Inorganic Chemistry

Chemical families - Halogens and Noble gases
Deriving formulae of compounds I

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

- Identify members of halogens and noble gases
- Describe common features of Group VII and Group VIII elements
- Connect halogens to uses like chlorine in water treatment and noble gases in lighting

- State the steps for writing formulae of compounds
- Derive formulae of simple ionic compounds
- Apply the cross-over method to write chemical formulae

- Identify elements in Group VII and Group VIII
- Discuss with peers common features of halogens
- Search for information on properties of noble gases

- Discuss the steps for writing formulae of compounds
- Study worked examples on deriving formulae
- Practise writing formulae using the cross-over method

Why are noble gases called inert gases?
How do you write the formula of a compound?

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

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

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

Inorganic Chemistry

Deriving formulae of compounds II

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

- Derive formulae of compounds containing radicals
- Write formulae of compounds with transition elements
- Apply formulae writing skills to complex compounds

- 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 containing a radical?

- 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

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

- 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

How does electron arrangement determine the organization of the periodic table?

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

- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

Role of electron arrangement in the periodic table - Project
Chemical Bonding - Role of valence electrons in bonding

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

- Explain the role of valence electrons in bonding
- Identify the octet and duplet rule in bond formation
- Relate chemical bonding to everyday materials like plastics and metals

- 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

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

How does electron arrangement determine the organization of the periodic table?
Why do atoms form bonds with other 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

- Project assessment - Peer evaluation - Observation
- Oral questions - Observation - Written exercises

Inorganic Chemistry

Chemical Bonding - Types of chemical bonds

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

- 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

- 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

What determines the type of bond formed between atoms?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Digital devices
- Charts showing bond types

- Oral questions - Group discussions - Written assignments

Inorganic Chemistry

Chemical Bonding - The ionic chemical bond
Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide

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

- Describe the formation of ionic bonds
- Illustrate electron transfer using dot and cross diagrams
- Relate ionic bonding to common substances like table salt

- Discuss the formation of ionic bonds between metals and non-metals
- Draw dot (.) and cross (x) diagrams to show ionic bonding
- Identify examples of ionic compounds

How do metals and non-metals combine to form ionic compounds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Digital devices
- Periodic table

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Giant ionic structures and lattice

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

- Describe giant ionic structures
- Model a 3-dimensional ionic lattice structure
- Link crystal structures to materials like gemstones and minerals

- Model a 3-dimensional sodium chloride ionic structure using locally available materials
- Discuss the arrangement of ions in a crystal lattice
- Compare models with diagrams of giant ionic lattices

How does the arrangement of ions affect the properties of ionic compounds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 76
- Modelling materials (clay, toothpicks)
- Charts of ionic lattices

- Project work - 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
Chemical Bonding - The covalent chemical bond

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

- 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

- 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

- 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

Why do ionic compounds conduct electricity only when molten or in solution?
How do non-metal atoms bond with each other?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 79
- Dry cells
- Bulb/ammeter
- Connecting wires
- Carbon rods
- Lead (II) bromide
- Access & Learn Chemistry Learner's Book Grade 10 pg. 81
- Digital devices
- Samples of ionic compounds

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

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

Inorganic Chemistry

Chemical Bonding - The covalent chemical bond

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

- 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

How do non-metal atoms bond with each other?

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

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Double and triple covalent bonds

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

- Illustrate double and triple covalent bonds
- Draw Lewis structures for oxygen and nitrogen molecules
- Relate multiple bonds to atmospheric gases we breathe

- Use dot (.) and cross (x) diagrams to show double bonds in oxygen molecules
- Illustrate triple covalent bonds in nitrogen molecules
- Model multiple covalent bonds using locally available materials

Why do some molecules have double or triple bonds?

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

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride

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

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

- Differentiate between intermolecular and intramolecular forces
- Illustrate hydrogen bonding and Van der Waals forces
- Connect intermolecular forces to properties of water like surface tension

- 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

- 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

- Carry out experiments to determine melting point of naphthalene
- Investigate thermal and electrical conductivity of molecular substances
- Compare properties with ionic compounds

Why does water have a relatively high boiling point compared to other small molecules?
Why do molecular substances have low melting and boiling points?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 86
- Modelling materials
- Digital devices

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

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

Inorganic Chemistry

Chemical Bonding - Melting, boiling points and conductivity 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

- Carry out experiments to determine melting point of naphthalene
- Investigate thermal and electrical conductivity of molecular substances
- Compare properties with ionic compounds

Why do molecular substances have low melting and boiling points?

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

- Practical report - Written exercises - Observation

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

- 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

- 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
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

- 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 - Metallic bonding and delocalised electrons

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

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

Why are metals good conductors of electricity and heat?

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

- 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

- 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

- 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 - 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

- 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

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

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

- 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

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

- Analyse data on atomic radii, ionisation energy, melting and boiling points of noble gases
- Discuss why noble gases are unreactive
- Search for information on uses of helium, neon and argon

Why are noble gases called inert gases?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 148
- Periodic table
- Digital devices
- Reference materials

- 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

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

- 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

- 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

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

- 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

What are the characteristic properties of acids?

- 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

- Observation - Oral questions - Written assignments

Physical Chemistry

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

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

- Describe the reaction between dilute acids and metals
- Carry out experiments on acid-metal reactions
- Relate acid-metal reactions to corrosion of metallic structures and pipes

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

- Measure dilute hydrochloric acid and add zinc powder
- Observe effervescence and test gas produced using burning splint
- Write balanced equations for the reactions

- 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

What products are formed when acids react with metals?
How can hydrogen gas be identified in the laboratory?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 169
- Zinc powder
- Dilute hydrochloric acid
- Test tubes
- Wooden splints
- Rubber corks
- Access & Learn Chemistry Learner's Book Grade 10 pg. 170
- Dilute sulphuric acid
- Magnesium ribbon
- 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 - Observation - Written exercises
- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Reaction of acids with hydrogen carbonates

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

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Reaction of acids with metal oxides

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

- Explain neutralisation reactions involving metal oxides
- Carry out experiments on acid-metal oxide reactions
- Relate neutralisation to treatment of acidic soils in agriculture

- Warm dilute nitric (V) acid and add magnesium oxide
- Test the resulting solution using pH paper
- Record observations and determine nature of solution
- Write balanced equations for the reactions

What is a neutralisation reaction?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 172
- Magnesium oxide
- Dilute nitric (V) acid
- pH paper
- Beakers
- Bunsen burner

- Practical assessment - Observation - Written exercises

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

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

- 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
Acids and Bases - Strong and weak bases

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

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

- 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 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

- 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

Why do strong acids have lower pH values than weak acids?
How can strong and weak bases be distinguished?

- Chemistry Learner's Book Grade 10 pg. 175
- 0.1 M hydrochloric acid
- 0.1 M ethanoic acid
- Universal indicator
- pH scale chart
- Test tubes

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

- Practical assessment - Oral questions - Written exercises
- 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 - 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

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

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

How are bases applied in agriculture and industry?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 179
- Soil samples
- pH paper
- Litmus paper
- Vinegar
- Citrus peels
- Digital resources

- Practical assessment - Oral questions - Written exercises