question_id stringlengths 8 35 | subject stringclasses 3
values | chapter stringclasses 90
values | topic stringclasses 459
values | question stringlengths 17 24.5k | options stringlengths 2 4.26k | correct_option stringclasses 6
values | answer stringclasses 460
values | explanation stringlengths 1 10.6k | question_type stringclasses 3
values | paper_id stringclasses 154
values | __index_level_0__ int64 2 13.4k |
|---|---|---|---|---|---|---|---|---|---|---|---|
1ldppgyi8 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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 - II, B - I, C - III, D - IV"}, {"identifier": "B", "content": "A - II, B - I, C - IV, D - III"}, {"identifier": "C", "content": "A - IV, B - I, C - II, D - III"}, {"identifier": "D", "content": "A - IV, B - III, C - II, D - I"}] | ["B"] | null | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/1leh9wcqv/41039764-7736-413d-ace2-672e44c709ef/ae342970-b390-11ed-96ad-459254a85a5f/file-1leh9wcqw.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1leh9wcqv/41039764-7736-413d-ace2-672e44c709ef/ae342970-b390-11ed-96ad-459254a85a5f/fi... | mcq | jee-main-2023-online-31st-january-morning-shift | 873 |
1ldr4ho5x | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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 - II, B - I, C - IV, D - III"}, {"identifier": "B", "content": "A - IV, B - I, C - II, D - III"}, {"identifier": "C", "content": "A - IV, B - III, C - II, D - I"}, {"identifier": "D", "content": "A - II, B - III, C - IV, D - I"}] | ["C"] | null | <p>(A) IF$$_7$$ $$-$$ 0 lone pairs</p>
<p>(B) ICI$$_4^ - $$ $$-$$ 2 lone pairs</p>
<p>(C) XeF$$_6$$ $$-$$ 1 lone pair</p>
<p>(D) XeF$$_2$$ $$-$$ 3 lone pairs</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lepzncy5/03ee6ab7-d140-4db8-bd2d-97f2c0c7d311/a6a17fd0-b85b-11ed-8195-4f3c56fa1eb5/file-1l... | mcq | jee-main-2023-online-30th-january-morning-shift | 874 |
1ldv10o5c | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The total number of lone pairs of electrons on oxygen atoms of ozone is __________.</p> | [] | null | 6 | <p>Total no, of lone pairs on oxygen atoms = 6</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lebwzzd6/9bf8acbe-9e54-4d5f-a5e8-daffdbfcaa39/512da2a0-b09e-11ed-a1d6-7715f24e8c48/file-1lebwzzd7.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lebwzzd6/9bf8acbe-9e54-4d5f-a5e... | integer | jee-main-2023-online-25th-january-morning-shift | 875 |
lgnze5sm | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | The number of $\mathrm{P}-\mathrm{O}-\mathrm{P}$ bonds in $\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7},\left(\mathrm{HPO}_{3}\right)_{3}$ and $\mathrm{P}_{4} \mathrm{O}_{10}$ are respectively : | [{"identifier": "A", "content": "$1,3,6$"}, {"identifier": "B", "content": "$1,2,4$"}, {"identifier": "C", "content": "$0,3,4$"}, {"identifier": "D", "content": "$0,3,6$"}] | ["A"] | null | Let's analyze each compound separately:
<br><br>
1. $\mathrm{H}_{4} \mathrm{P}_{2} \mathrm{O}_{7}$: This compound is also known as pyrophosphoric acid. Its structure has two phosphorus atoms (P) connected by one oxygen atom (O), forming a P-O-P bond. There are no other P-O-P bonds in its structure.
Number of P-O-P bond... | mcq | jee-main-2023-online-15th-april-morning-shift | 876 |
1lgq472j1 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | $$\mathrm{ClF}_{5}$$ at room temperature is a: | [{"identifier": "A", "content": "Colourless liquid with square pyramidal geometry"}, {"identifier": "B", "content": "Colourless gas with square pyramidal geometry"}, {"identifier": "C", "content": "Colourless gas with trigonal bipyramidal geometry."}, {"identifier": "D", "content": "Colourless liquid with trigonal bipy... | ["A"] | null | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lgtthcsj/24428c52-a29a-4693-b7e1-f2c2c9a5e1de/1a3c7530-e20f-11ed-9e52-3dd25100c100/file-1lgtthcsk.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lgtthcsj/24428c52-a29a-4693-b7e1-f2c2c9a5e1de/1a3c7530-e20f-11ed-9e52-3dd25100c100/fi... | mcq | jee-main-2023-online-13th-april-morning-shift | 877 |
1lgsz22g1 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The maximum number of lone pairs of electrons on the central atom from the following species is ____________.</p>
<p>$$\mathrm{ClO}_{3}{ }^{-}, \mathrm{XeF}_{4}, \mathrm{SF}_{4}$$ and $$\mathrm{I}_{3}{ }^{-}$$</p> | [] | null | 3 | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/1libj9fix/3a3c9e8e-e382-40b1-8b6a-179c32cfb663/75a6ac90-ff99-11ed-8d3c-6fd4c50a7427/file-1libj9fiy.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1libj9fix/3a3c9e8e-e382-40b1-8b6a-179c32cfb663/75a6ac90-ff99-11ed-8d3c-6fd4c50a7427/fi... | integer | jee-main-2023-online-11th-april-evening-shift | 878 |
1lguzfmzq | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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:sol... | [{"identifier": "A", "content": "A-III, B-I, C-II, D-IV"}, {"identifier": "B", "content": "A-III, B-II, C-I, D-IV"}, {"identifier": "C", "content": "A-III, B-IV, C-I, D-II"}, {"identifier": "D", "content": "A-III, B-IV, C-II, D-I"}] | ["B"] | null | <p>Let's consider each species in List I and determine their geometries/shapes.</p>
<p>A. $\mathrm{H_3O^+}$: This ion is formed by the addition of a proton to a water molecule. The central atom (O) is surrounded by three Hydrogen atoms and one lone pair, making its shape pyramidal.</p>
<p>B. Acetylide anion: The ac... | mcq | jee-main-2023-online-11th-april-morning-shift | 879 |
1lgvv5z7m | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of molecules from the following which contain only two lone pair of electrons is ________</p>
<p>$$\mathrm{H}_{2} \mathrm{O}, \mathrm{N}_{2}, \mathrm{CO}, \mathrm{XeF}_{4}, \mathrm{NH}_{3}, \mathrm{NO}, \mathrm{CO}_{2}, \mathrm{~F}_{2}$$</p> | [] | null | 3 | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1lixqco47/38985813-f5e4-4424-ba74-edb4b5dd5979/6de7f270-0bce-11ee-acbf-7f9d4e788425/file-6y3zli1lixqco48.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/6y3zli1lixqco47/38985813-f5e4-4424-ba74-edb4b5dd5979/6de7f270-0bce-11ee-ac... | integer | jee-main-2023-online-10th-april-evening-shift | 880 |
1lgyfyt7u | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The compound which does not exist is</p> | [{"identifier": "A", "content": "(NH$$_4$$)$$_2$$BeF$$_4$$"}, {"identifier": "B", "content": "PbEt$$_4$$"}, {"identifier": "C", "content": "BeH$$_2$$"}, {"identifier": "D", "content": "NaO$$_2$$"}] | ["D"] | null | Sodium superoxide (NaO$_2$) is not a stable compound. It is not found in normal conditions due to its high reactivity. | mcq | jee-main-2023-online-10th-april-morning-shift | 881 |
1lgyhijw5 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of bent-shaped molecule/s from the following is __________</p>
<p>N$$_3^-$$, NO$$_2^-$$, I$$_3^-$$, O$$_3$$, SO$$_2$$</p> | [] | null | 3 | <p>A bent-shaped molecule has a molecular geometry with a central atom bonded to two other atoms and one or two pairs of non-bonding electrons. The VSEPR (Valence Shell Electron Pair Repulsion) theory helps us predict the shapes of molecules.</p>
<p>Let's consider the given molecules:</p>
<ol>
<li><p>N$_3^-$: The a... | integer | jee-main-2023-online-10th-april-morning-shift | 882 |
1lgyhlpij | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The sum of lone pairs present on the central atom of the interhalogen IF$$_5$$ and IF$$_7$$ is _________</p> | [] | null | 1 | <p>Interhalogen compounds are the substances that consist of two different halogens. The most common type of interhalogen compounds are binary, containing only two different elements.</p>
<p>In IF$_5$, iodine (I) is the central atom. Iodine has 7 valence electrons, 5 of which are used for bonding with the 5 fluorine (F... | integer | jee-main-2023-online-10th-april-morning-shift | 883 |
1lh27wei6 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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-II, B-I, C-III, D-IV"}, {"identifier": "B", "content": "A-III, B-I, C-II, D-IV"}, {"identifier": "C", "content": "A-III, B-I, C-IV, D-II"}, {"identifier": "D", "content": "A-II, B-IV, C-III, D-I"}] | ["B"] | null | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1llm9poeo/b606cdcb-1706-473e-ad1b-625b32825c55/63727d00-40e5-11ee-8358-1796f8234e47/file-6y3zli1llm9poep.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/6y3zli1llm9poeo/b606cdcb-1706-473e-ad1b-625b32825c55/63727d00-40e5-11ee-83... | mcq | jee-main-2023-online-6th-april-morning-shift | 885 |
1lh29lf3g | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of species from the following which have square pyramidal structure is _________</p>
<p>$$\mathrm{PF}_{5}, \mathrm{BrF}_{4}^{-}, \mathrm{IF}_{5}, \mathrm{BrF}_{5}, \mathrm{XeOF}_{4}, \mathrm{ICl}_{4}^{-}$$</p> | [] | null | 3 | <p>A square pyramidal structure has five bonds and one lone pair, making a total of six electron pairs around the central atom. The geometry of such a molecule can be analyzed using the VSEPR theory.</p>
<ol>
<li>$\mathrm{PF}_{5}$: 5 bond pairs and 0 lone pairs, so its geometry is trigonal bipyramidal, not square pyram... | integer | jee-main-2023-online-6th-april-morning-shift | 886 |
1lh32lx4j | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of species having a square planar shape from the following is __________.</p>
<p>$$\mathrm{XeF}_{4}, \mathrm{SF}_{4}, \mathrm{SiF}_{4}, \mathrm{BF}_{4}^{-}, \mathrm{BrF}_{4}^{-},\left[\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},\left[\mathrm{FeCl}_{4}\right]^{2-},\left[\mathrm{PtCl}_{4}\right]... | [] | null | 4 | $\mathrm{XeF}_4 \rightarrow$ Square planar<br/><br/>
$\mathrm{SF}_4 \rightarrow$ See saw<br/><br/>
$\mathrm{SiF}_4 \rightarrow$ Tetrahedral<br/><br/>
$\mathrm{BF}_4^{-} \rightarrow$ Tetrahedral<br/><br/>
$\left[\mathrm{Cu}\left(\mathrm{NH}_3\right)_4\right]^{2+} \rightarrow$ Square planar<br/><br/>
$\left[\mathrm{FeCl}... | integer | jee-main-2023-online-6th-april-evening-shift | 887 |
lsbn2unr | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | The number of molecules/ion/s having trigonal bipyramidal shape is _______.
