Inorganic Chemistry

Deriving formulae of compounds I
Deriving formulae of compounds II
Writing balanced chemical equations I

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
- Digital devices
- Charts showing chemical equations

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations II
Writing balanced chemical equations III

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
- Access and Learn Chemistry Learner's Book pg. 66

- 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

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

- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide
Chemical Bonding - Giant ionic structures and lattice
Chemical Bonding - Solubility of ionic compounds
Chemical Bonding - Thermal conductivity, melting and boiling points of ionic compounds

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
- 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

- Written assignments - Practical observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Electrical conductivity in molten and aqueous ionic compounds
Chemical Bonding - Uses of ionic compounds
Chemical Bonding - The covalent chemical bond
Chemical Bonding - Double and triple covalent bonds
Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride

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

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

- 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

- 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 ionic compounds conduct electricity only when molten or in solution?
Why do some molecules have double or triple bonds?

- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 83
- Modelling materials
- Charts of molecular structures
- Access & Learn Chemistry Learner's Book Grade 10 pg. 84
- Charts showing molecular structures
- Digital devices

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

Inorganic Chemistry

Chemical Bonding - Dative covalent (coordinate) bonding
Chemical Bonding - Hydrogen bonding and Van der Waals forces

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

- Written exercises - Oral questions - Group discussions

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

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of diamond
Chemical Bonding - Giant atomic structure of graphite

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

- Model assessment - Written exercises - Oral questions

Inorganic Chemistry

Chemical Bonding - Uses of diamond, graphite and silicon (IV) oxide
Chemical Bonding - Metallic bonding and delocalised electrons
Chemical Bonding - Physical properties of giant metallic structures
Chemical Bonding - Uses of metallic structures related to properties
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:

- Outline uses of diamond, graphite and silicon (IV) oxide
- Relate uses to their structural properties
- Identify applications in drilling, electronics and glass making

- 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 giant atomic structures
- Discuss why diamond is used in drilling bits
- Explain the use of graphite as a lubricant and in electrodes

- 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 do the structures of diamond and graphite determine their uses?
How does metallic bonding make metals suitable for electrical wiring?

- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 99
- Metal and wood pieces
- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 106
- Sodium metal
- Scalpel blade
- Petri dish

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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 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

- 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

Why is the ionic radius of sodium smaller than its atomic radius?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 107
- Periodic table
- Graph paper
- Digital devices

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Periodicity - Ionisation energy and electronegativity 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

- Written exercises - Data analysis - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy and electronegativity 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

- Written exercises - Data analysis - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy and electronegativity 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

- Written exercises - Data analysis - Oral questions

Inorganic Chemistry

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 melting and boiling points of group I elements
- Investigate electrical conductivity of alkali metals
- Relate conductivity to use of sodium in sodium-vapour lamps

- Analyse data on melting and boiling points of group I elements
- Set up apparatus to investigate electrical conductivity of lithium and sodium
- Discuss the relationship between metallic bond strength and melting points

Why do melting points decrease down group I elements?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 110
- Connecting wires
- Dry cells
- Bulb
- Sodium metal
- Lithium metal

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen

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

- 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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen

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

- 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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen

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

- 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

- Practical report - Written exercises - Observation

Inorganic Chemistry

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 group I elements with chlorine and cold water
- Write balanced equations for the reactions
- Connect vigorous reactions to safety precautions in laboratories and industries

- Lower molten lithium and sodium into jars of dry chlorine gas
- Place lithium and sodium metals in beakers with cold water
- Test products with litmus paper
- Write chemical equations for reactions

Why does sodium react more vigorously with water than lithium?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 114
- Chlorine gas
- Cold water
- Beakers
- Lithium and sodium metals
- Litmus paper

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group I 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

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Applications of group I 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

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Applications of group I 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

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Applications of group I 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

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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

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

- Describe the physical appearance of group II elements
- Describe trends in atomic and ionic radii of group II elements
- Relate alkaline earth metals to materials like magnesium in aircraft construction

- Observe samples of group II elements and describe appearance
- Scrape oxide layer from magnesium ribbon
- Analyse data on atomic and ionic radii of group II elements
- Draw electron arrangements of group II atoms and ions

Why do group II elements have a dull appearance when exposed to air?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

- Observation - Written exercises - Oral questions

Inorganic Chemistry

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

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

- Describe the physical appearance of group II elements
- Describe trends in atomic and ionic radii of group II elements
- Relate alkaline earth metals to materials like magnesium in aircraft construction

- Observe samples of group II elements and describe appearance
- Scrape oxide layer from magnesium ribbon
- Analyse data on atomic and ionic radii of group II elements
- Draw electron arrangements of group II atoms and ions

Why do group II elements have a dull appearance when exposed to air?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

- Observation - Written exercises - Oral questions

Inorganic Chemistry

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

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

- Describe the physical appearance of group II elements
- Describe trends in atomic and ionic radii of group II elements
- Relate alkaline earth metals to materials like magnesium in aircraft construction

- Observe samples of group II elements and describe appearance
- Scrape oxide layer from magnesium ribbon
- Analyse data on atomic and ionic radii of group II elements
- Draw electron arrangements of group II atoms and ions

Why do group II elements have a dull appearance when exposed to air?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

- Observation - Written exercises - Oral questions

Inorganic Chemistry

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

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

- Describe the physical appearance of group II elements
- Describe trends in atomic and ionic radii of group II elements
- Relate alkaline earth metals to materials like magnesium in aircraft construction

- Observe samples of group II elements and describe appearance
- Scrape oxide layer from magnesium ribbon
- Analyse data on atomic and ionic radii of group II elements
- Draw electron arrangements of group II atoms and ions

Why do group II elements have a dull appearance when exposed to air?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

- Observation - Written exercises - 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
Periodicity - Reactions of group II elements with dilute acids and chlorine
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:

- 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

- Outline applications of group II elements
- Relate properties to specific uses
- Identify uses in construction, medicine, alloys and agriculture

- 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

- 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

Why does magnesium react slowly with cold water but vigorously with steam?
How is calcium used in the construction industry?

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

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

Inorganic Chemistry

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

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

- Describe trends in melting and boiling points of halogens
- Describe trends in atomic and ionic radii of group VII elements
- Relate physical states to intermolecular forces and room temperature applications

- Analyse data on melting and boiling points of halogens
- Plot graphs of melting and boiling points against atomic number
- Analyse data on atomic and ionic radii
- Discuss Van der Waals forces in halogens

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

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

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Displacement reactions and bleaching action of chlorine
Periodicity - Applications of group VII elements

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Physical properties and applications of noble gases
Periodicity - Atomic size, ionisation energy and electronegativity across period 3
Periodicity - Reactions of period 3 elements with oxygen and water
Periodicity - Reactions of period 3 elements with chlorine and dilute acids

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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Data tables
- Access & Learn Chemistry Learner's Book Grade 10 pg. 155
- Sodium, magnesium, sulphur
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner

- Written exercises - Oral questions - Group discussions