Inorganic Chemistry

The Periodic Table - Valency of elements

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

- Define valency and determine valency from group number
- Identify valencies of common elements
- Use valency to predict how elements combine in fertilisers and medicines

- Discuss the relationship between valency and oxidation number
- Infer valency from electron arrangement
- Complete tables showing valencies

What is valency and how is it determined?

- Front Row Chemistry Grade 10 pg. 33
- Periodic table
- Valency charts

- Oral questions - Written exercises - Individual assessment

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

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

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 elements of same valency
- Simplify chemical formulae appropriately
- Apply formula writing to common compounds like table salt (NaCl)

- 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 same valencies
- Simplify formulae to lowest terms
- Complete exercises on formula writing

How do we write chemical formulae using valencies?
How do we simplify chemical formulae?

- Front Row Chemistry Grade 10 pg. 36
- Valency charts
- Exercise books
- Front Row Chemistry Grade 10 pg. 37
- Exercise books
- Worked examples
- Practice worksheets

- Written exercises - Individual assessment - Peer assessment
- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

The Periodic Table - Formulae of compounds containing radicals

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

- Written exercises - Individual assessment - Oral questions

Inorganic Chemistry

The Periodic Table - Writing word equations

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

- Represent chemical reactions using word equations
- Identify reactants and products
- Describe reactions occurring in cooking and cleaning

- Write word equations for simple chemical reactions
- Identify reactants and products in reactions
- Practice converting descriptions to word equations

How do we represent chemical reactions using words?

- Front Row Chemistry Grade 10 pg. 39
- Exercise books
- Reaction examples

- Written exercises - Oral questions - Observation

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

Inorganic Chemistry

The Periodic Table - Balancing chemical equations
Chemical Bonding - Stability of atoms
Chemical Bonding - Valence electrons in bonding
Chemical Bonding - Introduction to bond types
Chemical Bonding - Formation of ionic bonds

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

- Identify different types of chemical bonds
- Classify substances by bond type
- Relate bond types to properties of common materials like salt and water

- Write balanced chemical equations for simple reactions
- Practice balancing various equations
- Share solutions with classmates for review

- Discuss different types of chemical bonds
- Examine various substances and predict bond types
- Categorise materials by bonding

Why must chemical equations be balanced?
What are the main types of chemical bonds?

- Front Row Chemistry Grade 10 pg. 40
- Exercise books
- Practice worksheets
- Front Row Chemistry Grade 10 pg. 56
- Periodic table
- Diagrams of electron configurations
- 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

- Written exercises - Individual assessment - Oral questions
- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

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:

- Draw Lewis structures for various ionic compounds
- Apply electron transfer principles
- Illustrate bonding in compounds like magnesium chloride and lithium sulphide

- Draw Lewis diagrams for magnesium chloride
- Draw Lewis diagrams for lithium sulphide
- Share diagrams with peers for review

How do we represent ionic bonding using diagrams?

- 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 - Peer assessment - Individual assessment

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

Inorganic Chemistry

Chemical Bonding - Covalent bonding in diatomic molecules

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

- Written exercises - Peer assessment - Individual assessment

Inorganic Chemistry

Chemical Bonding - Covalent bonding in compounds
Chemical Bonding - Formation of dative (coordinate) bonds

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

- Draw Lewis structures for covalent compounds
- Apply bonding principles to multi-atom molecules
- Relate compound structures to properties of water and carbon dioxide

- Explain how dative covalent bonds form
- Draw structures showing coordinate bonds
- Apply dative bonding to understand ammonium ion formation in fertilisers

- Draw Lewis structures for HF, H₂O, NH₃, CO₂
- Discuss bonding in each compound
- Share diagrams with peers for review

- Discuss formation of dative covalent bonds
- Draw structure of ammonium ion
- Identify donor and acceptor atoms

How do we represent covalent bonding in compounds?
How is a dative bond different from a normal covalent bond?

- Front Row Chemistry Grade 10 pg. 69
- Exercise books
- Molecular diagrams

- Front Row Chemistry Grade 10 pg. 71
- Exercise books
- Diagrams of dative bonding

- Written exercises - Individual assessment - Observation
- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Chemical Bonding - Properties of simple molecular substances
Chemical Bonding - Van der Waals forces and hydrogen bonding

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

- Investigate properties of molecular substances
- Compare melting points of molecular compounds
- Discuss intermolecular forces

Why do molecular substances have low melting points?

