Inorganic Chemistry

Relative Atomic Mass - Calculations from isotopic abundances I
Historical development of the periodic table II
Groups and periods I
Groups and periods II
Position of an element and electron arrangement

By the end of the lesson, the learner should be able to:
- Apply the formula for calculating R.A.M from isotopic abundances
- Calculate R.A.M for elements with two isotopes
- Solve numerical problems involving simple isotopic compositions
- Explain Mendeleev's contribution to the periodic table
- Describe Moseley's work on atomic numbers
- Recognize Mendeleev as the father of the periodic table

In groups, learners are guided to:
- Study worked examples on calculating R.A.M
- Calculate the R.A.M of elements with two isotopes
- Compare calculations with classmates for peer learning
- Search for information on Mendeleev's and Moseley's contributions
- Discuss why Mendeleev is called the father of the periodic table
- Compare Mendeleev's table with the modern periodic table

How do you calculate the Relative Atomic Mass of an element from its isotopic abundances?
Why is Mendeleev called the father of the periodic table?

- Access and Learn Chemistry Learner's Book pg. 27
- Scientific calculators
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 46
- Digital devices
- Periodic table charts
- Access and Learn Chemistry Learner's Book pg. 49
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 51
- Manila paper
- Graph paper
- Scissors

- Written exercises - Oral questions - Observation
- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Chemical families - Alkali metals and Alkaline earth metals
Chemical families - Halogens and Noble gases
Transition elements
Stability of atoms

By the end of the lesson, the learner should be able to:
- Identify members of alkali metals and alkaline earth metals
- Describe common features of Group I and Group II elements
- Recognize everyday applications of these elements like sodium in salt and calcium in bones

In groups, learners are guided to:
- Identify elements in Group I and Group II
- Discuss with peers common features of alkali metals
- Search for information on properties of alkaline earth metals

What are the characteristics of alkali metals and alkaline earth metals?

- Access and Learn Chemistry Learner's Book pg. 53
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 54
- Coloured pencils
- Access and Learn Chemistry Learner's Book pg. 55

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Cations and anions

By the end of the lesson, the learner should be able to:
- Define cations and anions
- Predict the type of ion formed from electron arrangement
- Draw ion formation using dot and cross diagrams

In groups, learners are guided to:
- Study diagrams showing ion formation
- Draw ion formation of metals and non-metals using dot and cross structures
- Discuss with peers the difference between cations and anions

How do atoms form ions?

- Access and Learn Chemistry Learner's Book pg. 56
- Digital devices
- Charts showing ion formation

- Oral questions - Written exercises - Practical drawings

Inorganic Chemistry

Valency and oxidation number I
Valency and oxidation number II

By the end of the lesson, the learner should be able to:
- Define valency and oxidation number
- Determine valency from electron arrangement
- Differentiate between valency and oxidation number

In groups, learners are guided to:
- Discuss with peers the meaning of valency and oxidation number
- Determine valency of elements from their electron arrangements
- Compare valency and oxidation number of elements

What is the difference between valency and oxidation number?

- Access and Learn Chemistry Learner's Book pg. 58
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 59

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Radicals
Electron arrangement of ions using s and p notation
Deriving formulae of compounds I
Deriving formulae of compounds II

By the end of the lesson, the learner should be able to:
- Define radicals in chemistry
- Identify common radicals and their valencies
- Apply knowledge of radicals in writing chemical formulae
- State the steps for writing formulae of compounds
- Derive formulae of simple ionic compounds
- Apply the cross-over method to write chemical formulae

In groups, learners are guided to:
- Discuss with peers the meaning of radicals
- Complete the table of radicals and their valencies
- Identify radicals in common compounds
- Discuss the steps for writing formulae of compounds
- Study worked examples on deriving formulae
- Practise writing formulae using the cross-over method

What are radicals and how are they used in Chemistry?
How do you write the formula of a compound?

- Access and Learn Chemistry Learner's Book pg. 60
- Charts showing radicals
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 62
- Periodic table
- Access and Learn Chemistry Learner's Book pg. 63
- Valency tables
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 64

- Oral questions - Written exercises - Observation
- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations I
Writing balanced chemical equations II

By the end of the lesson, the learner should be able to:
- Identify reactants and products in a chemical reaction
- Write word equations for chemical reactions
- Convert word equations to chemical equations

In groups, learners are guided to:
- Read information on parts of a chemical equation
- Identify reactants and products in given reactions
- Write word equations for simple chemical reactions

What are the parts of a chemical equation?

