Inorganic Chemistry

Relative Atomic Mass - Atomic number and mass number
Relative Atomic Mass - Meaning of isotopes

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 an atom
- Use atomic notation to represent atoms of different elements

- Discuss with peers the relationship between atomic number, mass number and number of electrons
- Calculate the number of subatomic particles in given atoms
- Practise writing atomic notation for elements

What is the relationship between atomic number, mass number and number of neutrons?

- Access and Learn Chemistry Learner's Book pg. 24
- Periodic table
- Digital devices
- Digital devices
- Charts showing isotopes

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Relative Atomic Mass - Meaning and calculation
Relative Atomic Mass - Calculations from isotopic abundances I
Relative Atomic Mass - Calculations from isotopic abundances II

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

- Define Relative Atomic Mass (R.A.M)
- Explain the concept of isotopic abundance
- Connect R.A.M to the values shown on the periodic table

- Search for information on Relative Atomic Mass
- Discuss with peers the meaning of isotopic abundance
- Study the relationship between R.A.M and isotopes

What is Relative Atomic Mass and why is it not always a whole number?

- Access and Learn Chemistry Learner's Book pg. 27
- Digital devices
- Periodic table
- Scientific calculators
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 28

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Relative Atomic Mass - Determining relative abundance
Relative Atomic Mass - Practical activity with dice

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

- Calculate relative abundance of isotopes given R.A.M
- Solve reverse problems on isotopic abundances
- Apply mathematical skills to determine isotope compositions

- Study worked examples on determining relative abundance
- Calculate relative abundances from given R.A.M values
- Practise solving reverse problems

How can you determine the relative abundance of isotopes if you know the R.A.M?

- Access and Learn Chemistry Learner's Book pg. 29
- Scientific calculators
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 30
- Coloured dice
- Flashcards

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Electron arrangement - Energy levels and sub-levels
Electron arrangement - Types of orbitals
Electron arrangement - Aufbau's principle
Electron arrangement - Writing s and p notation I

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

- Define energy levels and sub-levels in an atom
- Identify the sub-levels present in the first four energy levels
- Relate energy levels to the floors of a building and sub-levels to apartments

- State the Aufbau's principle
- Apply the order of filling electrons in orbitals
- Compare electron filling to constructing a building from the foundation upwards

- Discuss the relationship between energy levels and orbitals
- Study the sub-levels for the first four energy levels
- Create a table showing energy levels and their sub-levels

- Search for information on Aufbau's principle
- Study the diagram showing order of filling electrons
- Discuss with peers how electrons fill orbitals

How are electrons organized within energy levels?
In what order do electrons fill the orbitals in an atom?

- Access and Learn Chemistry Learner's Book pg. 32
- Digital devices
- Charts showing energy levels
- Access and Learn Chemistry Learner's Book pg. 34
- Charts showing orbital shapes
- Access and Learn Chemistry Learner's Book pg. 36
- Digital devices
- Aufbau diagram
- Access and Learn Chemistry Learner's Book pg. 38
- Periodic table
- Digital devices

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Electron arrangement - Writing s and p notation II
Electron arrangement - Practical activity

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

- Write electron arrangement of elements 11-20 using s and p notation
- Complete the electron arrangement table for the first 20 elements
- Connect electron arrangements to the position of elements in the periodic table

- Copy and complete the table of electron arrangements for the first 20 elements
- Compare electron arrangements with classmates
- Identify patterns in electron arrangements

What patterns can you observe in the electron arrangements of the first 20 elements?

- Access and Learn Chemistry Learner's Book pg. 39
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 40
- Plastic beakers
- Beads or pebbles
- Labels

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Historical development of the periodic table I
Historical development of the periodic table II
Groups and periods I
Groups and periods II

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

- Describe the early attempts to classify elements
- Explain the law of triads and law of octaves
- Trace the evolution of element classification from ancient times

- Brainstorm in groups on the historical development of the periodic table
- Watch a video on the history of the periodic table
- Study the timeline of periodic table development

How did scientists first attempt to organize the elements?

