Chapter 2 – The Structure of the Atom
Activity 2.1 7 Diffusion of particles in a gas, liquid and solid Aim To investigate the diffusion of particles in a gas, liquid and solid Problem How diffusion does occur Statement through solid, a liquid and gas? Hypothesis Particles can diffuse through the spaces between the particles of a solid, a liquid and the gas. Apparatus A. Diffusion in a gas Gas jars Gas jar covers B. Diffusion in a liquid
Material
Number Pg. Title
A. Diffusion in a gas Liquid bromine, Br 2 B. Diffusion in a liquid
-3
1 mol dm potassium manganate (VII), KMnO4solution Water C. Diffusion in a solid
Variables
Droppers / Teat pipette Thistle funnel Spatula C. Diffusion in a solid
Potassium manganate(VII), KMnO4 crystal / Copper(II) sulphate, CuSO 4 crystal Hot liquid gel Manipulated variable: Type of medium Responding variable: Motion of the particles Controlled / Fixed variable: Temperature and pressure
Number Pg. Title
Stoppers Test tubes Test tube rack Retort stand and clamp
Activity 2.2 8 Rate of diffusion depends on the temperature Aim To show that the rate of diffusion depends on the temperature Problem How does rate of diffusion Statement depends on the temperature? Hypothesis Higher temperature can increase the rate of diffusion Apparatus Beakers Droppers
Material
Food colouring Water Ice water Hot water Variables Manipulated variable: Temperature of water Responding variable: Rate of diffusion Controlled / Fixed variable: Concentration and volume of food colouring and pressure Operational Higher temperature in water Definition increases the particles to move faster and increases the rate of
diffusion. / Higher temperature in water increases the kinetics energy than lower temperature in water.
Number Pg. Title
Activity 2.3 9 Rate of diffusion depends on the mass of the gas particles Aim To show that the rate of diffusion depends on the mass of the gas particles Problem How does rate of diffusion Statement depends on the mass of the gas particles? Hypothesis Low molecular masses diffuse faster than those with high molecular masses Apparatus Glass tube Stoppers Retort stand and clamp Beakers Droppers Material Glass wool Concentrated ammonia, NH3 solution Concentrated hydrochloric acid, HCl Variables Manipulated variable: Mass of the gas particles Responding variable: Rate of diffusion Controlled / Fixed variable: Temperature and pressure Operational Gas with low molecular masses Definition diffuse faster than those with high molecular masses.
Number Pg. Title
Activity 2.4 9 Melting and freezing points of
naphthalene, C 10H8 Aim To determine the melting and freezing points of naphthalene, C10H8 Problem How does rate of diffusion Statement depends on the mass of the gas particles? Hypothesis The temperature of naphthalene, C10H8 increase during heating except at its melting and solidification points Apparatus Boiling tube 3 250 cm beaker Thermometer (0 – 100˚C) Tripod stand Retort stand and clamp Bunsen burner Stopwatch Conical flask Wire gauze Material Naphthalene, C 10H8 Water Variables Manipulated variable: Heat supplied Responding variable: Temperature Controlled / Fixed variable: Naphthalene, C 10H8
Chapter 3 – Chemical Formulae and Equations
Number Pg. Title
Activity 3.4 23 Empirical formula of copper(II) oxide Aim To determine the empirical formula of copper(II) oxide Problem How does the formula of Statement copper(II) oxide determine? Hypothesis The empirical formula of copper(II) oxide can be determined by finding out the mass of copper and oxygen in a sample of copper(II) oxide
Apparatus
U tube Stoppers Glass tube Combustion tube with a small hole at the end Retort stand and clamp Spatula Porcelain dish Bunsen burner Balance Preparation for hydrogen gas
Tripod stand Pipe-clay triangle
Material
Variables
Thistle funnel Flat-bottomed flask Hydrogen gas, H 2 Copper(II) oxide Anhydrous calcium chloride, CaCl2 Wooden splinter Preparation for the hydrogen gas
10 cm magnesium ribbon Sandpaper Manipulated variable: Magnesium ribbon Responding variable: Mass of magnesium oxide Controlled / Fixed variable: Length / Mass of magnesium ribbon and excess air
Material
Variables
Number Pg. Title
Number Pg. Title Aim
