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SCHEME OF WORK
Chemistry
Grade 10 2026
TERM II
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WK LSN STRAND SUB-STRAND LESSON LEARNING OUTCOMES LEARNING EXPERIENCES KEY INQUIRY QUESTIONS LEARNING RESOURCES ASSESSMENT METHODS REFLECTION
1

opening and reporting
1 2
Inorganic Chemistry
The Atom - Sub-atomic particles
By the end of the lesson, the learner should be able to:
- Describe the structure of the atom
- Identify the location and properties of protons, neutrons and electrons
- Relate atomic structure to understanding matter around us
- Review with peers the concept of the structure of the atom
- Discuss the properties of sub-atomic particles
- Model the structure of an atom using locally available materials
What particles make up an atom?
- Front Row Chemistry Grade 10 pg. 14
- Modelling materials
- Charts showing atomic structure
- Observation - Oral questions - Model assessment
1 3
Inorganic Chemistry
The Atom - Atomic number and mass number
The Atom - Dalton's and Rutherford's atomic models
The Atom - Bohr's atomic model and Rutherford Gold Foil experiment
By the end of the lesson, the learner should be able to:
- Define atomic number and mass number
- Calculate the number of protons, neutrons and electrons in atoms
- Use atomic notation to identify elements in everyday materials
- Discuss the relationship between atomic number, mass number and electrons
- Calculate sub-atomic particles for given elements
- Draw atomic structures using dots and crosses
How do we determine the number of particles in an atom?
- Front Row Chemistry Grade 10 pg. 15
- Periodic table
- Exercise books
- Front Row Chemistry Grade 10 pg. 16
- Printed diagrams of atomic models
- Digital devices
- Front Row Chemistry Grade 10 pg. 17
- Digital devices with internet
- Simulation videos
- Written exercises - Oral questions - Individual assessment
1 4-5
Inorganic Chemistry
The Atom - Definition and examples of isotopes
The Atom - Calculating relative atomic mass
The Atom - Practice on relative atomic mass calculations
The Atom - Relationship between energy levels and orbitals
The Atom - Order of filling electrons in orbitals
By the end of the lesson, the learner should be able to:
- Define the term isotopes
- Identify isotopes of common elements
- Relate isotopes to applications in medicine and carbon dating
- Explain the relationship between energy levels and orbitals
- Identify s and p orbitals in atoms
- Connect electron arrangement to element properties like conductivity
- Brainstorm the meaning of isotopes
- Examine isotopes of carbon and hydrogen
- Discuss similarities and differences between isotopes
- Discuss energy levels and sub-shells
- Draw diagrams showing energy levels and orbitals
- Discuss electron capacity of different orbitals
Why do some atoms of the same element have different masses?
How are electrons organised around the nucleus?
- Front Row Chemistry Grade 10 pg. 17
- Periodic table
- Charts showing isotopes
- Front Row Chemistry Grade 10 pg. 18
- Calculators
- Worked examples
- Front Row Chemistry Grade 10 pg. 19
- Practice worksheets
- Front Row Chemistry Grade 10 pg. 20
- Diagrams of orbitals
- Coloured pencils
- Front Row Chemistry Grade 10 pg. 21
- Energy level diagrams
- Exercise books
- Oral questions - Written exercises - Individual assessment
- Oral questions - Written exercises - Observation
2 1
Inorganic Chemistry
The Atom - Writing electron configuration (Elements 1-10)
By the end of the lesson, the learner should be able to:
- Write electron arrangement using s and p notation
- Apply notation to elements 1-10
- Use electron configuration to explain why neon is used in lighting
- Draw electron arrangements for elements 1-10 using s and p notation
- Practice writing configurations
- Compare configurations with peers
How do we represent electron arrangement using s and p notation?
- Front Row Chemistry Grade 10 pg. 22
- Periodic table
- Exercise books
- Written exercises - Individual assessment - Peer assessment
2 2
Inorganic Chemistry
The Atom - Writing electron configuration (Elements 11-20)
The Atom - Modelling atomic structure
By the end of the lesson, the learner should be able to:
- Write electron arrangement for elements 11-20 using s and p notation
- Identify patterns in electron configurations
- Connect electron arrangement to element uses in batteries and construction
- Draw electron arrangements for elements 11-20
- Identify patterns across periods
- Share work with classmates for review
How does electron configuration change across periods?
