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1l58iwm7j | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Which of the following elements is considered as a metalloid?</p> | [{"identifier": "A", "content": "Sc"}, {"identifier": "B", "content": "Pb"}, {"identifier": "C", "content": "Bi"}, {"identifier": "D", "content": "Te"}] | ["D"] | null | Sc, Pb, Bi are metals<br/><br/>
Te is a metalloid | mcq | jee-main-2022-online-26th-june-evening-shift | 2,966 |
1l6f72be0 | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Match List I with List II:</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;b... | [{"identifier": "A", "content": "A-II, B-III, C-IV, D-I"}, {"identifier": "B", "content": "A-IV, B-III, C-II, D-I"}, {"identifier": "C", "content": "A-III, B-II, C-I, D-IV"}, {"identifier": "D", "content": "A-III, B-II, C-IV, D-I"}] | ["C"] | null | Sodium arsinite - Herbicide
<br/><br/>
Nicotine - Pesticide
<br/><br/>
Sulphate - Laxative effect
<br/><br/>
Fluoride - Bending of bones | mcq | jee-main-2022-online-25th-july-evening-shift | 2,967 |
1l6jki5g8 | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Given below are two statements. One is labelled as Assertion A and the other is labelled as Reason R.</p>
<p>Assertion A : Activated charcoal adsorbs SO<sub>2</sub> more efficiently than CH<sub>4</sub>.</p>
<p>Reason R : Gases with lower critical temperatures are readily adsorbed by activated charcoal.</p>
<p>In the... | [{"identifier": "A", "content": "Both A and R are correct and R is the correct explanation of A."}, {"identifier": "B", "content": "Both A and R are correct but R is NOT the correct explanation of A."}, {"identifier": "C", "content": "A is correct but R is not correct."}, {"identifier": "D", "content": "A is not correc... | ["C"] | null | More polar gases easily adsorbs on activated charcoal.
<br/><br/>
And more polar gases has more (higher) critical temperature as compared to non-polar or less polar gases.
<br/><br/>
$\therefore$ Gases with higher critical temperature adsorbed more. | mcq | jee-main-2022-online-27th-july-morning-shift | 2,968 |
1ldwuzqem | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>$$\mathrm{K_2Cr_2O_7}$$ paper acidified with dilute $$\mathrm{H_2SO_4}$$ turns green when exposed to :</p> | [{"identifier": "A", "content": "Sulphur dioxide"}, {"identifier": "B", "content": "Sulphur trioxide"}, {"identifier": "C", "content": "Hydrogen sulphide"}, {"identifier": "D", "content": "Carbon dioxide"}] | ["A"] | null | $\mathrm{SO}_{2}$ gets oxidised in presence of $\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ and it converts to $\mathrm{Cr}^{+3}$ in presence of dil. $\mathrm{H}_{2} \mathrm{SO}_{4}$.
<br/><br/>
Similarly, $\mathrm{H}_{2} \mathrm{~S}$ can also get oxidized to sulphur.
<br/><br/>
However, most appropriate is (A) Sulp... | mcq | jee-main-2023-online-24th-january-evening-shift | 2,969 |
1lgsy0dph | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Which one of the following pairs is an example of polar molecular solids?</p> | [{"identifier": "A", "content": "$$\\mathrm{HCl}(\\mathrm{s}), \\mathrm{AlN}(\\mathrm{s})$$"}, {"identifier": "B", "content": "$$\\mathrm{MgO}(\\mathrm{s}), \\mathrm{SO}_{2}(\\mathrm{s})$$"}, {"identifier": "C", "content": "$$\\mathrm{SO}_{2}(\\mathrm{s}), \\mathrm{NH}_{3}(\\mathrm{s})$$"}, {"identifier": "D", "content... | ["C"] | null | <p>Polar molecular solids are formed by molecules that have polar covalent bonds and possess a net dipole moment. A net dipole moment arises when there is an asymmetric distribution of charge in the molecule, resulting in a separation of positive and negative charges.</p>
<p>Out of the given options, only option C cons... | mcq | jee-main-2023-online-11th-april-evening-shift | 2,971 |
lsbn0i1b | chemistry | p-block-elements | group-16-elements-(oxygen-family) | Among the following oxides of p-block elements, number of oxides having amphoteric nature is ________.<br/><br/>$\mathrm{Cl}_2 \mathrm{O}_7, \mathrm{CO}, \mathrm{PbO}_2, \mathrm{~N}_2 \mathrm{O}, \mathrm{NO}, \mathrm{Al}_2 \mathrm{O}_3, \mathrm{SiO}_2, \mathrm{~N}_2 \mathrm{O}_5, \mathrm{SnO}_2$ | [] | null | 3 | <p>An amphoteric oxide is one that displays both acidic and basic properties; such substances react with both acids and bases. In the p-block, several elements can form amphoteric oxides, particularly those elements that are metallic or metalloid in nature. It's essential to recognize which oxides among the provided li... | integer | jee-main-2024-online-1st-february-morning-shift | 2,972 |
jaoe38c1lscs2ec1 | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>1 mole of $$\mathrm{PbS}$$ is oxidised by "$$\mathrm{X}$$" moles of $$\mathrm{O}_3$$ to get "$$\mathrm{Y}$$" moles of $$\mathrm{O}_2$$. $$\mathrm{X}+\mathrm{Y}=$$ _________.</p> | [] | null | 8 | <p>$$\begin{aligned}
& \mathrm{PbS}+4 \mathrm{O}_3 \rightarrow \mathrm{PbSO}_4+4 \mathrm{O}_2 \\
& \mathrm{x}=4, \mathrm{y}=4
\end{aligned}$$</p> | integer | jee-main-2024-online-27th-january-evening-shift | 2,975 |
jaoe38c1lsd93acx | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Choose the correct statements from the following</p>
<p>A. All group 16 elements form oxides of general formula $$\mathrm{EO}_2$$ and $$\mathrm{EO}_3$$, where $$\mathrm{E}=\mathrm{S}, \mathrm{Se}, \mathrm{Te}$$ and $$\mathrm{Po}$$. Both the types of oxides are acidic in nature.</p>
<p>B. $$\mathrm{TeO}_2$$ is an oxi... | [{"identifier": "A", "content": "A and B only"}, {"identifier": "B", "content": "C and D only"}, {"identifier": "C", "content": "A and D only"}, {"identifier": "D", "content": "B and C only"}] | ["A"] | null | <p>(A) All group 16 elements form oxides of the $$\mathrm{EO}_2$$ and $$\mathrm{EO}_3$$ type where $$\mathrm{E}=\mathrm{S}, \mathrm{Se}, \mathrm{Te}$$ or $$\mathrm{Po}$$.</p>
<p>(B) $$\mathrm{SO}_2$$ is reducing while $$\mathrm{TeO}_2$$ is an oxidising agent.</p>
<p>(C) The reducing property increases from $$\mathrm{H}... | mcq | jee-main-2024-online-31st-january-evening-shift | 2,977 |
1lsg7hu98 | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>A and B formed in the following reactions are:</p>
<p>$$\begin{aligned}
& \mathrm{CrO}_2 \mathrm{Cl}_2+4 \mathrm{NaOH} \rightarrow \mathrm{A}+2 \mathrm{NaCl}+2 \mathrm{H}_2 \mathrm{O}, \\
& \mathrm{A}+2 \mathrm{HCl}+2 \mathrm{H}_2 \mathrm{O}_2 \rightarrow \mathrm{B}+3 \mathrm{H}_2 \mathrm{O}
\end{aligned}$$<... | [{"identifier": "A", "content": "$$\\mathrm{A}=\\mathrm{Na}_2 \\mathrm{Cr}_2 \\mathrm{O}_7, \\mathrm{~B}=\\mathrm{CrO}_5$$\n"}, {"identifier": "B", "content": "$$\\mathrm{A}=\\mathrm{Na}_2 \\mathrm{CrO}_4, \\mathrm{~B}=\\mathrm{CrO}_5$$\n"}, {"identifier": "C", "content": "$$\\mathrm{A}=\\mathrm{Na}_2 \\mathrm{Cr}_2 \\... | ["B"] | null | <p>$$\mathrm{Cr{O_2} + 4NaOH \to \mathop {N{a_2}Cr{O_4}}\limits_{(A)} + 2NaCl + 2{H_2}O}$$</p>
<p>$$\mathrm{N{a_2}Cr{O_4} + 2{H_2}{O_2} + 2HCl \to \mathop {Cr{O_5}}\limits_{(B)} + \mathop {2NaCl}\limits_{(Mis\sin g\,from\,balanced\,equation)} + 3{H_2}O}$$</p> | mcq | jee-main-2024-online-30th-january-evening-shift | 2,978 |
luy1mx0u | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Number of oxygen atoms present in chemical formula of fuming sulphuric acid is ___________.</p> | [] | null | 7 | <p>Fuming sulfuric acid, often known as oleum, can be represented chemically using the formula $ H_2S_2O_7 $. This compound is formed by adding excess sulfur trioxide ($ SO_3 $) to sulfuric acid ($ H_2SO_4 $). The chemical reaction can be represented as follows:</p>
<p>$ H_2SO_4 + SO_3 \rightarrow H_2S_2O_7 $</p>
<p>... | integer | jee-main-2024-online-9th-april-evening-shift | 2,980 |
luz2uzrj | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).</p>
<p>Assertion (A) : Both rhombic and monoclinic sulphur exist as $$\mathrm{S}_8$$ while oxygen exists as $$\mathrm{O}_2$$.</p>
<p>Reason (R) : Oxygen forms $$p \pi-p \pi$$ multiple bonds with itself and othe... | [{"identifier": "A", "content": "Both (A) and (R) are correct but (R) is not the correct explanation of (A)\n"}, {"identifier": "B", "content": "(A) is correct but (R) is not correct\n"}, {"identifier": "C", "content": "(A) is not correct but (R) is correct\n"}, {"identifier": "D", "content": "Both $$(\\mathbf{A})$$ an... | ["D"] | null | <p>Oxygen exists as $$\mathrm{O}_2$$</p>
<p>Sulphur exists as $$\mathrm{S}_8$$</p>
<p>Because of small size of oxygen, oxygen can form $$2 \mathrm{p}_\pi-2 \mathrm{p}_\pi$$ bond.</p>
<p>$$\Rightarrow$$ Assertion (A) is correct.</p>
<p>$$\Rightarrow$$ Reason (R) is correct.</p>
<p>Reason (R) is correct explanation of As... | mcq | jee-main-2024-online-9th-april-morning-shift | 2,981 |
luz2ux88 | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>On reaction of Lead Sulphide with dilute nitric acid which of the following is not formed?</p> | [{"identifier": "A", "content": "Sulphur\n"}, {"identifier": "B", "content": "Nitric oxide\n"}, {"identifier": "C", "content": "Lead nitrate\n"}, {"identifier": "D", "content": "Nitrous oxide"}] | ["D"] | null | <p>When lead sulphide (PbS) reacts with dilute nitric acid, the reaction is a redox process where lead sulphide is oxidized and nitric acid is reduced. The overall reaction involves the transformation of PbS and HNO<sub>3</sub> to form lead nitrate (Pb(NO<sub>3</sub>)<sub>2</sub>), sulphur, and nitrogen oxides, along w... | mcq | jee-main-2024-online-9th-april-morning-shift | 2,982 |
lv3xmazc | chemistry | p-block-elements | group-16-elements-(oxygen-family) | <p>Identify the correct statements about p-block elements and their compounds.</p>
<p>(A) Non metals have higher electronegativity than metals.</p>
<p>(B) Non metals have lower ionisation enthalpy than metals.</p>
<p>(C) Compounds formed between highly reactive nonmetals and highly reactive metals are generally ionic.<... | [{"identifier": "A", "content": "(B) and (D) only\n"}, {"identifier": "B", "content": "(B) and (E) only\n"}, {"identifier": "C", "content": "(D) and (E) only\n"}, {"identifier": "D", "content": "(A) and (C) only"}] | ["D"] | null | <p>Let's analyze each statement provided about p-block elements and determine their correctness:</p>
<p><strong>(A) Non metals have higher electronegativity than metals.</strong></p>
<p>This statement is correct. Non-metals, especially those in the upper right of the periodic table like fluorine, oxygen, and nitrogen,... | mcq | jee-main-2024-online-8th-april-evening-shift | 2,983 |
GXWI3vRQPRPREhET | chemistry | p-block-elements | group-17-elements-(halogen-family) | Oxidation number of Cl in CaOCl<sub>2</sub> (bleaching powder) is : | [{"identifier": "A", "content": "zero, since it contains Cl<sub>2</sub>"}, {"identifier": "B", "content": "-1, since it contains Cl<sup>-</sup>"}, {"identifier": "C", "content": "+1, since it contains ClO<sup>-</sup>"}, {"identifier": "D", "content": "+1 and -1 since it contains ClO<sup>-</sup> and Cl<sup>-</sup>"}] | ["D"] | null | $$CaOC{l_2} - $$or it can also be written as $$Ca\mathop {\left( {OCl} \right)}\limits_{{x_1}} \mathop {Cl}\limits_{{x_2}} $$
<br><br>hence oxidation no of $$Cl$$ in $$OC{l^ - }$$ is
<br><br>$$\eqalign{
& \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, - 2 + {x_2} = - 1 \cr
& \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,... | mcq | aieee-2002 | 2,984 |
KY82dAZgEvXWviOs | chemistry | p-block-elements | group-17-elements-(halogen-family) | The correct statement for the molecule, CsI<sub>3</sub> is : | [{"identifier": "A", "content": "it contains Cs<sup>3+</sup> and I<sup>-</sup> ions."}, {"identifier": "B", "content": "it contains Cs<sup>+</sup>, I<sup>-</sup> and lattice I<sub>2</sub> molecule."}, {"identifier": "C", "content": "it is a covalent molecule"}, {"identifier": "D", "content": "it contains Cs<sup>+</sup>... | ["D"] | null | $$Cs{l_3}\,\,$$ dissociates as
<br><br>$$Cs{l_3} \to C{s^ + } + I_3^ - $$ | mcq | jee-main-2014-offline | 2,985 |
pXwqIEIZisW3YuevRoBHt | chemistry | p-block-elements | group-17-elements-(halogen-family) | The non-metal that does <b>not</b> exhibit positive oxidation state is : | [{"identifier": "A", "content": "Oxygen"}, {"identifier": "B", "content": "Iodine"}, {"identifier": "C", "content": "Chlorine"}, {"identifier": "D", "content": "Fluorine"}] | ["D"] | null | Fluorine is the most electronegative element and it
shows only –1 oxidation state. | mcq | jee-main-2016-online-9th-april-morning-slot | 2,986 |
pmp5nPrrzoRq1nDAYsV10 | chemistry | p-block-elements | group-17-elements-(halogen-family) | Aqueous solution of which salt will not contain ions with the electronic
configuration 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup> ? | [{"identifier": "A", "content": "NaF"}, {"identifier": "B", "content": "NaCl"}, {"identifier": "C", "content": "KBr"}, {"identifier": "D", "content": "CaI<sub>2</sub>"}] | ["A"] | null | NaF is composed of Na<sup>+</sup>
and F<sup>–</sup>.
