Inorganic Chemistry

Deriving formulae of compounds I
Deriving formulae of compounds II

By the end of the lesson, the learner should be able to:
- State the steps for writing formulae of compounds
- Derive formulae of simple ionic compounds
- Apply the cross-over method to write chemical formulae
- Derive formulae of compounds containing radicals
- Write formulae of compounds with transition elements
- Apply formulae writing skills to complex compounds

- Discuss the steps for writing formulae of compounds
- Study worked examples on deriving formulae
- Practise writing formulae using the cross-over method
- Write formulae of compounds containing radicals
- Practise writing formulae of compounds with variable oxidation numbers
- Compare formulae with classmates for peer learning

How do you write the formula of a compound?
How do you write the formula of a compound containing a radical?

- Access and Learn Chemistry Learner's Book pg. 63
- Valency tables
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 64
- Valency tables
- Digital devices

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations I

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

- 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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Writing balanced chemical equations II

By the end of the lesson, the learner should be able to:
- Write state symbols in chemical equations
- Balance chemical equations by adjusting coefficients
- Apply the law of conservation of mass to balance equations

- Study the steps for balancing chemical equations
- Study worked examples on balancing equations
- Practise balancing simple chemical equations

How do you balance a chemical equation?

- Access and Learn Chemistry Learner's Book pg. 65
- Digital devices
- Practice worksheets

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations III

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

- 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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Role of electron arrangement in the periodic table - Project
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:
- Make a periodic table for the first 20 elements using locally available materials
- Explain the role of electron arrangement in the periodic table
- Apply creative skills to design and construct educational resources
- Identify different types of chemical bonds
- Distinguish between ionic, covalent and metallic bonds
- Connect different bond types to substances used in daily life like salt and water

- Use locally available materials to create a periodic table
- Include element names, symbols, atomic numbers and electron arrangements
- Display the periodic table for peer assessment
- Discuss with peers different types of chemical bonds (ionic, covalent, dative covalent, hydrogen bond, Van der Waals forces and metallic)
- Use models to represent different bond types
- Search for information using digital resources on bond types

How does electron arrangement determine the organization of the periodic table?
What determines the type of bond formed between atoms?

- Access and Learn Chemistry Learner's Book pg. 67
- Manila paper or carton box
- Coloured pencils
- Flashcards
- 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
- Digital devices
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices

- Project assessment - Peer evaluation - Observation
- Oral questions - Group discussions - Written assignments

Inorganic Chemistry

Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide
Chemical Bonding - Giant ionic structures and lattice

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

- 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

What holds sodium and chloride ions together in sodium chloride?

- 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

- Written assignments - Practical observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Solubility of ionic compounds
Chemical Bonding - Thermal conductivity, melting and boiling points of ionic compounds

By the end of the lesson, the learner should be able to:
- Investigate the solubility of ionic compounds
- Explain why ionic compounds dissolve in water
- Apply knowledge of solubility to dissolving salt in cooking

- Carry out experiments to investigate solubility of sodium chloride and copper (II) chloride in water and ethanol
- Record and discuss observations
- Relate solubility to polarity of water molecules

Why do ionic compounds dissolve in water but not in organic solvents?

- 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

- Practical report - Observation - Written exercises

Inorganic Chemistry

Chemical Bonding - Electrical conductivity in molten and aqueous ionic compounds
Chemical Bonding - Uses of ionic compounds

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

- 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

Why do ionic compounds conduct electricity only when molten or in solution?

- 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

- Practical report - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - The covalent chemical bond
Chemical Bonding - Double and triple covalent bonds

By the end of the lesson, the learner should be able to:
- Describe the formation of covalent bonds
- Illustrate single covalent bonds using dot and cross diagrams
- Connect covalent bonding to common molecules like water and oxygen
- Illustrate double and triple covalent bonds
- Draw Lewis structures for oxygen and nitrogen molecules
- Relate multiple bonds to atmospheric gases we breathe

- Discuss how atoms share electrons to form covalent bonds
- Draw dot (.) and cross (x) diagrams for hydrogen and chlorine molecules
- Use modelling clay to represent covalent bonding
- 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

How do non-metal atoms bond with each other?
Why do some molecules have double or triple bonds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 82
- Modelling clay
- Wooden splints
- Charts showing covalent bonds
- Access & Learn Chemistry Learner's Book Grade 10 pg. 83
- Modelling materials
- Charts of molecular structures

- Written exercises - Observation - Oral questions
- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride

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

- 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

- Written exercises - Observation - Oral questions

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

- 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

- 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

- 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 - 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

- 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

- 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

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

- 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

How do the structures of diamond and graphite determine their uses?

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

- Written assignments - Group presentations - Oral questions

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
- Describe physical properties of metallic structures
- Investigate thermal conductivity of metals
- Connect metallic properties to uses in cooking utensils and electrical wires

- 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
- 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 good conductors of electricity and heat?
Why are metals malleable and ductile?

- 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
- Digital devices

- Written exercises - Oral questions - Observation
- Practical observation - Written exercises - Oral questions

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

- 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

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

- 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

- Observation - Practical report - Oral questions

Inorganic Chemistry

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 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

- 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 does lithium have a higher ionisation energy than sodium?

- 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 - 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
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:
- Investigate reactions of lithium and sodium with oxygen
- Write balanced equations for reactions with oxygen
- Relate metal oxide formation to rusting and corrosion processes
- Outline applications of group I elements
- Relate properties to specific uses
- Identify uses in batteries, street lights, medicine and photography

- 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
- 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

What type of oxides do alkali metals form when they burn in oxygen?
How are the properties of alkali metals utilised in modern technology?