- Access and Learn Chemistry Learner's Book pg. 64
- Digital devices
- Charts showing chemical equations
- Access and Learn Chemistry Learner's Book pg. 65
- Practice worksheets

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Writing balanced chemical equations III
Role of electron arrangement in the periodic table - Project

By the end of the lesson, the learner should be able to:
- Write balanced equations for reactions of acids with metals
- Write balanced equations for reactions of acids with carbonates
- Apply balancing skills to more complex reactions

In groups, learners are guided to:
- Write balanced equations for reactions involving acids
- Practise writing equations for reactions with carbonates
- Compare equations with classmates for peer learning

How do you write balanced equations for reactions involving acids?

- Access and Learn Chemistry Learner's Book pg. 66
- Digital devices
- Practice worksheets
- Access and Learn Chemistry Learner's Book pg. 67
- Manila paper or carton box
- Coloured pencils
- Flashcards

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Role of valence electrons in bonding
Chemical Bonding - Types of chemical bonds
Chemical Bonding - The ionic chemical bond

By the end of the lesson, the learner should be able to:
- Explain the role of valence electrons in bonding
- Identify the octet and duplet rule in bond formation
- Relate chemical bonding to everyday materials like plastics and metals

In groups, learners are guided to:
- Review the concept of stability of atoms (gaining and/or losing electrons)
- Discuss in groups the role of valence electrons in bonding (octet/duplet noble gas configuration)
- Use digital devices to watch animations on atomic stability

Why do atoms form bonds with other atoms?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 70
- Digital devices
- Modelling clay or plasticine
- Wooden splints
- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices

- Oral questions - Observation - Written exercises

Inorganic Chemistry

Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide
Chemical Bonding - Giant ionic structures and lattice
Chemical Bonding - Solubility of ionic compounds
Chemical Bonding - Thermal conductivity, melting and boiling points of ionic compounds
Chemical Bonding - Electrical conductivity in molten and aqueous ionic compounds
Chemical Bonding - Uses of ionic compounds
Chemical Bonding - The covalent chemical bond

By the end of the lesson, the learner should be able to:
- Illustrate ionic bonding in sodium chloride and magnesium oxide
- Draw Lewis structures for ionic compounds
- Connect ionic compounds to household items like cooking salt
- Investigate electrical conductivity in molten and aqueous ionic compounds
- Explain why ionic compounds conduct electricity when molten or dissolved
- Relate conductivity to battery technology and electrolysis

In groups, learners are guided to:
- Use dot (.) and cross (x) diagrams to show electron donation and acceptance in NaCl and MgO
- Calculate net charges on ions formed
- Watch animations on ionic bond formation using digital devices
- Set up apparatus to investigate conductivity in molten lead (II) bromide
- Investigate conductivity in aqueous sodium chloride solution
- Compare conductivity in solid, molten and aqueous states

What holds sodium and chloride ions together in sodium chloride?
Why do ionic compounds conduct electricity only when molten or in solution?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Digital devices
- Periodic table
- Access & Learn Chemistry Learner's Book Grade 10 pg. 76
- Modelling materials (clay, toothpicks)
- Charts of ionic lattices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 77
- Sodium chloride
- Copper (II) chloride
- Distilled water
- Ethanol
- Test tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 78
- Bunsen burner
- Test tubes
- Copper (II) chloride
- Access & Learn Chemistry Learner's Book Grade 10 pg. 79
- Dry cells
- Bulb/ammeter
- Connecting wires
- Carbon rods
- Lead (II) bromide
- Access & Learn Chemistry Learner's Book Grade 10 pg. 81
- Digital devices
- Samples of ionic compounds
- Access & Learn Chemistry Learner's Book Grade 10 pg. 82
- Modelling clay
- Wooden splints
- Charts showing covalent bonds

- Written assignments - Practical observation - Oral questions
- Practical report - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Double and triple covalent bonds

By the end of the lesson, the learner should be able to:
- Illustrate double and triple covalent bonds
- Draw Lewis structures for oxygen and nitrogen molecules
- Relate multiple bonds to atmospheric gases we breathe

In groups, learners are guided to:
- Use dot (.) and cross (x) diagrams to show double bonds in oxygen molecules
- Illustrate triple covalent bonds in nitrogen molecules
- Model multiple covalent bonds using locally available materials