<br/><br/>$\mathrm{PF}_5, \mathrm{BrF}_5, \mathrm{PCl}_5,\left[\mathrm{Pt} \mathrm{Cl}_4\right]^{2-}, \mathrm{BF}_3, \mathrm{Fe}(\mathrm{CO})_5$ | [] | null | 3 | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1lsfah88p/a66619bb-5ed5-4177-af56-d7795c400dad/68b8ce90-c7a4-11ee-a4c7-e152a9884fc5/file-6y3zli1lsfah88q.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/6y3zli1lsfah88p/a66619bb-5ed5-4177-af56-d7795c400dad/68b8ce90-c7a4-11ee-a4... | integer | jee-main-2024-online-1st-february-morning-shift | 888 |
jaoe38c1lscs8hzs | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of non-polar molecules from the following is _________. $$\mathrm{HF}, \mathrm{H}_2 \mathrm{O}, \mathrm{SO}_2, \mathrm{H}_2, \mathrm{CO}_2, \mathrm{CH}_4, \mathrm{NH}_3, \mathrm{HCl}, \mathrm{CHCl}_3, \mathrm{BF}_3$$</p> | [] | null | 4 | <p>To determine whether a molecule is polar or non-polar, we must consider the difference in electronegativity between the atoms and the symmetry of the molecule. Polar molecules occur when there is an electronegativity difference between the bonded atoms. Non-polar molecules either do not have any polar bonds or the p... | integer | jee-main-2024-online-27th-january-evening-shift | 889 |
jaoe38c1lsfk70hj | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>Number of compounds with one lone pair of electrons on central atom amongst following is _________.</p>
<p>$$\mathrm{O}_3, \mathrm{H}_2 \mathrm{O}, \mathrm{SF}_4, \mathrm{ClF}_3, \mathrm{NH}_3, \mathrm{BrF}_5, \mathrm{XeF}_4$$</p> | [] | null | 4 | <p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lt2oifv6/1f764780-52ba-411c-a9aa-a11f5170d5e2/512a7230-d481-11ee-ac6c-b973c46afe12/file-1lt2oifv7.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lt2oifv6/1f764780-52ba-411c-a9aa-a11f5170d5e2/512a7230-d481-11ee-ac6c-b973c46afe12... | integer | jee-main-2024-online-29th-january-morning-shift | 891 |
1lsg7kbq3 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The molecule / ion with square pyramidal shape is</p> | [{"identifier": "A", "content": "$$\\mathrm{PCl}_5$$\n"}, {"identifier": "B", "content": "$$\\left[\\mathrm{Ni}(\\mathrm{CN})_4\\right]^{2-}$$\n"}, {"identifier": "C", "content": "$$\\mathrm{PF}_5$$\n"}, {"identifier": "D", "content": "$$\\mathrm{BrF}_5$$"}] | ["D"] | null | <p>$$\mathrm{BrF_5}$$</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1lspvcpn2/a7b05e75-c4d1-4eca-8add-63d4a0a5db32/e1529ee0-cd75-11ee-9be1-85ca54b9efcb/file-6y3zli1lspvcpn3.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/6y3zli1lspvcpn2/a7b05e75-c4d1-4eca-8add-63d4a... | mcq | jee-main-2024-online-30th-january-evening-shift | 892 |
1lsgxnho5 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>Aluminium chloride in acidified aqueous solution forms an ion having geometry</p> | [{"identifier": "A", "content": "Square planar\n"}, {"identifier": "B", "content": "Octahedral\n"}, {"identifier": "C", "content": "Trigonal bipyramidal\n"}, {"identifier": "D", "content": "Tetrahedral"}] | ["B"] | null | <p>$$\mathrm{AlCl}_3$$ in acidified aqueous solution forms octahedral geometry $$[\mathrm{Al}(\mathrm{H}_2 \mathrm{O})_6]^{3+}$$</p> | mcq | jee-main-2024-online-30th-january-morning-shift | 893 |
1lsgy08ma | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>Match List I with List II.</p>
<p><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padding:10px 5px;word-break:normal;}
.tg th{border-color:black;border-style:solid;b... | [{"identifier": "A", "content": "(A)-(I), (B)-(II), (C)-(IV), (D)-(III)\n"}, {"identifier": "B", "content": "(A)-(IV), (B)-(III), (C)-(I), (D)-(II)\n"}, {"identifier": "C", "content": "(A)-(III), (B)-(IV), (C)-(I), (D)-(II)\n"}, {"identifier": "D", "content": "(A)-(II), (B)-(I), (C)-(III), (D)-(IV)"}] | ["B"] | null | <img src="https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1lsqmhidy/bdac6e90-3aaf-4cbe-9e2a-a19aaadc1c8f/fd40af60-cddf-11ee-a0d3-7b75c4537559/file-6y3zli1lsqmhidz.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/6y3zli1lsqmhidy/bdac6e90-3aaf-4cbe-9e2a-a19aaadc1c8f/fd40af60-cddf-11ee-a0... | mcq | jee-main-2024-online-30th-january-morning-shift | 894 |
luxzq9h9 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The correct increasing order for bond angles among $$\mathrm{BF}_3, \mathrm{PF}_3$$ and $$\mathrm{ClF}_3$$ is :</p> | [{"identifier": "A", "content": "$$\\mathrm{BF}_3=\\mathrm{PF}_3<\\mathrm{ClF}_3$$\n"}, {"identifier": "B", "content": "$$\\mathrm{BF}_3<\\mathrm{PF}_3<\\mathrm{ClF}_3$$\n"}, {"identifier": "C", "content": "$$\\mathrm{ClF}_3<\\mathrm{PF}_3<\\mathrm{BF}_3$$\n"}, {"identifier": "D", "content": "$$\\mathrm{PF}_3<\\mathrm{... | ["C"] | null | <p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lw2xkwii/4c270791-c55b-4947-92e4-4c0873ba2d87/6df13890-1009-11ef-bffa-cb0d0a489c35/file-1lw2xkwij.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lw2xkwii/4c270791-c55b-4947-92e4-4c0873ba2d87/6df13890-1009-11ef-bffa-cb0d0a489c35... | mcq | jee-main-2024-online-9th-april-evening-shift | 895 |
lv0vyqj5 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>Number of molecules/ions from the following in which the central atom is involved in $$\mathrm{sp}^3$$ hybridization is ________.</p>
<p>$$\mathrm{NO}_3^{-}, \mathrm{BCl}_3, \mathrm{ClO}_2^{-}, \mathrm{ClO}_3^{-}$$</p> | [{"identifier": "A", "content": "2"}, {"identifier": "B", "content": "4"}, {"identifier": "C", "content": "1"}, {"identifier": "D", "content": "3"}] | ["A"] | null | <p>To determine the number of molecules/ions in which the central atom is involved in $$\mathrm{sp}^3$$ hybridization, we must analyze the hybridization state for each central atom. Hybridization is typically determined by the number of sigma bonds and lone pairs on the central atom.</p>
<p>Let's evaluate each molecul... | mcq | jee-main-2024-online-4th-april-morning-shift | 897 |
lv2es2q1 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The number of species from the following that have pyramidal geometry around the central atom is _________</p>
<p>$$\mathrm{S}_2 \mathrm{O}_3^{2-}, \mathrm{SO}_4^{2-}, \mathrm{SO}_3^{2-}, \mathrm{S}_2 \mathrm{O}_7^{2-}$$</p> | [{"identifier": "A", "content": "4"}, {"identifier": "B", "content": "3"}, {"identifier": "C", "content": "2"}, {"identifier": "D", "content": "1"}] | ["D"] | null | <p>$$\mathrm{SO}_3^{2-}$$ is the only species with pyramidal geometry.</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lwhsvaob/e56e6438-5a66-40f1-a233-1345578a2fd3/c311a9b0-1836-11ef-9081-0ded966256d8/file-1lwhsvaoc.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lwhsvao... | mcq | jee-main-2024-online-4th-april-evening-shift | 898 |
lv3xmasa | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>The shape of carbocation is :</p> | [{"identifier": "A", "content": "tetrahedral\n"}, {"identifier": "B", "content": "diagonal pyramidal\n"}, {"identifier": "C", "content": "diagonal\n"}, {"identifier": "D", "content": "trigonal planar"}] | ["D"] | null | <p>Carbocation is $$s p^2$$ hybridised hence it's shape is trigonal planar</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lw572fuz/7d920da9-b2af-44a2-8fce-743980ccd75b/191aa9b0-1148-11ef-b5fc-89359a20637a/file-1lw572fv0.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lw5... | mcq | jee-main-2024-online-8th-april-evening-shift | 899 |
lv5gsw7q | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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-II, B-IV, C-I, D-III\n"}, {"identifier": "B", "content": "A-III, B-I, C-IV, D-II\n"}, {"identifier": "C", "content": "A-IV, B-III, C-I, D-II\n"}, {"identifier": "D", "content": "A-III, B-IV, C-I, D-II"}] | ["B"] | null | <p>To match the molecules in List I with their corresponding shapes in List II, we need to consider the electronic geometry and the VSEPR (Valence Shell Electron Pair Repulsion) theory. Here’s the detailed analysis:</p>
<p><b>$$\mathrm{NH_3}$$ (Ammonia)</b>: Ammonia has a central nitrogen atom bonded to three hydrogen... | mcq | jee-main-2024-online-8th-april-morning-shift | 900 |
lv9s26z7 | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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)-(I), (B)-(IV), (C)-(III), (D)-(II)\n"}, {"identifier": "B", "content": "(A)-(IV), (B)-(I), (C)-(II), (D)-(III)\n"}, {"identifier": "C", "content": "(A)-(I), (B)-(III), (C)-(II), (D)-(IV)\n"}, {"identifier": "D", "content": "(A)-(IV), (B)-(III), (C)-(II), (D)-(I)"}] | ["B"] | null | <p>$$\begin{aligned}