- Access and Learn Chemistry Learner's Book pg. 45
- Digital devices
- Timeline charts
- Access and Learn Chemistry Learner's Book pg. 46
- Periodic table charts
- Access and Learn Chemistry Learner's Book pg. 49
- Periodic table
- Digital devices

- Oral questions - Group discussions - Written exercises

Inorganic Chemistry

Position of an element and electron arrangement
Chemical families - Alkali metals and Alkaline earth metals
Chemical families - Halogens and Noble gases
Transition elements
Stability of atoms
Cations and anions

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

- Relate the position of an element to its electron arrangement
- Determine group number from valence electrons
- Determine period number from number of energy levels

- Explain the stability of noble gas atoms
- Describe how atoms gain stability through electron loss or gain
- Relate atomic stability to the octet rule and full outer shells

- Create element cards showing electron arrangements
- Place element cards in correct positions on a periodic table template
- Discuss how electron arrangement relates to group and period

- Draw atomic structures of helium, neon and argon
- Discuss with peers the meaning of stability of an atom
- Identify what makes noble gases stable

How can you predict an element's position in the periodic table from its electron arrangement?
Why are noble gases stable?

- Access and Learn Chemistry Learner's Book pg. 51
- Manila paper
- Graph paper
- Scissors
- Access and Learn Chemistry Learner's Book pg. 53
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 54
- Coloured pencils
- Access and Learn Chemistry Learner's Book pg. 55
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 56
- Digital devices
- Charts showing ion formation

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

Inorganic Chemistry

Valency and oxidation number I
Valency and oxidation number II

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

- Define valency and oxidation number
- Determine valency from electron arrangement
- Differentiate between valency and oxidation number

- Discuss with peers the meaning of valency and oxidation number
- Determine valency of elements from their electron arrangements
- Compare valency and oxidation number of elements

What is the difference between valency and oxidation number?

- Access and Learn Chemistry Learner's Book pg. 58
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 59

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Radicals
Electron arrangement of ions using s and p notation

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

- Define radicals in chemistry
- Identify common radicals and their valencies
- Apply knowledge of radicals in writing chemical formulae

- Discuss with peers the meaning of radicals
- Complete the table of radicals and their valencies
- Identify radicals in common compounds

What are radicals and how are they used in Chemistry?

- Access and Learn Chemistry Learner's Book pg. 60
- Charts showing radicals
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 62
- Periodic table

- Oral questions - Written exercises - Observation

Inorganic Chemistry

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

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

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

- Identify reactants and products in a chemical reaction
- Write word equations for chemical reactions
- Convert word equations to chemical equations

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

- Read information on parts of a chemical equation
- Identify reactants and products in given reactions
- Write word equations for simple chemical reactions

How do you write the formula of a compound?
What are the parts of a chemical equation?

- Access and Learn Chemistry Learner's Book pg. 63
- Valency tables
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 64
- Access and Learn Chemistry Learner's Book pg. 64
- Digital devices
- Charts showing chemical equations
- Access and Learn Chemistry Learner's Book pg. 65
- Practice worksheets

- Written exercises - Oral questions - Observation
- Oral questions - Written exercises - Observation

Inorganic Chemistry

Writing balanced chemical equations III
Role of electron arrangement in the periodic table - Project
Chemical Bonding - Role of valence electrons in bonding

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

- Write balanced equations for reactions of acids with metals
- Write balanced equations for reactions of acids with carbonates
- Apply balancing skills to more complex reactions

- Write balanced equations for reactions involving acids
- Practise writing equations for reactions with carbonates
- Compare equations with classmates for peer learning

How do you write balanced equations for reactions involving acids?

- Access and Learn Chemistry Learner's Book pg. 66
- Digital devices
- Practice worksheets
- 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
- Modelling clay or plasticine
- Wooden splints

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Types of chemical bonds
Chemical Bonding - The ionic chemical bond
Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide
Chemical Bonding - Giant ionic structures and lattice

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

- Identify different types of chemical bonds
- Distinguish between ionic, covalent and metallic bonds
- Connect different bond types to substances used in daily life like salt and water

- Discuss with peers different types of chemical bonds (ionic, covalent, dative covalent, hydrogen bond, Van der Waals forces and metallic)
- Use models to represent different bond types
- Search for information using digital resources on bond types

What determines the type of bond formed between atoms?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Digital devices
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Periodic table
- Access & Learn Chemistry Learner's Book Grade 10 pg. 76
- Modelling materials (clay, toothpicks)
- Charts of ionic lattices

- Oral questions - Group discussions - Written assignments

Inorganic Chemistry

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

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

- Investigate the solubility of ionic compounds
- Explain why ionic compounds dissolve in water
- Apply knowledge of solubility to dissolving salt in cooking

- Describe the formation of covalent bonds
- Illustrate single covalent bonds using dot and cross diagrams
- Connect covalent bonding to common molecules like water and oxygen

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

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

Why do ionic compounds dissolve in water but not in organic solvents?
How do non-metal atoms bond with each other?