Why do some molecules have double or triple bonds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 83
- Modelling materials
- Charts of molecular structures

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride
Chemical Bonding - Dative covalent (coordinate) bonding

By the end of the lesson, the learner should be able to:
- Illustrate covalent bonding in ammonia and hydrogen chloride molecules
- Identify lone pairs of electrons in molecules
- Connect molecular compounds to household chemicals like cleaning ammonia

In groups, learners are guided to:
- Draw dot (.) and cross (x) structures for ammonia and hydrogen chloride
- Identify shared pairs and lone pairs in molecules
- Discuss the shape of ammonia molecule

What is the role of lone pairs in covalent molecules?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 84
- Charts showing molecular structures
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 85
- Charts showing dative bonds

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Hydrogen bonding and Van der Waals forces
Chemical Bonding - Melting, boiling points and conductivity of molecular substances

By the end of the lesson, the learner should be able to:
- Differentiate between intermolecular and intramolecular forces
- Illustrate hydrogen bonding and Van der Waals forces
- Connect intermolecular forces to properties of water like surface tension

In groups, learners are guided to:
- Discuss types of intermolecular forces using print or digital materials
- Illustrate hydrogen bonding in water molecules using models
- Draw diagrams showing Van der Waals forces

Why does water have a relatively high boiling point compared to other small molecules?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 86
- Modelling materials
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 89
- Naphthalene
- Thermometer
- Bunsen burner
- Melting point tube

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Solubility and uses of molecular substances
Chemical Bonding - Giant atomic structure of diamond
Chemical Bonding - Giant atomic structure of graphite
Chemical Bonding - Uses of diamond, graphite and silicon (IV) oxide

By the end of the lesson, the learner should be able to:
- Investigate solubility of molecular substances
- Relate uses of molecular substances to their properties
- Identify molecular substances in products like fuels and medicines
- Describe the layered structure of graphite
- Model the structure of graphite using locally available materials
- Relate graphite structure to its use in pencils and lubricants

In groups, learners are guided to:
- Carry out experiments to investigate solubility of sulphur and sugar in water and ethanol
- Discuss uses of molecular substances related to their properties
- Search for information on applications of molecular compounds
- Discuss the hexagonal layered structure of graphite
- Model a graphite structure showing layers
- Explain why graphite conducts electricity while diamond does not

Why do some molecular substances dissolve in organic solvents but not in water?
Why can graphite conduct electricity while diamond cannot?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol
- Access & Learn Chemistry Learner's Book Grade 10 pg. 93
- Modelling clay
- Toothpicks
- Charts of diamond structure
- Access & Learn Chemistry Learner's Book Grade 10 pg. 94
- Modelling clay
- Toothpicks
- Charts of graphite structure
- Access & Learn Chemistry Learner's Book Grade 10 pg. 96
- Digital devices
- Charts showing applications

- Practical report - Written assignments - Oral questions
- Model assessment - Written exercises - Group discussions

Inorganic Chemistry

Chemical Bonding - Metallic bonding and delocalised electrons
Chemical Bonding - Physical properties of giant metallic structures

By the end of the lesson, the learner should be able to:
- Describe the formation of metallic bonds
- Illustrate the sea of delocalised electrons model
- Relate metallic bonding to properties of metals used in wiring and construction

In groups, learners are guided to:
- Discuss how metallic bonds form through electron delocalisation
- Draw diagrams showing metallic bonding in sodium, magnesium and aluminium
- Explain the concept of positive ions in a sea of electrons

Why are metals good conductors of electricity and heat?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 97
- Charts showing metallic bonding
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 99
- Metal and wood pieces

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Uses of metallic structures related to properties
Periodicity - Introduction to periodic properties

By the end of the lesson, the learner should be able to:
- Outline uses of metallic structures
- Relate uses of metals to their bond type and properties
- Identify applications of metals in vehicles, buildings and electronics

In groups, learners are guided to:
- Search for information on uses of metallic structures
- Complete a table relating substances, bond types, properties and uses
- Discuss uses of copper, aluminium and iron in daily life

How does metallic bonding make metals suitable for electrical wiring?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 101
- Digital devices
- Samples of metal products
- Access & Learn Chemistry Learner's Book Grade 10 pg. 104
- Periodic table charts
- Digital devices

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Physical appearance and density of group I elements
Periodicity - Gradation in size of atoms and ions of group I elements
Periodicity - Ionisation energy and electronegativity of group I elements
Periodicity - Melting, boiling points and electrical conductivity of group I elements