& \mathrm{ICl} \rightarrow s p^3 \rightarrow 1 \mathrm{bp}+3 \mathrm{lp} \rightarrow \text { Linear } \\
& \mathrm{ICl}_3 \rightarrow s p^3 d \rightarrow 3 \mathrm{bp}+2 \mathrm{lp} \rightarrow \mathrm{T} \text {-shape } \\
& \mathrm{CIF}_5 \rightarrow s p^3 d^2 \rightarrow 5 \mathrm{bp}+1 \mathrm{... | mcq | jee-main-2024-online-5th-april-evening-shift | 901 |
lvb2acem | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <p>Total number of species from the following with central atom utilising $$\mathrm{sp}^2$$ hybrid orbitals for bonding is ________.</p> <p>$$\mathrm{NH}_3, \mathrm{SO}_2, \mathrm{SiO}_2, \mathrm{BeCl}_2, \mathrm{C}_2 \mathrm{H}_2, \mathrm{C}_2 \mathrm{H}_4, \mathrm{BCl}_3, \mathrm{HCHO}, \mathrm{C}_6 \mathrm{H}_6, \ma... | [] | null | 6 | <p>$$\mathrm{SO}_2, \mathrm{C}_2 \mathrm{H}_4, \mathrm{BCl}_3, \mathrm{HCHO}, \mathrm{C}_6 \mathrm{H}_6, \mathrm{BF}_3$$ are $$s p^2$$ hybridised central atom</p> | integer | jee-main-2024-online-6th-april-evening-shift | 902 |
lvc57i5y | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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-III, B-II, C-IV, D-I\n"}, {"identifier": "B", "content": "A-III, B-IV, C-II, D-I\n"}, {"identifier": "C", "content": "A-II, B-IV, C-III, D-I\n"}, {"identifier": "D", "content": "A-II, B-III, C-I, D-IV"}] | ["B"] | null | <p>$$\begin{aligned}
& \text { A } \rightarrow \text { Sea-saw (III) } \\
& \text { B } \rightarrow \text { Bent T-shape (IV) } \\
& \text { C } \rightarrow \text { Pyramidal (II) } \\
& \text { D } \rightarrow \text { Tetrahedral (I) }
\end{aligned}$$</p> | mcq | jee-main-2024-online-6th-april-morning-shift | 903 |
lvc588zk | chemistry | chemical-bonding-and-molecular-structure | hybridization-and-vsepr-theory | <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-II, B-III, C-I, D-IV\n"}, {"identifier": "B", "content": "A-III, B-I, C-II, D-IV\n"}, {"identifier": "C", "content": "A-IV, B-I, C-III, D-II\n"}, {"identifier": "D", "content": "A-III, B-IV, C-II, D-I"}] | ["B"] | null | <p>$$\begin{aligned}
& \mathrm{A} \rightarrow \text { Tetrahedral (III) } \\
& \mathrm{B} \rightarrow \text { Paramagnetic (I) } \\
& \mathrm{C} \rightarrow \text { Diamagnetic (II) } \\
& \mathrm{D} \rightarrow \text { Linear (IV) }
\end{aligned}$$</p> | mcq | jee-main-2024-online-6th-april-morning-shift | 904 |
RduOhjDepCS6jqrz | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | Which of the following hydrogen bonds is the strongest? | [{"identifier": "A", "content": "O\u2212H\u2026\u2026.N"}, {"identifier": "B", "content": "F\u2212H\u2026\u2026.F "}, {"identifier": "C", "content": "O\u2212H\u2026\u2026.O "}, {"identifier": "D", "content": "O\u2212H\u2026\u2026.F "}] | ["B"] | null | Among F, O and N, F is most electronegative so F pulls bond pair of electron in F - H towards itself and develops highly positive charge on H atom.
<br><br>This highly positive charged H atom creates stongest hydrogen bonding by taking lone pair of electron form electronegative atom F/N/O. Hence among the given option... | mcq | aieee-2007 | 905 |
InA3umoGpofamZ2t | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | The intermolecular interaction that is dependent on the inverse cube of distance between the molecule is: | [{"identifier": "A", "content": "ion-dipole interaction"}, {"identifier": "B", "content": "London force"}, {"identifier": "C", "content": "hydrogen bond"}, {"identifier": "D", "content": "ion-ion interaction"}] | ["C"] | null | Hydrogen bond is a type of strong electrostatic dipole- dipole intersection and dependent on the inverse cube of distance between the molecular ion-dipole -
<br><br> interaction $$ \propto {1 \over {{r^3}}}.$$ | mcq | jee-main-2015-offline | 906 |
C8wM97uJad4kiBxUSAxvh | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | HF has highest boiling point among hydrogen
halides, because it has : | [{"identifier": "A", "content": "lowest dissociation enthalpy"}, {"identifier": "B", "content": "strongest hydrogen bonding"}, {"identifier": "C", "content": "lowest ionic character"}, {"identifier": "D", "content": "strongest van der Waals' interactions"}] | ["B"] | null | Due to strong H-bonding
between HF molecules, HF has highest boiling point among the
hydrogen halides. | mcq | jee-main-2019-online-9th-april-evening-slot | 907 |
2San0gkpPqtZNXmtsbjgy2xukfjfemc7 | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | The potential energy curve for the H<sub>2</sub>
molecule as a function of internuclear distance is : | [{"identifier": "A", "content": "<img src=\"https://res.cloudinary.com/dckxllbjy/image/upload/v1734263495/exam_images/ebsqxtpz2rbzxfo0v6jf.webp\" style=\"max-width: 100%;height: auto;display: block;margin: 0 auto;\" loading=\"lazy\" alt=\"JEE Main 2020 (Online) 5th September Morning Slot Chemistry - Chemical Bonding &a... | ["C"] | null | Potential energy curve for H<sub>2</sub> molecules is
<img src="https://res.cloudinary.com/dckxllbjy/image/upload/v1734267306/exam_images/gfgvygdqedrzud5q17zp.webp" style="max-width: 100%;height: auto;display: block;margin: 0 auto;" loading="lazy" alt="JEE Main 2020 (Online) 5th September Morning Slot Chemistry - Chemi... | mcq | jee-main-2020-online-5th-september-morning-slot | 908 |
jrIpSPZ42eyUlUxyKk1klud2nda | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R.<br/><br/>Assertion A : Dipole-dipole interactions are the only non-covalent interactions, resulting in hydrogen bond formation.<br/><br/>Reason R : Fluorine is the most electronegative element and hydrogen bonds in HF... | [{"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": "A is false but R is true"}, {"identifier": "D", "content": "Both A and R are true but R is NOT the correct explanation of A"}] | ["C"] | null | Dipole - Dipole are not only the interaction
responsible for hydrogen bond formation.
Ion-dipole can also be responsible for
hydrogen bond formation.
<br><br> F is most electronegative element and
anhydrous HF in solid phase has
symmetrical hydrogen bonding. | mcq | jee-main-2021-online-26th-february-morning-slot | 909 |
1ktiha5vq | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | The number of hydrogen bonded water molecule(s) associated with stoichiometry CuSO<sub>4</sub>.5H<sub>2</sub>O is ____________. | [] | null | 1 | <img src="https://res.cloudinary.com/dckxllbjy/image/upload/v1734264346/exam_images/uhagajtbrpgxxvbseqkp.webp" style="max-width: 100%;height: auto;display: block;margin: 0 auto;" loading="lazy" alt="JEE Main 2021 (Online) 31st August Morning Shift Chemistry - Chemical Bonding & Molecular Structure Question 115 Engl... | integer | jee-main-2021-online-31st-august-morning-shift | 910 |
1l56wur7s | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | <p>The correct order of increasing intermolecular hydrogen bond strength is</p> | [{"identifier": "A", "content": "HCN < H<sub>2</sub>O < NH<sub>3</sub>"}, {"identifier": "B", "content": "HCN < CH<sub>4</sub> < NH<sub>3</sub>"}, {"identifier": "C", "content": "CH<sub>4</sub> < HCN < NH<sub>3</sub>"}, {"identifier": "D", "content": "CH<sub>4</sub> < NH<sub>3</sub> < HCN"}] | ["C"] | null | Due to the high difference in electronegativity of H and
N the H-bond strength of NH<sub>3</sub> is highest. There is
no H-bond in CH<sub>4</sub>.<br/><br/>
CH<sub>4</sub> < HCN < NH<sub>3</sub> | mcq | jee-main-2022-online-27th-june-evening-shift | 911 |
1ldyfls2h | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | <p>Decreasing order of the hydrogen bonding in following forms of water is correctly represented by</p>
<p>A. Liquid water</p>
<p>B. Ice</p>
<p>C. Impure water</p>
<p>Choose the correct answer from the options given below :</p> | [{"identifier": "A", "content": "A = B > C"}, {"identifier": "B", "content": "B > A > C"}, {"identifier": "C", "content": "A > B > C"}, {"identifier": "D", "content": "C > B > A"}] | ["B"] | null | Extent of hydrogen bonding :
<br/><br/>
Ice $>$ liquid water $>$ impure water
<br/><br/>
- In ice, 4 molecules of $\mathrm{H}_{2} \mathrm{O}$ are connected to $\mathrm{H}_{2} \mathrm{O}$ molecule.