Dilute hydrochloric acid Zinc pieces Manipulated variable: Mass of copper oxide Responding variable: Mass of copper formed Controlled / Fixed variable: An excess of hydrogen gas
Activity 3.5 25 Empirical formula of magnesium oxide Aim To determine the empirical formula of magnesium oxide Problem How does the formula of Statement magnesium oxide determine? Hypothesis The empirical formula of magnesium oxide is MgO Apparatus Crucible with lid Tongs Bunsen burner
Activity 3.6 27 Chemical equations To construct balanced chemical equations A. Heating of copper(II) carbonate B. Reaction of ammonia gas and hydrochloric acid / Formation of ammonium chloride C. Reaction of lead(II) nitrate and potassium iodide / Precipitation of lead(II) iodide
Problem How does the chemical Statement equations determine? Hypothesis A. The chemical equation of copper(II) carbonate is CuCO 3 – > CuO + CO2 B. The chemical equation of Apparatus
Boiling tube Test tubes Rubber bung with delivery tube Test tube rack Test tube holder
Stoppers Bunsen burner Material Copper(II) carbonate powder Lime water Concentrated ammonia solution Concentrated hydrochloric acid Lead(II) nitrate solution Potassium iodide solution Variables A. Heating of copper(II) carbonate Manipulated variable: Mass of copper(II) carbonate Responding variable: Mass of copper oxide formed / Volume of carbon dioxide liberated Controlled / Fixed variable: Pressure B. Reaction of ammonia gas and hydrochloric acid / Formation of ammonium chloride
Chapter 4 – Periodic Table of Elements
Number Pg. Title Aim
Problem Statement
Hypothesis
Apparatus
Experiment 4.1 35 Chemical properties of lithium, sodium and potassium To investigate the chemical properties of lithium, sodium and potassium How does the reactivity of Group 1 elements change when they react with water and oxygen gas, O 2? When going down Group 1, alkali metals become reactive in their reactions with water Water troughs Small knife Forceps Gas jars Gas jar spoons Gas jar covers Small pieces of lithium, sodium and potassium Filter paper Distilled water Red litmus paper Three gas jars filled with oxygen gas, O 2 Manipulated variable: Different types of alkali metals Responding variable: Reactivity of metals Controlled / Fixed variable: Water, size of metals An alkali metal that reacts more vigorously with water is more reactive metal
Manipulated variable: Concentration of ammonia and hydrochloric acid Responding variable: Ammonium chloride formed Controlled / Fixed variable: Temperature and pressure C. Reaction of lead(II) nitrate and potassium iodide / Precipitation of lead(II) iodide
Material
Variables
Manipulated variable: Volume of lead(II) nitrate solution and volume of potassium iodide solution Responding variable: Mass of lead(II) iodide formed Controlled / Fixed variable: Temperature and pressure
Operational Definition
Number Pg.
Experiment 4.2 39
Title Aim
Chemical properties of Group 17 elements To investigate the chemical properties of Group 17 elements (A) Reactions of halogens with water
sodium hydroxide solution Apparatus
Test tubes Dropper Test tube holders Stoppers Combustion tubes Delivery tubes Bunsen burner Retort stand and clamp Chlorine gas, Cl 2 (produce after mixing potassium manganate(VII) salts with concentrated hydrochloric acid) Liquid bromine, Br 2 Solid iodine, I2 Blue litmus paper Water Iron wool Soda lime -3 2 mol dm sodium hydroxide, NaOH solution (A) Reactions of halogens with water Manipulated variable: Type of halogens Responding variable: Change in colour of the blue litmus paper / Reactivity of halogens Controlled / Fixed variable: Water (B) Reactions of halogens with iron
(B) Reactions of halogens with iron
(C) Reactions of halogens with sodium hydroxide, NaOH solution Problem How do halogens react with Statement water, iron and sodium hydroxide, NaOH solution? Hypothesis (A) Reactions of halogens with water 1. Halogens forms acidic solutions when they react with water 2. Halogens show bleaching properties when they react with water (B) Reactions of halogens with iron Halogens form iron(III) halides when they react with iron / When going down Group 17, halogens become less reactive in their reactions with iron (C) ) Reactions of halogens with sodium hydroxide, NaOH solution
Material
Variables