- 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

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Structure and properties of diamond

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

- Describe the structure of diamond
- Explain properties of diamond in terms of structure
- Relate diamond's hardness to its use in cutting tools and jewellery

- Understand physical properties of giant covalent structures
- Build models of diamond structure
- Discuss uses of diamond

Why is diamond the hardest naturally occurring substance?

- Front Row Chemistry Grade 10 pg. 76
- Models of diamond structure
- Modelling materials

- Observation - Written exercises - Project work

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

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
Periodicity - Reaction of alkali metals with air/oxygen
Periodicity - Reaction of alkali metals with water

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

- Define ionisation energy
- Explain trends in ionisation energy down Group I
- Relate ionisation energy to reactivity of elements like caesium in atomic clocks

- Observe appearance of freshly cut alkali metals
- Investigate hardness by cutting metals
- Discuss reasons for trends observed

- Investigate ionisation energy of alkali metals
- Discuss factors affecting ionisation energy
- Explain trend using shielding effect

Why are alkali metals soft and shiny when freshly cut?
Why does ionisation energy decrease down Group I?

- 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
- 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

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

Inorganic Chemistry

Periodicity - Reaction of alkali metals with chlorine and dilute acids
Periodicity - Applications of alkali metals

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

- Describe reactions of alkali metals with chlorine
- Explain reactions with dilute acids
- Relate sodium chloride formation to table salt production

- Investigate reaction of sodium with chlorine
- Discuss reactions with dilute acids (video)
- Write balanced equations

Why are reactions of alkali metals with acids dangerous?

- Front Row Chemistry Grade 10 pg. 94
- Gas jar of chlorine
- Deflagrating spoon
- Digital devices
- Front Row Chemistry Grade 10 pg. 96
- Digital devices
- Pictures of applications

- Written exercises - Observation - Oral questions

Inorganic Chemistry

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:

- Describe trends in atomic and ionic radii of Group II elements
- Compare trends with Group I
- Relate atomic size to reactivity of calcium in bone formation

- Observe trends in atomic and ionic radii
- Complete tables showing radii data
- Compare with Group I trends

How do atomic sizes of Group II elements compare with Group I?

- 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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Periodicity - Physical properties of alkaline earth metals (melting points and ionisation energy)

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

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Reaction of alkaline earth metals with air/oxygen
Periodicity - Reaction of alkaline earth metals with water and steam

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

- Investigate reactions of Group II metals with oxygen
- Write balanced equations for the reactions
- Relate magnesium burning to its use in flares and fireworks

- Investigate reactions with water and steam
- Compare reactivity of magnesium and calcium
- Relate calcium hydroxide formation to lime water used in construction

- Burn magnesium and calcium in air
- Observe products formed
- Write word and chemical equations

- React magnesium and calcium with cold water
- React magnesium with steam
- Test gas produced and write equations

What products form when alkaline earth metals burn in air?
Why does magnesium react slowly with cold water but vigorously with steam?

- Front Row Chemistry Grade 10 pg. 106
- Magnesium ribbon
- Calcium metal
- Bunsen burner

- Front Row Chemistry Grade 10 pg. 107
- Magnesium, calcium
- Trough
- Steam apparatus

- Practical assessment - Written exercises - Observation

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

Inorganic Chemistry

Periodicity - Introduction to halogens

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

- Determine chemical family of chlorine and fluorine
- Write electron configurations
- List other halogens

Why are halogens called "salt formers"?

- Front Row Chemistry Grade 10 pg. 114
- Periodic table
- Digital devices

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Periodicity - Laboratory preparation of chlorine gas

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

- Prepare chlorine gas in the laboratory
- Describe properties of chlorine gas
- Relate chlorine properties to its use in bleach and water purification

- Prepare chlorine gas from HCl and MnO₂
- Collect chlorine gas
- Observe properties of chlorine

How is chlorine gas prepared and collected safely?

- Front Row Chemistry Grade 10 pg. 115
- MnO₂, conc. HCl
- Round bottomed flask
- Gas jars

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Trends in physical properties of halogens (atomic radii, melting and boiling points)
Periodicity - Appearance, physical state and solubility of halogens
Periodicity - Electrical conductivity of halogens

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

- Describe trends in atomic radii of halogens
- Explain trends in melting and boiling points
- Relate physical state changes to molecular size and intermolecular forces

- 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

- Review atomic structure of halogens
- Study trends in physical properties
- Explain trends using intermolecular forces

- Observe appearance of chlorine, bromine and iodine
- Test solubility in water
- Compare solubility of halogens

Why do halogens change from gas to solid down the group?
Why do halogens have different colours and physical states?