- Front Row Chemistry Grade 10 pg. 22
- Periodic table
- Exercise books
- Front Row Chemistry Grade 10 pg. 23
- Locally available materials
- Modelling clay
- Written exercises - Oral questions - Individual assessment
2 3
Inorganic Chemistry
The Periodic Table - Historical development
The Periodic Table - Arrangement into groups and periods
The Periodic Table - Alkali metals and alkaline earth metals
By the end of the lesson, the learner should be able to:
- Describe the historical development of the periodic table
- Identify contributions of Mendeleev and Moseley
- Value scientific collaboration that led to the modern periodic table
- Brainstorm on historical development of the periodic table
- Search for information on contributions of scientists
- Discuss evolution of the periodic table
How did scientists organise elements into the periodic table?
- Front Row Chemistry Grade 10 pg. 24
- Digital devices
- Printed periodic tables
- Front Row Chemistry Grade 10 pg. 26
- Periodic table charts
- Exercise books
- Front Row Chemistry Grade 10 pg. 28
- Periodic table
- Charts showing chemical families
- Oral questions - Written exercises - Group discussions
2 4-5
Inorganic Chemistry
The Periodic Table - Halogens and noble gases
The Periodic Table - Duplet and octet rule
The Periodic Table - Formation of cations
The Periodic Table - Formation of anions
The Periodic Table - Writing electron configuration of ions using s and p notation
The Periodic Table - Valency of elements
By the end of the lesson, the learner should be able to:
- Describe properties of halogens and noble gases
- Compare different chemical families
- Relate noble gas stability to their use in light bulbs and balloons
- Explain how non-metallic atoms form anions
- Draw ionic structures of anions
- Relate anion formation to salt production in food industry
- Discuss characteristics of Group VII and VIII elements
- Compare properties of different chemical families
- Present findings to classmates
- Discuss how non-metallic atoms gain electrons
- Draw ionic structures of anions
- Compare cation and anion formation
Why are noble gases called inert gases?
How do non-metal atoms form negative ions?
- Front Row Chemistry Grade 10 pg. 28
- Periodic table
- Digital devices
- Front Row Chemistry Grade 10 pg. 29
- Diagrams of stable configurations
- Front Row Chemistry Grade 10 pg. 30
- Exercise books
- Diagrams showing ion formation
- Front Row Chemistry Grade 10 pg. 31
- Exercise books
- Diagrams showing anion formation
- Front Row Chemistry Grade 10 pg. 32
- Periodic table
- Exercise books
- Front Row Chemistry Grade 10 pg. 33
- Valency charts
- Written exercises - Oral questions - Observation
- Written exercises - Peer assessment - Oral questions
3

Opener exam
3 2
Inorganic Chemistry
The Periodic Table - Elements with variable oxidation numbers
By the end of the lesson, the learner should be able to:
- Identify elements with variable oxidation numbers
- Explain why some elements show variable valency
- Connect variable valency to rust formation (iron) and paint pigments (lead)
- Discuss elements with variable oxidation numbers
- Examine examples like iron, copper and lead
- Practice identifying oxidation states
Why do some elements have more than one oxidation number?
- Front Row Chemistry Grade 10 pg. 34
- Periodic table
- Examples of compounds
- Written exercises - Oral questions - Observation
3 3
Inorganic Chemistry
The Periodic Table - Common radicals and their valencies
By the end of the lesson, the learner should be able to:
- Define radicals and identify common radicals
- State valencies of common radicals
- Apply knowledge of radicals to understand compound names in cleaning products
- List examples of radicals and their valencies
- Discuss characteristics of radicals
- Practice identifying radicals in compounds
What are radicals and how do they combine with other elements?
