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On adding chlorine water, bromine and Iodine are displaced from their solutions by chlorine. Bromine is more electronegative than iodide but less 6than chlorine. On adding Bromine water, iodine is displaced from its solution but not chlorine. Table showing the displacement of the halogens (V) means there is displacemen... | {
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- Reduce tooth decay when added in small amounts/quantities in tooth paste. NB –large small quantities of fluorine /fluoride ions in water cause browning of teeth/flourosis. - Hydrogen fluoride is used to engrave words /pictures in glass. (ii) Bromine - Silver bromide is used to make light sensitive photographic paper/... | {
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They therefore do not acquire/gain extra electron in the outer energy level or donate/lose. They therefore are therefore zerovalent . The number of energy levels increases down the group from Helium to Randon. The more the number of energy levels the bigger/larger the atomic size/radius. e.g. The atomic size/radius of ... | {
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The intermolecular/van-der-waals forces increase down the group as the atomic radius/size increase from Helium to Radon. The melting and boiling points thus increase also down the group. Noble gases are insoluble in water and are poor conductors of electricity. Element Formula of molecule Electrical conductivity Solubi... | {
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The trends in physical and chemical properties of elements in the same group vary down the group. Elements in the same group thus constitute a chemical family. (a) Group I elements: Alkali metals Group I elements are called Alkali metals except Hydrogen which is a non metal. The alkali metals include: Element Symbol At... | {
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The atomic radius of Francium is bigger/larger than that of sodium because Francium has more/7 energy levels than sodium (3 energy levels). Atomic radius and ionic radius of alkali metals increase down the group as the number of energy levels increases. The atomic radius of alkali metals is bigger than the ionic radius... | {
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For alkali metals the 1st ionization energy decrease down the group as the atomic radius increase and the effective nuclear attraction on outer energy level electrons decrease. e.g. The 1st ionization energy of sodium is 496 kJmole-1 while that of potassium is 419 kJmole-1 .This is because atomic radius increase and th... | {
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Summary of some physical properties of the 1st three alkali metals Alkali metal Appearance Ease of cutting Melting point (oC) Boiling point (oC) Conductivity 1st ionization energy Lithium Silvery white Not easy 180 1330 Good 520 Sodium Shiny grey Easy 98 890 Good 496 Potassium Shiny grey Very easy 64 774 Good 419
4 Che... | {
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Put three drops of phenolphthalein indicator. Put about 0.5g of Lithium metal into the beaker. Determine the pH of final product Repeat the experiment using about 0.1 g of Sodium and Potassium. Caution: Keep a distance Observations
5 Alkali metal Observations Comparative speed/rate of the reaction Lithium -Metal floats... | {
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Potassium is more reactive than sodium .Sodium is more reactive than Lithium. The reactivity increases as electropositivity increases of the alkali increases. This is because as the atomic radius increases , the ease of donating/losing outer electron increase during chemical reactions. 6 Chemical equations 2Li(s) + 2H2... | {
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Lithium metal continues to burn with a crimson flame forming white solid / fumes. Alkali metal react with chlorine gas to form the corresponding metal chlorides. The reactivity increase as electropositivity increase down the group from Lithium to Francium.The ease of donating/losing the outer electrons increase as the ... | {
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(v)Sodium is used as a reducing agent for the extraction of titanium from Titanium(IV)chloride. (vi)Lithium is used in making special high strength glasses (vii)Lithium compounds are used to make dry cells in mobile phones and computer laptops. Group II elements: Alkaline earth metals Group II elements are called Alkal... | {