- 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
- 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

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

Inorganic Chemistry

Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride
Chemical Bonding - Dative covalent (coordinate) bonding

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

- Illustrate covalent bonding in ammonia and hydrogen chloride molecules
- Identify lone pairs of electrons in molecules
- Connect molecular compounds to household chemicals like cleaning ammonia

- Draw dot (.) and cross (x) structures for ammonia and hydrogen chloride
- Identify shared pairs and lone pairs in molecules
- Discuss the shape of ammonia molecule

What is the role of lone pairs in covalent molecules?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 84
- Charts showing molecular structures
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 85
- Charts showing dative bonds

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Hydrogen bonding and Van der Waals forces
Chemical Bonding - Melting, boiling points and conductivity of molecular substances

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

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

- Discuss types of intermolecular forces using print or digital materials
- Illustrate hydrogen bonding in water molecules using models
- Draw diagrams showing Van der Waals forces

Why does water have a relatively high boiling point compared to other small molecules?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 86
- Modelling materials
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 89
- Naphthalene
- Thermometer
- Bunsen burner
- Melting point tube

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Solubility and uses of molecular substances
Chemical Bonding - Giant atomic structure of diamond
Chemical Bonding - Giant atomic structure of graphite
Chemical Bonding - Uses of diamond, graphite and silicon (IV) oxide

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

- Investigate solubility of molecular substances
- Relate uses of molecular substances to their properties
- Identify molecular substances in products like fuels and medicines

- Describe the layered structure of graphite
- Model the structure of graphite using locally available materials
- Relate graphite structure to its use in pencils and lubricants

- Carry out experiments to investigate solubility of sulphur and sugar in water and ethanol
- Discuss uses of molecular substances related to their properties
- Search for information on applications of molecular compounds

- Discuss the hexagonal layered structure of graphite
- Model a graphite structure showing layers
- Explain why graphite conducts electricity while diamond does not

Why do some molecular substances dissolve in organic solvents but not in water?
Why can graphite conduct electricity while diamond cannot?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol
- 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
- Modelling clay
- Toothpicks
- Charts of graphite structure
- Access & Learn Chemistry Learner's Book Grade 10 pg. 96
- Digital devices
- Charts showing applications

- Practical report - Written assignments - Oral questions
- Model assessment - Written exercises - Group discussions

Inorganic Chemistry

Chemical Bonding - Metallic bonding and delocalised electrons
Chemical Bonding - Physical properties of giant metallic structures

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

- Describe the formation of metallic bonds
- Illustrate the sea of delocalised electrons model
- Relate metallic bonding to properties of metals used in wiring and construction

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

Why are metals good conductors of electricity and heat?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 97
- Charts showing metallic bonding
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 99
- Metal and wood pieces

- Written exercises - Oral questions - Observation

Inorganic Chemistry

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 metallic structures
- Relate uses of metals to their bond type and properties
- Identify applications of metals in vehicles, buildings and electronics

- Search for information on uses of metallic structures
- Complete a table relating substances, bond types, properties and uses
- Discuss uses of copper, aluminium and iron in daily life

How does metallic bonding make metals suitable for electrical wiring?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 101
- Digital devices
- Samples of metal products
- Access & Learn Chemistry Learner's Book Grade 10 pg. 104
- Periodic table charts
- Digital devices
- 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
Periodicity - Ionisation energy and electronegativity of group I elements
Periodicity - Melting, boiling points and electrical conductivity of group I elements
Periodicity - Reactions of group I elements with oxygen
Periodicity - Reactions of group I elements with chlorine and cold water
Periodicity - Applications of group I elements
Periodicity - Appearance, atomic and ionic radii of group II elements

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

- 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

- 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

- 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

- 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 is the ionic radius of sodium smaller than its atomic radius?
Why does sodium react more vigorously with water than lithium?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 107
- Periodic table
- Graph paper
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 108
- Data tables
- Access & Learn Chemistry Learner's Book Grade 10 pg. 110
- Connecting wires
- Dry cells
- Bulb
- Sodium metal
- Lithium metal
- Access & Learn Chemistry Learner's Book Grade 10 pg. 112
- Gas jar of oxygen
- Deflagrating spoon
- Bunsen burner
- Lithium and sodium metals
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 114
- Chlorine gas
- Cold water
- Beakers
- Lithium and sodium metals
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 117
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