<br><br>Na<sup>+</sup> : 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>
<br><br>F<sup>-</sup> : 1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>
<br><br>Hence do not match with the configuration given in the question. | mcq | jee-main-2016-online-10th-april-morning-slot | 2,987 |
1l56xjz72 | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R.</p>
<p>Assertion A : Fluorine forms one oxoacid.</p>
<p>Reason R : Fluorine has smallest size amongst all halogens and is highly electronegative.</p>
<p>In the light of the above statements, choose the most appropr... | [{"identifier": "A", "content": "Both A and R are correct and R is the correct explanation of A."}, {"identifier": "B", "content": "Both A and R are correct but R is NOT the correct explanation of A."}, {"identifier": "C", "content": "A is correct but R is not correct."}, {"identifier": "D", "content": "A is not correc... | ["A"] | null | Due to its smaller size, fluorine forms only one oxoacid.<br/><br/>
Both the Assertion and Reason are correct and The reason is the correct explanation. | mcq | jee-main-2022-online-27th-june-evening-shift | 2,989 |
1ldo2rv99 | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>For electron gain enthalpies of the elements denoted as $$\Delta_{\mathrm{eg}} \mathrm{H}$$, the incorrect option is :</p> | [{"identifier": "A", "content": "$$\\Delta_{\\mathrm{eg}} \\mathrm{H}(\\mathrm{I})<\\Delta_{\\mathrm{eg}} \\mathrm{H}(\\mathrm{At})$$"}, {"identifier": "B", "content": "$$\\Delta_{\\mathrm{eg}} \\mathrm{H}(\\mathrm{Te})<\\Delta_{\\mathrm{eg}} \\mathrm{H}(\\mathrm{Po})$$"}, {"identifier": "C", "content": "$$\\Delta_{\\m... | ["C"] | null | $
\Delta \mathrm{H}_{\mathrm{eg}}(\mathrm{Cl})=-349 \mathrm{~kJ} / \text { mole } $
<br/><br/>$\Delta \mathrm{H}_{\mathrm{eg}}(\mathrm{F})=-333 \mathrm{~kJ} / \mathrm{mole} $<br/><br/>$
\Delta \mathrm{H}_{\mathrm{eg}}(\mathrm{I})=-296 \mathrm{~kJ} / \mathrm{mole} $<br/><br/>$
\Delta \mathrm{H}_{\mathrm{eg}}(\mathrm... | mcq | jee-main-2023-online-1st-february-evening-shift | 2,991 |
1lgyhrwmm | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>In the following reactions, the total number of oxygen atoms in X and Y is ___________.</p>
<p>Na$$_2$$O + H$$_2$$O $$\to$$ 2X</p>
<p>Cl$$_2$$O$$_7$$ + H$$_2$$O $$\to$$ 2Y</p> | [] | null | 5 | $$
\begin{aligned}
& \mathrm{Na}_2 \mathrm{O}+\mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{NaOH}(\mathrm{X}) \\\\
& \mathrm{Cl}_2 \mathrm{O}_7+\mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{HClO}_4(\mathrm{Y})
\end{aligned}
$$<br/><br/>
$X$ has one $O$ and $Y$ has four $O$ | integer | jee-main-2023-online-10th-april-morning-shift | 2,993 |
jaoe38c1lsc4tvpg | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>Element not showing variable oxidation state is :</p> | [{"identifier": "A", "content": "Bromine\n"}, {"identifier": "B", "content": "Iodine\n"}, {"identifier": "C", "content": "Chlorine\n"}, {"identifier": "D", "content": "Fluorine"}] | ["D"] | null | <p>Fluorine is the element among the options that does not exhibit a variable oxidation state, unlike its fellow halogens. This is because fluorine is the most electronegative element, and it always forms compounds in the oxidation state of -1 as it has a strong tendency to gain one electron to achieve a stable electro... | mcq | jee-main-2024-online-27th-january-morning-shift | 2,994 |
jaoe38c1lsfj8sve | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>Identify the incorrect pair from the following :</p> | [{"identifier": "A", "content": "Fluoroapatite $$-3 \\mathrm{Ca}_3\\left(\\mathrm{PO}_4\\right)_2 \\cdot \\mathrm{CaF}_2$$\n"}, {"identifier": "B", "content": "Carnallite $$-\\mathrm{KCl} \\cdot \\mathrm{MgCl}_2 \\cdot 6 \\mathrm{H}_2 \\mathrm{O}$$\n"}, {"identifier": "C", "content": "Cryolite $$-\\mathrm{Na}_3 \\mathr... | ["D"] | null | <p>(1) Fluorspar is $$\mathrm{CaF}_2$$</p> | mcq | jee-main-2024-online-29th-january-morning-shift | 2,995 |
1lsgy6q5x | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>The Lassiagne's extract is boiled with dil $$\mathrm{HNO}_3$$ before testing for halogens because,</p> | [{"identifier": "A", "content": "Silver halides are soluble in $$\\mathrm{HNO}_3$$.\n"}, {"identifier": "B", "content": "$$\\mathrm{AgCN}$$ is soluble in $$\\mathrm{HNO}_3$$.\n"}, {"identifier": "C", "content": "$$\\mathrm{Na}_2 \\mathrm{S}$$ and $$\\mathrm{NaCN}$$ are decomposed by $$\\mathrm{HNO}_3$$.\n"}, {"identifi... | ["C"] | null | <p>If nitrogen or sulphur is also present in the compound, the sodium fusion extract is first boiled with concentrated nitric acid to decompose cyanide or sulphide of sodium during Lassaigne's test</p> | mcq | jee-main-2024-online-30th-january-morning-shift | 2,996 |
lv5gt1te | chemistry | p-block-elements | group-17-elements-(halogen-family) | <p>Among the following halogens</p>
<p>$$\mathrm{F}_2, \mathrm{Cl}_2, \mathrm{Br}_2 \text { and } \mathrm{I}_2$$</p>
<p>Which can undergo disproportionation reactions?</p> | [{"identifier": "A", "content": "$$\\mathrm{F}_2$$ and $$\\mathrm{Cl}_2$$\n"}, {"identifier": "B", "content": "$$\\mathrm{Cl}_2, \\mathrm{Br}_2$$ and $$\\mathrm{I}_2$$\n"}, {"identifier": "C", "content": "Only $$\\mathrm{I}_2$$\n"}, {"identifier": "D", "content": "$$\\mathrm{F}_2, \\mathrm{Cl}_2$$ and $$\\mathrm{Br}_2$... | ["B"] | null | <p>To determine which halogens among $$\mathrm{F}_2, \mathrm{Cl}_2, \mathrm{Br}_2$$, and $$\mathrm{I}_2$$ can undergo disproportionation reactions, we need to understand what a disproportionation reaction is.</p>
<p>In a disproportionation reaction, a single substance is simultaneously oxidized and reduced, forming tw... | mcq | jee-main-2024-online-8th-april-morning-shift | 2,997 |
VpItfWawj53nnHJ9 | chemistry | p-block-elements | group-18-elements-(inert-or-noble-gases) | Which one the following statement regarding helium is incorrect? | [{"identifier": "A", "content": "It is used to fill gas balloons instead of hydrogen because it is lighter and non\u2013inflammable "}, {"identifier": "B", "content": "It is used in gas \u2013 cooled nuclear reactors"}, {"identifier": "C", "content": "It is used to produce and sustain powerful superconducting reagents ... | ["A"] | null | Helium is heavier than hydrogen although it is non-inflammable | mcq | aieee-2004 | 2,998 |
Ut5uj1dVpqLXtlWr | chemistry | p-block-elements | group-18-elements-(inert-or-noble-gases) | Which one has the highest boiling point? | [{"identifier": "A", "content": "Ne"}, {"identifier": "B", "content": "Kr"}, {"identifier": "C", "content": "Xe"}, {"identifier": "D", "content": "He"}] | ["C"] | null | $$Xe.$$ As we move down the group, the melting and boiling points show a regular increase due to corresponding increase in the magnitude of their van der waal forces of attraction as the size of the atom increases. | mcq | jee-main-2015-offline | 2,999 |
fEIuz17rr6XPqPBBuX2nZ | chemistry | p-block-elements | group-18-elements-(inert-or-noble-gases) | Which intermolecular force is most responsible in allowing xenon gas to liquefy? | [{"identifier": "A", "content": "Dipole - dipole"}, {"identifier": "B", "content": "Ion - dipole"}, {"identifier": "C", "content": "Instantaneous dipole - induced dipole"}, {"identifier": "D", "content": "Ionic"}] | ["C"] | null | Instantaneous dipole-induced dipole forces or van der Waals’ forces are most responsible in allowing xenon gas to
liquify.