- Front Row Chemistry Grade 10 pg. 35
- Charts showing radicals
- Exercise books
- Written exercises - Oral questions - Individual assessment
3 4-5
Inorganic Chemistry
The Periodic Table - Deriving formulae using valencies
The Periodic Table - Formulae of compounds with same valency
The Periodic Table - Formulae of compounds with different valencies
By the end of the lesson, the learner should be able to:
- Derive chemical formulae using valencies
- Apply the cross-over method
- Write correct formulae for compounds used in daily life like baking soda and salt
- Write formulae for compounds with different valencies
- Apply the cross-over method correctly
- Derive formulae for compounds like carbon dioxide and sulphuric acid
- Practice writing formulae using valencies and oxidation states
- Apply cross-over method to derive formulae
- Verify formulae with peers
- Practice writing formulae for compounds with different valencies
- Apply cross-over method systematically
- Share solutions with classmates
How do we write chemical formulae using valencies?
How do we write formulae when elements have different valencies?
- Front Row Chemistry Grade 10 pg. 36
- Valency charts
- Exercise books
- Front Row Chemistry Grade 10 pg. 37
- Exercise books
- Worked examples
- Front Row Chemistry Grade 10 pg. 37
- Exercise books
- Practice worksheets
- Written exercises - Individual assessment - Peer assessment
- Written exercises - Peer assessment - Individual assessment
4 1
Inorganic Chemistry
The Periodic Table - Formulae of compounds containing radicals
The Periodic Table - Writing word equations
By the end of the lesson, the learner should be able to:
- Write formulae for compounds containing radicals
- Apply brackets correctly for polyatomic ions
- Write formulae for fertilisers like ammonium sulphate and calcium phosphate
- Practice writing formulae with radicals
- Use brackets for polyatomic ions when necessary
- Complete exercises on compounds with radicals
How do we write formulae for compounds with radicals?
- Front Row Chemistry Grade 10 pg. 38
- Radical valency charts
- Exercise books
- Front Row Chemistry Grade 10 pg. 39
- Exercise books
- Reaction examples
- Written exercises - Individual assessment - Oral questions
4 2
Inorganic Chemistry
The Periodic Table - Writing symbol equations
By the end of the lesson, the learner should be able to:
- Convert word equations to symbol equations
- Write correct chemical formulae in equations
- Represent reactions like burning magnesium and rusting of iron
- Convert word equations to symbol equations
- Apply correct formulae in equations
- Practice writing symbol equations
How do we write chemical equations using symbols?
- Front Row Chemistry Grade 10 pg. 39
- Exercise books
- Formula charts
- Written exercises - Individual assessment - Peer assessment
4 3
Inorganic Chemistry
The Periodic Table - Balancing chemical equations
Chemical Bonding - Stability of atoms
By the end of the lesson, the learner should be able to:
- Balance chemical equations using appropriate coefficients
- Apply the law of conservation of mass
- Relate balanced equations to industrial processes like fertiliser production
- Write balanced chemical equations for simple reactions
- Practice balancing various equations
- Share solutions with classmates for review
Why must chemical equations be balanced?
- Front Row Chemistry Grade 10 pg. 40
- Exercise books
- Practice worksheets
- Front Row Chemistry Grade 10 pg. 56
- Periodic table
- Diagrams of electron configurations
- Written exercises - Individual assessment - Oral questions
4 4-5
Inorganic Chemistry
Chemical Bonding - Valence electrons in bonding
Chemical Bonding - Introduction to bond types
Chemical Bonding - Formation of ionic bonds
Chemical Bonding - Drawing ionic bond diagrams
Chemical Bonding - Structure of ionic lattice
Chemical Bonding - Physical properties of ionic compounds
By the end of the lesson, the learner should be able to:
- Explain the role of valence electrons in bonding
- Draw dot and cross diagrams for atoms
- Connect valence electrons to reactivity of elements like sodium and chlorine
- Draw Lewis structures for various ionic compounds
- Apply electron transfer principles
- Illustrate bonding in compounds like magnesium chloride and lithium sulphide
- Investigate the role of valence electrons in bonding
- Draw valence electron diagrams
- Discuss with peers the importance of outer electrons
- Draw Lewis diagrams for magnesium chloride
- Draw Lewis diagrams for lithium sulphide
- Share diagrams with peers for review
How do valence electrons determine how atoms bond?
How do we represent ionic bonding using diagrams?
