Inorganic Chemistry

Chemical Bonding - Dative covalent (coordinate) bonding

By the end of the lesson, the learner should be able to:
- Describe the formation of dative covalent bonds
- Illustrate dative bonding in ammonium and hydroxonium ions
- Relate coordinate bonds to acid-base reactions in the stomach

In groups, learners are guided to:
- Discuss how both shared electrons come from one atom in dative bonding
- Draw structures showing dative bonds in ammonium ion (NH₄⁺)
- Illustrate dative bonding in hydroxonium ion (H₃O⁺)

How is a dative covalent bond different from an ordinary covalent bond?

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Chemical Bonding - Hydrogen bonding and Van der Waals forces

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

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Melting, boiling points and conductivity of molecular substances
Chemical Bonding - Solubility and uses of molecular substances

By the end of the lesson, the learner should be able to:
- Investigate melting and boiling points of molecular substances
- Explain why molecular substances have low melting points
- Relate molecular properties to everyday substances like sugar and wax
- Investigate solubility of molecular substances
- Relate uses of molecular substances to their properties
- Identify molecular substances in products like fuels and medicines

In groups, learners are guided to:
- Carry out experiments to determine melting point of naphthalene
- Investigate thermal and electrical conductivity of molecular substances
- Compare properties with ionic compounds
- 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

Why do molecular substances have low melting and boiling points?
Why do some molecular substances dissolve in organic solvents but not in water?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 89
- Naphthalene
- Thermometer
- Bunsen burner
- Melting point tube
- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol

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

Inorganic Chemistry

Chemical Bonding - Solubility and uses of molecular substances

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

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

Why do some molecular substances dissolve in organic solvents but not in water?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol

- Practical report - Written assignments - Oral questions

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of diamond

By the end of the lesson, the learner should be able to:
- Describe the giant atomic structure of diamond
- Model the structure of diamond using locally available materials
- Connect diamond's structure to its use in cutting tools and jewelry

In groups, learners are guided to:
- Discuss the tetrahedral structure of diamond
- Model a diamond structure using modelling clay and toothpicks
- Relate structure to properties (hardness, non-conductivity)

Why is diamond the hardest natural substance?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 93
- Modelling clay
- Toothpicks
- Charts of diamond structure

- Model assessment - Written exercises - Oral questions

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of graphite

By the end of the lesson, the learner should be able to:
- 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:
- Discuss the hexagonal layered structure of graphite
- Model a graphite structure showing layers
- Explain why graphite conducts electricity while diamond does not

Why can graphite conduct electricity while diamond cannot?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 94
- Modelling clay
- Toothpicks
- Charts of graphite structure

- Model assessment - Written exercises - Group discussions

Inorganic Chemistry

Chemical Bonding - Uses of diamond, graphite and silicon (IV) oxide
Chemical Bonding - Metallic bonding and delocalised electrons

By the end of the lesson, the learner should be able to:
- Outline uses of diamond, graphite and silicon (IV) oxide
- Relate uses to their structural properties
- Identify applications in drilling, electronics and glass making
- 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:
- Search for information on uses of giant atomic structures
- Discuss why diamond is used in drilling bits
- Explain the use of graphite as a lubricant and in electrodes
- 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

How do the structures of diamond and graphite determine their uses?
Why are metals good conductors of electricity and heat?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 96
- Digital devices
- Charts showing applications
- Access & Learn Chemistry Learner's Book Grade 10 pg. 97
- Charts showing metallic bonding
- Digital devices

- Written assignments - Group presentations - Oral questions
- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Physical properties of giant metallic structures

By the end of the lesson, the learner should be able to:
- Describe physical properties of metallic structures
- Investigate thermal conductivity of metals
- Connect metallic properties to uses in cooking utensils and electrical wires

In groups, learners are guided to:
- Investigate thermal conductivity by comparing metal and wood pieces in sunlight
- Discuss high melting and boiling points, malleability, ductility and conductivity
- Analyse data on melting points of different metals

Why are metals malleable and ductile?

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

- Practical observation - Written exercises - Oral questions

Inorganic Chemistry

Chemical Bonding - Uses of metallic structures related to 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Introduction to periodic properties
Periodicity - Physical appearance and density of group I elements

By the end of the lesson, the learner should be able to:
- Define periodicity and periodic properties
- Identify atomic size, ionisation energy, electron affinity and electronegativity
- Relate periodic trends to arrangement of elements in the periodic table

In groups, learners are guided to:
- Search for information on periodic properties using print or digital materials
- Discuss the meaning of atomic radius, ionisation energy, electron affinity and electronegativity
- Study sample periodic tables to identify patterns

What causes the repeating pattern of properties in the periodic table?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 104
- Periodic table charts
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 106
- Sodium metal
- Scalpel blade
- Petri dish

