Inorganic Chemistry

Periodicity - Introduction to periodic properties

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

- Define periodicity and periodic properties
- Identify atomic size, ionisation energy, electron affinity and electronegativity
- Relate periodic trends to arrangement of elements in the periodic table

- Search for information on periodic properties using print or digital materials
- Discuss the meaning of atomic radius, ionisation energy, electron affinity and electronegativity
- Study sample periodic tables to identify patterns

What causes the repeating pattern of properties in the periodic table?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 104
- Periodic table charts
- Digital devices

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Periodicity - Physical appearance and density of group I elements
Periodicity - Gradation in size of atoms and ions of group I elements

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

- Describe the 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

- Observation - Practical report - Oral questions

Inorganic Chemistry

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 trends in ionisation energy and electronegativity of group I elements
- Analyse data on ionisation energies
- Connect ionisation energy to reactivity of metals like sodium in fireworks

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

- Analyse data on ionisation energies of group I elements
- Discuss factors affecting ionisation energy (atomic radius, shielding effect)
- Create trend charts for electronegativity values

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

Why does lithium have a higher ionisation energy than sodium?
Why do melting points decrease down group I elements?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 108
- Data tables
- Graph paper
- Digital devices

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

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

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen
Periodicity - Reactions of group I elements with chlorine and cold water

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

- Investigate reactions of 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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group I elements

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

- Outline applications of group I elements
- Relate properties to specific uses
- Identify uses in batteries, street lights, medicine and photography

- Search for information on applications of group I elements using print or digital materials
- Discuss uses of lithium in batteries, sodium in lamps, potassium in fertilizers
- Create presentations on applications

How are the properties of alkali metals utilised in modern technology?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 117
- Digital devices
- Reference materials

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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

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

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

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

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

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

- Observation - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy, melting and boiling points of group II elements

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

- Describe trends in ionisation energy of group II elements
- Analyse melting and boiling point data
- Connect high melting points to use of magnesium oxide in furnace linings

- Analyse data on first and second ionisation energies of group II elements
- Plot graphs of melting and boiling points against atomic number
- Discuss factors affecting ionisation energy and melting points

Why do group II elements have two ionisation energies?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 121
- Graph paper
- Data tables
- Digital devices

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group II elements with water, steam and oxygen

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

- Investigate reactions of magnesium and calcium with water and oxygen
- Write balanced equations for the reactions
- Relate magnesium's reaction with oxygen to its use in flares and fireworks

- Investigate reactions of magnesium ribbon with cold water and steam
- Investigate reaction of calcium with cold water
- Burn magnesium and calcium in oxygen and test products
- Collect and test gases produced

Why does magnesium react slowly with cold water but vigorously with steam?

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

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

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

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

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group II elements
Periodicity - Preparation of chlorine and physical properties of group VII elements

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

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

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

- Search for information on applications of group II elements
- Discuss uses of magnesium in alloys, calcium in cement, barium in X-rays
- Create flashcards showing applications

- 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

How is calcium used in the construction industry?
Why is chlorine collected by downward delivery?

- 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

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

Inorganic Chemistry

Periodicity - Preparation of chlorine and physical properties of group VII elements

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

- 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 is chlorine collected by downward delivery?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 131
- Concentrated HCl
- Potassium manganate (VII)
- Gas jars
- Delivery tubes

- Practical report - Observation - Written exercises

Inorganic Chemistry

Periodicity - Melting, boiling points and gradation in size of group VII elements

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

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

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

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 135
- Graph paper
- Data tables
- Digital devices

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of group VII elements with water and metals

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

- Practical report - Written exercises - Observation

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

- Investigate displacement reactions of halogens
- Investigate the bleaching action of chlorine
- Relate displacement reactions to water purification and textile bleaching

- 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

- Bubble chlorine gas through solutions of potassium bromide and potassium iodide
- Observe colour changes and identify products
- Investigate bleaching action of chlorine on coloured cloth and flower petals
- Write chemical equations for displacement reactions

Why does chlorine turn moist blue litmus paper red and then white?
Why can chlorine displace bromine and iodine from their compounds?

- 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
- Chlorine gas
- Coloured cloth
- Flower petals

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group VII elements

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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Physical properties and applications of noble gases

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

- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging

- Analyse data on atomic radii, ionisation energy, melting and boiling points of noble gases
- Discuss why noble gases are unreactive
- Search for information on uses of helium, neon and argon

Why are noble gases called inert gases?

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Periodicity - Physical properties and applications of noble gases

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

- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging

- Analyse data on atomic radii, ionisation energy, melting and boiling points of noble gases
- Discuss why noble gases are unreactive
- Search for information on uses of helium, neon and argon

Why are noble gases called inert gases?

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Periodicity - Physical properties and applications of noble gases
Periodicity - Atomic size, ionisation energy and electronegativity across period 3

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

- Describe physical properties of noble gases
- Outline applications of group VIII elements
- Relate noble gas properties to uses in lighting, welding and medical imaging

- 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

- Analyse data on atomic radii, ionisation energy, melting and boiling points of noble gases
- Discuss why noble gases are unreactive
- Search for information on uses of helium, neon and argon

- 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 are noble gases called inert gases?
Why does atomic radius decrease across period 3?

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Periodic table
- Data tables

- Written exercises - Oral questions - Group discussions
- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of period 3 elements with oxygen and water

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

- Investigate reactions of period 3 elements with oxygen and water
- Write balanced equations for the reactions
- Relate oxide formation to acidic and basic properties of substances

- Burn sodium, magnesium and sulphur in oxygen
- Test products with litmus paper to determine acidic or basic nature
- Investigate reactions of sodium and magnesium with water and steam
- Write chemical equations for all reactions

Why are metallic oxides basic while non-metallic oxides are acidic?