By the end of the lesson, the learner should be able to:
- Describe the physical appearance of group I elements
- Observe and record properties of sodium metal
- Connect alkali metals to applications like sodium lamps in street lighting

In groups, learners are guided to:
- Observe the colour of sodium metal stored under paraffin
- Cut sodium metal and compare freshly cut surface to stored metal
- Watch videos on properties of group I metals
- Analyse densities of alkali metals

Why are alkali metals stored under oil or paraffin?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 106
- Sodium metal
- Scalpel blade
- Petri dish
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 107
- Periodic table
- Graph paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 108
- Data tables
- Access & Learn Chemistry Learner's Book Grade 10 pg. 110
- Connecting wires
- Dry cells
- Bulb
- Lithium metal

- Observation - Practical report - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen
Periodicity - Reactions of group I elements with chlorine and cold water
Periodicity - Applications of group I elements
Periodicity - Appearance, atomic and ionic radii of group II elements
Periodicity - Ionisation energy, melting and boiling points of group II elements

By the end of the lesson, the learner should be able to:
- Investigate reactions of lithium and sodium with oxygen
- Write balanced equations for reactions with oxygen
- Relate metal oxide formation to rusting and corrosion processes
- Describe trends in ionisation energy of group II elements
- Analyse melting and boiling point data
- Connect high melting points to use of magnesium oxide in furnace linings

In groups, learners are guided to:
- Burn lithium and sodium in gas jars of oxygen
- Test products with litmus paper to determine nature of oxides
- Write chemical equations for reactions
- Compare reactivity of different alkali metals
- Analyse data on first and second ionisation energies of group II elements
- Plot graphs of melting and boiling points against atomic number
- Discuss factors affecting ionisation energy and melting points

What type of oxides do alkali metals form when they burn in oxygen?
Why do group II elements have two ionisation energies?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 112
- Gas jar of oxygen
- Deflagrating spoon
- Bunsen burner
- Lithium and sodium metals
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 114
- Chlorine gas
- Cold water
- Beakers
- Access & Learn Chemistry Learner's Book Grade 10 pg. 117
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table
- Access & Learn Chemistry Learner's Book Grade 10 pg. 121
- Graph paper
- Data tables
- Digital devices

- Practical report - Written exercises - Observation
- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group II elements with water, steam and oxygen
Periodicity - Reactions of group II elements with dilute acids and chlorine

By the end of the lesson, the learner should be able to:
- Investigate reactions of magnesium and calcium with water and oxygen
- Write balanced equations for the reactions
- Relate magnesium's reaction with oxygen to its use in flares and fireworks

In groups, learners are guided to:
- Investigate reactions of magnesium ribbon with cold water and steam
- Investigate reaction of calcium with cold water
- Burn magnesium and calcium in oxygen and test products
- Collect and test gases produced

Why does magnesium react slowly with cold water but vigorously with steam?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 123
- Magnesium ribbon
- Calcium metal
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 127
- Dilute acids
- Chlorine gas
- Test tubes

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group II elements
Periodicity - Preparation of chlorine and physical properties of group VII elements

By the end of the lesson, the learner should be able to:
- Outline applications of group II elements
- Relate properties to specific uses
- Identify uses in construction, medicine, alloys and agriculture

In groups, learners are guided to:
- Search for information on applications of group II elements
- Discuss uses of magnesium in alloys, calcium in cement, barium in X-rays
- Create flashcards showing applications

How is calcium used in the construction industry?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 129
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 131
- Concentrated HCl
- Potassium manganate (VII)
- Gas jars
- Delivery tubes

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Melting, boiling points and gradation in size of group VII elements
Periodicity - Reactions of group VII elements with water and metals

By the end of the lesson, the learner should be able to:
- Describe trends in melting and boiling points of halogens
- Describe trends in atomic and ionic radii of group VII elements
- Relate physical states to intermolecular forces and room temperature applications

In groups, learners are guided to:
- Analyse data on melting and boiling points of halogens
- Plot graphs of melting and boiling points against atomic number
- Analyse data on atomic and ionic radii
- Discuss Van der Waals forces in halogens

Why is iodine a solid while chlorine is a gas at room temperature?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 135
- Graph paper
- Data tables
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 139
- Chlorine gas
- Bromine water
- Iodine crystals
- Iron wool
- Litmus paper