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

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 trend in atomic and ionic radii of group I elements
- Draw electron arrangements of group I atoms and ions
- Relate atomic size to the number of energy levels in atoms
- Describe trends in ionisation energy and electronegativity of group I elements
- Analyse data on ionisation energies
- Connect ionisation energy to reactivity of metals like sodium in fireworks

In groups, learners are guided to:
- Draw dot (.) and cross (x) structures of lithium, sodium and potassium atoms and ions
- Compare atomic and ionic radii of group I elements
- Analyse data on atomic and ionic radii trends
- Analyse data on ionisation energies of group I elements
- Discuss factors affecting ionisation energy (atomic radius, shielding effect)
- Create trend charts for electronegativity values

Why is the ionic radius of sodium smaller than its atomic radius?
Why does lithium have a higher ionisation energy than sodium?

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

- Written exercises - Oral questions - Group discussions
- Written exercises - Data analysis - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen
Periodicity - Reactions of group I elements with chlorine and cold water

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

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

What type of oxides do alkali metals form when they burn in oxygen?

- 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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group I elements
Periodicity - Appearance, atomic and ionic radii of group II elements

By the end of the lesson, the learner should be able to:
- Outline applications of group I elements
- Relate properties to specific uses
- Identify uses in batteries, street lights, medicine and photography

In groups, learners are guided to:
- Search for information on applications of group I elements using print or digital materials
- Discuss uses of lithium in batteries, sodium in lamps, potassium in fertilizers
- Create presentations on applications

How are the properties of alkali metals utilised in modern technology?

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy, melting and boiling points of group II elements

By the end of the lesson, the learner should be able to:
- 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:
- 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

Why do group II elements have two ionisation energies?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 121
- Graph paper
- Data tables
- Digital devices

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy, melting and boiling points of group II elements
Periodicity - Reactions of group II elements with water, steam and oxygen

By the end of the lesson, the learner should be able to:
- 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
- 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:
- 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
- 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 do group II elements have two ionisation energies?
Why does magnesium react slowly with cold water but vigorously with steam?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 121
- Graph paper
- Data tables
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 123
- Magnesium ribbon
- Calcium metal
- Gas jar of oxygen
- Bunsen burner
- Litmus paper

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

Inorganic Chemistry

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 group II elements with dilute acids and chlorine
- Write balanced equations for the reactions
- Relate reactions to production of hydrogen gas for industrial uses

In groups, learners are guided to:
- Investigate reactions of magnesium and calcium with dilute HCl, dilute H₂SO₄ and dilute HNO₃
- Test gases produced with burning splint
- Investigate reactions with chlorine gas
- Write chemical equations for all reactions

Why does the reaction of calcium with dilute sulphuric acid stop quickly?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 127
- Dilute acids
- Magnesium ribbon
- Calcium metal
- Chlorine gas
- Test tubes

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group II 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Prepare chlorine gas in the laboratory
- Describe physical properties of halogens
- Relate chlorine's properties to its use in water treatment and disinfection

In groups, learners are guided to:
- Set up apparatus to prepare chlorine gas from concentrated HCl and potassium manganate (VII)
- Observe colour, smell and solubility of chlorine
- Compare physical properties of fluorine, chlorine, bromine and iodine

Why is chlorine collected by downward delivery?

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

- Practical report - Observation - Written exercises

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
- Investigate reactions of halogens with water and metals
- Write balanced equations for the reactions
- Relate halogen reactivity to their use in antiseptics and disinfectants

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
- Bubble chlorine gas into distilled water and test with litmus paper
- Add bromine and iodine to water and observe
- Pass chlorine gas over heated iron wool
- Write chemical equations for reactions

Why is iodine a solid while chlorine is a gas at room temperature?
Why does chlorine turn moist blue litmus paper red and then white?

- 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
- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Displacement reactions and bleaching action of chlorine

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

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

Why can chlorine displace bromine and iodine from their compounds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 142
- Potassium bromide solution
- Potassium iodide solution
- Chlorine gas
- Coloured cloth
- Flower petals

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group VII elements

By the end of the lesson, the learner should be able to:
- Outline applications of group VII elements
- Relate properties to specific uses
- Identify uses in water treatment, photography, medicine and refrigeration

In groups, learners are guided to:
- Search for information on applications of halogens
- Discuss uses of chlorine in water treatment, bromine in photography, iodine in medicine
- Create presentations on halogen applications

How is chlorine used to make drinking water safe?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 147
- Digital devices
- Reference materials

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Applications of group VII elements

By the end of the lesson, the learner should be able to:
- Outline applications of group VII elements
- Relate properties to specific uses
- Identify uses in water treatment, photography, medicine and refrigeration

In groups, learners are guided to:
- Search for information on applications of halogens
- Discuss uses of chlorine in water treatment, bromine in photography, iodine in medicine
- Create presentations on halogen applications

How is chlorine used to make drinking water safe?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 147
- Digital devices
- Reference materials

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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:
- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging
- Describe trends in atomic size and ionisation energy across period 3
- Plot graphs showing trends across the period
- Relate effective nuclear charge to changes in atomic properties

In groups, learners are guided to:
- 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
- Draw atomic structures of period 3 elements
- Analyse data on atomic radii and ionisation energies
- Plot graphs of ionisation energy against atomic number
- Discuss the role of effective nuclear charge

Why are noble gases called inert gases?
Why does atomic radius decrease across period 3?