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They donate /lose the two outer electrons to have oxidation state M2+ The number of energy levels increases down the group from Beryllium to Radium. The more the number of energy levels the bigger/larger the atomic size. e.g. The atomic size/radius of Calcium is bigger/larger than that of Magnesium because Calcium has ... | {
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e.g. The 1st ionization energy of Magnesium is 900 kJmole-1 while that of Calcium is 590 kJmole-1 .This is because atomic radius increase and thus effective nuclear attraction on outer energy level electrons decrease down the group from magnesium to calcium. It requires therefore less energy to donate/lose outer electr... | {
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The surface slowly tarnishes on exposure to air. This is because the metal surface slowly undergoes oxidation to form an oxide. This oxide layer should be removed before using the alkaline earth metals. Melting and boiling points: Alkaline earth metals have a relatively high melting/ boiling point than alkali metals. T... | {
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The more delocalized electrons the better the electrical conductor. Calcium is a better conductor than magnesium. Calcium has bigger/larger atomic radius than magnesium because the delocalized electrons are less attracted to the nucleus of calcium and thus more free /mobile and thus better the electrical conductor Summ... | {
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Repeat with Calcium Observations -Magnesium burns with a bright blindening flame -White solid /ash produced -Solid dissolves in water to form a colourless solution -Blue litmus paper remain blue -Red litmus paper turns blue -colourless gas with pungent smell of urine Explanation Magnesium burns in air with a bright bli... | {
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Observations -Surface of magnesium covered by bubbles of colourless gas. -Colourless solution formed. -Effervescence/bubbles/fizzing takes place in Calcium. -Red litmus paper turns blue. -Blue litmus paper remains blue. Explanations Magnesium slowly reacts with cold water to form Magnesium hydroxide and bubbles of Hydr... | {
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-Pale green colour of chlorine fades. Explanation Magnesium continues to burn in chlorine gas forming white magnesium oxide solid. Mg(s) + Cl2 (g) -> MgCl2 (s) Calcium burns slightly in chlorine gas to form white calcium oxide solid. Calcium oxide formed coat unreacted Calcium stopping further reaction Ca(s) + Cl2 (g) ... | {
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15 Nitric(V)acid is a strong oxidizing agent. It quickly oxidizes the hydrogen produced to water. Calcium is very reactive with dilute acids and thus a very small piece of very dilute acid should be used. Chemical equations Mg(s) + H2SO4 (aq) -> MgSO4(aq) + H2 (g) Mg(s) + 2HNO3 (aq) -> Mg(NO3)2(aq) + H2 (g) Mg(s) + 2HC... | {
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Chemical equations Mg(s) + H2SO4 (aq) -> MgSO4(aq) + H2 (g) Mg(s) + 2HNO3 (aq) -> Mg(NO3)2(aq) + H2 (g) Mg(s) + 2HCl (aq) -> MgCl2(aq) + H2 (g) Ca(s) + H2SO4 (aq) -> CaSO4(s) + H2 (g) (insoluble CaSO4(s) coat/cover Ca(s)) Ca(s) + 2HNO3 (aq) -> Ca(NO3)2(aq) + H2 (g) Ca(s) + 2HCl (aq) -> CaCl2(aq) + H2 (g) Ba(s) + H2SO4 ... | {
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(ii)Making duralumin. Duralumin is an alloy of Magnesium and aluminium used for making aeroplane bodies because it is light. Beryllium Magnesium Calcium Barium Hydroxide Be(OH)2 Mg(OH)2 Ca(OH)2 Ba(OH)2 Oxide BeO MgO CaO BaO Sulphide - MgS CaS BaS Chloride BeCl2 MgCl2 CaCl2 BaCl2 Carbonate BeCO3 MgCO3 CaCO3 BaCO3 Nitrat... | {
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They are all non metals. They include: Element Symbol Atomic number Electronicc configuration Charge of ion Valency State at Room Temperature Fluorine Chlorine Bromine Iodine Astatine F Cl Br I At 9 17 35 53 85 2:7 2:8:7 2:8:18:7 2:8:18:18:7 2:8:18:32:18:7 F- Cl- Br- I- At- 1 1 1 1 1 Pale yellow gas Pale green gas Red ... | {
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Table showing the atomic and ionic radius of four Halogens Element Symbol Atomic number Atomic radius(nM) Ionic radius(nM) Fluorine F 9 0.064 0.136 Chlorine Cl 17 0.099 0.181 Bromine Br 35 0.114 0.195 Iodine I 53 0.133 0.216 The atomic radius of Chlorine is 0.099nM .The ionic radius of Cl- is 0.181nM. This is because C... | {
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The SI unit of electron affinity is kilojoules per mole/kJmole-1 . Electron affinity depend on atomic radius. The higher the atomic radius, the less effective the nuclear attraction on outer energy level electrons and thus the lower the electron affinity. For halogens the 1st electron affinity decrease down the group a... | {
