Inorganic Chemistry

Historical development of the periodic table I
Historical development of the periodic table II
Groups and periods I
Groups and periods II
Position of an element and electron arrangement
Chemical families - Alkali metals and Alkaline earth metals

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
- Define groups and periods in the periodic table
- Identify the number of groups and periods in the modern periodic table
- Relate groups to vertical columns and periods to horizontal rows

- 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
- Study the modern periodic table
- Discuss with peers the meaning of groups and periods
- Identify groups and periods in the periodic table

How did scientists first attempt to organize the elements?
What are groups and periods in the periodic table?

- 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
- Access and Learn Chemistry Learner's Book pg. 51
- Manila paper
- Graph paper
- Scissors
- Access and Learn Chemistry Learner's Book pg. 53

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

Inorganic Chemistry

Chemical families - Halogens and Noble gases
Transition elements
Stability of atoms

By the end of the lesson, the learner should be able to:
- Identify members of halogens and noble gases
- Describe common features of Group VII and Group VIII elements
- Connect halogens to uses like chlorine in water treatment and noble gases in lighting

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

Why are noble gases called inert gases?

- 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

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Cations and anions
Valency and oxidation number I

By the end of the lesson, the learner should be able to:
- Define cations and anions
- Predict the type of ion formed from electron arrangement
- Draw ion formation using dot and cross diagrams

- Study diagrams showing ion formation
- Draw ion formation of metals and non-metals using dot and cross structures
- Discuss with peers the difference between cations and anions

How do atoms form ions?

- Access and Learn Chemistry Learner's Book pg. 56
- Digital devices
- Charts showing ion formation
- Access and Learn Chemistry Learner's Book pg. 58
- Periodic table
- Digital devices

- Oral questions - Written exercises - Practical drawings

Inorganic Chemistry

Valency and oxidation number II
Radicals

By the end of the lesson, the learner should be able to:
- Identify elements with variable oxidation numbers
- Write oxidation numbers of transition elements
- Apply Roman numerals to represent variable oxidation states

- Discuss with peers elements with variable oxidation numbers
- Complete the table of oxidation numbers for transition elements
- Practise writing oxidation numbers using Roman numerals

Why do some elements have more than one oxidation number?

- Access and Learn Chemistry Learner's Book pg. 59
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 60
- Charts showing radicals

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Electron arrangement of ions using s and p notation
Deriving formulae of compounds I
Deriving formulae of compounds II
Writing balanced chemical equations I

By the end of the lesson, the learner should be able to:
- Write electron arrangement of ions using s and p notation
- Distinguish between electron arrangements of atoms and ions
- Apply electron arrangement to explain ion formation
- Derive formulae of compounds containing radicals
- Write formulae of compounds with transition elements
- Apply formulae writing skills to complex compounds

- Copy and complete the table showing electron arrangements of ions
- Compare electron arrangements of atoms and their ions
- List cations and anions from the table
- Write formulae of compounds containing radicals
- Practise writing formulae of compounds with variable oxidation numbers
- Compare formulae with classmates for peer learning

How does the electron arrangement of an ion differ from that of its atom?
How do you write the formula of a compound containing a radical?

- Access and Learn Chemistry Learner's Book pg. 62
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 63
- Valency tables
- Access and Learn Chemistry Learner's Book pg. 64
- Valency tables
- Digital devices
- Digital devices
- Charts showing chemical equations

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations II
Writing balanced chemical equations III

By the end of the lesson, the learner should be able to:
- Write state symbols in chemical equations
- Balance chemical equations by adjusting coefficients
- Apply the law of conservation of mass to balance equations

- Study the steps for balancing chemical equations
- Study worked examples on balancing equations
- Practise balancing simple chemical equations

How do you balance a chemical equation?