- 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

- Practical report - Written exercises - Observation
- 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

- 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 - Reactions of group II elements with water, steam and oxygen

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

- 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

- 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

- 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
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
- Prepare chlorine gas in the laboratory
- Describe physical properties of halogens
- Relate chlorine's properties to its use in water treatment and disinfection

- 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
- 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

How is calcium used in the construction industry?
Why is chlorine collected by downward delivery?

- 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
- Practical report - Observation - Written exercises

Inorganic Chemistry

Periodicity - Melting, boiling points and gradation in size of group VII elements

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

- 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

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group VII elements with water and metals

By the end of the lesson, the learner should be able to:
- Investigate reactions of halogens with water and metals
- Write balanced equations for the reactions
- Relate halogen reactivity to their use in antiseptics and disinfectants

- 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 does chlorine turn moist blue litmus paper red and then white?

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

- 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

- 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
Periodicity - Physical properties and applications of noble gases

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
- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging

- 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
- 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

How is chlorine used to make drinking water safe?
Why are noble gases called inert gases?

- 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

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

Inorganic Chemistry

Periodicity - Atomic size, ionisation energy and electronegativity across period 3

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

- 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 does atomic radius decrease across period 3?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Periodic table
- Data tables

- 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

- 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

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

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

- 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

- Practical report - Written exercises - Oral questions

Physical Chemistry

Acids and Bases - Dissociation of bases in aqueous solutions
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:
- Explain dissociation of bases in water
- Demonstrate dissociation of bases in aqueous solutions
- Connect dissociation of bases to household cleaning products like soap and detergents
- Describe the physical properties of bases
- Differentiate between bases and alkalis
- Connect properties of bases to cleaning agents and antacids used at home

- Carry out experiments to demonstrate dissociation of sodium hydroxide solution
- Test solutions using litmus paper and phenolphthalein indicator
- Record observations on release of hydroxide ions (OH⁻)
- 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 ions are released when bases dissolve in water?
What common household substances are basic in nature?

- 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
- 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

- Practical assessment - Oral questions - 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

- 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

- 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

- 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
Acids and Bases - Strong and weak acids

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
- Differentiate between strong and weak acids
- Classify acids based on their pH values
- Connect acid strength to battery acid (strong) versus citrus fruits (weak)

- 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
- 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

What does the pH scale measure?
Why do strong acids have lower pH values than weak acids?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 175
- Universal indicator
- pH scale chart
- Various acid and base solutions
- Test tubes
- Droppers
- 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 - Observation - Written exercises
- 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)

- 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

- 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

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

- 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

How are acids useful in our daily lives?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers

- Oral questions - Written assignments - Project assessment

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
Introduction to Salts - Acid 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
- Describe normal salts and their properties
- Identify examples of normal salts
- Connect normal salts to common table salt and fertilisers like potassium nitrate

- 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
- Discuss characteristics of normal salts (no replaceable hydrogen, pH of 7)
- Identify cations and anions in normal salts
- Write formulae of normal salts (NaCl, KNO₃, CaSO₄)
- Test solutions of normal salts with litmus paper

How are bases applied in agriculture and industry?
What are normal salts and their characteristics?

- 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
- Litmus paper
- Test tubes
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 183
- Sodium hydrogen carbonate
- pH paper

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

Physical Chemistry

Introduction to Salts - Basic and double salts
Introduction to Salts - Soluble and insoluble salts

By the end of the lesson, the learner should be able to:
- Describe basic salts and double salts
- Identify examples of basic and double salts
- Connect double salts to alum used in water purification and dyeing

- Discuss characteristics of basic salts (contain hydroxide ions, pH greater than 7)
- Discuss double salts (two different cations or anions)
- Write formulae of double salts
- Categorise provided salt samples into types

What distinguishes basic salts and double salts from other types?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 184
- Samples of basic and double salts
- Potassium aluminium sulphate (alum)
- Litmus paper
- pH paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 185
- Copper (II) sulphate
- Copper (II) carbonate
- Distilled water
- Beakers
- Bunsen burner

- Oral questions - Written exercises - Observation

Physical Chemistry

Introduction to Salts - Solubility rules
Introduction to Salts - Preparation by direct synthesis

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

- Study the solubility table for chlorides, nitrates, sulphates and carbonates
- Discuss exceptions to solubility rules
- Practise predicting solubility of given salts
- Test predictions experimentally

What rules govern the solubility of 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

- Oral questions - Written exercises - Practical assessment

Physical Chemistry

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 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

- Add zinc powder to dilute hydrochloric acid until excess
- Test gas produced with burning splint
- Filter to obtain filtrate
- Evaporate to saturation and crystallise

Why is the metal added in excess when preparing salts?

- 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

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
- Describe preparation of salts using acid and carbonate
- Prepare sodium nitrate from sodium carbonate and nitric acid
- Relate effervescence to carbon dioxide fire extinguishers

- 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
- 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 does phenolphthalein indicate the end point of neutralisation?
How can you tell when the reaction between acid and carbonate is complete?

- 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
- Practical assessment - Observation - Written assignments

Physical Chemistry

Introduction to Salts - Preparation by precipitation (double decomposition)

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

- 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

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Introduction to Salts - Hygroscopic, deliquescent and efflorescent salts

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

- 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

How do salts behave when exposed to air?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 196
- Iron (III) chloride
- Anhydrous copper (II) sulphate
- Sodium carbonate decahydrate
- Watch glasses

- 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

- 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