| mcq | jee-main-2016-online-9th-april-morning-slot | 3,000 |
W50NsUwBBAgAFpPgKe3rsa0w2w9jx0u14hm | chemistry | p-block-elements | group-18-elements-(inert-or-noble-gases) | The noble gas that does not occur in the atmosphere is : | [{"identifier": "A", "content": "Ne"}, {"identifier": "B", "content": "He"}, {"identifier": "C", "content": "Kr"}, {"identifier": "D", "content": "Ra"}] | ["D"] | null | Inert gas Radon(Ra) is not present in atmosphere. Remaining all the inert gas can be found in the atmosphere. | mcq | jee-main-2019-online-10th-april-evening-slot | 3,001 |
jaoe38c1lse755kb | chemistry | p-block-elements | group-18-elements-(inert-or-noble-gases) | <p>Give below are two statements:</p>
<p>Statement - I: Noble gases have very high boiling points.</p>
<p>Statement - II: Noble gases are monoatomic gases. They are held together by strong dispersion forces. Because of this they are liquefied at very low temperature. Hence, they have very high boiling points.</p>
<p>In... | [{"identifier": "A", "content": "Both Statement I and Statement II are false.\n"}, {"identifier": "B", "content": "Statement I is true but Statement II is false.\n"}, {"identifier": "C", "content": "Statement I is false but Statement II is true.\n"}, {"identifier": "D", "content": "Both Statement I and Statement II are... | ["A"] | null | <p><strong>Option A</strong> is the correct answer. Both Statement I and Statement II are false.</p>
<p>Noble gases actually have <strong>low boiling points</strong>, not high. This is because noble gases are indeed monoatomic gases that exist as single atoms. They have a completely filled valence shell and do not easi... | mcq | jee-main-2024-online-31st-january-morning-shift | 3,002 |
1LuevMRepxZ1WOcw | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | $$C{e^{ + 3}},\,\,L{a^{ + 3}},\,\,P{m^{ + 3}}\,\,$$ and $$Y{b^{ + 3}}\,\,$$ have ionic radial in the increasing order as | [{"identifier": "A", "content": "$$L{a^{ + 3}}\\,\\, < C{e^{ + 3}}\\,\\, < P{m^{ + 3}}\\,\\, < Y{b^{ + 3}}$$ "}, {"identifier": "B", "content": "$$Y{b^{ + 3}}\\,\\, < P{m^{ + 3}}\\,\\, < C{e^{ + 3}}\\,<\\,L{a^{ + 3}}$$ "}, {"identifier": "C", "content": "$$L{a^{ + 3}}\\,\\, = C{e^{ + 3}}\\,\\, < P{... | ["B"] | null | <img class="question-image" src="https://gateclass.static.cdn.examgoal.net/Ya3EoPx4umoN1Nqtf/k7nY8Lv0VSxN9NTDF2aG3JAEqZlUx/hwpzI4iETT58dbwvZHk1BL/uploadfile.jpg" loading="lazy" alt="AIEEE 2002 Chemistry - Periodic Table & Periodicity Question 116 English Explanation">
<br>Here $$C{e^{ + 3}},\,\,P{m^{ + 3}},\,\,Y{b^... | mcq | aieee-2002 | 3,004 |
WaYwgdseGSFeCX4V | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | Which one of the following ions has the highest value of ionic radius? | [{"identifier": "A", "content": "O<sup>2-</sup>"}, {"identifier": "B", "content": "B<sup>3+</sup>"}, {"identifier": "C", "content": "Li<sup>+</sup>"}, {"identifier": "D", "content": "F<sup>-</sup>"}] | ["A"] | null | From a neutral atom where a electron is removed then it become cation and when a electron is added to the atom then it becomes anion.
<br><br>For a atom $$x$$ when it loose a electron then it becomes cation $$x - {e^ - } \to {x^ + }$$
<br><br>Let atomic no. of $$x$$ is $$z$$
<br><br>then no. of proton in $${x^ + } = z$... | mcq | aieee-2004 | 3,006 |
MBshRPbtzuPwmK3h | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The increasing order of the ionic radii of the given isoelectronic species is : | [{"identifier": "A", "content": "Cl<sup>\u2013</sup>, Ca<sup>2+</sup> , K<sup>+</sup> , S<sup>2\u2013</sup>"}, {"identifier": "B", "content": "S<sup>2\u2013</sup>, Cl<sup>\u2013</sup>, Ca<sup>2+</sup> , K<sup>+</sup>"}, {"identifier": "C", "content": "Ca<sup>2+</sup> , K<sup>+</sup> , Cl<sup>\u2013</sup> , S<sup>2\u201... | ["C"] | null | <p>Iso-electronic ions have same number of electrons. So, for iso-electronic ions, number of electrons = constant.
<br/>$$ \therefore $$ $$\sigma $$(Slaten's Constant) = Constant. As $$\sigma $$ depends on number of electrons. If a element's number of electrons increases then that element's $$\sigma $$ increases.</p>
... | mcq | aieee-2012 | 3,009 |
mon03lcV7SBvYiyy | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The ionic radii (in Å) of N<sup>3–</sup>, O<sup>2–</sup> and F<sup>–</sup> are respectively: | [{"identifier": "A", "content": "1.36, 1.71 and 1.40"}, {"identifier": "B", "content": "1.71, 1.40 and 1.36"}, {"identifier": "C", "content": "1.71, 1.36 and 1.40"}, {"identifier": "D", "content": "1.36, 1.40 and 1.71"}] | ["B"] | null | Here all of them are isoelectric and for isoelectric species size of anion increases as negative charge increases.
<br><br>So, correct order is :
<br><br>N<sup>3–</sup> > O<sup>2–</sup> > F<sup>–</sup>
<br><br>$$ \therefore $$ Radius of N<sup>3–</sup> = 1.71 Å
<br><br>and Radius of
O<sup>2–</sup> = 1.40 Å
<br><b... | mcq | jee-main-2015-offline | 3,010 |
FIPtNdY8hkCMpNOBONkFM | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The correct order of the atomic radii of C, Cs, Al, and S is : | [{"identifier": "A", "content": "S < C < Al < Cs "}, {"identifier": "B", "content": "S < C < Cs < Al"}, {"identifier": "C", "content": "C < S < Al < Cs "}, {"identifier": "D", "content": "C < S < Cs < Al \n"}] | ["C"] | null | Atomic radii increase by moving down the group and
decrease across a period. <br><br>Hence, the correct order of atomic
radii is : C < S < Al < Cs. | mcq | jee-main-2019-online-11th-january-morning-slot | 3,012 |
a4s1MRUaAsAzEitw5Tjgy2xukfp2zk7a | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The correct order of the ionic radii of<br/> O<sup>2–</sup>, N<sup>3–</sup>, F<sup>–</sup>
, Mg<sup>2+</sup>, Na<sup>+</sup> and Al<sup>3+</sup> is : | [{"identifier": "A", "content": "N<sup>3\u2013</sup> < O<sup>2\u2013</sup> < F<sup>\u2013</sup>\n < Na<sup>+</sup> < Mg<sup>2+</sup> < Al<sup>3+</sup>"}, {"identifier": "B", "content": "N<sup>3\u2013</sup> < F<sup>\u2013</sup>\n < O<sup>2\u2013</sup> < Mg<sup>2+</sup> < Na<sup>+</sup> < Al... | ["D"] | null | For isoelectronic species, as the no. of protons
increases, size of ions decreases.
<br><br>$$ \therefore $$ Correct order of size for isoelectronic species
<br><br>Al<sup>3+</sup> < Mg<sup>2+</sup> < Na<sup>+</sup> < F<sup>–</sup>
< O<sup>2–</sup> < N<sup>3–</sup> | mcq | jee-main-2020-online-5th-september-evening-slot | 3,013 |
LcSov41YJlz8ZZIt3Hjgy2xukf93pib6 | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The ionic radii of O<sup>2–</sup>, F<sup>–</sup>, Na<sup>+</sup> and Mg<sup>2+</sup> are in
the order : | [{"identifier": "A", "content": "F<sup>\u2013</sup> > O<sup>2\u2013</sup> > Na<sup>+</sup> > Mg<sup>2+</sup>"}, {"identifier": "B", "content": "Mg<sup>2+</sup> > Na<sup>+</sup> > F<sup>\u2013</sup> > O<sup>2\u2013</sup>"}, {"identifier": "C", "content": "O<sup>2\u2013</sup> > F<sup>\u2013</sup> >... | ["D"] | null | Among isoelectronic species, greater the Z<sub>eff</sub>
smaller will be the radius.
<br><br>Order of Z<sub>eff</sub> : Mg<sup>2+</sup> > Na<sup>+</sup> > F<sup>–</sup> > O<sup>2–</sup>
<br><br>Order of Ionic Radii : O<sup>2–</sup> > F<sup>–</sup> > Na<sup>+</sup> > Mg<sup>2+</sup> | mcq | jee-main-2020-online-4th-september-morning-slot | 3,014 |
sIztGaiqvF5GydHqwh7k9k2k5hl6qft | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The increasing order of the atomic radii of the
following elements is :-<br/>
(a) C (b) O<br/> (c) F (d) Cl<br/>
(e) Br | [{"identifier": "A", "content": "(a) < (b) < (c) < (d) < (e)"}, {"identifier": "B", "content": "(c) < (b) < (a) < (d) < (e)"}, {"identifier": "C", "content": "(b) < (c) < (d) < (a) < (e)"}, {"identifier": "D", "content": "(d) < (c) < (b) < (a) < (e)"}] | ["B"] | null | Generally in a period Left to Right Atomic radius decrease.
<br><br>In a Group Top to Bottom Atomic radius increase.