<br/><br/>
- Impure water will have less hydrogen bonding. | mcq | jee-main-2023-online-24th-january-morning-shift | 912 |
1lh333die | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | <p>In an ice crystal, each water molecule is hydrogen bonded to ____________ neighbouring molecules.</p> | [] | null | 4 | In an ice crystal, each water molecule is hydrogen bonded to four neighbouring molecules. | integer | jee-main-2023-online-6th-april-evening-shift | 913 |
lsap1fic | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | Select the compound from the following that will show intramolecular hydrogen bonding. | [{"identifier": "A", "content": "<img src=\"https://app-content.cdn.examgoal.net/fly/@width/image/6y3zli1lsar2vc6/4f0ca88f-8841-4a89-a07a-96469081fcba/695fec60-c525-11ee-94a9-d124b3795c4c/file-6y3zli1lsar2vc7.png?format=png\" data-orsrc=\"https://app-content.cdn.examgoal.net/image/6y3zli1lsar2vc6/4f0ca88f-8841-4a89-a07... | ["A"] | null | <p>Intramolecular hydrogen bonding occurs when a hydrogen atom is covalently bonded to a highly electronegative atom, like oxygen or nitrogen, and this hydrogen atom is also attracted to another electronegative atom within the same molecule. This phenomenon tends to happen when the molecule can form a six-membered or f... | mcq | jee-main-2024-online-1st-february-evening-shift | 914 |
lsbmkq49 | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | 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>: $\mathrm{PH}_3$ has lower boiling point than $\mathrm{NH}_3$.<br/><br/>
<b>Reason (R)</b> : In liquid state $\mathrm{NH}_3$ molecules are associated through vander Waal... | [{"identifier": "A", "content": "Both (A) and (R) are correct and (R) is the correct explanation of (A)"}, {"identifier": "B", "content": "(A) is not correct but (R) is correct"}, {"identifier": "C", "content": "(A) is correct but (R) is not correct"}, {"identifier": "D", "content": "Both $(\\mathbf{A})$ and $(\\mathbf... | ["C"] | null | <p>The correct answer is Option C: (A) is correct but (R) is not correct.</p>
<p><b>Assertion (A)</b>: $\mathrm{PH}_3$ has lower boiling point than $\mathrm{NH}_3$.</p>
<p>This assertion is true. The boiling point of ammonia ($\mathrm{NH}_3$) is higher than that of phosphine ($\mathrm{PH}_3$). Ammonia has a boiling p... | mcq | jee-main-2024-online-1st-february-morning-shift | 915 |
lv2erjdj | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | <p>The correct statement/s about Hydrogen bonding is/are</p>
<p>A. Hydrogen bonding exists when H is covalently bonded to the highly electro negative atom.</p>
<p>B. Intermolecular H bonding is present in $$o$$-nitro phenol</p>
<p>C. Intramolecular $$\mathrm{H}$$ bonding is present in HF.</p>
<p>D. The magnitude of $$\... | [{"identifier": "A", "content": "A, B, C only\n"}, {"identifier": "B", "content": "A only\n"}, {"identifier": "C", "content": "A, D, E only\n"}, {"identifier": "D", "content": "A, B, D only"}] | ["C"] | null | <p>In o-nitrophenol intra molecular hydrogen bonding
is present.</p>
<p>In HF intermolecular hydrogen bonding is present. </p>
<p>Other statements are correct except B and C. </p> | mcq | jee-main-2024-online-4th-april-evening-shift | 916 |
lvb2ackq | chemistry | chemical-bonding-and-molecular-structure | hydrogen-bonding | <p>Consider the following reactions</p>
<p><img src="data:image/png;base64,UklGRuIaAABXRUJQVlA4INYaAACwiQCdASoAA5EAPm00l0ekIyIhJRJbOIANiWlu/HyYw+tQ0f0z/sHaL/ev79+3Pid+g/x/5l+vjkr66Pn31R/lX2h/W/3/0I/5v+C8YflZqEe0v8pvQNqvQI9evo3+m/x/5FekF/dehf2F/5fuAfzn+7f9P2C77WgX/Pv8P+yfsMfYHoG+p/2t+A7+ff3L/r9hX0lCdWHKsLj/7GOIGoY2zVv2X... | [] | null | 12 | <p>$$\mathrm{NiS + HN{O_3} + HCl\buildrel {} \over
\longrightarrow \mathop {NiC{l_2}}\limits_{(A)} + S + NO + {H_2}O}$$</p>
<p>$$\mathrm{\mathop {NiC{l_2}}\limits_{(A)} + N{H_4}OH +}$$ Dimethylgyoxime $$\mathrm{\buildrel {} \over
\longrightarrow \mathop {Ni{{(dmg)}_2}}\limits_{(B)} + N{H_4}Cl + {H_2}O}$$</p>
<p><i... | integer | jee-main-2024-online-6th-april-evening-shift | 917 |
rSpvxqnXjBtwo9bfkI1klsd0e3n | chemistry | chemical-bonding-and-molecular-structure | hydrolysis | Among the following, the number of halide(s) which is/are inert to hydrolysis is _________.<br/><br/>(A) BF<sub>3</sub><br/><br/>(B) SiCl<sub>4</sub><br/><br/>(C) PCl<sub>5</sub><br/><br/>(D) SF<sub>6</sub> | [] | null | 1 | BF<sub>3</sub> – Shows Partial hydrolysis
<br><br>SiCl<sub>4</sub> – Undergoes hydrolysis readily
<br><br>PCl<sub>5</sub> – Undergoes hydrolysis by addition–
elimination mechanism.
<br><br>SF<sub>6</sub> – Due to crowding Inert towards hydrolysis. | integer | jee-main-2021-online-25th-february-morning-slot | 919 |
fq1DNfNhwProQ708 | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | Lattice energy of an ionic compounds depends upon | [{"identifier": "A", "content": "Charge on the ion only"}, {"identifier": "B", "content": "Size of the ion only "}, {"identifier": "C", "content": "Packing of ions only"}, {"identifier": "D", "content": "Charge on the ion and size of the ion"}] | ["D"] | null | <p>The lattice energy of an ionic compound is a measure of the strength of the bonds in that ionic compound. Specifically, it is the energy required to separate one mole of an ionic solid into its constituent ions in the gaseous state. The lattice energy depends on several factors, primarily the charge on the ions and ... | mcq | aieee-2005 | 920 |
RWNDdbhUYKYBoil1 | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | The charge/size ratio of a cation determines its polarizing power. Which one of the following
sequences represents the increasing order of the polarizinig order of the polarizing power of the
cationic species, K<sup>+</sup>, Ca<sup>2+</sup>, Mg<sup>2+</sup>, Be<sup>2+</sup>? | [{"identifier": "A", "content": "Mg<sup>2+</sup> < Be<sup>2+</sup> < K<sup>+</sup> < Ca<sup>2+</sup>"}, {"identifier": "B", "content": "K<sup>+</sup> < Ca<sup>2+</sup> < Mg<sup>2+</sup> < Be<sup>2+</sup>"}, {"identifier": "C", "content": "Be<sup>2+</sup> < K<sup>+</sup> < Ca<sup>2+</sup> < Mg... | ["B"] | null | As charge/size ratio of a cation determines its polarizing power so high charge and small size of the cations increases
polarisation.
<br><br>As the size of the given cations decreases as
<br><br> K<sup>+</sup>
> Ca<sup>2+</sup> > Mg<sup>2+</sup> > Be<sup>2+</sup>
<br><br>Hence, polarising power decreases as
... | mcq | aieee-2007 | 921 |
NlQwrJQxyidRbufT | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | Among the following the maximum covalent character is shown by the compound : | [{"identifier": "A", "content": "SnCl<sub>2 </sub>"}, {"identifier": "B", "content": "AlCl<sub>3</sub> "}, {"identifier": "C", "content": "MgCl<sub>2 </sub>"}, {"identifier": "D", "content": "FeCl<sub>2</sub>"}] | ["B"] | null | Charge of cation/Size of cation is called polarising power.
<br><br>$$ \therefore $$ (i) Polarising power $$ \propto $$ charge of cation
<br><br>(ii) Polarising power $$ \propto $$ <span style="display: inline-block;vertical-align: middle;">
<div style="text-align: center;border-bottom: 1px solid black;">1</div>
... | mcq | aieee-2011 | 922 |
EKsMjnfbWj3zbUo1ppjgy2xukeyf4obe | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | Match the type of interaction in column A with
the distance dependence of their interaction
energy in column B
<br/><style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;}
.tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px;
overflow:hidden;padd... | [{"identifier": "A", "content": "(I)-(a), (II)-(b), (III)-(d)"}, {"identifier": "B", "content": "(I)-(b), (II)-(d), (III)-(c)"}, {"identifier": "C", "content": "(I)-(a), (II)-(b), (III)-(c)"}, {"identifier": "D", "content": "(I)-(a), (II)-(c), (III)-(d)"}] | ["D"] | null | Ion-ion interaction energy $$ \propto $$ $${1 \over r}$$
<br><br>Dipole-dipole interaction energy $$ \propto $$ $${1 \over {{r^3}}}$$
<br><br>London dispersion $$ \propto $$ $${1 \over {{r^6}}}$$ | mcq | jee-main-2020-online-2nd-september-evening-slot | 923 |
HFY7Xy1k19cqRCzppU1klru73v4 | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | The correct set from the following in which both pairs are in correct order of melting point is : | [{"identifier": "A", "content": "LiCl > LiF ; NaCl > MgO"}, {"identifier": "B", "content": "LiCl > LiF ; MgO > NaCl"}, {"identifier": "C", "content": "LiF > LiCl ; NaCl > MgO"}, {"identifier": "D", "content": "LiF > LiCl ; MgO > NaCl"}] | ["D"] | null | <p>Correct option is i.e. LiF > LiCl; MgO > NaCl. Melting point is directly proportional to lattice energy. Lattice energy is the energy required to separate a mole of an ionic solid into gaseous ions. It depends upon charge of ions and size of ions.</p>
<p>$$M.P. \propto L.E. \propto {{Charge} \over {Size}}$$</p>
<p>$... | mcq | jee-main-2021-online-24th-february-evening-slot | 924 |
1lh04mf3g | chemistry | chemical-bonding-and-molecular-structure | ionic-bond | <p>The number of following factors which affect the percent covalent character of the ionic bond is _________</p>
<p>(A) Polarising power of cation</p>
<p>(B) Extent of distortion of anion</p>
<p>(C) Polarisability of the anion</p>
<p>(D) Polarising power of anion</p> | [] | null | 3 | <p>The covalent character of an ionic bond is largely determined by the polarization of the ions involved in the bond. Polarization refers to the distortion of the electron cloud of an anion by a cation. This distortion leads to a shift in electron density towards the cation, thereby increasing the covalent character o... | integer | jee-main-2023-online-8th-april-morning-shift | 925 |
tRqcHUfZAks8ckvLOhjgy2xukfuqwaai | chemistry | chemical-bonding-and-molecular-structure | lewis-theory | The number of Cl = O bonds in perchloric acid
is, "________". | [] | null | 3 | The structure of perchloric acid is
<img src="https://res.cloudinary.com/dckxllbjy/image/upload/v1734266578/exam_images/jyszcvabceqqemsdzkut.webp" style="max-width: 100%;height: auto;display: block;margin: 0 auto;" loading="lazy" alt="JEE Main 2020 (Online) 6th September Morning Slot Chemistry - Chemical Bonding & ... | integer | jee-main-2020-online-6th-september-morning-slot | 928 |
1ldst4bbt | chemistry | chemical-bonding-and-molecular-structure | lewis-theory | <p>The number of molecules or ions from the following, which do not have odd number of electrons are _________.</p>
<p>(A) NO$$_2$$</p>
<p>(B) ICl$$_4^ - $$</p>
<p>(C) BrF$$_3$$</p>
<p>(D) ClO$$_2$$</p>
<p>(E) NO$$_2^ + $$</p>
<p>(F) NO</p> | [] | null | 3 | Only $\mathrm{ICl}_4^{-}, \mathrm{BrF}_3$ and $\mathrm{NO}_2^{+}$have even number of electrons.