- Front Row Chemistry Grade 10 pg. 57
- Coloured pencils
- Periodic table
- Front Row Chemistry Grade 10 pg. 58
- Samples of different substances
- Digital devices
- Front Row Chemistry Grade 10 pg. 59
- Exercise books
- Diagrams of ionic bonding
- Front Row Chemistry Grade 10 pg. 60
- Exercise books
- Coloured pencils
- Front Row Chemistry Grade 10 pg. 61
- Sodium chloride crystals
- Hand lens
- Watch glass
- Front Row Chemistry Grade 10 pg. 62
- Sodium chloride
- Distilled water
- Circuit with bulb
- Written exercises - Observation - Oral questions
- Written exercises - Peer assessment - Individual assessment
5 1
Inorganic Chemistry
Chemical Bonding - Formation of covalent bonds
Chemical Bonding - Single, double and triple covalent bonds
By the end of the lesson, the learner should be able to:
- Explain how covalent bonds form through electron sharing
- Distinguish between ionic and covalent bonding
- Relate covalent bonding to properties of water and oxygen we breathe
- Investigate role of valence electrons in covalent bonding
- Model covalent bond formation
- Compare ionic and covalent bonding
How do non-metal atoms share electrons to form covalent bonds?
- Front Row Chemistry Grade 10 pg. 66
- Modelling materials
- Diagrams of covalent bonding
- Front Row Chemistry Grade 10 pg. 67
- Exercise books
- Bond diagrams
- Oral questions - Written exercises - Observation
5 2
Inorganic Chemistry
Chemical Bonding - Covalent bonding in diatomic molecules
Chemical Bonding - Covalent bonding in compounds
By the end of the lesson, the learner should be able to:
- Draw Lewis structures for diatomic molecules
- Identify bonding and non-bonding electron pairs
- Relate diatomic molecules to atmospheric gases we depend on
- Draw Lewis diagrams for H₂, Cl₂, O₂, N₂
- Identify lone pairs and bonding pairs
- Practice drawing molecular structures
How do we draw covalent bonds in simple molecules?
- Front Row Chemistry Grade 10 pg. 68
- Exercise books
- Coloured pencils
- Front Row Chemistry Grade 10 pg. 69
- Molecular diagrams
- Written exercises - Peer assessment - Individual assessment
5 3
Inorganic Chemistry
Chemical Bonding - Formation of dative (coordinate) bonds
By the end of the lesson, the learner should be able to:
- Explain how dative covalent bonds form
- Draw structures showing coordinate bonds
- Apply dative bonding to understand ammonium ion formation in fertilisers
- Discuss formation of dative covalent bonds
- Draw structure of ammonium ion
- Identify donor and acceptor atoms
How is a dative bond different from a normal covalent bond?
- Front Row Chemistry Grade 10 pg. 71
- Exercise books
- Diagrams of dative bonding
- Written exercises - Oral questions - Individual assessment
5 4-5
Inorganic Chemistry
Chemical Bonding - Properties of simple molecular substances
Chemical Bonding - Van der Waals forces and hydrogen bonding
Chemical Bonding - Structure and properties of diamond
By the end of the lesson, the learner should be able to:
- Describe simple molecular structures
- Investigate properties of molecular substances
- Relate molecular properties to everyday substances like sugar and wax
- Distinguish between Van der Waals forces and hydrogen bonds
- Explain the effect of intermolecular forces on properties
- Relate hydrogen bonding to water's unique properties essential for life
- Investigate properties of molecular substances
- Compare melting points of molecular compounds
- Discuss intermolecular forces
- Visualise hydrogen bonding in water
- Compare substances with different intermolecular forces
- Discuss effect on boiling points
Why do molecular substances have low melting points?
Why does water have a higher boiling point than expected?
- Front Row Chemistry Grade 10 pg. 72
- Samples of molecular substances
- Bunsen burner
- Front Row Chemistry Grade 10 pg. 74
- Diagrams of hydrogen bonding
- Digital devices
- Front Row Chemistry Grade 10 pg. 76
- Models of diamond structure
- Modelling materials
- Practical assessment - Written exercises - Observation
- Written exercises - Oral questions - Observation
6 1
Inorganic Chemistry
Chemical Bonding - Structure and properties of graphite and silicon dioxide
Periodicity - Physical properties of alkali metals (atomic and ionic radii)
By the end of the lesson, the learner should be able to:
- Describe structures of graphite and silicon dioxide
- Compare properties of different giant covalent structures
- Relate graphite conductivity to pencil writing and lubricant uses
- Build models of graphite structure
- Compare graphite and diamond properties
- Discuss structure and uses of silicon dioxide
Why can graphite conduct electricity while diamond cannot?