<br><br>Atomic radius order : Br > Cl > C > O > F | mcq | jee-main-2020-online-8th-january-evening-slot | 3,015 |
trsye3E6Ydxm0hUECg1kmlm9w9n | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The ionic radius of Na<sup>+</sup> ions is 1.02 $$\mathop A\limits^o $$. The ionic radii (in $$\mathop A\limits^o $$) of Mg<sup>2+</sup> and Al<sup>3+</sup>, respectively, are | [{"identifier": "A", "content": "1.05 and 0.99"}, {"identifier": "B", "content": "0.72 and 0.54"}, {"identifier": "C", "content": "0.85 and 0.99"}, {"identifier": "D", "content": "0.68 and 0.72"}] | ["B"] | null | <p>The ionic radii (in $$\mathop A\limits^o $$) of $$\text{Mg}^{2+}$$ and $$\text{Al}^{3+}$$, respectively, are:</p>
<p><strong>Option B</strong>:</p>
<p><p>$$0.72 \mathop A\limits^o$$ for $$\text{Mg}^{2+}$$</p></p>
<p><p>$$0.54 \mathop A\limits^o$$ for $$\text{Al}^{3+}$$</p></p>
| mcq | jee-main-2021-online-18th-march-morning-shift | 3,016 |
1krusl2pj | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The ionic radii of K<sup>+</sup>, Na<sup>+</sup>, Al<sup>3+</sup> and Mg<sup>2+</sup> are in the order: | [{"identifier": "A", "content": "Na<sup>+</sup> < K<sup>+</sup> < Mg<sup>2+</sup> < Al<sup>3+</sup>"}, {"identifier": "B", "content": "Al<sup>3+</sup> < Mg<sup>2+</sup> < K<sup>+</sup> < Na<sup>+</sup>"}, {"identifier": "C", "content": "Al<sup>3+</sup> < Mg<sup>2+</sup> < Na<sup>+</sup> < K<s... | ["C"] | null | Al<sup>3+</sup>, Mg<sup>2+</sup> and Na<sup>+</sup> are isoelectronic ionic species. For monoatomic ionic isoelectronic species as positive charge increases ionic size decreases.<br><br>The order of size of Na<sup>+</sup> & K<sup>+</sup> is Na<sup>+</sup> < K<sup>+</sup><br><br>$$\therefore$$ Order of ionic radi... | mcq | jee-main-2021-online-25th-july-morning-shift | 3,017 |
1ktcoupty | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | Given below are two statements : one is labelled as Assertion (A) and the other is labelled as Reason (R).<br/><br/>Assertion (A) : Barium carbonate is insoluble in water and is highly stable.<br/><br/>Reason (R) : The thermal stability of the carbonates increases with increasing cationic size. | [{"identifier": "A", "content": "Both (A) and (R) are true and (R) is the true explanation of (A)"}, {"identifier": "B", "content": "(A) is true but (R) is false"}, {"identifier": "C", "content": "Both (A) and (R) are true but (R) is not the true explanation of (A)"}, {"identifier": "D", "content": "(A) is false but (R... | ["A"] | null | In IIA group on moving down the group size of cation increases and show thermal stability of carbonate increases. | mcq | jee-main-2021-online-26th-august-evening-shift | 3,019 |
1ktfs8ty7 | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | The correct order of ionic radii for the ions, P<sup>3$$-$$</sup>, S<sup>2$$-$$</sup>, Ca<sup>2+</sup>, K<sup>+</sup>, Cl<sup>$$-$$</sup> is : | [{"identifier": "A", "content": "P<sup>3$$-$$</sup> > S<sup>2$$-$$</sup> > Cl<sup>$$-$$</sup> > K<sup>+</sup> > Ca<sup>2+</sup>"}, {"identifier": "B", "content": "Cl<sup>$$-$$</sup> > S<sup>2$$-$$</sup> > P<sup>3$$-$$</sup> > Ca<sup>2+</sup> > K<sup>+</sup>"}, {"identifier": "C", "content": "P<s... | ["A"] | null | P<sup>3$$-$$</sup> > S<sup>2$$-$$</sup> > Cl<sup>$$-$$</sup> > K<sup>+</sup> > Ca<sup>2+</sup> (Correct order of ionic radii)<br><br>all the given species are isoelectronic species. In isoelectronic species size increases with increase of negative charge and size decreases with increase in positive charge. | mcq | jee-main-2021-online-27th-august-evening-shift | 3,020 |
1l56wx7p2 | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>The correct order of increasing ionic radii is</p> | [{"identifier": "A", "content": "Mg<sup>2+</sup> < Na<sup>+</sup> < F<sup>$$-$$</sup> < O<sup>2$$-$$</sup> < N<sup>3$$-$$</sup>"}, {"identifier": "B", "content": "N<sup>3$$-$$</sup> < O<sup>2$$-$$</sup> < F<sup>$$-$$</sup> < Na<sup>+</sup> < Mg<sup>2+</sup>"}, {"identifier": "C", "content": "F<sup>$$-$$</sup> < Na<sup>... | ["A"] | null | For isoelectronic species<br/><br/>
Ionic radii $$\propto \frac{(-) \text { ve charge }}{(+) \text { ve charge }}$$<br/><br/>
Hence, correct order of ionic radii is<br/><br/>
Mg<sup>2+</sup> < Na<sup>+</sup> < F<sup>–</sup> < O<sup>2–</sup> < N<sup>3–</sup> | mcq | jee-main-2022-online-27th-june-evening-shift | 3,021 |
1l6gpsf7v | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>Given two statements below :</p>
<p>Statement I : In $$\mathrm{Cl}_{2}$$ molecule the covalent radius is double of the atomic radius of chlorine.</p>
<p>Statement II : Radius of anionic species is always greater than their parent atomic radius.</p>
<p>Choose the most appropriate answer from options given below :</p> | [{"identifier": "A", "content": "Both Statement I and Statement II are correct."}, {"identifier": "B", "content": "Both Statement I and Statement II are incorrect."}, {"identifier": "C", "content": "Statement I is correct but Statement II is incorrect."}, {"identifier": "D", "content": "Statement I is incorrect but Sta... | ["D"] | null | <p>The given statements pertain to the concepts of atomic and ionic radii in chemical bonding and periodic properties. Let's analyze each statement individually for clarity.</p>
<p><strong>Statement I: </strong>In $$\mathrm{Cl}_{2}$$ molecule the covalent radius is double of the atomic radius of chlorine.</p>
<p>The a... | mcq | jee-main-2022-online-26th-july-morning-shift | 3,023 |
1ldpofadj | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>The correct increasing order of the ionic radii is</p> | [{"identifier": "A", "content": "$$\\mathrm{Cl^- < Ca^{2+} < K^+ < S^{2-}}$$"}, {"identifier": "B", "content": "$$\\mathrm{K^+ < S^{2-} < Ca^{2+} < Cl^-}$$"}, {"identifier": "C", "content": "$$\\mathrm{Ca^{2+} < K^+ < Cl^- < S^{2-}}$$"}, {"identifier": "D", "content": "$$\\mathrm{S^{2-} < Cl^- < Ca^{2+} < K^+}$$"}] | ["C"] | null | In isoelectronic species size $\propto \frac{1}{Z}$
<br/><br/>$$
\mathrm{Ca}^{2+}<\mathrm{K}^{+}<\mathrm{Cl}^{-}<\mathrm{S}^{2-} \text { : Size }
$$
<br/><br/>$\begin{array}{lllll}Z: & 20 & 19 & 17 & 18\end{array}$ | mcq | jee-main-2023-online-31st-january-morning-shift | 3,024 |
jaoe38c1lsd9kj89 | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>Consider the following elements.</p>
<p><img src="data:image/png;base64,UklGRmIUAABXRUJQVlA4IFYUAACQdwCdASoAA74APm00l0ikIqKhItBaAIANiWlu4XKRG/Nj8if5Ltf/x3S+erPb/lCxQfjf3O/if3r3Dfx3+38F/V/6hH5R/Qv9HvO4APzz+xf8LwrNSzIA4K6gJ/Rv8r6JGff6w9hby3/YZ+843Qec8o5J3dEOZj6yyVoPOeUck7u7u7u7u7u7uh9oIeXeP+L223q69EbY3VNprSVpyfrx+CAUS... | [{"identifier": "A", "content": "A only"}, {"identifier": "B", "content": "B, C and D only"}, {"identifier": "C", "content": "A and B only"}, {"identifier": "D", "content": "A, B and D only"}] | ["D"] | null | <p>In general along the period from left to right, size decreases and metallic character decrease.</p>
<p>In general down the group, size increases and metallic character increases.</p>
<p>$$\begin{aligned}
& \mathrm{B}^{\prime}<\mathrm{A}^{\prime}(\text { size }) \quad \mathrm{C}^{\prime}>\mathrm{A}^{\prime}(\text { s... | mcq | jee-main-2024-online-31st-january-evening-shift | 3,025 |
lv7v3u1a | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>The statement(s) that are correct about the species $$\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{Na}^{+}$$ and $$\mathrm{Mg}^{2+}$$.</p>
<p>(A) All are isoelectronic</p>
<p>(B) All have the same nuclear charge</p>
<p>(C) $$\mathrm{O}^{2-}$$ has the largest ionic radii</p>
<p>(D) $$\mathrm{Mg}^{2+}$$ has the smallest i... | [{"identifier": "A", "content": "(C) and (D) only\n"}, {"identifier": "B", "content": "(A), (C) and (D) only\n"}, {"identifier": "C", "content": "(B), (C) and (D) only\n"}, {"identifier": "D", "content": "(A), (B), (C) and (D)"}] | ["B"] | null | <p>To answer this question, let's address each statement individually.</p>
<p><strong>(A) All are isoelectronic</strong></p>
<p>An isoelectronic species is a group of ions or atoms which have the same number of electrons. The electron configuration for each species is as follows:</p>
<ul>
<li>$$\mathrm{O}^{2-}$$: O... | mcq | jee-main-2024-online-5th-april-morning-shift | 3,026 |
lv9s2pz5 | chemistry | periodic-table-and-periodicity | atomic-and-ionic-radius | <p>Given below are two statements :</p>
<p>Statement I : The metallic radius of $$\mathrm{Na}$$ is $$1.86 \mathrm{~A}^{\circ}$$ and the ionic radius of $$\mathrm{Na}^{+}$$ is lesser than $$1.86 \mathrm{~A}^{\circ}$$</p>
<p>Statement II : Ions are always smaller in size than the corresponding elements.</p>
<p>In the lig... | [{"identifier": "A", "content": "Both Statement I and Statement II are true\n"}, {"identifier": "B", "content": "Statement I is incorrect but Statement II is true\n"}, {"identifier": "C", "content": "Both Statement I and Statement II are false\n"}, {"identifier": "D", "content": "Statement I is correct but Statement II... | ["D"] | null | <p>To determine the correctness of the given statements, let's analyze each one individually based on atomic and ionic radii concepts.</p>
<hr />
<h3><strong>Statement I:</strong></h3>
<p><strong>The metallic radius of $\mathrm{Na}$ is $1.86\, \text{Å}$ and the ionic radius of $\mathrm{Na}^+$ is lesser than $1.86\, \te... | mcq | jee-main-2024-online-5th-april-evening-shift | 3,027 |
eso2oclGrXSeMCidWb1LU | chemistry | periodic-table-and-periodicity | effective-nuclear-charge | The size of the iso-electronic species Cl<sup>–</sup>, Ar and Ca<sup>2+</sup> is affected by : | [{"identifier": "A", "content": "electron-electron interaction in the outer orbitals"}, {"identifier": "B", "content": "Principal quantum number of valence shell"}, {"identifier": "C", "content": "nuclear charge"}, {"identifier": "D", "content": "azimuthal quantum number of valence shell"}] | ["C"] | null | <table class="tg">
<tbody><tr>
<th class="tg-nrix"></th>
<th class="tg-nrix">Cl<sup>-</sup></th>
<th class="tg-nrix">Ar</th>
<th class="tg-nrix">Ca<sup>+2</sup></th>
</tr>
<tr>
<td class="tg-nrix">Protons</td>
<td class="tg-nrix">17</td>
<td class="tg-nrix">18</td>
<td class="tg-nr... | mcq | jee-main-2019-online-8th-april-morning-slot | 3,028 |
kwJYsjrMpmHiDMjZf83rsa0w2w9jx80b28u | chemistry | periodic-table-and-periodicity | effective-nuclear-charge | Among the following, the energy of 2s orbital is lowest in : | [{"identifier": "A", "content": "Li"}, {"identifier": "B", "content": "H"}, {"identifier": "C", "content": "Na"}, {"identifier": "D", "content": "K"}] | ["D"] | null | Here Z of K = 15, Na = 11, H = 1, Li = 3.
<br><br>In K, because of more number of protons (high atomic
number) the 2s electron experiences a higher effective nuclear
charge and is closer to nucleus, thus having less energy | mcq | jee-main-2019-online-12th-april-evening-slot | 3,029 |
34hIZ7U2TMLlH4Gj | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | In which of the following arrangements the order is NOT according to the property
indicated against it? | [{"identifier": "A", "content": "Li < Na < K < Rb Increasing metallic radius"}, {"identifier": "B", "content": "I < Br < F < Cl Increasing electron gain enthalpy (with negative sign) "}, {"identifier": "C", "content": "B < C < N < O Increasing first ionization enthalpy"}, {"identifier": "D", ... | ["C"] | null | $$\left( a \right)\,\,\,\,\,$$It is True.
<br><br>Here $$Li, Na, K$$ and $$Rb$$ all are belongs to the same group, so their effective nuclear charge is same but in a group from top to bottom the no. of shells increase in a atom. So the radius of atom increases.
<br><br>$$\left( b \right)\,\,\,\,\,$$ It is True.
<br... | mcq | aieee-2005 | 3,030 |
TmgEqBkT5dQNbcARJZ4nf | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | The correct order of electron affinity is : | [{"identifier": "A", "content": "F > Cl > O"}, {"identifier": "B", "content": "F > O > Cl"}, {"identifier": "C", "content": "Cl > F > O"}, {"identifier": "D", "content": "O > F > Cl"}] | ["C"] | null | Electron affinity means tendency of gaining an electron by an atom.