<br/><br/>$$
\begin{aligned}
& \mathrm{NO}_2 \Rightarrow 23 e^{-} ; \\\\
& \mathrm{ICl}_4^{-} \Rightarrow 122 e^{-} ; \\\\
& \mathrm{BrF}_3 \Rightarrow 62 e^{-} ; \\\\
& \mathrm{ClO}_2 \Rightarrow 33 e^{-} ; \\\\
& \mathrm{N... | integer | jee-main-2023-online-29th-january-morning-shift | 929 |
lv5gsw8c | chemistry | chemical-bonding-and-molecular-structure | lewis-theory | <p>Number of molecules from the following which are exceptions to octet rule is _________.</p>
<p>$$\mathrm{CO}_2, \mathrm{NO}_2, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{BF}_3, \mathrm{CH}_4, \mathrm{SiF}_4, \mathrm{ClO}_2, \mathrm{PCl}_5, \mathrm{BeF}_2, \mathrm{C}_2 \mathrm{H}_6, \mathrm{CHCl}_3, \mathrm{CBr}_4$$</p> | [] | null | 6 | <p>$$\mathrm{NO}_2, \mathrm{H}_2 \mathrm{SO}_4, \mathrm{BF}_3, \mathrm{ClO}_2, \mathrm{PCl}_5, \mathrm{BeF}_2$$</p>
<p>These are exception of octet rule</p> | integer | jee-main-2024-online-8th-april-morning-shift | 930 |
lv7v47s8 | chemistry | chemical-bonding-and-molecular-structure | lewis-theory | <p>In the lewis dot structure for $$\mathrm{NO}_2^{-}$$, total number of valence electrons around nitrogen is _________.</p> | [] | null | 8 | <p>$$\text { Lewis dot structure of } \mathrm{NO}_2^{-} \text {is: }$$</p>
<p><img src="https://app-content.cdn.examgoal.net/fly/@width/image/1lwh56zal/04a24314-4a60-43cf-8f6c-8ea5670b9184/2ce32dd0-17da-11ef-a722-71ab49de2419/file-1lwh56zam.png?format=png" data-orsrc="https://app-content.cdn.examgoal.net/image/1lwh56za... | integer | jee-main-2024-online-5th-april-morning-shift | 931 |
5ewmfVaZwhG6amZL | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following are arranged in an increasing order of their bond strengths? | [{"identifier": "A", "content": "$$O_2^-$$ < O<sub>2</sub> < $$O_2^+$$ < $$O_2^{2-}$$"}, {"identifier": "B", "content": "$$O_2^{2-}$$ < $$O_2^-$$ < $$O_2$$ < $$O_2^{+}$$"}, {"identifier": "C", "content": "$$O_2^-$$ < $$O_2^{2-}$$ < $$O_2$$ < $$O_2^{+}$$"}, {"identifier": "D", "content": "$$O_... | ["B"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,\,\,\,$$ Bond strength $$ \propto $$ Bond order
<br><br>(2) $$\,\,\,\,$$ Bond length $$ \propto $$ $${1 \over {Bond\,\,order}}$$
<br><br>(3) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbi... | mcq | aieee-2002 | 932 |
nZWgMrVC61t5mc6a | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The bond order in NO is 2.5 while that in NO<sup>+</sup> is 3. Which of the following statements is true for these two species? | [{"identifier": "A", "content": "Bond length in NO<sup>+</sup> is greater than in NO "}, {"identifier": "B", "content": "Bond length is unpredictable"}, {"identifier": "C", "content": "Bond length in NO<sup>+</sup> in equal to that in NO"}, {"identifier": "D", "content": "Bond length in NO is greater than in NO<sup>+</... | ["D"] | null | Molecular orbital configuration of NO (15 electrons) is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\sigma _{2p_z^2}}\,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * \, = \,\pi _{2p_y^o}^ * $$
<br><br>$$\therefore\,\,\,\,$$ N<sub>b</sub> = 10
<br><br>N<sub>a<... | mcq | aieee-2004 | 933 |
78vvWsuL3joAOjJY | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which one of the following species is diamagnetic in nature? | [{"identifier": "A", "content": "$$He_2^+$$"}, {"identifier": "B", "content": "H<sub>2</sub>"}, {"identifier": "C", "content": "$$H_2^+$$"}, {"identifier": "D", "content": "$$H_2^-$$"}] | ["B"] | null | <b>TIPS/Formulae :</b>
<br><br>A diamagnetic substance contains no unpaired electron.
<br><br>$${H_2}$$ is diamagnetic as it contains all paired electrons
<br><br>$$\mathop {{H_2} = \sigma _b^2}\limits_{\left( {diamagnetic} \right)} \,\,,\,\,\mathop {H_2^ + = \sigma _b^1,}\limits_{\left( {paramagnetic} \right)}... | mcq | aieee-2005 | 934 |
l1VU0nBBIoUEbBGm | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following molecules/ions does not contain unpaired electrons? | [{"identifier": "A", "content": "$$O_2^{2\u2212} $$"}, {"identifier": "B", "content": "B<sub>2</sub>"}, {"identifier": "C", "content": "$$N_2^+$$"}, {"identifier": "D", "content": "O<sub>2</sub>"}] | ["A"] | null | (A) Molecular orbital configuration of O $$_2^{2 - }$$ (18 electrons) is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\sigma _{2p_z^2}}\,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,\pi _{2p_x^2}^ * \, = \,\pi _{2p_y^2}^ * $$
<br><br>So O $$_2^{2 - }$$ has no unpaired electr... | mcq | aieee-2006 | 935 |
v25tvfRhzo8LhY59 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following species exhibits the diamagnetic behaviour? | [{"identifier": "A", "content": "$$O_2^{2\u2212}$$"}, {"identifier": "B", "content": "NO"}, {"identifier": "C", "content": "$$O_2^+$$"}, {"identifier": "D", "content": "O<sub>2</sub>"}] | ["A"] | null | Those species which have unpaired electrons are called paramagnetic species.
<br><br>And those species which have no unpaired electrons are called diamagnetic species.
<br><br>(a) $$O_2^{2−}$$ has 18 electrons.
<br><br>Moleculer orbital configuration of $$O_2^{2−}$$ is
<br><br>$${\sigma _{1{s^2}}}\,... | mcq | aieee-2007 | 936 |
Mk1EqYkRfu6bSrWr | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | In which of the following ionization processes, the bond order has increased and the magnetic
behaviour has changed? | [{"identifier": "A", "content": "$$C_2 \\to C_2^+$$"}, {"identifier": "B", "content": "$$N_2 \\to N_2^+$$"}, {"identifier": "C", "content": "$$NO \\to NO^+$$"}, {"identifier": "D", "content": "$$O_2 \\to O_2^+$$"}] | ["C"] | null | (A) Moleculer orbital configuration of $$C_2$$ (12 electrons)
<br><br>= $${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}$$
<br><br>$$\therefore\,\,\,\,$$N<sub>a</sub> = 4
<br><br>N<sub>b</sub> = 8
<br><br>$$\therefore\,\,\,\,$$ BO = $${1 \over 2... | mcq | aieee-2007 | 937 |
hVhRBuRAwNW6A8B1 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following pair of species have the same bond order? | [{"identifier": "A", "content": "CN<sup>-</sup> and NO<sup>+</sup>"}, {"identifier": "B", "content": "CN<sup>-</sup> and CN<sup>+</sup>"}, {"identifier": "C", "content": "$$O_2^-$$ and CN<sup>-</sup>"}, {"identifier": "D", "content": "NO<sup>+</sup> and CN<sup>+</sup>"}] | ["A"] | null | Number of electron in
NO<sup>+</sup>
= number of electron in CN<sup>–</sup>
= 14 electrons.
<br><br>As both have same number of electrons so their bond order is equal.
<br><br>Moleculer orbital configuration of NO<sup>+</sup> (14 electrons) is
<br><br>= $${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}... | mcq | aieee-2008 | 938 |
Vnurx6F2t4VBIDLe | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Using MO theory, predict which of the following species has the shortest bond length? | [{"identifier": "A", "content": "$$O_2^+$$"}, {"identifier": "B", "content": "$$O_2^-$$"}, {"identifier": "C", "content": "$$O_2^{2-}$$"}, {"identifier": "D", "content": "$$O_2^{2+}$$"}] | ["D"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,\,\,\,$$ Bond length $$ \propto $$ $${1 \over {Bond\,\,order}}$$
<br><br>(2) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbital
<br><br>N<sub>a</sub> $$=$$ No of electrons in anti bonding ... | mcq | aieee-2009 | 939 |
IVnAUloaajyf6Ciz | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which one of the following molecules is expected to exhibit diamagnetic behaviour? | [{"identifier": "A", "content": "N<sub>2</sub>"}, {"identifier": "B", "content": "O<sub>2</sub>"}, {"identifier": "C", "content": "S<sub>2</sub>"}, {"identifier": "D", "content": "C<sub>2</sub>"}] | null | null | Those species which have unpaired electrons are called paramagnetic species.
<br><br>And those species which have no unpaired electrons are called diamagnetic species.
<br><br>(A) $$N_2$$ has 14 electrons.
<br><br>Moleculer orbital configuration of $$N_2$$
<br><br>= $${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ ... | mcqm | jee-main-2013-offline | 940 |
e9ZZ6hVkVRrr20He | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | In which of the following pairs of molecules/ions, both the species are not likely to exist? | [{"identifier": "A", "content": "$$H_2^+$$ , $$He_2^{2-}$$"}, {"identifier": "B", "content": "$$H_2^-$$ , $$He_2^{2-}$$"}, {"identifier": "C", "content": "$$H_2^{2+}$$ , $$He_2$$"}, {"identifier": "D", "content": "$$H_2^-$$ , $$He_2^{2+}$$"}] | ["C"] | null | $$H_2^{2+}$$ , $$He_2$$
<br><br>Both have zero bond order. Thus, they do not exist. | mcq | jee-main-2013-offline | 941 |
71vVjiJV8KEZUIQD | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Stability of the species Li<sub>2</sub>, $$Li_2^−$$ and $$Li_2^+$$ increases in the order of: | [{"identifier": "A", "content": "Li<sub>2</sub> < $$Li_2^+$$ < $$Li_2^-$$"}, {"identifier": "B", "content": "$$Li_2^+$$ < $$Li_2^-$$ < Li<sub>2</sub>"}, {"identifier": "C", "content": "$$Li_2^-$$ <$$Li_2^+$$ < Li<sub>2</sub>"}, {"identifier": "D", "content": "$$Li_2^-$$ < Li<sub>2</sub> < $$Li_... | ["C"] | null | Li<sub>2</sub> = $${\sigma _{1{s^2}}}\,\,\sigma _{1{s^2}}^ * \,$$ $${\sigma _{2{s^2}}} \,$$
<br><br>$$ \therefore $$ Bond order = $${1 \over 2}\left( {4 - 2} \right)$$ = 1
<br><br>$$Li_2^+$$ = $${\sigma _{1{s^2}}}\,\,\sigma _{1{s^2}}^ * \,$$ $${\sigma _{2{s^1}}} \,$$
<br><br>$$ \therefore $$ Bond order = $${1 \over 2}\... | mcq | jee-main-2013-offline | 942 |
2I94DYV587XfHvOi | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following species is <b>not</b> paramagnetic?
| [{"identifier": "A", "content": "CO"}, {"identifier": "B", "content": "O<sub>2</sub>"}, {"identifier": "C", "content": "B<sub>2</sub>"}, {"identifier": "D", "content": "NO"}] | ["A"] | null | Those species which have unpaired electrons are called paramagnetic species.