- Front Row Chemistry Grade 10 pg. 117
- Data tables
- Periodic table
- Front Row Chemistry Grade 10 pg. 118
- Bromine, iodine samples
- Distilled water
- Test tubes
- Front Row Chemistry Grade 10 pg. 120
- Iodine crystals
- Circuit with bulb
- Beaker

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

Inorganic Chemistry

Periodicity - Electron affinity and ion formation of halogens

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

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Reaction of halogens with metals

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

- Investigate reactions of halogens with metals
- Write balanced equations for the reactions
- Relate iron chloride formation to industrial rust prevention

- React chlorine with iron and zinc
- Observe products formed
- Write balanced equations

What happens when halogens react with metals?

- Front Row Chemistry Grade 10 pg. 122
- Iron filings
- Chlorine gas
- Combustion tube

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of chlorine with water

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

- Prepare chlorine water
- Test with litmus paper
- Investigate decomposition in sunlight

How does chlorine react with water and why is it used as a bleach?

- Front Row Chemistry Grade 10 pg. 124
- Chlorine gas
- Distilled water
- Litmus paper

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Displacement reactions of halogens
Periodicity - Applications of halogens
Periodicity - Introduction to noble gases

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

- Investigate displacement reactions of halogens
- Explain order of reactivity of halogens
- Apply displacement reactions to understand water purification processes

- 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

- Add chlorine water to potassium bromide and iodide solutions
- Observe colour changes
- Write ionic equations

- Determine electronic configuration of noble gases
- Discuss stability of full electron shells
- List noble gas elements

Why can chlorine displace bromine and iodine from their salts?
Why are noble gases unreactive?

- 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

- Front Row Chemistry Grade 10 pg. 128
- Periodic table
- Digital devices

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

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

Inorganic Chemistry

Periodicity - Applications of noble gases

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

- Oral questions - Written exercises - Group presentations

Inorganic Chemistry

Periodicity - Introduction to Period 3 elements

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

- Identify Period 3 elements and their properties
- Classify elements as metals, metalloids or non-metals
- Relate Period 3 elements to common materials like aluminium foil and silicon chips

- List Period 3 elements from Na to Ar
- Discuss bonding and structure of each element
- Classify elements by type

What elements are found in Period 3 and how do their properties vary?

- Front Row Chemistry Grade 10 pg. 131
- Periodic table
- Element samples

- Oral questions - Written exercises - Observation

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 melting and boiling points across Period 3
- Explain trends using structure and bonding
- Relate silicon's high melting point to its use in computer chips

- Study data on atomic radii of Period 3 elements
- Plot graph of atomic radius vs atomic number
- Explain trend using nuclear charge

- Study data on melting and boiling points
- Relate trends to bonding and structure
- Explain anomalies

Why does atomic radius decrease across Period 3?
Why does silicon have the highest melting point in Period 3?

- Front Row Chemistry Grade 10 pg. 132
- Data tables
- Graph paper
- Front Row Chemistry Grade 10 pg. 133
- Digital devices

- Front Row Chemistry Grade 10 pg. 134
- Data tables
- Charts

- Written exercises - Graphical work - Oral questions
- Written exercises - Oral questions - Observation

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

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with oxygen (Na, Mg, Al)

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

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with oxygen (Si, P, S)
Periodicity - Reaction of Period 3 elements with chlorine (Na, Mg, Al)

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

- Describe reactions of Si, P and S with oxygen
- Write balanced equations for the reactions
- Relate sulphur dioxide formation to air pollution and acid rain

- Discuss reactions of silicon and phosphorus with oxygen
- Burn sulphur in oxygen
- Write balanced equations

What products form when Period 3 non-metals burn in oxygen?

- Front Row Chemistry Grade 10 pg. 136
- Sulphur powder
- Gas jar of oxygen
- Deflagrating spoon
- Front Row Chemistry Grade 10 pg. 137
- Na, Mg samples
- Chlorine gas

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with chlorine (Si, P)
Periodicity - Reaction of Period 3 elements with water (Na, Mg)

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

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

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with dilute acids

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

- Investigate reactions of Period 3 metals with dilute acids
- Write balanced equations for the reactions
- Relate hydrogen gas production to laboratory gas collection techniques

- React magnesium and aluminium with dilute HCl and H₂SO₄
- Test gas produced
- Write balanced equations

What products form when Period 3 metals react with dilute acids?