- Front Row Chemistry Grade 10 pg. 77
- Modelling materials
- Sand samples
- Front Row Chemistry Grade 10 pg. 85
- Periodic table
- Data tables
- Written exercises - Project work - Observation
6 2
Inorganic Chemistry
Periodicity - Physical properties of alkali metals (appearance and hardness)
Periodicity - Physical properties of alkali metals (conductivity, melting and boiling points)
Periodicity - Ionisation energy of alkali metals
By the end of the lesson, the learner should be able to:
- Observe and describe appearance of alkali metals
- Investigate hardness of alkali metals
- Connect softness of alkali metals to their easy cutting and handling
- Observe appearance of freshly cut alkali metals
- Investigate hardness by cutting metals
- Discuss reasons for trends observed
Why are alkali metals soft and shiny when freshly cut?
- Front Row Chemistry Grade 10 pg. 87
- Lithium, sodium, potassium samples
- Scalpel
- White tile
- Front Row Chemistry Grade 10 pg. 89
- Circuit with bulb
- Alkali metal samples
- Data tables
- Front Row Chemistry Grade 10 pg. 90
- Data tables
- Digital devices
- Practical assessment - Observation - Written exercises
6 3
Inorganic Chemistry
Periodicity - Reaction of alkali metals with air/oxygen
Periodicity - Reaction of alkali metals with water
Periodicity - Reaction of alkali metals with chlorine and dilute acids
By the end of the lesson, the learner should be able to:
- Investigate reaction of alkali metals with oxygen
- Write balanced equations for the reactions
- Relate oxidation of sodium to its storage under oil
- Carry out experiments on reaction with air
- Observe flame colours and products
- Write word and chemical equations
What happens when alkali metals burn in air?
- Front Row Chemistry Grade 10 pg. 91
- Sodium metal
- Deflagrating spoon
- Gas jar of oxygen
- Front Row Chemistry Grade 10 pg. 93
- Sodium, potassium
- Trough with water
- Phenolphthalein
- Front Row Chemistry Grade 10 pg. 94
- Gas jar of chlorine
- Digital devices
- Practical assessment - Written exercises - Observation
6 4-5
Inorganic Chemistry
Periodicity - Applications of alkali metals
Periodicity - Physical properties of alkaline earth metals (atomic and ionic radii)
Periodicity - Physical properties of alkaline earth metals (appearance, hardness, conductivity)
By the end of the lesson, the learner should be able to:
- Identify uses of alkali metals
- Relate properties to applications
- Connect lithium to battery technology in phones and electric vehicles
- Observe appearance of alkaline earth metals
- Test hardness and conductivity
- Connect magnesium's light weight to its use in aircraft alloys
- Search for information on uses of alkali metals
- Discuss applications of lithium, sodium and potassium
- Present findings to class
- Observe appearance of magnesium and calcium
- Test hardness and ductility
- Test electrical conductivity
How are alkali metals used in everyday life?
Why are alkaline earth metals harder than alkali metals?
- Front Row Chemistry Grade 10 pg. 96
- Digital devices
- Pictures of applications
- Front Row Chemistry Grade 10 pg. 98
- Periodic table
- Data tables
- Front Row Chemistry Grade 10 pg. 99
- Magnesium ribbon
- Calcium metal
- Circuit with bulb
- Oral questions - Written exercises - Group presentations
- Practical assessment - Written exercises - Observation
7 1
Inorganic Chemistry
Periodicity - Physical properties of alkaline earth metals (melting points and ionisation energy)
Periodicity - Reaction of alkaline earth metals with air/oxygen
By the end of the lesson, the learner should be able to:
- Describe trends in melting points and ionisation energy
- Compare first and second ionisation energies
- Relate ionisation energy to element reactivity in fireworks
- Study data on melting and boiling points
- Investigate ionisation energy trends
- Discuss factors affecting ionisation energy
Why do alkaline earth metals have higher ionisation energies than alkali metals?