- Access and Learn Chemistry Learner's Book pg. 65
- Digital devices
- Practice worksheets
- Access and Learn Chemistry Learner's Book pg. 66

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Role of electron arrangement in the periodic table - Project
Chemical Bonding - Role of valence electrons in bonding
Chemical Bonding - Types of chemical bonds
Chemical Bonding - The ionic chemical bond

By the end of the lesson, the learner should be able to:
- Make a periodic table for the first 20 elements using locally available materials
- Explain the role of electron arrangement in the periodic table
- Apply creative skills to design and construct educational resources

- Use locally available materials to create a periodic table
- Include element names, symbols, atomic numbers and electron arrangements
- Display the periodic table for peer assessment

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

- Access and Learn Chemistry Learner's Book pg. 67
- Manila paper or carton box
- Coloured pencils
- Flashcards
- Access & Learn Chemistry Learner's Book Grade 10 pg. 70
- Digital devices
- Modelling clay or plasticine
- Wooden splints
- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices

- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Illustrate ionic bonding in sodium chloride and magnesium oxide
- Draw Lewis structures for ionic compounds
- Connect ionic compounds to household items like cooking salt

- Use dot (.) and cross (x) diagrams to show electron donation and acceptance in NaCl and MgO
- Calculate net charges on ions formed
- Watch animations on ionic bond formation using digital devices

What holds sodium and chloride ions together in sodium chloride?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Digital devices
- Periodic table
- Access & Learn Chemistry Learner's Book Grade 10 pg. 76
- Modelling materials (clay, toothpicks)
- Charts of ionic lattices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 77
- Sodium chloride
- Copper (II) chloride
- Distilled water
- Ethanol
- Test tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 78
- Bunsen burner
- Test tubes
- Copper (II) chloride

- Written assignments - Practical observation - Oral questions

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Investigate electrical conductivity in molten and aqueous ionic compounds
- Explain why ionic compounds conduct electricity when molten or dissolved
- Relate conductivity to battery technology and electrolysis
- Illustrate double and triple covalent bonds
- Draw Lewis structures for oxygen and nitrogen molecules
- Relate multiple bonds to atmospheric gases we breathe

- Set up apparatus to investigate conductivity in molten lead (II) bromide
- Investigate conductivity in aqueous sodium chloride solution
- Compare conductivity in solid, molten and aqueous states
- Use dot (.) and cross (x) diagrams to show double bonds in oxygen molecules
- Illustrate triple covalent bonds in nitrogen molecules
- Model multiple covalent bonds using locally available materials

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 79
- Dry cells
- Bulb/ammeter
- Connecting wires
- Carbon rods
- Lead (II) bromide
- Access & Learn Chemistry Learner's Book Grade 10 pg. 81
- Digital devices
- Samples of ionic compounds
- Access & Learn Chemistry Learner's Book Grade 10 pg. 82
- Modelling clay
- Wooden splints
- Charts showing covalent bonds
- Access & Learn Chemistry Learner's Book Grade 10 pg. 83
- Modelling materials
- Charts of molecular structures
- Access & Learn Chemistry Learner's Book Grade 10 pg. 84
- Charts showing molecular structures
- Digital devices

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

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Describe the formation of dative covalent bonds
- Illustrate dative bonding in ammonium and hydroxonium ions
- Relate coordinate bonds to acid-base reactions in the stomach

- Discuss how both shared electrons come from one atom in dative bonding
- Draw structures showing dative bonds in ammonium ion (NH₄⁺)
- Illustrate dative bonding in hydroxonium ion (H₃O⁺)

How is a dative covalent bond different from an ordinary covalent bond?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 85
- Charts showing dative bonds
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 86
- Modelling materials

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Investigate melting and boiling points of molecular substances
- Explain why molecular substances have low melting points
- Relate molecular properties to everyday substances like sugar and wax

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

Why do molecular substances have low melting and boiling points?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 89
- Naphthalene
- Thermometer
- Bunsen burner
- Melting point tube
- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol

- Practical report - Written exercises - Observation

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Describe the giant atomic structure of diamond
- Model the structure of diamond using locally available materials
- Connect diamond's structure to its use in cutting tools and jewelry

- Discuss the tetrahedral structure of diamond
- Model a diamond structure using modelling clay and toothpicks
- Relate structure to properties (hardness, non-conductivity)

Why is diamond the hardest natural substance?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 93
- Modelling clay
- Toothpicks
- Charts of diamond structure
- Access & Learn Chemistry Learner's Book Grade 10 pg. 94
- Charts of graphite structure