<br><br>(a) CO has 14 electrons.
<br><br>Moleculer orbital configuration of CO is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\pi _{2p_x^2}} =\,{\pi _{2p_y^2}}\,{\sig... | mcq | jee-main-2017-offline | 943 |
YFVl81zZz9l5GTXPCmqsx | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Which of the following is paramagnetic ? | [{"identifier": "A", "content": "NO<sup>+</sup> "}, {"identifier": "B", "content": "CO"}, {"identifier": "C", "content": "$$O_2^{2 - }$$"}, {"identifier": "D", "content": "B<sub>2</sub>"}] | ["D"] | null | Those species which have unpaired electrons are called paramagnetic species.
<br><br>(a) NO<sup>+</sup> has 14 electrons.
<br><br>Moleculer orbital configuration of NO<sup>+</sup> is
<br><br>$${\sigma _{1{s^2}}}$$ $$\sigma _{1{s^2}}^ * $$ $${\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z... | mcq | jee-main-2017-online-8th-april-morning-slot | 944 |
xbbpwAyMOufn5c54 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | According to molecular orbital theory, which of the following will not be a viable molecule? | [{"identifier": "A", "content": "$${\\rm H}e_2^{2 + }$$ "}, {"identifier": "B", "content": "$${\\rm H}e_2^{ + }$$"}, {"identifier": "C", "content": "$${\\rm H}_2^{- }$$"}, {"identifier": "D", "content": "$${\\rm H}_2^{2 - }$$"}] | ["D"] | null | <b><u>Note</u> :</b>
<br><br>According to molecules orbital theory, when a molecule have bond order = 0 then that molecule does not exist.
<br><br>(a)$$\,\,\,$$ Configuration of $$He_2^{2 + }$$ (2 electrons) is = $${\sigma _{1{s^2}}}$$
<br><br>$$\therefore\,\,\,$$ Bond order = $${1 \over 2}$$ (2 $$-$$0) = 1
<br><br>(b... | mcq | jee-main-2018-offline | 947 |
5QPKgmMT1jSaJIB9R9HXC | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | According to molecular orbital theory, which of the following is true with respect to Li<sub>2</sub><sup>+</sup> and Li<sub>2</sub><sup>$$-$$</sup> ? | [{"identifier": "A", "content": "$$Li_2^ + $$ is unstable and $$Li_2^ - $$ is stable"}, {"identifier": "B", "content": "$$Li_2^ + $$ is stable and $$Li_2^ - $$ unstable"}, {"identifier": "C", "content": "Both are stable "}, {"identifier": "D", "content": "Both are unstable "}] | ["C"] | null | $$Li_2^ + $$ (5 electrons) = $${\sigma _{1{s^2}}}\,\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^1}}}$$
<br><br>$$Li_2^ - $$ (7 electrons) = $${\sigma _{1{s^2}}}\,\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}$$ $$\,\sigma _{2{s^1}}^ * \,$$
<br><br>$$ \therefore $$ Bond order of $$Li_2^ ... | mcq | jee-main-2019-online-9th-january-morning-slot | 948 |
tajJ8St48Q1lcW1qdYfUS | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Among the following species, the diamagnetic
molecule is | [{"identifier": "A", "content": "CO"}, {"identifier": "B", "content": "B<sub>2</sub>"}, {"identifier": "C", "content": "O<sub>2</sub>"}, {"identifier": "D", "content": "NO"}] | ["A"] | null | Those species which have unpaired electrons are called paramagnetic species.
<br><br>And those species which have no unpaired electrons are called diamagnetic species.
<br><br>(a) CO has 14 electrons.
<br><br>Moleculer orbital configuration of CO is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * ... | mcq | jee-main-2019-online-9th-april-evening-slot | 950 |
4kAdZGcAFWDgiyauTrdhC | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Among the following, the molecule expected
to be stabilized by anion formation is :<br/>
C<sub>2</sub>, O<sub>2</sub>, NO, F<sub>2</sub> | [{"identifier": "A", "content": "C<sub>2</sub>"}, {"identifier": "B", "content": "NO"}, {"identifier": "C", "content": "O<sub>2</sub>"}, {"identifier": "D", "content": "F<sub>2</sub>"}] | ["A"] | null | C<sub>2</sub> has 12 electrons.
<br><br>Moleculer orbital configuration of C<sub>2</sub> is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\pi _{2p_x^2}} =\,{\pi _{2p_y^2}}$$
<br><br>Bond order of C<sub>2</sub> = $${{8 - 4} \over 2}$$ = 2
<br><br>C<sub>2</sub><sup>... | mcq | jee-main-2019-online-9th-april-morning-slot | 951 |
jyTyBEbXoLWjxRE6s2Jln | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Two pi and half sigma bonds are present in : | [{"identifier": "A", "content": "O<sub>2</sub>"}, {"identifier": "B", "content": "N$$_2^ + $$"}, {"identifier": "C", "content": "O$$_2^ + $$"}, {"identifier": "D", "content": "N<sub>2</sub>"}] | ["B"] | null | Two pi and half sigma bonds are presents in molecule with bond order 2.5.
<br><br>Moleculer orbital configuration of $$N_2^+$$ (13 electrons)
<br><br>= $${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,{\sigma _{2p_z^1}}$$
<br><br>Bond order = $... | mcq | jee-main-2019-online-10th-january-morning-slot | 953 |
rZmnCDvb0RMeec8w5Dkta | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | In which of the following process, the bond order has increased and paramagnetic character has charged to diamagnetic ? | [{"identifier": "A", "content": "NO $$ \\to $$ NO<sup>+</sup>"}, {"identifier": "B", "content": "N<sub>2</sub> $$ \\to $$ N<sub>2</sub><sup>+</sup>"}, {"identifier": "C", "content": "O<sub>2</sub> $$ \\to $$ O<sub>2</sub><sup>+</sup>"}, {"identifier": "D", "content": "O<sub>2</sub> $$ \\to $$ O... | ["A"] | null | Molecular orbital configuration of NO (15 electrons) is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,{\sigma _{2{s^2}}}\,\sigma _{2{s^2}}^ * \,{\sigma _{2p_z^2}}\,{\pi _{2p_x^2}}\, = \,{\pi _{2p_y^2}}\,\pi _{2p_x^1}^ * \, = \,\pi _{2p_y^o}^ * $$
<br><br>$$\therefore\,\,\,\,$$ N<sub>b</sub> = 10
<br><br>N<sub>a<... | mcq | jee-main-2019-online-9th-january-evening-slot | 954 |
39uduN98fcC5Wjng4F7k9k2k5epf47d | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The bond order and the magnetic characteristics of CN<sup>-</sup>
are : | [{"identifier": "A", "content": "3, paramagnetic"}, {"identifier": "B", "content": "$$2{1 \\over 2}$$, paramagnetic"}, {"identifier": "C", "content": "3, diamagnetic"}, {"identifier": "D", "content": "$$2{1 \\over 2}$$, diamagnetic"}] | ["C"] | null | CN<sup>-</sup> has 14 electrons.
<br><br>Moleculer orbital configuration of CN<sup>-</sup> is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\pi _{2p_x^2}} =\,{\pi _{2p_y^2}}\,{\sigma _{2p_z^2}}$$
<br><br>Here is no unpaired electron so it is dia... | mcq | jee-main-2020-online-7th-january-evening-slot | 955 |
OJ4HXN2l6O25EZHBDR7k9k2k5icjff5 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | If the magnetic moment of a dioxygen species
is 1.73 B.M, it may be : | [{"identifier": "A", "content": "$$O_2^ - $$ or $$O_2^ + $$"}, {"identifier": "B", "content": "O<sub>2</sub>, $$O_2^ - $$ or $$O_2^ + $$"}, {"identifier": "C", "content": "O<sub>2</sub> or $$O_2^ + $$"}, {"identifier": "D", "content": "O<sub>2</sub> or $$O_2^ - $$"}] | ["A"] | null | Magnetic moment = 1.73 BM
<br><br>$$ \therefore $$ Unpaired electron = 1
<br><br>(1) $$O_2$$ has 16 electrons.
<br><br>Moleculer orbital configuration of $$O_2$$ is
<br><br>$${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^ * \,\,{\sigma _{2{s^2}}}\,\,\sigma _{2{s^2}}^ * \,\,{\sigma _{2p_z^2}}\,\,{\pi _{2p_x^2}}\,= \,{\pi _{2p_... | mcq | jee-main-2020-online-9th-january-morning-slot | 956 |
mHQPHyo2fQemHaqz1Fjgy2xukf2b5jgn | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Of the species, NO, NO<sup>+</sup>, NO<sup>2+</sup> and NO<sup>-</sup>
, the one with minimum bond strength is : | [{"identifier": "A", "content": "NO<sup>\u2013</sup>"}, {"identifier": "B", "content": "NO"}, {"identifier": "C", "content": "NO<sup>+</sup>"}, {"identifier": "D", "content": "NO<sup>2+</sup>"}] | ["A"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,\,\,\,$$ Bond strength $$ \propto $$ Bond order
<br><br>(2) $$\,\,\,\,$$ Bond length $$ \propto $$ $${1 \over {Bond\,\,order}}$$
<br><br>(3) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbi... | mcq | jee-main-2020-online-3rd-september-morning-slot | 957 |
LWpA0sfVy1vp0ZMoaD1kls92xym | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | According to molecular orbital theory, the species among the following that does not exist is : | [{"identifier": "A", "content": "$${O_2}^{2 - }$$"}, {"identifier": "B", "content": "$$B{e_2}$$"}, {"identifier": "C", "content": "$$H{e_2}^ - $$"}, {"identifier": "D", "content": "$$H{e_2}^ + $$"}] | ["B"] | null | <b><u>Note</u> :</b>
<br><br>According to molecules orbital theory, when a molecule have bond order = 0 then that molecule does not exist.