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Melting/Boiling point The strength of intermolecular/Van-der-waals forces of attraction increase with increase in molecular size/atomic radius. Iodine has therefore the largest atomic radius and thus strongest intermolecular forces to make it a solid. Iodine sublimes when heated to form (caution: highly toxic/poisonous... | {
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The level of water in chlorine is higher than in bromine and the level of tetrachloromethane in chlorine is lower than in bromine. Caution: Tetrachloromethane , Bromine vapour and Chlorine gas are all highly toxic/poisonous. 20 Table showing the physical properties of Halogens Halogen Formula of molecule Electrical con... | {
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On adding chlorine water, bromine and Iodine are displaced from their solutions by chlorine. Bromine is more electronegative than iodide but less 6than chlorine. 21 On adding Bromine water, iodine is displaced from its solution but not chlorine. Table showing the displacement of the halogens (V) means there is displace... | {
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- Reduce tooth decay when added in small amounts/quantities in tooth paste. NB –large small quantities of fluorine /fluoride ions in water cause browning of teeth/flourosis. - Hydrogen fluoride is used to engrave words /pictures in glass. (ii) Bromine - Silver bromide is used to make light sensitive photographic paper/... | {
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They therefore do not acquire/gain extra electron in the outer energy level or donate/lose. They therefore are therefore zerovalent . The number of energy levels increases down the group from Helium to Randon. The more the number of energy levels the bigger/larger the atomic size/radius. e.g. The atomic size/radius of ... | {
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The intermolecular/van-der-waals forces increase down the group as the atomic radius/size increase from Helium to Radon. The melting and boiling points thus increase also down the group. Noble gases are insoluble in water and are poor conductors of electricity. Element Formula of molecule Electrical conductivity Solubi... | {
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Ionic bonding in sodium chloride Sodium (2,8,1) has 1 electron more than a stable noble gas structure (2,8). If it gave away that electron it would become more stable. Chlorine (2,8,7) has 1 electron short of a stable noble gas structure (2,8,8). If it could gain an electron from somewhere it too would become more stab... | {
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They conduct electricity in the aqueous state because the ions are free to move. Most ionic substances are soluble in water because the polar water molecules can accommodate the charged ions. COVALENT BONDING - SINGLE BONDS As well as achieving noble gas structures by transferring electrons from one atom to another... | {
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As there are weak, Van der Waal's forces between the molecules, they are not held in rigid position. The state depends on the bond energy. If the bond energy is very low, they stay as gases, if it is appreciable they are volatile liquids. If very high, they exist as soft solids. 3) Covalent compounds generally have low... | {
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This is again due to the need to break very strong covalent bonds operating in 3dimensions. Doesnಬt conduct electricity. All the electrons are held tightly between the atoms, and aren't free to move. Is insoluble in water and organic solvents. There are no possible attractions which could occur between solvent mole... | {
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You can think of graphite rather like a pack of cards - each card is strong, but the cards will slide over each other, or even fall off the pack altogether. When you use a pencil, sheets are rubbed off and stick to the paper. Has a lower density than diamond. This is because of the relatively large amount of space th... | {
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Uses of Silica i) Quartz glass is used for manufacturing optical instruments. ii) Colored quartz is used for manufacturing gems. iii) Sand is used in manufacture of glass, porcelain, sand paper and mortar etc. iv) Sand stone is used as a building material. CO-ORDINATE (DATIVE COVALENT) BONDING Co-ordinate (dative coval... | {
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The forces of attraction which hold an individual molecule together (for example, the covalent bonds) are known as