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

Inorganic Chemistry

Periodicity - Ionisation energy, melting and boiling points of group II elements
Periodicity - Reactions of group II elements with water, steam and oxygen

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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 123
- Magnesium ribbon
- Calcium metal
- Gas jar of oxygen
- Bunsen burner
- Litmus paper

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group II elements with dilute acids and chlorine
Periodicity - Applications of group II elements

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

- Investigate reactions of group II elements with dilute acids and chlorine
- Write balanced equations for the reactions
- Relate reactions to production of hydrogen gas for industrial uses

- Investigate reactions of magnesium and calcium with dilute HCl, dilute H₂SO₄ and dilute HNO₃
- Test gases produced with burning splint
- Investigate reactions with chlorine gas
- Write chemical equations for all reactions

Why does the reaction of calcium with dilute sulphuric acid stop quickly?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 127
- Dilute acids
- Magnesium ribbon
- Calcium metal
- Chlorine gas
- Test tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 129
- Digital devices
- Reference materials

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Preparation of chlorine and physical properties of group VII elements
Periodicity - Melting, boiling points and gradation in size of group VII elements
Periodicity - Reactions of group VII elements with water and metals
Periodicity - Displacement reactions and bleaching action of chlorine

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

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

- Investigate reactions of halogens with water and metals
- Write balanced equations for the reactions
- Relate halogen reactivity to their use in antiseptics and disinfectants

- Set up apparatus to prepare chlorine gas from concentrated HCl and potassium manganate (VII)
- Observe colour, smell and solubility of chlorine
- Compare physical properties of fluorine, chlorine, bromine and iodine

- Bubble chlorine gas into distilled water and test with litmus paper
- Add bromine and iodine to water and observe
- Pass chlorine gas over heated iron wool
- Write chemical equations for reactions

Why is chlorine collected by downward delivery?
Why does chlorine turn moist blue litmus paper red and then white?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 131
- Concentrated HCl
- Potassium manganate (VII)
- Gas jars
- Delivery tubes
- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 142
- Potassium bromide solution
- Potassium iodide solution
- Coloured cloth
- Flower petals

- Practical report - Observation - Written exercises
- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group VII elements
Periodicity - Physical properties and applications of noble gases

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

- Outline applications of group VII elements
- Relate properties to specific uses
- Identify uses in water treatment, photography, medicine and refrigeration

- Search for information on applications of halogens
- Discuss uses of chlorine in water treatment, bromine in photography, iodine in medicine
- Create presentations on halogen applications

How is chlorine used to make drinking water safe?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 147
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 148
- Periodic table

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Atomic size, ionisation energy and electronegativity across period 3
Periodicity - Reactions of period 3 elements with oxygen and water

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

- Describe trends in atomic size and ionisation energy across period 3
- Plot graphs showing trends across the period
- Relate effective nuclear charge to changes in atomic properties

- Draw atomic structures of period 3 elements
- Analyse data on atomic radii and ionisation energies
- Plot graphs of ionisation energy against atomic number
- Discuss the role of effective nuclear charge

Why does atomic radius decrease across period 3?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Periodic table
- Data tables
- Access & Learn Chemistry Learner's Book Grade 10 pg. 155
- Sodium, magnesium, sulphur
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Distilled water

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry
Physical Chemistry
Physical Chemistry
Physical Chemistry

Periodicity - Reactions of period 3 elements with chlorine and dilute acids
Acids and Bases - Dissociation of acids in aqueous solutions
Acids and Bases - Dissociation of bases in aqueous solutions
Acids and Bases - Properties of acids
Acids and Bases - Properties of bases
Acids and Bases - Reaction of dilute acids with metals
Acids and Bases - Confirmatory test for hydrogen gas
Acids and Bases - Reaction of acids with carbonates

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

- Investigate reactions of period 3 elements with chlorine and dilute acids
- Write balanced equations for the reactions
- Connect periodic trends to prediction of element behaviour in chemical reactions

- Describe the physical properties of bases
- Differentiate between bases and alkalis
- Connect properties of bases to cleaning agents and antacids used at home

- Pass chlorine gas over heated sodium and magnesium
- Investigate reactions of magnesium with dilute HCl, dilute H₂SO₄ and dilute HNO₃
- Test gases produced
- Write chemical equations for all reactions
- Summarise trends in chemical properties across period 3