<br><br>In a period from left ot right the electron affinity increases and in a group it decreases from top to bottom.
<br><br>So according to this theory Fluorine(F) should have most electron affinity. But when an electron is added to the F atom, elec... | mcq | jee-main-2018-online-15th-april-evening-slot | 3,031 |
xGTiBQSTwqlHk9EiI3sKk | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | When the first electron gain enthalpy $$\left( {{\Delta _{eg}}H} \right)$$ of oxygen is $$-$$ 141 kJ/mol, its second electron gain enthalpy is : | [{"identifier": "A", "content": "a more negative value than the first"}, {"identifier": "B", "content": "almost the same as that of the first"}, {"identifier": "C", "content": "negative, but less negative than the first"}, {"identifier": "D", "content": "a positive value"}] | ["D"] | null | Second electron gain enthalpy is always positive for every element.
<br>O<sup>$$-$$</sup><sub>(g)</sub> + e<sup>$$-$$</sup> $$ \to $$ O<sup>$$-$$2</sup><sub>(g)</sub> ; $$\Delta $$H = positive | mcq | jee-main-2019-online-9th-january-evening-slot | 3,032 |
bymMlZOak3pTMyxTzM7k9k2k5dz3vg6 | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | The electron gain enthalpy (in KJ/mol) of fluorine, chlorine, bromine and iodine, respectively are: | [{"identifier": "A", "content": "-296, -325, -333 and -349"}, {"identifier": "B", "content": "349, -333, -325 and -296 "}, {"identifier": "C", "content": "-333, -349, -325 and -296"}, {"identifier": "D", "content": "-333, -325, -349 and -296\n"}] | ["C"] | null | Order of electron gain enthalpy (magnitude) is
Cl > F > Br > I
<br><br><b>Note:</b> Electron gain enthalpy increases with electro negativity but chlorine has higher electron gain enthalpy than
fluorine (exception). | mcq | jee-main-2020-online-7th-january-morning-slot | 3,033 |
hZFvmUgreGYpgoXGSz7k9k2k5eq0i7i | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | Within each pair of elements F & Cl, S & Se, and Li & Na, respectively, the elements that release
more energy upon and electron gain are : | [{"identifier": "A", "content": "F, S and Li"}, {"identifier": "B", "content": "Cl, Se and Na"}, {"identifier": "C", "content": "Cl, S and Li "}, {"identifier": "D", "content": "F, Se and Na"}] | ["C"] | null | Electron affinity of second period p-block
element is less than third period p-block element
due to small size of second period p-block element.
<br><br>$$ \therefore $$ Electron affinity order : F $$<$$ Cl
<br><br>Down the group electron affinity decreases due
to size increases.
<br><br>$$ \therefore $$ Electron af... | mcq | jee-main-2020-online-7th-january-evening-slot | 3,034 |
d3hIRdXrR1rAdv98XH1klusfda4 | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | The correct order of electron gain enthalpy is : | [{"identifier": "A", "content": "Te > Se > S > O"}, {"identifier": "B", "content": "S > Se > Te > O"}, {"identifier": "C", "content": "S > O > Se > Te"}, {"identifier": "D", "content": "O > S > Se > Te"}] | ["B"] | null | Oxygen is the second most electronegative element in comparison to fluorine. In group - 16 family $(\mathrm{O}, \mathrm{S}, \mathrm{Se}, \mathrm{Te})$, O-atom is smallest in size. So, electron density on O-atom is very high in group -16
During addition of a free electron to gaseous $\mathrm{O}$-atom,<br/><br/>
$$
\math... | mcq | jee-main-2021-online-26th-february-evening-slot | 3,035 |
5MXK0IIzT59kN5CVrU1kmj67h8f | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | The absolute value of the electron gain enthalpy of halogens satisfies : | [{"identifier": "A", "content": "Cl > Br > F > I"}, {"identifier": "B", "content": "Cl > F > Br > I"}, {"identifier": "C", "content": "I > Br > Cl > F"}, {"identifier": "D", "content": "F > Cl > Br > I"}] | ["B"] | null | The magnitude of electron gain enthalpy of halogen
atoms down the group show abnormal behavior.
The |ΔH<sub>eg</sub>| of F is lower than that of Cl due to its
smaller size. The incoming electron experiences
higher repulsive force due to valence electrons of
F than Cl. The correct order is Cl > F > Br > I. | mcq | jee-main-2021-online-17th-march-morning-shift | 3,036 |
1l59qpre3 | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>The correct order of electron gain enthalpies of Cl, F, Te and Po is</p> | [{"identifier": "A", "content": "F < Cl < Te < Po"}, {"identifier": "B", "content": "Po < Te < F < Cl"}, {"identifier": "C", "content": "Te < Po < Cl < F"}, {"identifier": "D", "content": "Cl < F < Te < Po"}] | ["B"] | null | Te → –190 kJ mol<sup>–1</sup><br/><br/>
Po → –174 kJ mol<sup>–1</sup><br/><br/>
F → –333 kJ mol<sup>–1</sup><br/><br/>
Cl → –349 kJ mol<sup>–1</sup><br/><br/>
Hence, correct order is Cl > F > Te > Po | mcq | jee-main-2022-online-25th-june-evening-shift | 3,038 |
1l6mcidmt | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>In which of the following pairs, electron gain enthalpies of constituent elements are nearly the same or identical?</p>
<p>(A) Rb and Cs</p>
<p>(B) Na and K</p>
<p>(C) Ar and Kr</p>
<p>(D) I and At</p>
<p>Choose the correct answer from the options given below :</p> | [{"identifier": "A", "content": "(A) and (B) only"}, {"identifier": "B", "content": "(B) and (C) only"}, {"identifier": "C", "content": "(A) and (C) only"}, {"identifier": "D", "content": "(C) and (D) only"}] | ["C"] | null | $\mathrm{Rb} \,\& \,\mathrm{Cs}$ have nearly same electron gain enthalpy electron gain enthalpy $=-46\, \mathrm{kj} / \mathrm{ml}$<br/><br/>
Ar & Kr have same $\Delta \mathrm{H}_{\mathrm{eq}} .$ Value is $+96 \,\mathrm{kj} / \mathrm{ml}$ | mcq | jee-main-2022-online-28th-july-morning-shift | 3,040 |
1lh28surs | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>The difference between electron gain enthalpies will be maximum between :</p> | [{"identifier": "A", "content": "Ar and Cl"}, {"identifier": "B", "content": "Ne and Cl"}, {"identifier": "C", "content": "Ne and F"}, {"identifier": "D", "content": "Ar and F"}] | ["B"] | null | $\Delta \mathrm{H}_{\mathrm{eg}}$ for chlorine $=-349 \mathrm{~kJ} \mathrm{~mole}^{-1}$<br/><br/>
$\Delta \mathrm{H}_{\mathrm{eg}}$ for Neon $=+116 \mathrm{~kJ} \mathrm{~mole}^{-1}$ | mcq | jee-main-2023-online-6th-april-morning-shift | 3,042 |
jaoe38c1lsfmk12q | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>Given below are two statements:</p>
<p>Statement I : Fluorine has most negative electron gain enthalpy in its group.</p>
<p>Statement II : Oxygen has least negative electron gain enthalpy in its group.</p>
<p>In the light of the above statements, choose the most appropriate from the options given below</p> | [{"identifier": "A", "content": "Both Statement I and Statement II are true\n"}, {"identifier": "B", "content": "Both Statement I and Statement II are false\n"}, {"identifier": "C", "content": "Statement I is false but Statement II is true\n"}, {"identifier": "D", "content": "Statement I is true but Statement II is fal... | ["C"] | null | <p>Statement- 1 is false because chlorine has most negative electron gain enthalpy in its group.</p> | mcq | jee-main-2024-online-29th-january-evening-shift | 3,044 |
luz2usqx | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>Given below are two statements :</p>
<p>Statement (I) : The oxidation state of an element in a particular compound is the charge acquired by its atom on the basis of electron gain enthalpy consideration from other atoms in the molecule.</p>
<p>Statement (II) : $$\mathrm{p} \pi-\mathrm{p} \pi$$ bond formation is more... | [{"identifier": "A", "content": "Statement I is correct but Statement II is incorrect\n"}, {"identifier": "B", "content": "Both Statement I and Statement II are correct\n"}, {"identifier": "C", "content": "Statement I is incorrect but Statement II is correct\n"}, {"identifier": "D", "content": "Both Statement I and Sta... | ["C"] | null | <p>To evaluate the given statements, we need to consider the concepts of oxidation states and bonding tendencies across different periods in the periodic table.</p>
<p>Statement (I) describes the oxidation state of an element in a compound as the hypothetical charge an atom would have if all bonds to atoms of differen... | mcq | jee-main-2024-online-9th-april-morning-shift | 3,045 |
lvc584o4 | chemistry | periodic-table-and-periodicity | electron-gain-enthalpy | <p>The electron affinity value are negative for</p>
<p>A. $$\mathrm{Be} \rightarrow \mathrm{Be}^{-}$$</p>
<p>B. $$\mathrm{N} \rightarrow \mathrm{N}^{-}$$</p>
<p>C. $$\mathrm{O} \rightarrow \mathrm{O}^{2-}$$</p>
<p>D. $$\mathrm{Na} \rightarrow \mathrm{Na}^{-}$$</p>
<p>E. $$\mathrm{Al} \rightarrow \mathrm{Al}^{-}$$</p>
<... | [{"identifier": "A", "content": "A, B, D and E only\n"}, {"identifier": "B", "content": "D and E only\n"}, {"identifier": "C", "content": "A and D only\n"}, {"identifier": "D", "content": "A, B and C only"}] | ["D"] | null | <p>To determine which elements have <strong>negative electron affinity values</strong>, we'll analyze each option individually.</p>
<h3>Understanding Electron Affinity</h3>
<p><p><strong>Electron Affinity (EA):</strong> The energy change when an electron is added to a neutral atom in the gas phase to form a negative i... | mcq | jee-main-2024-online-6th-april-morning-shift | 3,046 |
czSLorwmhSeJucEt | chemistry | periodic-table-and-periodicity | electronegativity | The formation of the oxide ion O<sup>2-</sup>(g) requires first an exothermic and then an endothermic
step as shown below <br/><br/>
O<sub>(g)</sub> + e<sup>-</sup> = $$O_{(g)}^{-}$$ $$\Delta $$H<sup>o</sup> = -142 kJmol<sup>-1</sup><br/><br/>
$$O_{(g)}^{-}$$ + e<sup>-</sup> = $$O_{(g)}^{2-}$$ $$\Delta $$H<sup>o</sup>... | [{"identifier": "A", "content": "O<sup>-</sup> ion will tend to resist the addition of another electron "}, {"identifier": "B", "content": "Oxygen has high electron affinity"}, {"identifier": "C", "content": "Oxygen is more electronegative "}, {"identifier": "D", "content": "O<sup>-</sup> ion has comparatively larger s... | ["A"] | null | $$O$$ atom is highly electronegative so will add first electron easily by releasing energy. So it is an exothermic.
<br><br>After adding first electron $$O$$ becomes $${O^ - }\,\,$$ and size of $${O^ - }\,\,$$ becomes slightly more than $$O$$ atom. Now when a new electron is trying to add into $$\,\,{O^ - }$$ ion, tw... | mcq | aieee-2004 | 3,047 |
zt41lVfktVcLf4z4SxX2r | chemistry | periodic-table-and-periodicity | electronegativity | In general, the properties that decrease and increase down a group in the periodic table, respectively, are : | [{"identifier": "A", "content": "Atomic Radius and Electronegativity"}, {"identifier": "B", "content": "Electron Gain Enthalpy and Electronegativity. "}, {"identifier": "C", "content": "Electronegativity and Atomic Radius."}, {"identifier": "D", "content": "Electronegativity and Electron Gain Enthalpy."}] | ["C"] | null | Electronegativity decreases down the group because the increased number of energy levels puts the outer electrons very far away from the pull of nucleus.