intramolecular attractions. All molecules experience intermolecular attractions, although in some cases those attractions are very weak. Even in a gas like hydrogen, H2, if you slow the molecules down by c... | {
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Hydrogen bonding makes water molecules "stick" together. This makes water have high melting and boiling points compared to other covalent compounds such as ammonia (NH3) which have similar molecular mass but are gases Ice and Hydrogen Bonding The structure that forms in the solid ice crystal actually has large holes in... | {
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The hydrogen bonding is limited by the fact that there is only one hydrogen in each ethanol molecule with sufficient + charge. In methoxymethane, the lone pairs on the oxygen are still there, but the hydrogens aren't sufficiently + for hydrogen bonds to form. Except in some rather unusual cases, the hydrogen atom has... | {
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His type of bonding (called metallic boding) is present in alloys as well. Alloys, for example solder and brass, will conduct electricity. The physical properties of metals: This strong bonding generally results in dense, strong materials with high melting and boiling points. Usually a relatively large amount of energy... | {
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(c) Some salts are normal salts while other are acid salts. (i)A normal salt is formed when all the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. (ii)An acid salt is formed when part/portion the ionizable /replaceable hydrogen in an acid is replaced by a metal or metal... | {
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(i)A normal salt is formed when all the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. (ii)An acid salt is formed when part/portion the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. Table showing normal and acid salts d... | {
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(ii)An acid salt is formed when part/portion the ionizable /replaceable hydrogen in an acid is replaced by a metal or metallic /ammonium radical. Table showing normal and acid salts derived from common acids Acid name Chemical formula Basicity Normal salt Acid salt Hydrochloric acid HCl Monobasic Chloride(Cl-) None Nit... | {
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Table showing normal and acid salts derived from common acids Acid name Chemical formula Basicity Normal salt Acid salt Hydrochloric acid HCl Monobasic Chloride(Cl-) None Nitric(V)acid HNO3 Monobasic Nitrate(V)(NO3-) None Nitric(III)acid HNO2 Monobasic Nitrate(III)(NO2-) None Sulphuric(VI)acid H2SO4 Dibasic Sulphate(VI... | {
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Base/alkali Cation Acid Anion Salt Chemical name of salts NaOH Na+ HCl Cl NaCl Sodium(I)chloride Mg(OH)2 Mg2+ H2SO4 SO42 MgSO4 Mg(HSO4)2 Magnesium sulphate(VI) Magnesium hydrogen sulphate(VI) Pb(OH)2 Pb2+ HNO3 NO3 Pb(NO3)2 Lead(II)nitrate(V) Ba(OH)2 Ba2+ HNO3 NO3 Ba(NO3)2 Barium(II)nitrate(V) Ca(OH)2 Ba2+ H2SO4 SO42 Mg... | {
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(ii)Deliquescent salts /compounds are those that absorb water from the atmosphere and form a solution. Some salts which are deliquescent include: Sodium nitrate(V),Calcium chloride, Sodium hydroxide, Iron(II)chloride, Magnesium chloride. (iii)Efflorescent salts/compounds are those that lose their water of crystallizati... | {
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Table showing some hydrated salts. Name of hydrated salt Chemical formula Copper(II)sulphate(VI)pentahydrate CuSO4.5H2O Aluminium(III)sulphate(VI)hexahydrate Al2 (SO4) 3.6H2O Zinc(II)sulphate(VI)heptahydrate ZnSO4.7H2O Iron(II)sulphate(VI)heptahydrate FeSO4.7H2O Calcium(II)sulphate(VI)heptahydrate CaSO4.7H2O Magnesium(... | {
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Below are some complex salts. Table of some complex salts Name of complex salt Chemical formula Colour of the complex salt Tetraamminecopper(II)sulphate(VI) Cu(NH3) 4 SO4 H2O Royal/deep blue solution
Tetraamminezinc(II)nitrate(V) Zn(NH3) 4 (NO3 )2 Colourless solution Tetraamminecopper(II) nitrate(V) Cu(NH3) 4 (NO3 )2 R... | {
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They are said to be soluble. Others do not dissolve in water. They form a suspension/precipitate in water. Table of solubility of salts Soluble salts Insoluble salts All nitrate(V)salts All sulphate(VI)/SO42- salts except Barium(II) sulphate(VI)/BaSO4 Calcium(II) sulphate(VI)/CaSO4 Lead(II) sulphate(VI)/PbSO4 All sulph... | {