- Front Row Chemistry Grade 10 pg. 102
- Data tables
- Digital devices
- Front Row Chemistry Grade 10 pg. 106
- Magnesium ribbon
- Calcium metal
- Bunsen burner
- Written exercises - Oral questions - Individual assessment
7 2
Inorganic Chemistry
Periodicity - Reaction of alkaline earth metals with water and steam
By the end of the lesson, the learner should be able to:
- Investigate reactions with water and steam
- Compare reactivity of magnesium and calcium
- Relate calcium hydroxide formation to lime water used in construction
- React magnesium and calcium with cold water
- React magnesium with steam
- Test gas produced and write equations
Why does magnesium react slowly with cold water but vigorously with steam?
- Front Row Chemistry Grade 10 pg. 107
- Magnesium, calcium
- Trough
- Steam apparatus
- Practical assessment - Written exercises - Observation
7 3
Inorganic Chemistry
Periodicity - Reaction of alkaline earth metals with chlorine and dilute acids
Periodicity - Applications of alkaline earth metals
By the end of the lesson, the learner should be able to:
- Describe reactions with chlorine gas
- Investigate reactions with dilute acids
- Relate magnesium chloride formation to uses in dust control on roads
- React magnesium with chlorine gas
- React magnesium and calcium with dilute acids
- Write balanced equations
What products form when alkaline earth metals react with chlorine and acids?
- Front Row Chemistry Grade 10 pg. 110
- Magnesium ribbon
- Chlorine gas
- Dilute HCl and H₂SO₄
- Front Row Chemistry Grade 10 pg. 112
- Digital devices
- Pictures of applications
- Practical assessment - Written exercises - Observation
7 4-5
Inorganic Chemistry
Periodicity - Introduction to halogens
Periodicity - Laboratory preparation of chlorine gas
Periodicity - Trends in physical properties of halogens (atomic radii, melting and boiling points)
By the end of the lesson, the learner should be able to:
- Identify elements in the halogen family
- Describe electron configuration of halogens
- Relate halogen reactivity to their use in water treatment and disinfectants
- Prepare chlorine gas in the laboratory
- Describe properties of chlorine gas
- Relate chlorine properties to its use in bleach and water purification
- Determine chemical family of chlorine and fluorine
- Write electron configurations
- List other halogens
- Prepare chlorine gas from HCl and MnO₂
- Collect chlorine gas
- Observe properties of chlorine
Why are halogens called "salt formers"?
How is chlorine gas prepared and collected safely?
- Front Row Chemistry Grade 10 pg. 114
- Periodic table
- Digital devices
- Front Row Chemistry Grade 10 pg. 115
- MnO₂, conc. HCl
- Round bottomed flask
- Gas jars
- Front Row Chemistry Grade 10 pg. 117
- Data tables
- Periodic table
- Oral questions - Written exercises - Observation
- Practical assessment - Written exercises - Observation
8-9

mid term and break
10 1
Inorganic Chemistry
Periodicity - Appearance, physical state and solubility of halogens
By the end of the lesson, the learner should be able to:
- Describe appearance and physical states of halogens
- Investigate solubility in water and organic solvents
- Relate iodine's colour to its use as antiseptic in wound treatment
- Observe appearance of chlorine, bromine and iodine
- Test solubility in water
- Compare solubility of halogens
Why do halogens have different colours and physical states?
- Front Row Chemistry Grade 10 pg. 118
- Bromine, iodine samples
- Distilled water
- Test tubes
- Practical assessment - Written exercises - Observation
10 2
Inorganic Chemistry
Periodicity - Electrical conductivity of halogens
By the end of the lesson, the learner should be able to:
- Investigate electrical conductivity of halogens
- Explain why halogens do not conduct electricity
- Contrast halogen non-conductivity with metal conductivity in wiring
- Test electrical conductivity of iodine crystals
- Discuss results in terms of structure
- Compare with ionic and metallic substances
Why don't halogens conduct electricity?