<br><br>Atomic radius increases down the group because the number of energy levels increases when you move down the group. Each subsequent energy level is further f... | mcq | jee-main-2019-online-9th-january-morning-slot | 3,048 |
SYfp09gAHw5vszkNGPdPk | chemistry | periodic-table-and-periodicity | electronegativity | The electronegativity of aluminium is similar to : | [{"identifier": "A", "content": "Beryllium"}, {"identifier": "B", "content": "Carbon"}, {"identifier": "C", "content": "Boron"}, {"identifier": "D", "content": "Lithium"}] | ["A"] | null | E.N. of Al = (1.5) $$ \cong $$ Be (1.5) | mcq | jee-main-2019-online-10th-january-morning-slot | 3,049 |
1NYoLvdsw8RDFpOlqJnUx | chemistry | periodic-table-and-periodicity | electronegativity | The correct option with respect to the Pauling electronegativity values of the element is : | [{"identifier": "A", "content": "Ga < Ge"}, {"identifier": "B", "content": "Si < Al"}, {"identifier": "C", "content": "Te > Se"}, {"identifier": "D", "content": "P > S"}] | ["A"] | null | Electronegativity increases from left to right in a period and decreases down the group. The correct orders are
<br><br>Si > Al, Ga < Ge, Te < Se and P < S. | mcq | jee-main-2019-online-11th-january-evening-slot | 3,050 |
kUkJbCnwVC6Xpxdirgjgy2xukevlra8w | chemistry | periodic-table-and-periodicity | electronegativity | In general the property (magnitudes only) that
show an opposite trend in comparison to other
properties across a period is | [{"identifier": "A", "content": "Electron gain enthalpy"}, {"identifier": "B", "content": "Electronegativity"}, {"identifier": "C", "content": "Ionization enthalpy"}, {"identifier": "D", "content": "Atomic radius"}] | ["D"] | null | Atomic radius decreases on moving left to right
in periodic table, while other three properties
given increases (in magnitude) on moving left
to right across a period. | mcq | jee-main-2020-online-2nd-september-morning-slot | 3,051 |
Ik8bdwg3HEN3lvci | chemistry | periodic-table-and-periodicity | ionization-energy | The atomic numbers of Vanadium (V), Chromium (cr), Manganese (Mn) and Iron (Fe), respectively, $$23,24,25$$ and $$26$$. Which one of these may be expected to have the higher second ionization enthalpy? | [{"identifier": "A", "content": "Cr"}, {"identifier": "B", "content": "Mn"}, {"identifier": "C", "content": "Fe"}, {"identifier": "D", "content": "V"}] | ["A"] | null | Ionization enthalpy is the energy required to remove the electron from the outer most orbit.
<br><br><u><b>Electronic configuration</b> :</u>
<br><br>$$\eqalign{
& \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,V\left( {23} \right) = \left[ {Ar} \right]\,\,\,3{d^3}\,\,\,4{S^2} \cr
& \,\,\,\,\,\,\,\,\,\,\,\,\,Cr\left(... | mcq | aieee-2003 | 3,054 |
fiVb9ZmMM2eIsnsx | chemistry | periodic-table-and-periodicity | ionization-energy | The increasing order of the first ionization enthalpies of the elements B, P, S and F (lowest first) is : | [{"identifier": "A", "content": "F < S < P < B "}, {"identifier": "B", "content": "P < S < B < F"}, {"identifier": "C", "content": "B < P < S < F "}, {"identifier": "D", "content": "B < S < P < F "}] | ["D"] | null | The correct order of ionisation enthalpies is $$F > P > S > B$$
<br><br><b>NOTE :</b> On moving along a period ionization enthalpy increases from left to right and decreases from top to bottom in a group. But this trend breaks up in case of atom having fully or half filled stable orbitals.
<br><br>In this cas... | mcq | aieee-2006 | 3,055 |
0L67JQ4Hlh6dXi0w | chemistry | periodic-table-and-periodicity | ionization-energy | Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se
and Ar? | [{"identifier": "A", "content": "S < Se < Ca < Ba < Ar "}, {"identifier": "B", "content": "Ba < Ca < Se < S < Ar "}, {"identifier": "C", "content": "Ca < Ba < S < Se < Ar "}, {"identifier": "D", "content": "Ca < S < Ba < Se < Ar "}] | ["B"] | null | Those elements are present in periodic table like this -
<br><br>
<style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;border-color:#999;}
.tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:#999;color... | mcq | jee-main-2013-offline | 3,057 |
EFht6grTUGVQ7GXkQErPQ | chemistry | periodic-table-and-periodicity | ionization-energy | Consider the following ionization enthalpies of two elements 'A' and 'B' .
<br/><br/><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;}
.... | [{"identifier": "A", "content": "Both \u2018A\u2019 and \u2018B\u2019 belong to group-1where \u2018B\u2019 comes below \u2018A\u2019.\n"}, {"identifier": "B", "content": "Both \u2018A\u2019 and \u2018B\u2019 belong to group-1 where \u2018A\u2019 comes below \u2018B\u2019."}, {"identifier": "C", "content": "Both \u2018A... | ["C"] | null | From the table you can see ionization enthalpy of A is greater than B in all the cases.
<br><br>So, B comes below A in the group as in a group from top to bottom ionization enthalpy decreases.
<br><br>After 1<sup>st</sup> ionization enthalpy each element become cation by removing a electron. In A<sup>+</sup> and B<sup... | mcq | jee-main-2017-online-8th-april-morning-slot | 3,058 |
ZKx2nRw6gDyMaNAe8vJou | chemistry | periodic-table-and-periodicity | ionization-energy | The electronic configuration with the highest ionization enthalpy is : | [{"identifier": "A", "content": "[Ne] 3s<sup>2</sup> 3p<sup>1</sup>"}, {"identifier": "B", "content": "[Ne] 3s<sup>2</sup> 3p<sup>2</sup> "}, {"identifier": "C", "content": "[Ne] 3s<sup>2</sup> 3p<sup>3</sup>"}, {"identifier": "D", "content": "[Ar] 3d<sup>10</sup> 4s<sup>2</sup> 4p<sup>3</sup>"}] | ["C"] | null | In option (D) electron is removed from 4p subshell for 1<sup>st</sup> ionization enthalpy, but in all other options electron is removed from 3p subshell. As 3p subshell is closer to nucleus than 4p, then attraction to the electrons in 3p subshell is more compared to the electrons in 4p subhell. That is why removal of e... | mcq | jee-main-2017-online-9th-april-morning-slot | 3,059 |
aWEoBg2Pl5wdFEL7xEISy | chemistry | periodic-table-and-periodicity | ionization-energy | The element having greatest difference between
its first and second ionization energies, is : | [{"identifier": "A", "content": "Ba"}, {"identifier": "B", "content": "Ca"}, {"identifier": "C", "content": "Sc"}, {"identifier": "D", "content": "K"}] | ["D"] | null | Electronic configuration of Potassium (K) :
<br><br>1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>4s<sup>1</sup>
<br><br>After first ionisation enthalpy its configuration becomes :
<br><br>1s<sup>2</sup>2s<sup>2</sup>2p<sup>6</sup>3s<sup>2</sup>3p<sup>6</sup>
<br><br>which is a inert gas configu... | mcq | jee-main-2019-online-9th-april-morning-slot | 3,060 |
vdQzSMKy5Al82WwiLQ3rsa0w2w9jx926uap | chemistry | periodic-table-and-periodicity | ionization-energy | In comparison to boron, berylium has : | [{"identifier": "A", "content": "lesser nuclear charge and greater first ionisation enthalpy"}, {"identifier": "B", "content": "greater nuclear charge and greater first ionisation enthalpy"}, {"identifier": "C", "content": "greater nuclear charge and lesser first ionisation enthalpy"}, {"identifier": "D", "content": "l... | ["A"] | null | Electronic configuration of Be(4) = 1s<sup>2</sup>2s<sup>2</sup>
<br>Electronic configuration of B(5) = 1s<sup>2</sup>2s<sup>2</sup>2p<sup>1</sup>
<br><br>Removing electron from outer most shell of Be is harder compare to B, as for Be 2s orbital is full filled so it is stable therefore required more ionization enthalpy... | mcq | jee-main-2019-online-12th-april-evening-slot | 3,061 |
EWBol1WNgzzZ5s6rgu7k9k2k5h10ay2 | chemistry | periodic-table-and-periodicity | ionization-energy | The third ionization enthalpy is minimum for : | [{"identifier": "A", "content": "Ni"}, {"identifier": "B", "content": "Co"}, {"identifier": "C", "content": "Mn"}, {"identifier": "D", "content": "Fe"}] | ["D"] | null | Electronic configuration of
<br><br><sub>25</sub>Mn = [Ar]3d<sup>5</sup>4s<sup>2</sup>
<br><br><sub>25</sub>Mn<sup>2+</sup> = [Ar]3d<sup>5</sup>4s<sup>0</sup>
<br><br><sub>26</sub>Fe = [Ar]3d<sup>6</sup>4s<sup>2</sup>
<br><br><sub>26</sub>Fe<sup>2+</sup> = [Ar]3d<sup>6</sup>4s<sup>0</sup>
<br><br><sub>27</sub>Co = [Ar]... | mcq | jee-main-2020-online-8th-january-morning-slot | 3,062 |
2Mg8RHzSwYaiLtI0ly7k9k2k5h6kkpk | chemistry | periodic-table-and-periodicity | ionization-energy | The first ionization energy (in kJ/mol) of Na, Mg, Al and Si respectively, are : | [{"identifier": "A", "content": "496, 577, 786, 737"}, {"identifier": "B", "content": "496, 737, 577, 786"}, {"identifier": "C", "content": "786, 737, 577, 496"}, {"identifier": "D", "content": "496, 577, 737, 786"}] | ["B"] | null | Elecronic configuration of Na = [Ne] 3s<sup>1</sup>
<br>Mg = [Ne] 3s<sup>2</sup>
<br>Al = [Ne] 3s<sup>2</sup>3p<sup>1</sup>
<br>Si = [Ne] 3s<sup>2</sup>3p<sup>2</sup>
<br><br>Correct order is :
<br><br>Na $$<$$ Al $$<$$ Mg $$<$$ Si | mcq | jee-main-2020-online-8th-january-morning-slot | 3,063 |
PNpMWKAgPnACxm6HWa7k9k2k5lfq2nr | chemistry | periodic-table-and-periodicity | ionization-energy | The first and second ionisation enthalpies of a
metal are 496 and 4560 kJ mol<sup>–1</sup>, respectively.
How many moles of HCl and H<sub>2</sub>SO<sub>4</sub>,
respectively, will be needed to react completely
with 1 mole of the metal hydroxide ? | [{"identifier": "A", "content": "1 and 2"}, {"identifier": "B", "content": "1 and 0.5"}, {"identifier": "C", "content": "1 and 1"}, {"identifier": "D", "content": "2 and 0.5"}] | ["B"] | null | First ionization enthalpies = 496 kJ/mole
<br><br>Second ionization enthalpies = 4560 kJ/mol
<br><br>According to the given information, the difference between first and second ionization enthalpy is very high so Metal belong to 1st group i.e. Monovalent cation.
<br><br>Metal hydroxide will be of type, MOH.
<br><br>MOH... | mcq | jee-main-2020-online-9th-january-evening-slot | 3,065 |
287GCn5IPHqKhcuBwBjgy2xukf3ipq51 | chemistry | periodic-table-and-periodicity | ionization-energy | The five successive ionization enthalpies of an
element are 800, 2427, 3658, 25024 and 32824
kJ mol<sup>–1</sup>. The number of valence electrons in
the element is : | [{"identifier": "A", "content": "2"}, {"identifier": "B", "content": "3"}, {"identifier": "C", "content": "4"}, {"identifier": "D", "content": "5"}] | ["B"] | null | There is a sudden jump after 3<sup>rd</sup> I.E. due to
attainment of noble gas configuration.