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The filtrate is heated to concentrate then allowed to crystallize. Washing with distilled water then drying between filter papers produces a sample crystal of the salt. i.e. M(s) + H2X -> MX(aq) + H2(g) Examples Mg(s) + H2SO4(aq) -> MgSO4 (aq) + H2(g) Zn(s) + H2SO4(aq) -> ZnSO4 (aq) + H2(g) Pb(s) + 2HNO3(aq) -> Pb(NO3)... | {
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M(s) + H2X -> MX(aq) + H2(g) Examples Mg(s) + H2SO4(aq) -> MgSO4 (aq) + H2(g) Zn(s) + H2SO4(aq) -> ZnSO4 (aq) + H2(g) Pb(s) + 2HNO3(aq) -> Pb(NO3) 2(aq) + H2(g) Ca(s) + 2HNO3(aq) -> Ca(NO3) 2(aq) + H2(g) Mg(s) + 2HNO3(aq) -> Mg(NO3) 2(aq) + H2(g) Mg(s) + 2HCl(aq) -> MgCl 2(aq) + H2(g) Zn(s) + 2HCl(aq) -> ZnCl 2(aq) + H... | {
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Excess of the base is filtered off. The filtrate is heated to concentrate ,allowed to crystallize then washed with distilled water before drying between filter papers e.g. PbO(s) + 2HNO3(aq) -> Pb(NO3) 2(aq) + H2O (l) Pb(OH)2(s) + 2HNO3(aq) -> Pb(NO3) 2(aq) + 2H2O (l) CaO (s) + 2HNO3(aq) -> Ca(NO3) 2(aq) + H2O (l) MgO ... | {
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By adding an excess of a soluble /insoluble carbonate or hydrogen carbonate to adilute acid, effervescence /fizzing/bubbling out of carbon(IV)oxide gas shows the
reaction is taking place. When effervescence /fizzing/bubbling out of the gas is over, excess of the insoluble carbonate is filtered off. The filtrate is heat... | {
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When effervescence /fizzing/bubbling out of the gas is over, excess of the insoluble carbonate is filtered off. The filtrate is heated to concentrate ,allowed to crystallize then washed with distilled water before drying between filter paper papers e.g. PbCO3 (s) + 2HNO3(aq) -> Pb(NO3) 2(aq) + H2O (l)+ CO2(g) ZnCO3 (s)... | {
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PbCO3 (s) + 2HNO3(aq) -> Pb(NO3) 2(aq) + H2O (l)+ CO2(g) ZnCO3 (s) + 2HNO3(aq) -> Zn(NO3) 2(aq) + H2O (l)+ CO2(g) CaCO3 (s) + 2HNO3(aq) -> Ca(NO3) 2(aq) + H2O (l)+ CO2(g) MgCO3 (s) + H2SO4(aq) -> MgSO4(aq) + H2O (l)+ CO2(g) Cu CO3 (s) + H2SO4(aq) -> CuSO4(aq) + H2O (l) + CO2(g) Ag2CO3 (s) + 2HNO3(aq) -> 2AgNO3(aq) + H2... | {
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The procedure is then repeated without the indicator .The solution mixture is then heated to concentrate , allowed to crystallize ,washed with distilled water before drying with filter papers. e.g. NaOH (aq) + HNO3(aq) -> NaNO3(aq) + H2O (l) KOH (aq) + HNO3(aq) -> KNO3(aq) + H2O (l) KOH (aq) + HCl(aq) -> KCl(aq) + H2O ... | {
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Care should be taken to avoid water/moisture into the reaction flask during their preparation.Such salts include aluminium(III)chloride(AlCl3) and iron (III)chloride(FeCl3)
1. Heated aluminium foil reacts with chlorine to form aluminium(III)chloride that sublimes away from the source of heating then deposited as solid ... | {
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FeCl3(s)+ 3H2 O(g) -> Fe(OH)3 (aq) + 3HCl(g) (b)Insoluble salts can be prepared by reacting two suitable soluble salts to form one soluble and one insoluble. This is called double decomposition or precipitation. The mixture is filtered and the residue is washed with distilled water then dried. CuSO4(aq) + Na2CO3 (aq) -... | {
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Ammonium chloride sublimes on gentle heating. It dissociate into the constituent ammonia and hydrogen chloride gases on strong heating. NH4Cl(s) NH4Cl(g) NH3(g) + HCl(g) (sublimation) (dissociation) (b)effect of heat on nitrate(V) (i) Potassium nitrate(V)/KNO3 and sodium nitrate(V)/NaNO3 decompose on heating to form Po... | {
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2Ca(NO3)2 (s) -> 2CaO(s) + 4NO2(g) + O2(g) 2Mg(NO3)2(s) -> 2MgO(s) + 4NO2(g) + O2(g) 2Zn(NO3)2(s) -> 2ZnO(s) + 4NO2(g) + O2(g) 2Pb(NO3)2(s) -> 2PbO(s) + 4NO2(g) + O2(g) 2Cu(NO3)2(s) -> 2CuO(s) + 4NO2(g) + O2(g) 2Fe(NO3)2(s) -> 2FeO(s) + 4NO2(g) + O2(g) (iii)Silver(I)nitrate(V) and mercury(II) nitrate(V) are lowest in t... | {
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2AgNO3(s) -> 2Ag (s) + 2NO2(g) + O2(g) 2Hg(NO3)2 (s) -> 2Hg (s) + 4NO2(g) + O2(g) (iv)Ammonium nitrate(V) and Ammonium nitrate(III) decompose on heating to Nitrogen(I)oxide(relights/rekindles glowing splint) and nitrogen gas respectively.Water is also formed.i.e. NH4NO3(s) -> N2O (g) + H2O(l) NH4NO2(s) -> N2 (g) + H2O(... | {
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e.g. CuCO3 (s) -> CuO(s) + CO2(g) CaCO3 (s) -> CaO(s) + CO2(g) PbCO3 (s) -> PbO(s) + CO2(g) FeCO3 (s) -> FeO(s) + CO2(g) ZnCO3 (s) -> ZnO(s) + CO2(g) (iii)Sodium hydrogen carbonate(IV) and Potassium hydrogen carbonate(IV)decompose on heating to give the corresponding carbonate (IV) and form water and carbon(IV)oxide ga... | {