- 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
- Periodic table
- Data tables

- Written exercises - Oral questions - Group discussions
- Data analysis - Written exercises - Oral questions

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

Periodicity - Reactions of period 3 elements with chlorine and dilute 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

- Practical report - Written exercises - Oral questions

Physical Chemistry

Acids and Bases - Dissociation of acids in aqueous solutions
Acids and Bases - Dissociation of bases in aqueous solutions

By the end of the lesson, the learner should be able to:
- Define dissociation of acids in water
- Demonstrate dissociation of acids in aqueous solutions
- Relate dissociation of acids to everyday substances like vinegar and lemon juice

In groups, learners are guided to:
- Discuss with peers the meaning of dissociation of acids in water
- Carry out experiments to demonstrate dissociation of dilute hydrochloric acid
- Record observations on release of hydrogen ions (H⁺)

How do acids behave when dissolved in water?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 164
- Dilute hydrochloric acid
- Test tubes
- 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

- Observation - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Properties of acids
Acids and Bases - Properties of bases
Acids and Bases - Reaction of dilute acids with metals

By the end of the lesson, the learner should be able to:
- Describe the physical properties of acids
- Identify acids based on their characteristics
- Relate properties of acids to food preservation using citric acid and vinegar
- Describe the reaction between dilute acids and metals
- Carry out experiments on acid-metal reactions
- Relate acid-metal reactions to corrosion of metallic structures and pipes

In groups, learners are guided to:
- Discuss with peers the properties of acids (sour taste, effect on litmus paper, pH values)
- Classify acids as organic and mineral acids
- Identify common acids found at home and in the laboratory
- Measure dilute hydrochloric acid and add zinc powder
- Observe effervescence and test gas produced using burning splint
- Write balanced equations for the reactions

What are the characteristic properties of acids?
What products are formed when acids react with metals?

- Chemistry Learner's Book Grade 10 pg. 166
- Samples of acids
- pH indicator paper
- Blue litmus paper
- Digital resources
- 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

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

Physical Chemistry

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:
- Perform the confirmatory test for hydrogen gas
- Record observations accurately
- Connect hydrogen gas production to industrial processes like welding

In groups, learners are guided to:
- Collect hydrogen gas produced from acid-metal reactions
- Test the gas using a burning splint
- Record the pop sound observation
- Write equations for reactions of different metals with acids

How can hydrogen gas be identified in the laboratory?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 170
- Dilute sulphuric acid
- Magnesium ribbon
- Test tubes
- Wooden splints
- Delivery tubes
- Chemistry Learner's Book Grade 10 pg. 170
- Sodium carbonate
- Dilute hydrochloric acid
- Calcium hydroxide
- Delivery tubes
- Test tubes

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Reaction of acids with hydrogen carbonates
Acids and Bases - Reaction of acids with metal oxides

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

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

How is carbon (IV) oxide gas tested in the laboratory?

- 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

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Reaction of acids with metal hydroxides

By the end of the lesson, the learner should be able to:
- 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 sulphuric (VI) acid to sodium hydroxide with phenolphthalein
- Observe colour change from pink to colourless
- Write balanced equations for the neutralisation reaction

How do indicators show the end point of neutralisation?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 173
- Sodium hydroxide solution
- Dilute sulphuric (VI) acid
- Phenolphthalein indicator
- Beakers
- Measuring cylinders

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Universal indicator and pH scale

By the end of the lesson, the learner should be able to:
- Explain the pH scale and its use
- Determine pH values using universal indicator
- Relate pH values to water quality testing and swimming pool maintenance

In groups, learners are guided to:
- Prepare solutions of various acids and bases
- Add universal indicator to each solution
- Compare colours with pH scale chart
- Record pH values and classify solutions

What does the pH scale measure?

- 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 - Observation - Written exercises

Physical Chemistry

Acids and Bases - Strong and weak acids

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

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Strong and weak bases

By the end of the lesson, the learner should be able to:
- Differentiate between strong and weak bases
- Classify bases based on their pH values
- Relate base strength to drain cleaners (strong) versus baking soda (weak)

In groups, learners are guided to:
- Test 0.1 M sodium hydroxide and 0.1 M ammonium hydroxide using universal indicator
- Compare pH values of strong and weak bases
- Discuss characteristics of strong and weak bases

How can strong and weak bases be distinguished?