- Front Row Chemistry Grade 10 pg. 139
- Mg ribbon
- Dilute HCl, H₂SO₄
- Test tubes

- Practical assessment - Written exercises - Observation

Inorganic Chemistry
Physical Chemistry
Physical Chemistry

Periodicity - Comparison of trends across Period 3 and down groups
Acids and Bases - Dissociation of acids in water
Acids and Bases - Dissociation of bases in water

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

- Compare periodic trends across periods and down groups
- Summarise factors affecting periodic properties
- Apply periodic trends to predict element behaviour in new materials

- Compare trends across Period 3 with trends down groups
- Create summary tables of periodic trends
- Discuss patterns and exceptions

How do trends across a period differ from trends down a group?

- Front Row Chemistry Grade 10 pg. 141
- Summary charts
- Periodic table
- Front Row Chemistry Learner's Book pg. 143
- Distilled water
- Hydrochloric acid
- Blue and red litmus papers
- Beakers
- Stirring rod
- Sodium hydroxide
- Measuring cylinder

- Written exercises - Oral questions - Individual assessment

Physical Chemistry

Acids and Bases - Reaction of acids with metals
Acids and Bases - Reaction of acids with metals (continued)

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

- Describe the reaction between acids and metals
- Test for hydrogen gas produced during the reaction
- Connect the corrosion of metal roofs by acid rain to acid-metal reactions

- Carry out experiments on reactions between dilute acids and metals (zinc, magnesium, iron)
- Test for hydrogen gas using a burning splint
- Write balanced chemical equations for the reactions

What gas is produced when metals react with acids?

- Front Row Chemistry Learner's Book pg. 144
- Zinc granules
- Magnesium ribbon
- Iron filings
- Dilute HCl and H₂SO₄
- Test tubes
- Wooden splints
- Front Row Chemistry Learner's Book pg. 146
- Aluminium foil
- Copper turnings
- Dilute HCl
- Dilute H₂SO₄
- Test tubes

- Practical assessment - Written equations - Oral questions

Physical Chemistry

Acids and Bases - Reaction of acids with carbonates and hydrogen carbonates
Acids and Bases - Reaction of acids with hydrogen carbonates
Acids and Bases - Reaction of acids with metal hydroxides
Acids and Bases - Reaction of acids with metal oxides
Acids and Bases - Amphoteric oxides and hydroxides
Acids and Bases - Universal indicator and pH scale

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

- Describe reactions between acids and carbonates
- Test for carbon (IV) oxide gas produced
- Connect the effervescence of antacid tablets in water to carbonate-acid reactions

- Explain reactions between acids and insoluble metal oxides
- Write balanced chemical equations for acid-metal oxide reactions
- Relate the cleaning of rusted surfaces using acids to acid-metal oxide reactions

- Carry out experiments on reactions of acids with sodium carbonate and calcium carbonate
- Pass gas produced through lime water
- Write balanced chemical equations for the reactions
- Carry out experiments on reactions of dilute acids with zinc oxide and copper (II) oxide
- Filter the mixture and test pH of filtrate
- Discuss why excess metal oxide is added

How can you confirm the presence of carbon (IV) oxide gas?
How do acids react with metal oxides?

- Front Row Chemistry Learner's Book pg. 147
- Sodium carbonate
- Calcium carbonate
- Dilute HCl
- Lime water
- Delivery tubes
- Test tubes
- Sodium hydrogen carbonate
- Test tubes
- Delivery tubes
- Front Row Chemistry Learner's Book pg. 148
- Sodium hydroxide
- Phenolphthalein indicator
- Droppers
- Beakers
- Stirring rod
- Front Row Chemistry Learner's Book pg. 150
- Zinc oxide
- Copper (II) oxide
- Dilute HCl
- Universal indicator
- Filter funnel and paper
- Front Row Chemistry Learner's Book pg. 151
- Sodium hydroxide
- Test tubes
- Spatula
- Front Row Chemistry Learner's Book pg. 152
- pH chart
- Sulphuric (VI) acid
- Ethanoic acid
- Test tubes

- Practical assessment - Written equations - Oral questions
- Observation - Written tests - Practical assessment