<br><br>We know, Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbital
<br><br>N<sub>a</sub> $$=$... | mcq | jee-main-2021-online-25th-february-morning-slot | 958 |
OJX2Tfv6pbCnjqppz81klurauoc | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Match List - I with List - II.<br/><br/><table>
<thead>
<tr>
<th></th>
<th>List - I (Molecule)</th>
<th></th>
<th>List - II (Bond order)</th>
</tr>
</thead>
<tbody>
<tr>
<td>(a)</td>
<td>$$N{e_2}$$</td>
<td>(i)</td>
<td>1</td>
</tr>
<tr>
<td>(b)</td>
<td>$${N_2}$$</td>
<td>(ii)</td>
<td>2</td>
</tr>
<tr>
<td>(c)</td>
<... | [{"identifier": "A", "content": "(a) $$ \\to $$ (i), (b) $$ \\to $$ (ii), (c) $$ \\to $$ (iii), (d) $$ \\to $$ (iv)"}, {"identifier": "B", "content": "(a) $$ \\to $$ (iv), (b) $$ \\to $$ (iii), (c) $$ \\to $$ (ii), (d) $$ \\to $$ (i)"}, {"identifier": "C", "content": "(a) $$ \\to $$ (iii), (b) $$ \\to $$ (iv), (c) $$ \... | ["C"] | null | Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbital
<br><br>N<sub>a</sub> $$=$$ No of electrons in anti bonding molecular orbital
<br><br>(4) $$\,\,\,\,$$ upto 14 electrons, molecular orbital configuration is
<br><br><img class="que... | mcq | jee-main-2021-online-26th-february-evening-slot | 959 |
9ZObK2CT7396w4lhw01kmlnkmj6 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | AX is a covalent diatomic molecule where A and X are second row elements of periodic table. Based on Molecular orbital theory, the bond order of AX is 2.5. The total number of electrons in AX is __________. (Round off to the Nearest Integer). | [] | null | 15 | The compound AX is NO its bond order is 2.5 and it has total 15 electrons.
<br><br><b>Note :</b> Total number of electrons equal to 13 will
also have the 2.5 bond order. But in this case
neutral diatomic molecule will not be possible. | integer | jee-main-2021-online-18th-march-morning-shift | 960 |
1krx4sr8p | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | In the following the correct bond order sequence is : | [{"identifier": "A", "content": "$$O_2^{2 - } > O_2^ + > O_2^ - > {O_2}$$"}, {"identifier": "B", "content": "$$O_2^ + > O_2^ - > O_2^{2 - } > {O_2}$$"}, {"identifier": "C", "content": "$$O_2^ + > {O_2} > O_2^ - > O_2^{2 - }$$"}, {"identifier": "D", "content": "$${O_2} > O_2^ - > ... | ["C"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,\,\,\,$$ Bond strength $$ \propto $$ Bond order
<br><br>(2) $$\,\,\,\,$$ Bond length $$ \propto $$ $${1 \over {Bond\,\,order}}$$
<br><br>(3) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbi... | mcq | jee-main-2021-online-25th-july-evening-shift | 961 |
1krz3371p | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The difference between bond orders of CO and NO$$^ \oplus $$ is $${x \over 2}$$ where x = _____________. (Round off to the Nearest Integer) | [] | null | 0 | Bond order of CO = 3<br><br>Bond order of NO<sup>+</sup> = 3<br><br>Difference = 0 = $${x \over 2}$$<br><br>$$ \Rightarrow $$ x = 0
<br><br><b><u>Note</u> :</b>
<br><br>(1) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bending molecular orbital
... | integer | jee-main-2021-online-27th-july-morning-shift | 962 |
1ks1jnmhr | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The total number of electrons in all bonding molecular orbitals of $$O_2^{2 - }$$ is ______________.<br/><br/>(Round off to the nearest integer) | [] | null | 10 | N<sub>b</sub> = No of electrons in bonding molecular orbital
<br><br>N<sub>a</sub> $$=$$ No of electrons in anti bonding molecular orbital
<br><br>(1) $$\,\,\,\,$$ upto 14 electrons, molecular orbital configuration is
<br><br><img class="question-image" src="https://res.cloudinary.com/dckxllbjy/image/upload/v1734264... | integer | jee-main-2021-online-27th-july-evening-shift | 963 |
1ktcnvdv8 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The bond order and magnetic behaviour of $$O_2^ - $$ ion are respectively : | [{"identifier": "A", "content": "1.5 and paramagnetic "}, {"identifier": "B", "content": "1.5 and diamagnetic"}, {"identifier": "C", "content": "2 and diamagnetic"}, {"identifier": "D", "content": "1 and paramagnetic "}] | ["A"] | null | $$O_2^ - = {({\sigma _{1s}})^2}{(\sigma _{1s}^*)^2}{({\sigma _{2s}})^2}{(\sigma _{2s}^*)^2}{({\sigma _{2{p_z}}})^2}$$$$\left( {\pi _{2{p_x}}^2 = \pi _{2{p_y}}^2} \right)\left( {\pi _{2{p_x}}^{*2} = \pi _{2{p_y}}^{*1}} \right)$$<br><br>Bond order = $${{10 - 7} \over 2} = 1.5$$ <br><br>and paramagnetic. | mcq | jee-main-2021-online-26th-august-evening-shift | 964 |
1ktebop1v | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Match items of List-I with those of List-II :<br/><br/><table>
<thead>
<tr>
<th></th>
<th>List - I<br/>(Property)</th>
<th></th>
<th>List - II<br/>(Example)</th>
</tr>
</thead>
<tbody>
<tr>
<td>(a)</td>
<td>Diamagnetism</td>
<td>(i)</td>
<td>MnO</td>
</tr>
<tr>
<td>(b)</td>
<td>Ferrimagnetism</td>
<td>(ii)</td>
<td>$${... | [{"identifier": "A", "content": "(a)-(ii), (b)-(i), (c)-(iii), (d)-(iv)"}, {"identifier": "B", "content": "(a)-(i), (b)-(iii), (c)-(iv), (d)-(ii)"}, {"identifier": "C", "content": "(a)-(iii), (b)-(iv), (c)-(ii), (d)-(i)"}, {"identifier": "D", "content": "(a)-(iv), (b)-(ii), (c)-(i), (d)-(iii)"}] | ["C"] | null | <p> A. NaCl is diamagnetic because all electrons are paired in Na<sup>+</sup> and in Cl<sup>−</sup> . So, it shows diamagnetism. </p>
<p> B. Fe<sub>3</sub>O<sub>4</sub> is ferrimagnetic because of the presence of the unequal alignment of magnetic moment in opposite direction. </p>
<p> C. O<sub>2</sub> molecule has two ... | mcq | jee-main-2021-online-27th-august-morning-shift | 965 |
1ktn2xa2s | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | The spin-only magnetic moment value of $$B_2^ + $$ species is _____________ $$\times$$ 10<sup>$$-$$2</sup> BM. (Nearest integer) [Given : $$\sqrt 3 $$ = 1.73] | [] | null | 173 | $$B_2^ + \Rightarrow \sigma _{1s}^2\sigma _{1s}^{*2}\sigma _{2s}^2\sigma _{2s}^{*2}\pi _{2py}^1 \simeq \pi _{2pz}^0$$<br><br> It has one
unpaired electron.<br><br>Spin - only magnetic moment = $$\mu
$$
<br><br>= $$\sqrt {n\left( {n + 1} \right)} $$
<br><br>n = Number of unpaired electrons
<br><br>$$= \sqrt {1(1 + 2)... | integer | jee-main-2021-online-1st-september-evening-shift | 968 |
1l58di4xa | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>Consider the ions/molecule</p>
<p>O$$_2^ + $$, O<sub>2</sub>, O$$_2^ - $$, O$$_2^ {2-} $$</p>
<p>For increasing bond order the correct option is :</p> | [{"identifier": "A", "content": "O$$_2^ {2-} $$ < O$$_2^ - $$ < O<sub>2</sub> < O$$_2^ + $$"}, {"identifier": "B", "content": "O$$_2^ - $$ < O$$_2^ {2-} $$ < O<sub>2</sub> < O$$_2^ + $$"}, {"identifier": "C", "content": "O$$_2^ - $$ < O$$_2^ {2-} $$ < O$$_2^ + $$ < O<sub>2</sub>"}, {"identifier": "D", "content": "O$$_2... | ["A"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,\,\,\,$$ Bond strength $$ \propto $$ Bond order
<br><br>(2) $$\,\,\,\,$$ Bond length $$ \propto $$ $${1 \over {Bond\,\,order}}$$
<br><br>(3) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = Number of electrons in bonding molecular ... | mcq | jee-main-2022-online-26th-june-morning-shift | 969 |
1l5alkri6 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>Bonding in which of the following diatomic molecule(s) become(s) stronger, on the basis of MO Theory, by removal of an electron?</p>
<p>(A) NO</p>
<p>(B) N<sub>2</sub></p>
<p>(C) O<sub>2</sub></p>
<p>(D) C<sub>2</sub></p>
<p>(E) B<sub>2</sub></p>
<p>Choose the most appropriate answer from the options given below :</... | [{"identifier": "A", "content": "(A), (B), (C) only"}, {"identifier": "B", "content": "(B), (C), (E) only"}, {"identifier": "C", "content": "(A), (C) only"}, {"identifier": "D", "content": "(D) only"}] | ["C"] | null | If an electron is removed from the anti-bonding
orbital, then it will tend to increase the bond order.
The HOMO in NO and O<sub>2</sub> is antibonding molecular
orbital .<br/><br/>
Hence, in NO and O<sub>2</sub> bond order will increase on
loss of electron. | mcq | jee-main-2022-online-25th-june-morning-shift | 970 |
1l5bcwle0 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The correct order of bond orders of $${C_2}^{2 - }$$, $${N_2}^{2 - }$$ and $${O_2}^{2 - }$$</p> is, respectively | [{"identifier": "A", "content": "$${C_2}^{2 - }$$ < $${N_2}^{2 - }$$ < $${O_2}^{2 - }$$"}, {"identifier": "B", "content": "$${O_2}^{2 - }$$ < $${N_2}^{2 - }$$ < $${C_2}^{2 - }$$"}, {"identifier": "C", "content": "$${C_2}^{2 - }$$ < $${O_2}^{2 - }$$ < $${N_2}^{2 - }$$"}, {"identifier": "D", "content": "$${N_2}^{2 - }$$ ... | ["B"] | null | <b><u>Note</u> :</b>
<br><br>(1) $$\,$$ Bond order $$ = {1 \over 2}$$ [N<sub>b </sub> $$-$$ N<sub>a</sub>]
<br><br>N<sub>b</sub> = No of electrons in bonding molecular orbital
<br><br>N<sub>a</sub> $$=$$ No of electrons in anti bonding molecular orbital
<br><br>(2) $$\,\,\,\,$$ upto 14 electrons, molecular orbital... | mcq | jee-main-2022-online-24th-june-evening-shift | 971 |
1l6e1w620 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>Among the following species</p>
<p>$$\mathrm{N}_{2}, \mathrm{~N}_{2}^{+}, \mathrm{N}_{2}^{-}, \mathrm{N}_{2}^{2-}, \mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{-}, \mathrm{O}_{2}^{2-}$$</p>
<p>the number of species showing diamagnesim is _______________.</p> | [] | null | 2 | Those species which have unpaired electrons are called paramagnetic species.