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

- Practical assessment - Observation - Written assignments

Physical Chemistry

Acids and Bases - Electrical conductivity of acids and bases

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

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

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

By the end of the lesson, the learner should be able to:
- Outline the uses of acids in various sectors
- Search for information on industrial applications of acids
- Relate acids to food preservation, fertiliser production and metal cleaning
- 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:
- Search for information on uses of acids using print or digital materials
- Discuss uses in food industry, manufacturing and cleaning
- Prepare charts showing applications of acids
- 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 acids useful in our daily lives?
How are bases applied in agriculture and industry?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers
- Access & Learn Chemistry Learner's Book Grade 10 pg. 179
- Soil samples
- pH paper
- Litmus paper
- Vinegar
- Citrus peels
- Digital resources

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

Physical Chemistry

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:
- Define the term salt
- Explain how salts are formed from neutralisation reactions
- Relate salt formation to table salt production and food seasoning

In groups, learners are guided to:
- Study equations showing neutralisation reactions
- Identify reactants and products in salt formation
- Discuss how hydrogen ions in acids are replaced by metal ions
- Examine samples of different salts

What is a salt and how is it formed?

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

- Oral questions - Written exercises - Observation

Physical Chemistry

Introduction to Salts - Acid salts
Introduction to Salts - Basic and double salts

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

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

How do acid salts differ from normal salts?

- 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

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Introduction to Salts - Soluble and insoluble salts

By the end of the lesson, the learner should be able to:
- Define soluble and insoluble salts
- Carry out experiments to determine solubility of salts
- Relate solubility to water treatment and removal of hardness in water

In groups, learners are guided to:
- Place spatulaful of different salts in beakers with distilled water
- Stir and observe dissolution
- Warm mixtures and observe changes
- Record observations and classify salts as soluble or insoluble

How can soluble salts be distinguished from insoluble salts?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 185
- Copper (II) sulphate
- Copper (II) carbonate
- Distilled water
- Beakers
- Bunsen burner

- Practical assessment - Observation - Written exercises

Physical Chemistry

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:
- State solubility rules for common salts
- Apply solubility rules to predict salt solubility
- Connect solubility rules to choosing appropriate chemicals for water softening
- Describe preparation of soluble salts using acid and metal
- Prepare zinc chloride from zinc and hydrochloric acid
- Connect this method to production of hydrogen gas for industrial use

In groups, learners are guided to:
- Study the solubility table for chlorides, nitrates, sulphates and carbonates
- Discuss exceptions to solubility rules
- Practise predicting solubility of given salts
- Test predictions experimentally
- Add zinc powder to dilute hydrochloric acid until excess
- Test gas produced with burning splint
- Filter to obtain filtrate
- Evaporate to saturation and crystallise

What rules govern the solubility of salts?
Why is the metal added in excess when preparing salts?

- Chemistry Learner's Book Grade 10 pg. 185
- Solubility table charts
- Various salt samples
- Distilled water
- Test tubes
- 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

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

Physical Chemistry

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

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

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

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 carbonate
- Prepare sodium nitrate from sodium carbonate and nitric acid
- Relate effervescence to carbon dioxide fire extinguishers

In groups, learners are guided to:
- Add sodium carbonate to dilute nitric (V) acid until no more gas bubbles
- Test gas with calcium hydroxide
- Filter, evaporate and crystallise
- Write balanced equation for the reaction

How can you tell when the reaction between acid and carbonate is complete?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 191
- Sodium carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Filter funnel
- Evaporating dish

- Practical assessment - Observation - Written assignments

Physical Chemistry

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 carbonate
- Prepare sodium nitrate from sodium carbonate and nitric acid
- Relate effervescence to carbon dioxide fire extinguishers

In groups, learners are guided to:
- Add sodium carbonate to dilute nitric (V) acid until no more gas bubbles
- Test gas with calcium hydroxide
- Filter, evaporate and crystallise
- Write balanced equation for the reaction

How can you tell when the reaction between acid and carbonate is complete?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 191
- Sodium carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Filter funnel
- Evaporating dish

- Practical assessment - Observation - Written assignments

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
- Describe behaviour of salts when exposed to atmosphere
- Carry out experiments to investigate salt behaviour in air
- Connect hygroscopic salts to silica gel sachets used to keep products dry

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
- Place samples of different salts on watch glasses
- Leave uncovered for 24 hours
- Observe and record changes in appearance
- Classify salts as hygroscopic, deliquescent or efflorescent

What is double decomposition and how is it used to prepare insoluble salts?
How do salts behave when exposed to air?

- 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
- Practical assessment - Observation - 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