Manipulated variable: Types of halogens Responding variable: Appearance of brown solid / Reactivity of halogens Controlled / Fixed variable: Iron (C) ) Reactions of halogens with sodium hydroxide, NaOH
Halogens form sodium halide, sodium halite(I) and water when they react with sodium hydroxide / When going down Group 17, halogens become less reactive in their reactions with
solution Manipulated variable: Types of halogens Responding variable: Formation of a colourless solution from a coloured halogen / Reactivity of halogens Controlled / Fixed variable: Sodium hydroxide solution Operational (A) Reactions of halogens with Definition water 1. When blue litmus paper turns red, the solution formed shows acidic property 2. When blue litmus paper turns white, the solution formed shows bleaching property (B) Reactions of halogens with iron
Aim
To study the properties of the oxides of elements in Period 3 Problem How do the acid-base Statement properties of the oxides of elements change across Period 3? Hypothesis Acidic properties of the oxides of elements increase whereas basic properties of the oxides of elements decrease across Period 3 Apparatus Boiling tubes Test tubes Test tube holder Glass rod Spatula Gas jar Gas cover 3 100 cm measuring cylinder Material Sodium oxide, Na 2O Magnesium oxide, MgO Aluminium oxide, Al 2O3 Silicon(IV) oxide, SiO 2 Phosphorus pentoxide, P2O5 Sulphur dioxide gas, SO2 Dichlorine heptoxide, Cl2O7 Universal Indicator -3 2 mol dm nitric acid, HNO3 -3 2 mol dm sodium hydroxide, NaOH solution Variables Manipulated variable: Oxides of elements of Period 3 Responding variable: pH values in water and solubility in acid or alkali Controlled / Fixed variable: Water or nitric
The appearance of a brown solid shows the formation of iron(III) halides
(C) ) Reactions of halogens with sodium hydroxide, NaOH solution
The formation of a colourless solution indicates that salts of sodium halide, sodium halite(I) and water are formed
Number Pg. Title
Experiment 4.3 45 Properties of the oxides of elements in Period 3
Operational 1. Definition
2.
3.
4.
acid, HNO3 or sodium hydroxide, NaOH solution Oxide that dissolves in water to form solution with pH less than 7 is acidic and pH more than 7 is alkaline Oxide that can dissolve in an acid exhibits basic properties Oxide that can dissolve in an alkali exhibits acidic properties Oxide that can dissolve in both acid and alkali exhibits amphoteric properties
Chapter 5 – Chemical Bonds
Number Pg. Title Aim
Gas jar spoon / Deflagrating spoon Gas jar cover Gas jar (C) Preparation of iron(III) chloride, FeCl3 Spatula Asbestos paper Combustion tube Stopper with delivery tube Retort stand and clamp Bunsen burner
Material (A) Preparation of magnesium oxide, MgO Magnesium ribbon (B) Preparation of sodium chloride, NaCl
Activity 5.1 52 Ionic compound To prepare ionic compounds(A) Preparation of magnesium oxide, MgO (B) Preparation of sodium chloride, NaCl
(C) Preparation of iron(III) chloride, FeCl 3 Apparatus (A) Preparation of magnesium oxide, MgO Sandpaper Crucible Spatula Pipe-clay triangle Tripod stand Bunsen burner (B) Preparation of sodium chloride, NaCl
Sodium Chlorine gas, Cl 2 (C) Preparation of iron(III) chloride, FeCl3 Iron filling Chlorine gas, Cl 2
Number Pg. Title Aim
Activity 5.3 55 Properties of ionic and covalent compounds To compare the properties of ionic and covalent compounds(A) Melting point and boiling point (B) Solubility in water and organic solvents (C) Electrical conductivity
Knife Forceps Filter paper Spatula
Apparatus (A) Melting point and boiling point Spatula Evaporating dish Dropper (B) Solubility in water and organic solvents
(C) Electrical conductivity
Spatula Glass rod Test tubes Test tube rack (C) Electrical conductivity
Spatula Glass rod Switch Connecting wires with crocodile clips Batteries Bulb Carbon electrodes Beakers Crucible Tripod stand Pipe-clay triangle Bunsen burner (A) Melting point and boiling point Magnesium chloride, MgCl2 Sodium sulphate, Na 2SO4 Diethyl ether, (C 2H5)2O Hexane, C 6H14 (B) Solubility in water and organic solvents
Material
Distilled water Magnesium chloride, MgCl2 Cyclohexane, C 6H12 Sodium sulphate, Na 2SO4 Diethyl ether, (C 2H5)2O Hexane, C 6H14
Solid lead(II) bromide, PbBr2 Magnesium chloride, MgCl2 solution Naphthalene, C 10H8