- Carry out experiments to investigate properties of bases
- Test bases using litmus paper and phenolphthalein indicator
- Discuss with peers the slippery feel and bitter taste of bases

How do the chemical properties of elements change across period 3?
What common household substances are basic in nature?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner
- Access & Learn Chemistry Learner's Book Grade 10 pg. 164
- Dilute hydrochloric acid
- pH indicator paper
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 166
- Sodium hydroxide solution
- Phenolphthalein indicator
- Red and blue litmus paper
- Test tubes
- Chemistry Learner's Book Grade 10 pg. 166
- Samples of acids
- Blue litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 167
- Sodium hydroxide solution
- Baking soda
- Soap solution
- Red litmus paper
- Phenolphthalein
- Access & Learn Chemistry Learner's Book Grade 10 pg. 169
- Zinc powder
- Dilute hydrochloric acid
- Test tubes
- Wooden splints
- Rubber corks
- Access & Learn Chemistry Learner's Book Grade 10 pg. 170
- Dilute sulphuric acid
- Magnesium ribbon
- Delivery tubes
- Chemistry Learner's Book Grade 10 pg. 170
- Sodium carbonate
- Calcium hydroxide
- Delivery tubes
- Test tubes

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

Physical Chemistry

Acids and Bases - Reaction of acids with hydrogen carbonates
Acids and Bases - Reaction of acids with metal oxides
Acids and Bases - Reaction of acids with metal hydroxides

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

- Describe reactions of acids with hydrogen carbonates
- Perform the confirmatory test for carbon (IV) oxide
- Connect the reaction to baking powder action in bread and cakes

- Add dilute nitric (V) acid to sodium hydrogen carbonate
- Collect and test gas produced using limewater
- Observe white precipitate formation
- Write balanced equations for the reactions

How is carbon (IV) oxide gas tested in the laboratory?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 171
- Sodium hydrogen carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Test tubes
- Delivery tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 172
- Magnesium oxide
- pH paper
- Beakers
- Bunsen burner
- Access & Learn Chemistry Learner's Book Grade 10 pg. 173
- Sodium hydroxide solution
- Dilute sulphuric (VI) acid
- Phenolphthalein indicator
- Measuring cylinders

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Universal indicator and pH scale
Acids and Bases - Strong and weak acids

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

- Explain the pH scale and its use
- Determine pH values using universal indicator
- Relate pH values to water quality testing and swimming pool maintenance

- Prepare solutions of various acids and bases
- Add universal indicator to each solution
- Compare colours with pH scale chart
- Record pH values and classify solutions

What does the pH scale measure?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 175
- Universal indicator
- pH scale chart
- Various acid and base solutions
- Test tubes
- Droppers
- Chemistry Learner's Book Grade 10 pg. 175
- 0.1 M hydrochloric acid
- 0.1 M ethanoic acid
- Test tubes

- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Strong and weak bases
Acids and Bases - Electrical conductivity of acids and bases
Acids and Bases - Uses of acids in day-to-day life
Acids and Bases - Uses of bases in day-to-day life

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

- Differentiate between strong and weak bases
- Classify bases based on their pH values
- Relate base strength to drain cleaners (strong) versus baking soda (weak)

- Outline the uses of acids in various sectors
- Search for information on industrial applications of acids
- Relate acids to food preservation, fertiliser production and metal cleaning

- Test 0.1 M sodium hydroxide and 0.1 M ammonium hydroxide using universal indicator
- Compare pH values of strong and weak bases
- Discuss characteristics of strong and weak bases

- Search for information on uses of acids using print or digital materials
- Discuss uses in food industry, manufacturing and cleaning
- Prepare charts showing applications of acids

How can strong and weak bases be distinguished?
How are acids useful in our daily lives?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 176
- 0.1 M sodium hydroxide
- 0.1 M ammonium hydroxide
- Universal indicator
- pH scale chart
- Test tubes
- Chemistry Learner's Book Grade 10 pg. 176
- Dry cells
- Bulbs with holders
- Connecting wires
- Nails/electrodes
- Various acid and base solutions
- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers
- Access & Learn Chemistry Learner's Book Grade 10 pg. 179
- Soil samples
- pH paper
- Litmus paper
- Vinegar
- Citrus peels
- Digital resources