<br><br>And those species which have no unpaired electrons are called diamagnetic species.
<br><br>(1) $$N_2$$ has 14 electrons.
<br><br>Moleculer orbital configuration of $$N_2$$
<br><br>= $${\sigma _{1{s^2}}}\,\sigma _{1{s^2}}^... | integer | jee-main-2022-online-25th-july-morning-shift | 972 |
1l6jn1ls9 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>According to MO theory, number of species/ions from the following having identical bond order is ________.</p>
<p>$$\mathrm{CN}^{-}, \mathrm{NO}^{+}, \mathrm{O}_{2}, \mathrm{O}_{2}^{+}, \mathrm{O}_{2}^{2+}$$</p> | [] | null | 3 | $\mathrm{CN}^{-}, \mathrm{NO}^{+}$and $\mathrm{O}_{2}^{2+}$ have bond order of 3
<br/><br/>
$\mathrm{O}_{2}$ has bond order of 2
<br/><br/>
$\mathrm{O}_{2}^{+}$ has bond order of $2.5$
<br/><br/>
$\therefore 3$ species have similar bond order. | integer | jee-main-2022-online-27th-july-morning-shift | 974 |
1ldscb4vt | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>According to MO theory the bond orders for $$\mathrm{O}$$$$_2^{2 - }$$, $$\mathrm{CO}$$ and $$\mathrm{NO^+}$$ respectively, are</p> | [{"identifier": "A", "content": "1, 3 and 3"}, {"identifier": "B", "content": "2, 3 and 3"}, {"identifier": "C", "content": "1, 2 and 3"}, {"identifier": "D", "content": "1, 3 and 2"}] | ["A"] | null | <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;border-width:1px;font-family:Arial,... | mcq | jee-main-2023-online-29th-january-evening-shift | 976 |
1ldwsjb3e | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>What is the number of unpaired electron(s) in the highest occupied molecular orbital of the following species : $$\mathrm{{N_2};N_2^ + ;{O_2};O_2^ + }$$ ?</p> | [{"identifier": "A", "content": "0, 1, 0, 1"}, {"identifier": "B", "content": "2, 1, 0, 1"}, {"identifier": "C", "content": "0, 1, 2, 1"}, {"identifier": "D", "content": "2, 1, 2, 1"}] | ["C"] | null | <style type="text/css">
.tg {border-collapse:collapse;border-spacing:0;width:100%}
.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;border-width:1px;font-family... | mcq | jee-main-2023-online-24th-january-evening-shift | 978 |
1lgq3vwp7 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>In which of the following processes, the bond order increases and paramagnetic character changes to diamagnetic one ?</p> | [{"identifier": "A", "content": "$$\\mathrm{O}_{2} \\rightarrow \\mathrm{O}_{2}^{2-}$$"}, {"identifier": "B", "content": "$$\\mathrm{N}_{2} \\rightarrow \\mathrm{N}_{2}^{+}$$"}, {"identifier": "C", "content": "$$\\mathrm{NO} \\rightarrow \\mathrm{NO}^{+}$$"}, {"identifier": "D", "content": "$$\\mathrm{O}_{2} \\rightarr... | ["C"] | null | Let's analyze each option:
<br/><br/>
Option A: $\mathrm{O}_{2} \rightarrow \mathrm{O}_{2}^{2-}$<br/><br/>
The bond order of $\mathrm{O}_{2}$ is 2 and it is paramagnetic. When two electrons are added to form $\mathrm{O}_{2}^{2-}$, the bond order becomes 1 (decreases) and it becomes diamagnetic. This option does not mee... | mcq | jee-main-2023-online-13th-april-morning-shift | 979 |
1lgrkbmlp | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The bond order and magnetic property of acetylide ion are same as that of</p> | [{"identifier": "A", "content": "$$\\mathrm{O}_{2}^{+}$$"}, {"identifier": "B", "content": "$$\\mathrm{O}_{2}^{-}$$"}, {"identifier": "C", "content": "$$\\mathrm{N}_{2}^{+}$$"}, {"identifier": "D", "content": "$$\\mathrm{NO}^{+}$$"}] | ["D"] | null | <p>The acetylide ion has the formula $$\mathrm{C}_{2}^{2-}$$. To determine its bond order, we need to first write the molecular orbital (MO) diagram for this ion. </p>
<p>The MO diagram for $$\mathrm{C}_{2}^{2-}$$ is:</p>
<p>$$\mathrm{σ_{1s}^{2}}\mathrm{σ_{1s}^{2}}\mathrm{σ_{2s}^{2}}\mathrm{σ_{2s}^{2}}\mathrm{π_{2p}^{4... | mcq | jee-main-2023-online-12th-april-morning-shift | 980 |
lsaowhvy | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | Given below are two statements :<br/><br/>
<b>Statement (I)</b> : A $\pi$ bonding MO has lower electron density above and below the inter-nuclear axis.
<br/><br/>
<b>Statement (II)</b> : The $\pi^*$ antibonding MO has a node between the nuclei.<br/><br/>
In the light of the above statements, choose the <b>most appropri... | [{"identifier": "A", "content": "Both Statement I and Statement II are true"}, {"identifier": "B", "content": "Both Statement I and Statement II are false"}, {"identifier": "C", "content": "Statement I is true but Statement II is false"}, {"identifier": "D", "content": "Statement I is false but Statement II is true"}] | ["D"] | null | <p>Let's analyze both statements:</p>
<p><b>Statement (I)</b>: "A $\pi$ bonding MO has lower electron density above and below the inter-nuclear axis."</p>
<p>This statement is false. In molecular orbital (MO) theory, a pi bond ($\pi$ bond) is formed by the sideways overlap of p-orbitals from two adjacent atoms. The c... | mcq | jee-main-2024-online-1st-february-evening-shift | 981 |
jaoe38c1lsc6u3er | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>Sum of bond order of CO and NO$$^+$$ is ________.</p> | [] | null | 6 | <p>$$\begin{array}{lcl}
\mathrm{CO} \Rightarrow & \overline{\mathrm{C}} \equiv \stackrel{+}{\mathrm{O}} & : \mathrm{BO}=3 \\
\mathrm{NO}^{+} \Rightarrow & \mathrm{N} \equiv \mathrm{O}^{+} & : \mathrm{BO}=3
\end{array}$$</p> | integer | jee-main-2024-online-27th-january-morning-shift | 982 |
jaoe38c1lse7imu1 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The linear combination of atomic orbitals to form molecular orbitals takes place only when the combining atomic orbitals</p>
<p>A. have the same energy</p>
<p>B. have the minimum overlap</p>
<p>C. have same symmetry about the molecular axis</p>
<p>D. have different symmetry about the molecular axis</p>
<p>Choose the... | [{"identifier": "A", "content": "B, C, D only"}, {"identifier": "B", "content": "A, B, C only"}, {"identifier": "C", "content": "B and D only"}, {"identifier": "D", "content": "A and C only"}] | ["D"] | null | <p>* Molecular orbital should have maximum overlap</p>
<p>* Symmetry about the molecular axis should be similar</p> | mcq | jee-main-2024-online-31st-january-morning-shift | 983 |
jaoe38c1lsfk4s5c | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The number of species from the following which are paramagnetic and with bond order equal to one is _________.</p>
<p>$$\mathrm{H}_2, \mathrm{He}_2^{+}, \mathrm{O}_2^{+}, \mathrm{N}_2^{2-}, \mathrm{O}_2^{2-}, \mathrm{F}_2, \mathrm{Ne}_2^{+}, \mathrm{B}_2$$</p> | [] | null | 1 | <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;border-width:1px;font-family:Arial,... | integer | jee-main-2024-online-29th-january-morning-shift | 984 |
jaoe38c1lsfplid6 | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The total number of anti bonding molecular orbitals, formed from $$2 s$$ and $$2 p$$ atomic orbitals in a diatomic molecule is _______.</p> | [] | null | 4 | <p>Antibonding molecular orbital from $$2 \mathrm{~s}=1$$</p>
<p>Antibonding molecular orbital from $$2 p=3$$</p>
<p>Total $$=4$$</p> | integer | jee-main-2024-online-29th-january-evening-shift | 985 |
1lsgyk5tt | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>The total number of molecular orbitals formed from $$2 \mathrm{s}$$ and $$2 \mathrm{p}$$ atomic orbitals of a diatomic molecule is __________.</p> | [] | null | 8 | <p>Two molecular orbitals $$\sigma 2 \mathrm{s}$$ and $$\sigma * 2 \mathrm{s}$$.</p>
<p>Six molecular orbitals $$\sigma 2 \mathrm{p}_z$$ and $$\sigma * 2 \mathrm{p}_{\mathrm{z}}$$.</p>
<p>$$\pi 2 \mathrm{p}_{\mathrm{x}}, \pi 2 \mathrm{p}_{\mathrm{y}}$$ and $$\pi * 2 \mathrm{p}_{\mathrm{x}}, \pi^* 2 \mathrm{p}_{\mathrm{... | integer | jee-main-2024-online-30th-january-morning-shift | 986 |
luy1mwmf | chemistry | chemical-bonding-and-molecular-structure | molecular-orbital-theory | <p>Total number of electrons present in $$\left(\pi^*\right)$$ molecular orbitals of $$\mathrm{O}_2, \mathrm{O}_2^{+}$$ and $$\mathrm{O}_2^{-}$$ is ________.</p> | [] | null | 6 | <p>$$\begin{aligned}
& \mathrm{O}_2(16 \mathrm{e}):\left(\sigma_{1 \mathrm{~s}}\right)^2\left(\sigma_{1 \mathrm{~s}}^*\right)^2\left(\sigma_{2 \mathrm{~s}}\right)^2\left(\sigma_{2 \mathrm{~s}}^*\right)^2 \\
& \left(\sigma_{2 \mathrm{p}}\right)^2\left[\left(\pi_{2 \mathrm{p}}\right)^2=\left(\pi_{2 \mathrm{p}}\right)^2\r... | integer | jee-main-2024-online-9th-april-evening-shift | 987 |
Subsets and Splits
No community queries yet
The top public SQL queries from the community will appear here once available.