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Common weak electrolytes include: (i)all organic acids (ii)all bases except sodium hydroxide/potassium hydroxide. (iii)Water 4. A compound that is not decomposed by an electric current is called nonelectrolyte. Non-electrolytes are those compounds /substances that exist as molecules and thus cannot ionize/dissociate in... | {
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M(l) -> M+(l) + e (for cations from molten electrolytes) M(s) -> M+(aq) + e (for cations from electrolytes in aqueous state / solution / dissolved in water) The neutral atoms /molecules form the products of electrolysis at the anode. This is called discharge at anode 10. During electrolysis, free cations are attracted ... | {
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3 BatteryAnode(+)Cathode(-)ElectrolyteSimple set up of electrolytic cellGaseous product at anodeGaseous product at cathode 12. For a compound /salt containing only two ion/binary salt the products of electrolysis in an electrolytic cell can be determined as in the below examples: a)To determine the products of electrol... | {
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II.At the anode pale green chlorine gas. b)To determine the products of electrolysis of molten Zinc bromide
4 (i)Decomposition of electrolyte into free ions; ZnBr2 (l) -> Zn 2+(l) + 2Br-(l) (Compound decomposed into free cation and anion in liquid state) (ii)At the cathode/negative electrode(-); Zn 2+(l) + 2e -> Zn(l) ... | {
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II.At the anode red bromine liquid / red/brown bromine gas. c)To determine the products of electrolysis of molten sodium chloride (i)Decomposition of electrolyte into free ions; NaCl (l) -> Na +(l) + Cl-(l) (Compound decomposed into free cation and anion in liquid state) (ii)At the cathode/negative electrode(-); 2Na+(l... | {
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Potassium, sodium ,magnesium, and aluminium are extracted from their ores using electrolytic methods. (b)Purifying copper after exraction from copper pyrites ores. Copper obtained from copper pyrites ores is not pure. After extraction, the copper is refined by electrolysing copper(II)sulphate(VI) solution using the imp... | {
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Example: During the electroplating of a spoon with silver (i)the spoon/impure is placed as the cathode(negative terminal of battery) (ii)the pure silver is placed as the anode(positive terminal of battery) (iii)the pure silver erodes/ionizes/dissociates to release electrons: Ag(s) ->Ag+ (aq) + e (impure silver erodes/d... | {
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(ii)amorphous carbon in coal, peat ,charcoal and coke. (iii)carbon(IV)oxide gas accounting 0.03% by volume of normal air in the atmosphere. (b)Allotropes of Carbon Carbon naturally occur in two main crystalline allotropic forms, carbon-graphite and carbon-diamond Carbon-diamond Carbon-graphite Shiny crystalline solid B... | {
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Explanation Carbon burns in air and faster in Oxygen with a blue non-sooty/non-smoky flame forming Carbon (IV) oxide gas. Carbon burns in limited supply of air with a blue non-sooty/non-smoky flame forming Carbon (IV) oxide gas. Carbon (IV) oxide gas dissolve in water to form weak acidic solution of Carbonic (IV)acid. ... | {
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Heat strongly. Observation Colour change from black to brown Explanation
3 Carbon is a reducing agent. For ages it has been used to reducing metal oxide ores to metal, itself oxidized to carbon(IV)oxide gas. Carbon reduces black copper(II)oxide to brown copper metal Chemical Equation 2CuO(s) + C(s) -> 2Cu(s) + CO2(g) (... | {
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(b)School Laboratory preparation In the school laboratory carbon(IV)oxide can be prepared in the school laboratory from the reaction of marble chips(CaCO3)or sodium hydrogen carbonate(NaHCO3) with dilute hydrochloric acid. 5 (c)Properties of carbon(IV)oxide gas(Questions) 1.Write the equation for the reaction for the s... | {
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6 Chemical equation NaHCO3(s) + HCl(aq) -> Na2CO3 (aq) + H2O(l) + CO2 (g) (c)concentrated sulphuric(VI)acid? To dry the gas/as a drying agent 4.Describe the smell of carbon(IV)oxide gas Colourless and odourless 5. Effect on lime water. Experiment Bubbled carbon(IV)oxide gas into a test tube containing lime water for ab... | {
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Chemical equation 2Mg(s) + CO2 (g) -> C (s) + 2MgO(l)
