(a) Arrange the three states of matter in order of decreasing:
(i) kinetic energy;
(ii) force of cohesion.
(b) Consider the redox reaction equation:
(i) State the change in oxidation number of:
I. magnesium;
II. hydrogen.
(ii) Which of the species is being:
I. oxidized;
II. reduced?
(iii) Identify the oxidizing agent.
(c) (i) State two differences between boiling and evaporation.
(ii) What will be the effect of reduction of atmospheric pressure on the boiling point of water?
(d) For a given chemical equilibrium system, what is the significance of the equilibrium constant \(K\)?
(e) Consider the following organic compounds:
\(\mathrm{C_3H_7COOH}\); \(\mathrm{(CH_3)_3COH}\).
Give the IUPAC name of each compound.
(f) Why are organic compounds classified on the basis of functional groups?
(g) State three differences between the solubility of solids in liquids and gases in liquids.
(h) Write a balanced chemical equation for the reaction between fluorine and water.
(i) Define the term basicity of an acid.
(a)
(i) Decreasing kinetic energy: gas > liquid > solid.
(ii) Decreasing force of cohesion: solid > liquid > gas.
(b) For the reaction \( \text{Mg} + 2\text{HCl} \to \text{MgCl}_2 + \text{H}_2 \):
- (i) I. Magnesium: oxidation number changes from 0 to +2. II. Hydrogen: from +1 to 0.
- (ii) I. Oxidized: magnesium (Mg). II. Reduced: hydrogen (H+).
- (iii) Oxidizing agent: hydrochloric acid (HCl / H+).
(c)(i) Two differences between boiling and evaporation:
- Boiling occurs at a fixed temperature (the boiling point) and throughout the whole liquid with bubbles forming, whereas evaporation occurs at any temperature and only at the surface of the liquid.
- Boiling requires an external supply of heat and produces no cooling, whereas evaporation uses the internal energy of the liquid and produces cooling.
(c)(ii) Reducing the atmospheric pressure lowers the boiling point of water, so it boils at a temperature below 100 °C.
(d) The equilibrium constant K indicates the extent to which a reaction proceeds and where the position of equilibrium lies: a large K means the products are favoured (reaction nearly complete), while a small K means the reactants are favoured.
(e) C3H7COOH is butanoic acid; (CH3)3COH is 2-methylpropan-2-ol.
(f) Because a functional group is the atom or group of atoms responsible for the characteristic chemical reactions of a compound. Compounds sharing the same functional group have similar chemical properties, so classifying by functional group makes their study systematic and their reactions predictable.
(g) Three differences between solubility of solids and of gases in liquids:
- The solubility of most solids increases with a rise in temperature, whereas the solubility of gases decreases with a rise in temperature.
- The solubility of gases increases markedly with pressure, whereas that of solids is virtually unaffected by pressure.
- Dissolving a solid is generally accompanied by absorption of heat (endothermic), whereas dissolving a gas is generally accompanied by release of heat (exothermic).
(h) \[ 2\text{F}_2 + 2\text{H}_2\text{O} \to 4\text{HF} + \text{O}_2 \]
(i) The basicity of an acid is the number of replaceable (ionizable) hydrogen ions produced by one molecule of the acid in aqueous solution.
(a)
(i) Decreasing kinetic energy: gas > liquid > solid.
(ii) Decreasing force of cohesion: solid > liquid > gas.
(b) For the reaction \( \text{Mg} + 2\text{HCl} \to \text{MgCl}_2 + \text{H}_2 \):
- (i) I. Magnesium: oxidation number changes from 0 to +2. II. Hydrogen: from +1 to 0.
- (ii) I. Oxidized: magnesium (Mg). II. Reduced: hydrogen (H+).
- (iii) Oxidizing agent: hydrochloric acid (HCl / H+).
(c)(i) Two differences between boiling and evaporation:
- Boiling occurs at a fixed temperature (the boiling point) and throughout the whole liquid with bubbles forming, whereas evaporation occurs at any temperature and only at the surface of the liquid.
- Boiling requires an external supply of heat and produces no cooling, whereas evaporation uses the internal energy of the liquid and produces cooling.
(c)(ii) Reducing the atmospheric pressure lowers the boiling point of water, so it boils at a temperature below 100 °C.
(d) The equilibrium constant K indicates the extent to which a reaction proceeds and where the position of equilibrium lies: a large K means the products are favoured (reaction nearly complete), while a small K means the reactants are favoured.
(e) C3H7COOH is butanoic acid; (CH3)3COH is 2-methylpropan-2-ol.
(f) Because a functional group is the atom or group of atoms responsible for the characteristic chemical reactions of a compound. Compounds sharing the same functional group have similar chemical properties, so classifying by functional group makes their study systematic and their reactions predictable.
(g) Three differences between solubility of solids and of gases in liquids:
- The solubility of most solids increases with a rise in temperature, whereas the solubility of gases decreases with a rise in temperature.
- The solubility of gases increases markedly with pressure, whereas that of solids is virtually unaffected by pressure.
- Dissolving a solid is generally accompanied by absorption of heat (endothermic), whereas dissolving a gas is generally accompanied by release of heat (exothermic).
(h) \[ 2\text{F}_2 + 2\text{H}_2\text{O} \to 4\text{HF} + \text{O}_2 \]
(i) The basicity of an acid is the number of replaceable (ionizable) hydrogen ions produced by one molecule of the acid in aqueous solution.