<br><br>So, the number of valence electrons in this
element are 3. | mcq | jee-main-2020-online-3rd-september-evening-slot | 3,067 |
s1BB1rArLsvSgZvLU51klre8bvz | chemistry | periodic-table-and-periodicity | ionization-energy | Consider the elements Mg, Al, S, P and Si, the correct increasing order of their first ionization
enthalpy is : | [{"identifier": "A", "content": "Al < Mg < Si < S < P"}, {"identifier": "B", "content": "Al < Mg < S < Si < P"}, {"identifier": "C", "content": "Mg < Al < Si < S < P"}, {"identifier": "D", "content": "Mg < Al < Si < P < S"}] | ["A"] | null | <p>On moving left to right in a period of the periodic table,
Ionisation energy (I.E.) increases due to increase in effective nuclear
charge i.e. Z<sub>eff</sub>.</p>
<p>But due to extra stability of fully filled and half-filled electronic
configuration of Mg and P required ionisation enthalpy is more from
neighbouring... | mcq | jee-main-2021-online-24th-february-morning-slot | 3,068 |
vw5UG91COQjGHgYD0k1klucntlw | chemistry | periodic-table-and-periodicity | ionization-energy | Match List - I with List - II.<br/><br/><table>
<thead>
<tr>
<th></th>
<th>List I<br/> Electronic configuration</th>
<th></th>
<th>List II<br/> $${\Delta _i}H$$ in kJ $$mo{l^{ - 1}}$$</th>
</tr>
</thead>
<tbody>
<tr>
<td>(a)</td>
<td>$$1{s^2}2{s^2}$$</td>
<td>(i)</td>
<td>801</td>
</tr>
<tr>
<td>(b)</td>
<td>$$1{s^2}2{... | [{"identifier": "A", "content": "(a) $$ \\to $$ (i), (b) $$ \\to $$ (iii), (c) $$ \\to $$ (iv), (d) $$ \\to $$ (iii)"}, {"identifier": "B", "content": "(a) $$ \\to $$ (iv), (b) $$ \\to $$ (i), (c) $$ \\to $$ (ii), (d) $$ \\to $$ (iii)"}, {"identifier": "C", "content": "(a) $$ \\to $$ (ii), (b) $$ \\to $$ (iii), (c) $$ ... | ["C"] | null | (a) 1s<sup>2</sup> 2s<sup>2</sup> $$ \to $$ Be<br><br>
(b) 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>4</sup> $$ \to $$ O<br><br>
(c) 1s<sup>2</sup> 2s<sup>2</sup> 2p3 $$ \to $$ N<br><br>
(d) 1s<sup>2</sup> 2s<sup>2</sup> 2p<sup>1</sup> $$ \to $$ B<br><br>
The ionization enthalpy order is<br><br>
B < Be < O < N<br>... | mcq | jee-main-2021-online-26th-february-morning-slot | 3,069 |
rweUtYFJ4i6wJFXbRw1kmitzd6m | chemistry | periodic-table-and-periodicity | ionization-energy | Identify the elements X and Y using the ionisation energy values given below :<br/><br/><table>
<thead>
<tr>
<th></th>
<th>Ionization energy (kJ/mol)</th>
<th></th>
</tr>
</thead>
<tbody>
<tr>
<td></td>
<td>1$${st}$$</td>
<td>2$${nd}$$</td>
</tr>
<tr>
<td>X</td>
<td>495</td>
<td>4563</td>
</tr>
<tr>
<td>Y</td>
<td>731<... | [{"identifier": "A", "content": "X = F; Y = Mg"}, {"identifier": "B", "content": "X = Mg; Y = F"}, {"identifier": "C", "content": "X = Na; Y = Mg"}, {"identifier": "D", "content": "X = Mg; Y = Na"}] | ["C"] | null | Due to 2p<sup>6</sup>, noble gas electronic configuration, the
second ionisation enthalpy of Na is very high. That’s
why has large difference between IE<sub>1</sub>, and IE<sub>2</sub><br><br>
Mg<sup>+</sup> is 2p<sup>6</sup>, 3s<sup>1</sup>.<br><br>
After the loss of one electron, Mg<sup>+</sup> will be formed
with no... | mcq | jee-main-2021-online-16th-march-evening-shift | 3,070 |
2hTGONkgwIUqTCaGI31kmm13av5 | chemistry | periodic-table-and-periodicity | ionization-energy | The first ionization energy of magnesium is smaller as compared to that of elements X and Y, but higher than that of Z. The elements X, Y and Z, respectively, are : | [{"identifier": "A", "content": "neon, sodium and chlorine"}, {"identifier": "B", "content": "argon, chlorine and sodium"}, {"identifier": "C", "content": "chlorine, lithium and sodium"}, {"identifier": "D", "content": "argon, lithium and sodium"}] | ["B"] | null | Order of I.E.<br><br>
3rd period $$ \to $$ Na < Al < Mg < Si < S < P < Cl < Ar | mcq | jee-main-2021-online-18th-march-evening-shift | 3,071 |
1l54y9cxc | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Given below are two statements. One is labelled as Assertion A and the other is labelled as Reason R.</p>
<p>Assertion A : The first ionization enthalpy for oxygen is lower than that of nitrogen.</p>
<p>Reason R : The four electrons in 2p orbitals of oxygen experience more electron-electron repulsion.</p>
<p>In the ... | [{"identifier": "A", "content": "Both A and R are are correct and R is the correct explanation of A."}, {"identifier": "B", "content": "Both A and R are are correct but R is NOT the correct explanation of A."}, {"identifier": "C", "content": "A is correct but R is not correct."}, {"identifier": "D", "content": "A is no... | ["B"] | null | Nitrogen has half-filled p-orbitals which is stable.
Due to this, its 1<sup>st</sup> ionization energy is more than
oxygen. | mcq | jee-main-2022-online-29th-june-evening-shift | 3,073 |
1l6jkoy8d | chemistry | periodic-table-and-periodicity | ionization-energy | <p>The incorrect statement is</p> | [{"identifier": "A", "content": "The first ionization enthalpy of K is less than that of Na and Li."}, {"identifier": "B", "content": "Xe does not have the lowest first ionization enthalpy in its group."}, {"identifier": "C", "content": "The first ionization enthalpy of element with atomic number 37 is lower than that ... | ["D"] | null | On moving down in a group ionisation energy decrease
<br/><br/>
$\therefore 1^{\text {st }}$ ionisation enthalpy order is $\mathrm{Li}>\mathrm{Na}>\mathrm{K}$
<br/><br/>
$\mathrm{Zn}$ has more ionisation energy as compared to Ga because of their pseudo inert gas configuration. | mcq | jee-main-2022-online-27th-july-morning-shift | 3,075 |
1l6p70irf | chemistry | periodic-table-and-periodicity | ionization-energy | <p>The first ionization enthalpy of Na, Mg and Si, respectively, are : 496, 737 and $$786 \mathrm{~kJ} \mathrm{~mol}^{-1}$$. The first ionization enthalpy ($$\mathrm{kJ} \,\mathrm{mol}^{-1}$$) of $$\mathrm{Al}$$ is :</p> | [{"identifier": "A", "content": "487"}, {"identifier": "B", "content": "768"}, {"identifier": "C", "content": "577"}, {"identifier": "D", "content": "856"}] | ["C"] | null | I.E. $\mathrm{Na}<\mathrm{Al}<\mathrm{Mg}<\mathrm{Si}$
<br/><br/>
$\because 496<$ I.E. (Al) $<737$
<br/><br/>
Option (C), matches the condition <br/><br/>i.e. I.E. $(\mathrm{Al})=577 \mathrm{~kJ} \mathrm{~mol}^{-1}$ | mcq | jee-main-2022-online-29th-july-morning-shift | 3,076 |
ldo9jka5 | chemistry | periodic-table-and-periodicity | ionization-energy | Given below are two statements : one is labelled as <b>Assertion (A)</b> and the other is labelled as <b>Reason (R)</b>
<br/><br/>
<b>Assertion (A):</b> The first ionization enthalpy of $3 \mathrm{~d}$ series elements is more than that of group 2 metals
<br/><br/>
<b>Reason (R):</b> In 3d series of elements successive ... | [{"identifier": "A", "content": "Both (A) and (R) are true and (R) is the correct explanation of (A)"}, {"identifier": "B", "content": "(A) is true but (R) is false"}, {"identifier": "C", "content": "Both (A) and (R) are true but $(\\mathbf{R})$ is not the correct explanation of (A)"}, {"identifier": "D", "content": "(... | ["D"] | null | From Sc to Mn ionization energy is less than that of Mg.