7 7. Dry and wet litmus papers were separately put in a gas jar containing dry carbon (IV)oxide gas. State and explain the observations made. Observation Blue dry litmus paper remain blue Red dry litmus paper remain Red Blue wet/damp/moist litmus paper turn red Red ... | {
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Reaction forms insoluble Lead(II)Chloride that cover/coat unreacted Lead(II) carbonate stopping further reaction unless the reaction mixture is heated. Lead(II)Chloride is soluble in hot water. Chemical equation PbCO3(s) + 2HCl (aq) -> PbCl2 (s) + H2O(l) + CO2 (g) 9. Describe the test for the presence of Carbon (IV)oxi... | {
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(ii) Carbon(II)Oxide (CO) (a)Occurrence Carbon(II)oxide is found is found from incomplete combustion of fuels like petrol charcoal, liquefied Petroleum Gas/LPG. (b)School Laboratory preparation In the school laboratory carbon(II)oxide can be prepared from dehydration of methanoic acid/Formic acid(HCOOH) or Ethan-1,2-di... | {
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Downward delivery because the gas is 1 ½ times denser than air . 3.What is the purpose of : (i) Potassium hydroxide/sodium hydroxide in Method 1 To absorb/ remove carbon (II) oxide produced during the reaction. 2KOH (aq) + CO2 (g) -> K2CO3 (s) + H2O(l) 2NaOH (aq) + CO2 (g) -> Na2CO3 (s) + H2O(l) (ii) Concentrated sulph... | {
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Observation Colour change from black to brown. Excess carbon (II)oxide burn with a blue flame. Flame K Dry carbon(II)oxide
11 Explanation Carbon is a reducing agent. It is used to reduce metal oxide ores to metal, itself oxidized to carbon(IV)oxide gas. Carbon(II)Oxide reduces black copper(II)oxide to brown copper meta... | {
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This reaction is exothermic(-∆H) producing more heat. Chemical equation C(s) + O2(g) -> CO2(g) Carbon(IV)oxide gas formed rises up to meet more charcoal which reduces it to Carbon(II)oxide gas. Chemical equation 2CO2 (g) + O2(g) -> 2CO (g) At the top of burner in region II, Carbon (II)oxide gas is further oxidized to C... | {
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State the main uses of carbon (II)oxide gas. (i) As a fuel /water gas (ii)As a reducing agent in the blast furnace for extracting iron from iron ore(Magnetite/Haematite) (iii)As a reducing agent in extraction of Zinc from Zinc ore/Zinc blende (iv) As a reducing agent in extraction of Lead from Lead ore/Galena (v) As a ... | {
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3.The following experiments show the effect of heat on Carbonate (IV) (CO32-) and Hydrogen carbonate (IV) (HCO3-) salts: Experiment In a clean dry test tube place separately about 1.0 of the following: Zinc(II)carbonate(IV), sodium hydrogen carbonate(IV), sodium carbonate(IV), Potassium carbonate(IV) ammonium carbonate... | {
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Chemical equation Na2CO3 .10H2O(s) -> Na2CO3 (s) + 10H2O(l)
14 K2CO3 .10H2O(s) -> K2CO3 (s) + 10H2O(l) 2. Carbonate (IV) (CO32-) and Hydrogen carbonate (IV) (HCO3-) salts decompose on heating except Sodium carbonate(IV) and Potassium carbonate(IV). (a) Sodium hydrogen carbonate(IV) and Potassium hydrogen carbonate(IV) ... | {
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Chemical equation 2NaHCO3 (s) -> Na2CO3 (s) + H2O(l) + CO2 (g) (white) (white) 2KHCO3 (s) -> K2CO3 (s) + H2O(l) + CO2 (g) (white) (white) (b) Calcium hydrogen carbonate(IV) and Magnesium hydrogen carbonate(IV) decompose on heating to form insoluble Calcium carbonate(IV) and Magnesium carbonate(IV).Water and carbon(IV)o... | {
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Chemical equation Ca(HCO3)2 (aq) -> CaCO3 (s) + H2O(l) + CO2 (g) (Colourless solution) (white) Mg(HCO3)2 (aq) -> MgCO3 (s) + H2O(l) + CO2 (g) (Colourless solution) (white) (c) Ammonium hydrogen carbonate(IV) decompose on heating to form ammonium carbonate(IV) .Water and carbon(IV)oxide gas are also produced. Chemical e... | {
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Observation inference White precipitate/ppt CO32- ,SO32- ,SO42- ,Cl- - II. To the preserved solution ,add six drops of dilutte nitric(V)acid. Preserve. Observation inference White precipitate/ppt persists White precipitate/ppt dissolves SO42- ,Cl- CO32- ,SO32- II. To the preserved sample( that forms a precipitate ),hea... | {
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To the preserved sample in (I) above, add six drops of 2M nitric(V) acid . Preserve. Observation 1 Observation Inference White precipitate/ppt persists SO42- , ions Observation 2 Observation Inference White precipitate/ppt dissolves SO32- , CO32- , ions III.To the preserved sample observation 2 in (II) above, add 4 dro... | {