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Displacement reactions and bleaching action of chlorine
Periodicity - Applications of group VII elements
Periodicity - Physical properties and applications of noble gases
Periodicity - Atomic size, ionisation energy and electronegativity across period 3

By the end of the lesson, the learner should be able to:
- Investigate displacement reactions of halogens
- Investigate the bleaching action of chlorine
- Relate displacement reactions to water purification and textile bleaching
- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging

In groups, learners are guided to:
- Bubble chlorine gas through solutions of potassium bromide and potassium iodide
- Observe colour changes and identify products
- Investigate bleaching action of chlorine on coloured cloth and flower petals
- Write chemical equations for displacement reactions
- Analyse data on atomic radii, ionisation energy, melting and boiling points of noble gases
- Discuss why noble gases are unreactive
- Search for information on uses of helium, neon and argon

Why can chlorine displace bromine and iodine from their compounds?
Why are noble gases called inert gases?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 142
- Potassium bromide solution
- Potassium iodide solution
- Chlorine gas
- Coloured cloth
- Flower petals
- Access & Learn Chemistry Learner's Book Grade 10 pg. 147
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 148
- Periodic table
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Data tables

- Practical report - Written exercises - Observation
- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Periodicity - Reactions of period 3 elements with oxygen and water

By the end of the lesson, the learner should be able to:
- Investigate reactions of period 3 elements with oxygen and water
- Write balanced equations for the reactions
- Relate oxide formation to acidic and basic properties of substances

In groups, learners are guided to:
- Burn sodium, magnesium and sulphur in oxygen
- Test products with litmus paper to determine acidic or basic nature
- Investigate reactions of sodium and magnesium with water and steam
- Write chemical equations for all reactions

Why are metallic oxides basic while non-metallic oxides are acidic?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 155
- Sodium, magnesium, sulphur
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Distilled water

- Practical report - Written exercises - Observation

Inorganic Chemistry
Physical Chemistry
Physical Chemistry
Physical Chemistry

Periodicity - Reactions of period 3 elements with chlorine and dilute acids
Acids and Bases - Dissociation of acids in aqueous solutions
Acids and Bases - Dissociation of bases in aqueous solutions
Acids and Bases - Properties of acids

By the end of the lesson, the learner should be able to:
- Investigate reactions of period 3 elements with chlorine and dilute acids
- Write balanced equations for the reactions
- Connect periodic trends to prediction of element behaviour in chemical reactions

In groups, learners are guided to:
- Pass chlorine gas over heated sodium and magnesium
- Investigate reactions of magnesium with dilute HCl, dilute H₂SO₄ and dilute HNO₃
- Test gases produced
- Write chemical equations for all reactions
- Summarise trends in chemical properties across period 3

How do the chemical properties of elements change across period 3?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner
- Access & Learn Chemistry Learner's Book Grade 10 pg. 164
- Dilute hydrochloric acid
- pH indicator paper
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 166
- Sodium hydroxide solution
- Phenolphthalein indicator
- Red and blue litmus paper
- Test tubes
- Chemistry Learner's Book Grade 10 pg. 166
- Samples of acids
- Blue litmus paper

- Practical report - Written exercises - Oral questions

Physical Chemistry

Acids and Bases - Properties of bases
Acids and Bases - Reaction of dilute acids with metals
Acids and Bases - Confirmatory test for hydrogen gas
Acids and Bases - Reaction of acids with carbonates

By the end of the lesson, the learner should be able to:
- Describe the physical properties of bases
- Differentiate between bases and alkalis
- Connect properties of bases to cleaning agents and antacids used at home

In groups, learners are guided to:
- Carry out experiments to investigate properties of bases
- Test bases using litmus paper and phenolphthalein indicator
- Discuss with peers the slippery feel and bitter taste of bases

What common household substances are basic in nature?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 167
- Sodium hydroxide solution
- Baking soda
- Soap solution
- Red litmus paper
- Phenolphthalein
- Access & Learn Chemistry Learner's Book Grade 10 pg. 169
- Zinc powder
- Dilute hydrochloric acid
- Test tubes
- Wooden splints
- Rubber corks
- Access & Learn Chemistry Learner's Book Grade 10 pg. 170
- Dilute sulphuric acid
- Magnesium ribbon
- Delivery tubes
- Chemistry Learner's Book Grade 10 pg. 170
- Sodium carbonate
- Calcium hydroxide
- Delivery tubes
- Test tubes