- Practical assessment - Observation - Written assignments
- Oral questions - Written assignments - Project assessment

Physical Chemistry

Introduction to Salts - Meaning and formation of salts
Introduction to Salts - Normal salts
Introduction to Salts - Acid salts
Introduction to Salts - Basic and double salts

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

- Define the term salt
- Explain how salts are formed from neutralisation reactions
- Relate salt formation to table salt production and food seasoning

- Study equations showing neutralisation reactions
- Identify reactants and products in salt formation
- Discuss how hydrogen ions in acids are replaced by metal ions
- Examine samples of different salts

What is a salt and how is it formed?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 181
- Samples of salts (sodium chloride, copper sulphate)
- Charts showing neutralisation equations
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 182
- Samples of normal salts
- Litmus paper
- Test tubes
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 183
- Sodium hydrogen carbonate
- pH paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 184
- Samples of basic and double salts
- Potassium aluminium sulphate (alum)
- pH paper

- Oral questions - Written exercises - Observation

Physical Chemistry

Introduction to Salts - Soluble and insoluble salts
Introduction to Salts - Solubility rules
Introduction to Salts - Preparation by direct synthesis
Introduction to Salts - Preparation using acid and metal

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

- Define soluble and insoluble salts
- Carry out experiments to determine solubility of salts
- Relate solubility to water treatment and removal of hardness in water

- Place spatulaful of different salts in beakers with distilled water
- Stir and observe dissolution
- Warm mixtures and observe changes
- Record observations and classify salts as soluble or insoluble

How can soluble salts be distinguished from insoluble salts?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 185
- Copper (II) sulphate
- Copper (II) carbonate
- Distilled water
- Beakers
- Bunsen burner
- Chemistry Learner's Book Grade 10 pg. 185
- Solubility table charts
- Various salt samples
- Test tubes
- Digital resources
- Access & Learn Chemistry Learner's Book Grade 10 pg. 186
- Copper metal
- Sulphur powder
- Crucible
- Bunsen burner
- Tripod stand
- Access & Learn Chemistry Learner's Book Grade 10 pg. 187
- Zinc powder
- Dilute hydrochloric acid
- Filter funnel and paper
- Evaporating dish

- Practical assessment - Observation - Written exercises

Physical Chemistry

Introduction to Salts - Preparation using acid and metal oxide
Introduction to Salts - Preparation using acid and alkali (titration)
Introduction to Salts - Preparation using acid and carbonate
Introduction to Salts - Preparation by precipitation (double decomposition)
Introduction to Salts - Hygroscopic, deliquescent and efflorescent salts
Introduction to Salts - Uses of salts and environmental impact of fertilisers

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

- Describe preparation of salts using acid and metal oxide
- Prepare copper (II) nitrate from copper oxide and nitric acid
- Relate this neutralisation method to pharmaceutical salt production

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

- Warm dilute nitric (V) acid and add copper (II) oxide in excess
- Filter to remove unreacted oxide
- Evaporate filtrate to saturation
- Allow to cool and crystallise

- Add sodium carbonate to dilute nitric (V) acid until no more gas bubbles
- Test gas with calcium hydroxide
- Filter, evaporate and crystallise
- Write balanced equation for the reaction

What is the role of warming the acid in salt preparation?
How can you tell when the reaction between acid and carbonate is complete?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 188
- Copper (II) oxide
- Dilute nitric (V) acid
- Filter funnel and paper
- Evaporating dish
- Beakers
- Access & Learn Chemistry Learner's Book Grade 10 pg. 190
- Sodium hydroxide solution
- Dilute hydrochloric acid
- Phenolphthalein
- Burette and stand
- Conical flask
- Access & Learn Chemistry Learner's Book Grade 10 pg. 191
- Sodium carbonate
- Dilute nitric (V) acid
- Calcium hydroxide
- Filter funnel
- Evaporating dish
- Access & Learn Chemistry Learner's Book Grade 10 pg. 193
- Zinc sulphate solution
- Lead nitrate solution
- Filter funnel and paper
- Beakers
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 196
- Iron (III) chloride
- Anhydrous copper (II) sulphate
- Sodium carbonate decahydrate
- Watch glasses
- Access & Learn Chemistry Learner's Book Grade 10 pg. 197
- Samples of inorganic fertilisers
- Digital devices
- Reference books
- Charts on eutrophication

- Practical assessment - Observation - Written exercises
- Practical assessment - Observation - Written assignments