- Model assessment - Written exercises - Oral questions

Inorganic Chemistry

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

By the end of the lesson, the learner should be able to:
- Outline uses of diamond, graphite and silicon (IV) oxide
- Relate uses to their structural properties
- Identify applications in drilling, electronics and glass making
- Describe physical properties of metallic structures
- Investigate thermal conductivity of metals
- Connect metallic properties to uses in cooking utensils and electrical wires

- Search for information on uses of giant atomic structures
- Discuss why diamond is used in drilling bits
- Explain the use of graphite as a lubricant and in electrodes
- Investigate thermal conductivity by comparing metal and wood pieces in sunlight
- Discuss high melting and boiling points, malleability, ductility and conductivity
- Analyse data on melting points of different metals

How do the structures of diamond and graphite determine their uses?
Why are metals malleable and ductile?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 96
- Digital devices
- Charts showing applications
- Access & Learn Chemistry Learner's Book Grade 10 pg. 97
- Charts showing metallic bonding
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 99
- Metal and wood pieces
- Digital devices
- 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

- Written assignments - Group presentations - Oral questions
- Practical observation - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Physical appearance and density of group I elements
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

By the end of the lesson, the learner should be able to:
- Describe the physical appearance of group I elements
- Observe and record properties of sodium metal
- Connect alkali metals to applications like sodium lamps in street lighting

- Observe the colour of sodium metal stored under paraffin
- Cut sodium metal and compare freshly cut surface to stored metal
- Watch videos on properties of group I metals
- Analyse densities of alkali metals

Why are alkali metals stored under oil or paraffin?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 106
- Sodium metal
- Scalpel blade
- Petri dish
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 107
- Periodic table
- Graph paper
- 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
- Lithium metal

- Observation - Practical report - Oral questions

Inorganic Chemistry

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:
- Investigate reactions of lithium and sodium with oxygen
- Write balanced equations for reactions with oxygen
- Relate metal oxide formation to rusting and corrosion processes

- Burn lithium and sodium in gas jars of oxygen
- Test products with litmus paper to determine nature of oxides
- Write chemical equations for reactions
- Compare reactivity of different alkali metals

What type of oxides do alkali metals form when they burn in oxygen?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 112
- Gas jar of oxygen
- Deflagrating spoon
- Bunsen burner
- Lithium and sodium metals
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 114
- Chlorine gas
- Cold water
- Beakers
- 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

- 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
Periodicity - Preparation of chlorine and physical properties of group VII elements
Periodicity - Melting, boiling points and gradation in size of group VII 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
- 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 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
- Set up apparatus to prepare chlorine gas from concentrated HCl and potassium manganate (VII)
- Observe colour, smell and solubility of chlorine
- Compare physical properties of fluorine, chlorine, bromine and iodine

Why does the reaction of calcium with dilute sulphuric acid stop quickly?
Why is chlorine collected by downward delivery?

- 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
- 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

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

Inorganic Chemistry

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

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

Why does chlorine turn moist blue litmus paper red and then white?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 139
- Chlorine gas
- Bromine water
- Iodine crystals
- Iron wool
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 142
- Potassium bromide solution
- Potassium iodide solution
- Coloured cloth
- Flower petals

- 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

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)

- 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

How can strong and weak bases be distinguished?

- 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

- Practical assessment - Observation - Written assignments

Physical Chemistry

Acids and Bases - Uses of acids in day-to-day life
Acids and Bases - Uses of bases in day-to-day life
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:
- 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
- Define the term salt
- Explain how salts are formed from neutralisation reactions
- Relate salt formation to table salt production and food seasoning

- 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
- 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

How are acids useful in our daily lives?
What is a salt and how is it formed?

- 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
- 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 assignments - Project assessment
- 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)

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

- 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

What is the role of warming the acid in salt preparation?

- 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

- Practical assessment - Observation - Written exercises

Physical Chemistry

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 carbonate
- Prepare sodium nitrate from sodium carbonate and nitric acid
- Relate effervescence to carbon dioxide fire extinguishers

- 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

How can you tell when the reaction between acid and carbonate is complete?

- 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 assignments