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Reaction of acids with hydrogen carbonates
Acids and Bases - Reaction of acids with metal oxides
Acids and Bases - Reaction of acids with metal hydroxides
Acids and Bases - Universal indicator and pH scale

By the end of the lesson, the learner should be able to:
- Describe reactions of acids with hydrogen carbonates
- Perform the confirmatory test for carbon (IV) oxide
- Connect the reaction to baking powder action in bread and cakes
- Describe reactions of acids with metal hydroxides
- Demonstrate neutralisation using indicators
- Connect neutralisation to antacid medication for treating stomach acidity

In groups, learners are guided to:
- Add dilute nitric (V) acid to sodium hydrogen carbonate
- Collect and test gas produced using limewater
- Observe white precipitate formation
- Write balanced equations for the reactions
- Add dilute sulphuric (VI) acid to sodium hydroxide with phenolphthalein
- Observe colour change from pink to colourless
- Write balanced equations for the neutralisation reaction

How is carbon (IV) oxide gas tested in the laboratory?
How do indicators show the end point of neutralisation?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 171
- Sodium hydrogen carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Test tubes
- Delivery tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 172
- Magnesium oxide
- pH paper
- Beakers
- Bunsen burner
- Access & Learn Chemistry Learner's Book Grade 10 pg. 173
- Sodium hydroxide solution
- Dilute sulphuric (VI) acid
- Phenolphthalein indicator
- Beakers
- Measuring cylinders
- Access & Learn Chemistry Learner's Book Grade 10 pg. 175
- Universal indicator
- pH scale chart
- Various acid and base solutions
- Test tubes
- Droppers

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Strong and weak acids
Acids and Bases - Strong and weak bases

By the end of the lesson, the learner should be able to:
- Differentiate between strong and weak acids
- Classify acids based on their pH values
- Connect acid strength to battery acid (strong) versus citrus fruits (weak)

In groups, learners are guided to:
- Test 0.1 M hydrochloric acid and 0.1 M ethanoic acid using universal indicator
- Compare pH values of strong and weak acids
- Discuss degree of dissociation in strong and weak acids

Why do strong acids have lower pH values than weak acids?

- Chemistry Learner's Book Grade 10 pg. 175
- 0.1 M hydrochloric acid
- 0.1 M ethanoic acid
- Universal indicator
- pH scale chart
- Test tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 176
- 0.1 M sodium hydroxide
- 0.1 M ammonium hydroxide

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Electrical conductivity of acids and bases
Acids and Bases - Uses of acids in day-to-day life

By the end of the lesson, the learner should be able to:
- Compare electrical conductivity of strong and weak acids and bases
- Set up circuits to test conductivity
- Connect conductivity to car battery technology and industrial electrochemistry

In groups, learners are guided to:
- Set up electrical circuits with bulb, dry cell and electrodes
- Test conductivity of strong and weak acids and bases
- Compare brightness of bulb in different solutions
- Record and discuss observations

Why do strong acids and bases conduct electricity better than weak ones?

- Chemistry Learner's Book Grade 10 pg. 176
- Dry cells
- Bulbs with holders
- Connecting wires
- Nails/electrodes
- Various acid and base solutions
- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Uses of bases in day-to-day life
Introduction to Salts - Meaning and formation of salts
Introduction to Salts - Normal salts

By the end of the lesson, the learner should be able to:
- Outline the uses of bases in various sectors
- Identify applications of bases in agriculture and construction
- Connect bases to soap making, cement production and soil treatment

In groups, learners are guided to:
- Discuss uses of bases in cleaning, food industry and construction
- Carry out soil pH testing activity
- Discuss role of calcium oxide in neutralising acidic soils
- Make natural citrus cleaner using vinegar and citrus peels

How are bases applied in agriculture and industry?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 179
- Soil samples
- pH paper
- Litmus paper
- Vinegar
- Citrus peels
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 181
- Samples of salts (sodium chloride, copper sulphate)
- Charts showing neutralisation equations
- Access & Learn Chemistry Learner's Book Grade 10 pg. 182
- Samples of normal salts
- Test tubes
- Distilled water

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Introduction to Salts - Acid salts
Introduction to Salts - Basic and double salts
Introduction to Salts - Soluble and insoluble salts
Introduction to Salts - Solubility rules
Introduction to Salts - Preparation by direct synthesis
Introduction to Salts - Preparation using acid and metal
Introduction to Salts - Preparation using acid and metal oxide