<br><br><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lecvglyj/efbdc808-6264-4683-8af0-7b4471f35f7c/15f816c0-b125-11ed-a8fc-b3bd3ab31931/file-1lecvglyk.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lecvglyj/efbdc808-62... | mcq | jee-main-2023-online-31st-january-evening-shift | 3,077 |
1ldsc2o1m | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Given below are two statements :</p>
<p>Statement I : The decrease in first ionization enthalpy from B to Al is much larger than that from Al to Ga.</p>
<p>Statement II : The d orbitals in Ga are completely filled.</p>
<p>In the light of the above statements, choose the most appropriate answer from the options given... | [{"identifier": "A", "content": "Statement I is correct but statement II is incorrect"}, {"identifier": "B", "content": "Statement I is incorrect but statement II is correct"}, {"identifier": "C", "content": "Both the statements I and II are correct"}, {"identifier": "D", "content": "Both the statements I and II are in... | ["C"] | null | <p><b>Statement I</b> is correct as the decrease in first ionization enthalpy from B to Al is indeed much larger than from Al to Ga. This is due to the shielding effect of the electron in the outermost shell and the increased effective nuclear charge as one moves from B to Al and from Al to Ga.</p>
<p><b>Statement II</... | mcq | jee-main-2023-online-29th-january-evening-shift | 3,078 |
1lguzhffg | chemistry | periodic-table-and-periodicity | ionization-energy | <p>For elements $$\mathrm{B}, \mathrm{C}, \mathrm{N}, \mathrm{Li}, \mathrm{Be}, \mathrm{O}$$ and $$\mathrm{F}$$, the correct order of first ionization enthalpy is</p> | [{"identifier": "A", "content": "$$\\mathrm{Li}<\\mathrm{Be}<\\mathrm{B}<\\mathrm{C}<\\mathrm{O}<\\mathrm{N}<\\mathrm{F}$$"}, {"identifier": "B", "content": "$$\\mathrm{B}>\\mathrm{Li}>\\mathrm{Be}>\\mathrm{C}>\\mathrm{N}>\\mathrm{O}>\\mathrm{F}$$"}, {"identifier": "C", "content": "$$\\mathrm{Li}<\\mathrm{Be}<\\mathrm{... | ["D"] | null | <p>The ionization energy of an atom or molecule describes the minimum amount of energy required to remove an electron from the atom or molecule in the gaseous state. It generally increases across a period (from left to right) on the periodic table because the number of protons is increasing, making the nucleus more pos... | mcq | jee-main-2023-online-11th-april-morning-shift | 3,079 |
1lgvu0oop | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Given below are two statements: one is labelled as Assertion $$\mathbf{A}$$ and the other is labelled as Reason $$\mathbf{R}$$</p>
<p>Assertion A : The energy required to form $$\mathrm{Mg}^{2+}$$ from $$\mathrm{Mg}$$ is much higher than that required to produce $$\mathrm{Mg}^+$$</p>
<p>Reason $$\mathbf{R}: \mathrm{... | [{"identifier": "A", "content": "A is false but R is true"}, {"identifier": "B", "content": "Both A and R are correct but R is NOT the correct explanation of A"}, {"identifier": "C", "content": "Both A and R are correct and R is the correct explanation of A"}, {"identifier": "D", "content": "A is true but R is false"}] | ["C"] | null | <p>The correct answer is <strong>Option C: Both A and R are correct and R is the correct explanation of A.</strong></p>
<ul>
<li><strong>Assertion A:</strong> The energy required to form Mg<sup>2+</sup> from Mg is much higher than that required to produce Mg<sup>+</sup>.</li>
</ul>
<p>This is true because it takes more... | mcq | jee-main-2023-online-10th-april-evening-shift | 3,080 |
lsaoc9af | chemistry | periodic-table-and-periodicity | ionization-energy | The transition metal having highest $3^{\text {rd }}$ ionisation enthalpy is : | [{"identifier": "A", "content": "$\\mathrm{Mn}$"}, {"identifier": "B", "content": "$\\mathrm{Fe}$"}, {"identifier": "C", "content": "$\\mathrm{Cr}$"}, {"identifier": "D", "content": "$V$"}] | ["A"] | null | <p>The third ionization enthalpy refers to the energy required to remove the third electron from a di-positive ion ($M^{2+}$) to form a tri-positive ion ($M^{3+}$). In the case of transition metals, the energies involved in removing the third electron are typically higher than for the first and second electrons due to ... | mcq | jee-main-2024-online-1st-february-evening-shift | 3,081 |
jaoe38c1lsfjay38 | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Given below are two statements : one is labelled as Assertion $$\mathbf{A}$$ and the other is labelled as Reason $$\mathbf{R}$$ :</p>
<p>Assertion A : The first ionisation enthalpy decreases across a period.</p>
<p>Reason $$\mathbf{R}$$ : The increasing nuclear charge outweighs the shielding across the period.</p>
<... | [{"identifier": "A", "content": "$$\\mathbf{A}$$ is false but $$\\mathbf{R}$$ is true\n"}, {"identifier": "B", "content": "Both $$\\mathbf{A}$$ and $$\\mathbf{R}$$ are true but $$\\mathbf{R}$$ is NOT the correct explanation of $$\\mathbf{A}$$\n"}, {"identifier": "C", "content": "Both $$\\mathbf{A}$$ and $$\\mathbf{R}$$... | ["A"] | null | <p>First ionisation energy increases along the period. Along the period $$\mathrm{Z}$$ increases which outweighs the shielding effect.</p> | mcq | jee-main-2024-online-29th-january-morning-shift | 3,082 |
luxzq97n | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Match List I with List II</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;bo... | [{"identifier": "A", "content": "A-IV, B-I, C-II, D-III\n"}, {"identifier": "B", "content": "A-I, B-II, C-III, D-IV\n"}, {"identifier": "C", "content": "A-III, B-IV, C-I, D-II\n"}, {"identifier": "D", "content": "A-II, B-III, C-IV, D-I"}] | ["A"] | null | <p>Melting point : $$\mathrm{B}>\mathrm{A} \ell>\mathrm{T} \ell>\mathrm{In}>\mathrm{Ga}$$</p>
<p>Ionic radius $$(\mathrm{M}^{+3} / \mathrm{pm}): \mathrm{T} \ell>\mathrm{In}>\mathrm{Ga}>\mathrm{A} \ell>\mathrm{B}$$</p>
<p>$$\left(\Delta_{\mathrm{IE}} \mathrm{H}\right)_1\left[\frac{\mathrm{kJ}}{\mathrm{mol}}\right]: \mat... | mcq | jee-main-2024-online-9th-april-evening-shift | 3,084 |
lv0vyqw9 | chemistry | periodic-table-and-periodicity | ionization-energy | <p>The correct order of first ionization enthalpy values of the following elements is :</p>
<p>(A) O</p>
<p>(B) N</p>
<p>(C) Be</p>
<p>(D) F</p>
<p>(E) B</p>
<p>Choose the correct answer from the options given below :</p> | [{"identifier": "A", "content": "$$\\mathrm{A}<\\mathrm{B}<\\mathrm{D}<\\mathrm{C}<\\mathrm{E}$$\n"}, {"identifier": "B", "content": "$$\\mathrm{C}<\\mathrm{E}<\\mathrm{A}<\\mathrm{B}<\\mathrm{D}$$\n"}, {"identifier": "C", "content": "$$\\mathrm{E}<\\mathrm{C}<\\mathrm{A}<\\mathrm{B}<\\mathrm{D}$$\n"}, {"identifier": "... | ["C"] | null | <p> Correct ionization enthalpy order : </p>
<p>$$\quad$$B < Be < O < N < F </p>
<p>or E < C < A < B < D</p> | mcq | jee-main-2024-online-4th-april-morning-shift | 3,085 |
lv2erzas | chemistry | periodic-table-and-periodicity | ionization-energy | <p>The correct order of the first ionization enthalpy is</p> | [{"identifier": "A", "content": "$$\\mathrm{Ga}>\\mathrm{Al}>\\mathrm{B}$$\n"}, {"identifier": "B", "content": "$$\\mathrm{Tl}>\\mathrm{Ga}>\\mathrm{Al}$$\n"}, {"identifier": "C", "content": "$$\\mathrm{Al}>\\mathrm{Ga}>\\mathrm{Tl}$$\n"}, {"identifier": "D", "content": "$$\\mathrm{B}>\\mathrm{Al}>\\mathrm{Ga}$$"}] | ["B"] | null | <p>I. $$\mathrm{E}_1$$ of $$\mathrm{TI}=589 \mathrm{~kJ} / \mathrm{mol}$$</p>
<p>I. $$\mathrm{E}_1$$ of $$\mathrm{Ga}=579 \mathrm{~kJ} / \mathrm{mol}$$</p>
<p>I. $$\mathrm{E_1}$$ of $$\mathrm{Al}=577 \mathrm{~kJ} / \mathrm{mol}$$</p> | mcq | jee-main-2024-online-4th-april-evening-shift | 3,086 |
lv2erj91 | chemistry | periodic-table-and-periodicity | ionization-energy | <p>Given below are two statements :</p>
<p>Statement I : The correct order of first ionization enthalpy values of $$\mathrm{Li}, \mathrm{Na}, \mathrm{F}$$ and $$\mathrm{Cl}$$ is $$\mathrm{Na}<\mathrm{Li}<\mathrm{Cl}<\mathrm{F}$$.</p>
<p>Statement II : The correct order of negative electron gain enthalpy values... | [{"identifier": "A", "content": "Statement I is true but Statement II is false\n"}, {"identifier": "B", "content": "Both Statement I and Statement II are false\n"}, {"identifier": "C", "content": "Statement I is false but Statement II is true\n"}, {"identifier": "D", "content": "Both Statement I and Statement II are tr... | ["D"] | null | <p>First ionization enthalpy of $$\mathrm{F}>\mathrm{Cl}$$ as first IE decreases down the group.</p>
<p>Similarly, first IE of $$\mathrm{Li}>\mathrm{Na}$$.</p>
<p>So, statement-I is correct.</p>
<p>Electron gain enthalpy of given elements are negative. Considering the magnitude the given order is correct.</p>
<p>Thus, ... | mcq | jee-main-2024-online-4th-april-evening-shift | 3,087 |
BhhYY8pJsndQGssB | chemistry | periodic-table-and-periodicity | nature-of-oxide | Which one of the following is an amphoteric oxide? | [{"identifier": "A", "content": "Na<sub>2</sub>O"}, {"identifier": "B", "content": "SO<sub>2</sub>"}, {"identifier": "C", "content": "B<sub>2</sub>O<sub>3</sub>"}, {"identifier": "D", "content": "ZnO"}] | ["D"] | null | These elements are called amphoteric which reacts with both acid and base.
<br><br>Following elements are amphoteric
<br><br>$$\left( 1 \right)\,\,\,\,Zn$$
<br><br>$$\left( 2 \right)\,\,\,\,Be$$
<br><br>$$\left( 3 \right)\,\,\,\,Al$$
<br><br>$$\left( 4 \right)\,\,\,\,B$$
<br><br>$$\left( 5 \right)\,\,\,\,Cr$$
<br><br... | mcq | aieee-2003 | 3,088 |
OXnfgb75B5dClK6j | chemistry | periodic-table-and-periodicity | nature-of-oxide | Among Al<sub>2</sub>O<sub>3</sub>, SiO<sub>2</sub>, P<sub>2</sub>O<sub>3</sub> and SO<sub>2</sub> the correct order of acid strength is | [{"identifier": "A", "content": "SO<sub>2</sub> < P<sub>2</sub>O<sub>3</sub> < SiO<sub>2</sub> < Al<sub>2</sub>O<sub>3</sub>"}, {"identifier": "B", "content": "Al<sub>2</sub>O<sub>3</sub> < SiO<sub>2</sub> < <sub>P2</sub>O<sub>3</sub> < SO<sub>2</sub>"}, {"identifier": "C", "content": "Al<sub>2</sub>O... | ["B"] | null | In periodic table from left to right (group $$1$$ to group $$18$$ ) acidic strength increases.
<br><br>$$Al$$ belongs to group $$13,$$ $$Si$$ belongs to group $$14,$$ $$P$$ belongs to group $$15$$ and $$S$$ belongs to group $$16$$.
<br><br>So, $$\,\,\,A{l_2}{O_3}$$ will be least acidic and $$S{o_2}$$ will most acidic... | mcq | aieee-2004 | 3,089 |
9BvtDiokWWAJbNgs | chemistry | periodic-table-and-periodicity | nature-of-oxide | Which one of the following order represents the correct sequence of the increasing basic nature of the
given oxides ? | [{"identifier": "A", "content": "MgO < K<sub>2</sub>O < Al<sub>2</sub>O<sub>3</sub> < Na<sub>2</sub>O"}, {"identifier": "B", "content": "Al<sub>2</sub>O<sub>3</sub> < MgO < Na<sub>2</sub>O < K<sub>2</sub>O"}, {"identifier": "C", "content": "Na<sub>2</sub>O < K<sub>2</sub>O < MgO < Al<sub>2</s... | ["B"] | null | You should know that,
<br><br>(1)$$\,\,\,$$ In a period, from left to right the acidic strength increases that mean basic nature decreases.
<br><br>(2)$$\,\,\,$$ In a group, from top to bottom the basic nature increases that means acidic nature decreases.
<br><br>Na, Mg, Al and K are present in periodic table like t... | mcq | aieee-2011 | 3,092 |
hWos1QbD2o6pGJCQcMXfX | chemistry | periodic-table-and-periodicity | nature-of-oxide | Which one of the following is an oxide? | [{"identifier": "A", "content": "KO<sub>2</sub> "}, {"identifier": "B", "content": "BaO<sub>2</sub> "}, {"identifier": "C", "content": "SiO<sub>2</sub> "}, {"identifier": "D", "content": "CsO<sub>2</sub>"}] | ["C"] | null | Na, H, Ba and Sr produce Peroxide.
<br><br>K, Rb and Cs produces Superoxide.
<br><br>So, SiO<sub>2</sub> will be oxide. | mcq | jee-main-2017-online-9th-april-morning-slot | 3,093 |
OqdbyXIPmG3ZzYVE4t7k9k2k5icuagp | chemistry | periodic-table-and-periodicity | nature-of-oxide | The acidic, basic and amphoteric oxides,
respectively, are : | [{"identifier": "A", "content": "Cl<sub>2</sub>O, CaO, P<sub>4</sub>O<sub>10</sub>"}, {"identifier": "B", "content": "N<sub>2</sub>O<sub>3</sub>, Li<sub>2</sub>O, Al<sub>2</sub>O<sub>3</sub>"}, {"identifier": "C", "content": "MgO, Cl<sub>2</sub>O, Al<sub>2</sub>O<sub>3</sub>"}, {"identifier": "D", "content": "Na<sub>2<... | ["B"] | null | Non metal oxide $$ \to $$ acidic.
<br><br>Metal oxide $$ \to $$ basic.
<br><br>Al<sub>2</sub>O<sub>3</sub> amphoteric. | mcq | jee-main-2020-online-9th-january-morning-slot | 3,094 |
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