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Chemical/ionic equation: Pb2+(aq) + Cl- (aq) -> PbCl2(s) Pb2+(aq) + SO42+ (aq) -> PbSO4 (s) Pb2+(aq) + SO32+ (aq) -> PbSO3 (s) Pb2+(aq) + CO32+ (aq) -> PbCO3 (s) (ii)When the insoluble precipitates are acidified with nitric(V) acid, - Lead(II)chloride and Lead(II)sulphate(VI) do not react with the acid and thus their w... | {
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Chemical/ionic equation: PbSO3 (s) + 2H+(aq) -> H2 O (l) + Pb2+(aq) + SO2 (g) PbCO3 (s) + 2H+(aq) -> H2 O (l) + Pb2+(aq) + CO2 (g) (iii)When Lead(II)chloride and Lead(II)sulphate(VI) are heated/warmed; - Lead(II)chloride dissolves in hot water/on boiling(recrystallizes on cooling) - Lead(II)sulphate(VI) do not dissolve... | {
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Chemical equation: 5SO32-(aq) + 2MnO4- (aq) +6H+(aq) -> 5SO42-(aq) + 2Mn2+(aq) + 3H2O(l) (purple) (colourless) 3SO32-(aq) + Cr2O72-(aq) +8H+(aq) -> 3SO42-(aq) + 2Cr3+(aq) + 4H2O(l) (Orange) (green) - Carbon(IV)oxide forms an insoluble white precipitate of calcium carbonate if three drops of lime water are added into th... | {
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Chemical/ionic equation: Ba2+(aq) + SO42+ (aq) -> BaSO4 (s) Ba2+(aq) + SO32+ (aq) -> BaSO3 (s) Ba2+(aq) + CO32+ (aq) -> BaCO3 (s) (ii)When the insoluble precipitates are acidified with nitric(V) acid, - Barium (II)sulphate(VI) do not react with the acid and thus its white precipitates remain/ persists. - Barium(II) sul... | {
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Carbon(IV)oxide will not. Chemical equation: 5SO32-(aq) + 2MnO4- (aq) +6H+(aq) -> 5SO42-(aq) + 2Mn2+(aq) + 3H2O(l) (purple) (colourless) 3SO32-(aq) + Cr2O72-(aq) +8H+(aq) -> 3SO42-(aq) + 2Cr3+(aq) + 4H2O(l) (Orange) (green) - Carbon(IV)oxide forms an insoluble white precipitate of calcium carbonate if three drops of li... | {
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Lake Magadi has no outlet. Solubility of Trona decrease with increase in temperature.High temperature during the day causes trona to naturally crystallize .It is mechanically scooped/dredged/dug and put in a furnace. Inside the furnace, trona decompose into soda ash/sodium carbonate. Chemical equation 2NaHCO3 .Na2CO3 .... | {
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-Water from rivers/lakes. (ii)Chemical processes Ammonia gas is passed up to meet a downward flow of sodium chloride solution / brine to form ammoniated brine/ammoniacal brine mixture in the ammoniated brine chamber The ammoniated brine mixture is then pumped up, atop the carbonator/ solvay tower. In the carbonator/ so... | {
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Water and carbon(IV)oxide gas are recycled back to the ammoniated brine/ammoniacal brine chamber. More carbon(IV)oxide is produced in the kiln/furnace. Limestone is heated to decompose into Calcium oxide and carbon(IV)oxide. Chemical equation CaCO3 (s) -> CaO(s) + CO2(g) Carbon(IV)oxide is recycled to the carbonator/so... | {
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Evaporation of most of the water takes place leaving a very concentrated solution. (b)(i) Name process: I. Filtration II. Decomposition (ii) Write the equation for the reaction in process: Process I Chemical equation CO2(g) + H2O(l) + NaCl (aq) + NH3(g) -> NaHCO3(s) + NH4Cl(aq) Process II Chemical equation 2NaHCO3 (s) ... | {
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Chemical equation Ca(OH)2 (aq) +2NH4Cl (aq) -> CaCl2(s) + 2NH3(g) + H2O(l) (d)In an experiment to determine the % purity of Sodium carbonate produced in the Solvay process ,2.15g of the sample reacted with exactly 40.0cm3 of 0.5M Sulphuric(VI)acid. (i)Calculate the number of moles of sodium carbonate that reacted. Chem... | {
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(i) during making glass/lowering the melting point of mixture of sand/SiO2 from 1650oC and CaO from 2500oC to around 1500oC (ii) in softening hard water (iii) in the manufacture of soapless detergents. (iv) swimming pool “pH increaser”. (f)The diagram below shows a simple ammonia soda tower used in manufacturing sodium... | {
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Describe how you would differentiate between carbon (IV)oxide and carbon(II)oxide using chemical method. Method I -Bubble both gases in lime water/Ca(OH)2 -white precipitate is formed if the gas is carbon (IV) oxide - No white precipitate is formed if the gas is carbon (II) oxide Method II
27 -ignite both gases - Carbo... | {
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