- Front Row Chemistry Grade 10 pg. 120
- Iodine crystals
- Circuit with bulb
- Beaker
- Practical assessment - Written exercises - Observation
10 3
Inorganic Chemistry
Periodicity - Electron affinity and ion formation of halogens
Periodicity - Reaction of halogens with metals
By the end of the lesson, the learner should be able to:
- Define electron affinity
- Explain trends in electron affinity down Group VII
- Relate electron affinity to halogen reactivity in forming salts
- Understand how halogen atoms form ions
- Discuss electron affinity values
- Explain trend down the group
Why does electron affinity decrease down Group VII?
- Front Row Chemistry Grade 10 pg. 121
- Data tables
- Digital devices
- Front Row Chemistry Grade 10 pg. 122
- Iron filings
- Chlorine gas
- Combustion tube
- Written exercises - Oral questions - Individual assessment
10 4-5
Inorganic Chemistry
Periodicity - Reaction of chlorine with water
Periodicity - Displacement reactions of halogens
Periodicity - Applications of halogens
By the end of the lesson, the learner should be able to:
- Investigate reaction of chlorine with water
- Describe bleaching action of chlorine water
- Relate chlorine water to swimming pool disinfection
- Investigate displacement reactions of halogens
- Explain order of reactivity of halogens
- Apply displacement reactions to understand water purification processes
- Prepare chlorine water
- Test with litmus paper
- Investigate decomposition in sunlight
- Add chlorine water to potassium bromide and iodide solutions
- Observe colour changes
- Write ionic equations
How does chlorine react with water and why is it used as a bleach?
Why can chlorine displace bromine and iodine from their salts?
- Front Row Chemistry Grade 10 pg. 124
- Chlorine gas
- Distilled water
- Litmus paper
- Front Row Chemistry Grade 10 pg. 125
- Chlorine, bromine water
- KBr, KI solutions
- Test tubes
- Front Row Chemistry Grade 10 pg. 127
- Digital devices
- Product samples
- Practical assessment - Written exercises - Observation
11 1
Inorganic Chemistry
Periodicity - Introduction to noble gases
By the end of the lesson, the learner should be able to:
- Identify noble gases and their electron configurations
- Explain why noble gases are chemically inert
- Relate noble gas stability to their use in light bulbs and balloons
- Determine electronic configuration of noble gases
- Discuss stability of full electron shells
- List noble gas elements
Why are noble gases unreactive?
- Front Row Chemistry Grade 10 pg. 128
- Periodic table
- Digital devices
- Oral questions - Written exercises - Observation
11 2
Inorganic Chemistry
Periodicity - Trends in physical properties of noble gases
By the end of the lesson, the learner should be able to:
- Describe trends in physical properties of noble gases
- Explain trends in ionisation energy
- Relate noble gas properties to neon signs and helium balloons
- Review atomic structure of noble gases
- Study trends in atomic radii and ionisation energy
- Discuss reactivity based on electron configuration
Why do noble gases have very high ionisation energies?
- Front Row Chemistry Grade 10 pg. 129
- Data tables
- Periodic table
- Written exercises - Oral questions - Observation
11 3
Inorganic Chemistry
Periodicity - Applications of noble gases
Periodicity - Introduction to Period 3 elements
By the end of the lesson, the learner should be able to:
- Identify uses of noble gases
- Relate properties to applications
- Connect argon's inertness to its use in welding and light bulbs
- Search for information on uses of noble gases
- Discuss applications of He, Ne and Ar
- Present findings to class
How are noble gases used despite being unreactive?
- Front Row Chemistry Grade 10 pg. 131
- Digital devices
- Pictures of applications
- Periodic table
- Element samples
- Oral questions - Written exercises - Group presentations
11 4-5
Inorganic Chemistry
Periodicity - Trends in atomic radii across Period 3
Periodicity - Trends in ionisation energy across Period 3
Periodicity - Trends in melting and boiling points across Period 3
By the end of the lesson, the learner should be able to:
- Describe trends in atomic radii across Period 3
- Explain reasons for the observed trend
- Relate atomic size to element reactivity in sodium vs chlorine
- Describe trends in ionisation energy across Period 3
- Explain factors affecting ionisation energy
- Relate ionisation energy to metallic character of sodium vs non-metallic chlorine
- Study data on atomic radii of Period 3 elements
- Plot graph of atomic radius vs atomic number
- Explain trend using nuclear charge
- Study ionisation energy data for Period 3
- Discuss trend and anomalies
- Explain using atomic structure
Why does atomic radius decrease across Period 3?