By the end of the lesson, the learner should be able to:
- Describe acid salts and their formation
- Identify examples of acid salts
- Relate acid salts to baking soda (sodium hydrogen carbonate) used in cooking
- Describe preparation of salts by direct combination
- Carry out experiments on direct synthesis
- Relate direct synthesis to industrial production of iron sulphide

In groups, learners are guided to:
- Discuss characteristics of acid salts (contain replaceable hydrogen, pH less than 7)
- Write formulae of acid salts (NaHCO₃, NaHSO₄)
- Test solutions of acid salts with litmus paper
- Compare acid salts with normal salts
- Place copper metal and sulphur powder in crucible
- Heat mixture strongly and observe reaction
- Allow product to cool and examine crystals
- Write equation for reaction between copper and sulphur

How do acid salts differ from normal salts?
How are salts prepared by direct combination of elements?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 183
- Sodium hydrogen carbonate
- Litmus paper
- pH paper
- Test tubes
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 184
- Samples of basic and double salts
- Potassium aluminium sulphate (alum)
- pH paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 185
- Copper (II) sulphate
- Copper (II) carbonate
- Distilled water
- Beakers
- Bunsen burner
- Chemistry Learner's Book Grade 10 pg. 185
- Solubility table charts
- Various salt samples
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 186
- Copper metal
- Sulphur powder
- Crucible
- Bunsen burner
- Tripod stand
- Access & Learn Chemistry Learner's Book Grade 10 pg. 187
- Zinc powder
- Dilute hydrochloric acid
- Filter funnel and paper
- Evaporating dish
- Bunsen burner
- Access & Learn Chemistry Learner's Book Grade 10 pg. 188
- Copper (II) oxide
- Dilute nitric (V) acid
- Beakers

- Practical assessment - Oral questions - Written assignments
- Practical assessment - Observation - Written exercises

Physical Chemistry

Introduction to Salts - Preparation using acid and alkali (titration)
Introduction to Salts - Preparation using acid and carbonate

By the end of the lesson, the learner should be able to:
- Describe preparation of salts using acid and alkali
- Carry out titration using phenolphthalein indicator
- Connect titration to quality control in food and pharmaceutical industries

In groups, learners are guided to:
- Measure sodium hydroxide into conical flask and add phenolphthalein
- Fill burette with dilute hydrochloric acid
- Titrate until colour changes from pink to colourless
- Evaporate and crystallise to obtain sodium chloride

How does phenolphthalein indicate the end point of neutralisation?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 190
- Sodium hydroxide solution
- Dilute hydrochloric acid
- Phenolphthalein
- Burette and stand
- Conical flask
- Access & Learn Chemistry Learner's Book Grade 10 pg. 191
- Sodium carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Filter funnel
- Evaporating dish

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Introduction to Salts - Preparation by precipitation (double decomposition)
Introduction to Salts - Hygroscopic, deliquescent and efflorescent salts

By the end of the lesson, the learner should be able to:
- Describe preparation of insoluble salts by precipitation
- Prepare lead (II) sulphate by double decomposition
- Connect precipitation to water treatment and removal of heavy metals

In groups, learners are guided to:
- Mix zinc sulphate solution with lead nitrate solution
- Observe precipitate formation
- Filter, wash and dry the precipitate
- Write ionic equations for precipitation reactions

What is double decomposition and how is it used to prepare insoluble salts?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 193
- Zinc sulphate solution
- Lead nitrate solution
- Filter funnel and paper
- Beakers
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 196
- Iron (III) chloride
- Anhydrous copper (II) sulphate
- Sodium carbonate decahydrate
- Watch glasses

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Introduction to Salts - Uses of salts and environmental impact of fertilisers

By the end of the lesson, the learner should be able to:
- Outline applications of salts in various sectors
- Discuss effects of inorganic fertilisers on the environment
- Relate salts to food preservation, agriculture and water pollution from fertiliser runoff

In groups, learners are guided to:
- Search for uses of salts in agriculture, medicine, food and glass industries
- Discuss positive and negative effects of inorganic fertilisers
- Discuss eutrophication and mitigation measures
- Present findings on sustainable use of fertilisers

How do salts contribute to agriculture and what are the environmental concerns?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 197
- Samples of inorganic fertilisers
- Digital devices
- Reference books
- Charts on eutrophication

- Oral questions - Written assignments - Project assessment