Why does ionisation energy generally increase across Period 3?
- Front Row Chemistry Grade 10 pg. 132
- Data tables
- Graph paper
- Front Row Chemistry Grade 10 pg. 133
- Data tables
- Digital devices
- Front Row Chemistry Grade 10 pg. 134
- Charts
- Written exercises - Graphical work - Oral questions
- Written exercises - Oral questions - Individual assessment
12 1
Inorganic Chemistry
Periodicity - Electron affinity and electronegativity across Period 3
By the end of the lesson, the learner should be able to:
- Define electron affinity and electronegativity
- Describe trends across Period 3
- Relate electronegativity to bond polarity in water molecules
- Discuss electron affinity trends
- Study electronegativity values across Period 3
- Explain factors affecting these properties
Why does electronegativity increase across Period 3?
- Front Row Chemistry Grade 10 pg. 135
- Data tables
- Digital devices
- Written exercises - Oral questions - Individual assessment
12 2
Inorganic Chemistry
Periodicity - Reaction of Period 3 elements with oxygen (Na, Mg, Al)
Periodicity - Reaction of Period 3 elements with oxygen (Si, P, S)
By the end of the lesson, the learner should be able to:
- Investigate reactions of Na, Mg and Al with oxygen
- Write balanced equations for the reactions
- Relate magnesium oxide formation to its use in antacids and refractory materials
- Burn sodium, magnesium and aluminium in air
- Observe products formed
- Write word and chemical equations
What products form when Period 3 metals burn in oxygen?
- Front Row Chemistry Grade 10 pg. 136
- Na, Mg, Al samples
- Bunsen burner
- Deflagrating spoon
- Sulphur powder
- Gas jar of oxygen
- Practical assessment - Written exercises - Observation
12 3
Inorganic Chemistry
Periodicity - Reaction of Period 3 elements with chlorine (Na, Mg, Al)
By the end of the lesson, the learner should be able to:
- Investigate reactions of Period 3 metals with chlorine
- Write balanced equations for the reactions
- Relate aluminium chloride to its use as catalyst in industry
- React sodium, magnesium and aluminium with chlorine
- Observe products formed
- Write balanced equations
What happens when Period 3 metals react with chlorine?
- Front Row Chemistry Grade 10 pg. 137
- Na, Mg samples
- Chlorine gas
- Deflagrating spoon
- Practical assessment - Written exercises - Observation
12 4-5
Inorganic Chemistry
Periodicity - Reaction of Period 3 elements with chlorine (Si, P)
Periodicity - Reaction of Period 3 elements with water (Na, Mg)
Periodicity - Reaction of Period 3 elements with dilute acids
Periodicity - Comparison of trends across Period 3 and down groups
By the end of the lesson, the learner should be able to:
- Describe reactions of Si and P with chlorine
- Write balanced equations for the reactions
- Relate silicon tetrachloride to semiconductor manufacturing
- Investigate reactions of sodium and magnesium with water
- Compare reactivity of the two metals
- Relate sodium hydroxide formation to soap making
- Discuss reactions of silicon and phosphorus with chlorine
- Write balanced equations
- Compare metal and non-metal chlorides
- React sodium and magnesium with cold water
- React magnesium with steam
- Write balanced equations
What are the products when Period 3 non-metals react with chlorine?
Why does sodium react more vigorously with water than magnesium?
- Front Row Chemistry Grade 10 pg. 138
- Reference materials
- Digital devices
- Front Row Chemistry Grade 10 pg. 140
- Sodium, magnesium
- Trough with water
- Phenolphthalein
- Front Row Chemistry Grade 10 pg. 139
- Mg ribbon
- Dilute HCl, H₂SO₄
- Test tubes
- Front Row Chemistry Grade 10 pg. 141
- Summary charts
- Periodic table
- Written exercises - Oral questions - Observation
- Practical assessment - Written exercises - Observation
13

End term exam
14

end term break

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