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reactions of period 3 elements with chlorine and dilute acids

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

- 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

How do the chemical properties of elements change across period 3?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner

- Practical report - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reactions of period 3 elements with chlorine and dilute acids

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

- 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

How do the chemical properties of elements change across period 3?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner

- Practical report - Written exercises - Oral questions

Physical Chemistry

Acids and Bases - Dissociation of acids in aqueous solutions
Acids and Bases - Dissociation of bases in aqueous solutions
Acids and Bases - Properties of acids

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

- Define dissociation of acids in water
- Demonstrate dissociation of acids in aqueous solutions
- Relate dissociation of acids to everyday substances like vinegar and lemon juice

- Explain dissociation of bases in water
- Demonstrate dissociation of bases in aqueous solutions
- Connect dissociation of bases to household cleaning products like soap and detergents

- Discuss with peers the meaning of dissociation of acids in water
- Carry out experiments to demonstrate dissociation of dilute hydrochloric acid
- Record observations on release of hydrogen ions (H⁺)

- Carry out experiments to demonstrate dissociation of sodium hydroxide solution
- Test solutions using litmus paper and phenolphthalein indicator
- Record observations on release of hydroxide ions (OH⁻)

How do acids behave when dissolved in water?
What ions are released when bases dissolve in water?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 164
- Dilute hydrochloric acid
- Test tubes
- 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
- pH indicator paper
- Blue litmus paper
- Digital resources

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

Physical Chemistry

Acids and Bases - Properties of bases

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

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

- 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

What common household substances are basic in nature?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 167
- Sodium hydroxide solution
- Baking soda
- Soap solution
- Red litmus paper
- Phenolphthalein

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Reaction of dilute acids with metals

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

- Describe the reaction between dilute acids and metals
- Carry out experiments on acid-metal reactions
- Relate acid-metal reactions to corrosion of metallic structures and pipes

- Measure dilute hydrochloric acid and add zinc powder
- Observe effervescence and test gas produced using burning splint
- Write balanced equations for the reactions

What products are formed when acids react with metals?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 169
- Zinc powder
- Dilute hydrochloric acid
- Test tubes
- Wooden splints
- Rubber corks

- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Confirmatory test for hydrogen gas

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

- Perform the confirmatory test for hydrogen gas
- Record observations accurately
- Connect hydrogen gas production to industrial processes like welding

- Collect hydrogen gas produced from acid-metal reactions
- Test the gas using a burning splint
- Record the pop sound observation
- Write equations for reactions of different metals with acids

How can hydrogen gas be identified in the laboratory?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 170
- Dilute sulphuric acid
- Magnesium ribbon
- Test tubes
- Wooden splints
- Delivery tubes

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

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

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

- Describe reactions of acids with carbonates
- Carry out experiments on acid-carbonate reactions
- Relate the reaction to effervescence in baking and antacid tablets

- Explain neutralisation reactions involving metal oxides
- Carry out experiments on acid-metal oxide reactions
- Relate neutralisation to treatment of acidic soils in agriculture

- Add dilute hydrochloric acid to sodium carbonate
- Observe effervescence and collect gas produced
- Test gas using calcium hydroxide (limewater)
- Write balanced equations for the reactions

- Warm dilute nitric (V) acid and add magnesium oxide
- Test the resulting solution using pH paper
- Record observations and determine nature of solution
- Write balanced equations for the reactions

What gas is produced when acids react with carbonates?
What is a neutralisation reaction?

- Chemistry Learner's Book Grade 10 pg. 170
- Sodium carbonate
- Dilute hydrochloric acid
- Calcium hydroxide
- Delivery tubes
- Test tubes
- Access & Learn Chemistry Learner's Book Grade 10 pg. 171
- Sodium hydrogen carbonate
- Dilute nitric (V) acid
- Test tubes
- Delivery tubes

- Access & Learn Chemistry Learner's Book Grade 10 pg. 172
- Magnesium oxide
- Dilute nitric (V) acid
- pH paper
- Beakers
- Bunsen burner

- Practical assessment - Observation - Written exercises

Physical Chemistry

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 metal hydroxides
- Demonstrate neutralisation using indicators
- Connect neutralisation to antacid medication for treating stomach acidity

- Add dilute sulphuric (VI) acid to sodium hydroxide with phenolphthalein
- Observe colour change from pink to colourless
- Write balanced equations for the neutralisation reaction

How do indicators show the end point of neutralisation?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 173
- Sodium hydroxide solution
- Dilute sulphuric (VI) acid
- Phenolphthalein indicator
- Beakers
- Measuring cylinders

- Practical assessment - Oral questions - Written assignments

Physical Chemistry

Acids and Bases - Universal indicator and pH scale

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

- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Universal indicator and pH scale

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

- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Strong and weak acids

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

- Differentiate between strong and weak acids
- Classify acids based on their pH values
- Connect acid strength to battery acid (strong) versus citrus fruits (weak)

- Test 0.1 M hydrochloric acid and 0.1 M ethanoic acid using universal indicator
- Compare pH values of strong and weak acids
- Discuss degree of dissociation in strong and weak acids

Why do strong acids have lower pH values than weak acids?

- Chemistry Learner's Book Grade 10 pg. 175
- 0.1 M hydrochloric acid
- 0.1 M ethanoic acid
- Universal indicator
- pH scale chart
- Test tubes

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Electrical conductivity of acids and bases

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

- Compare electrical conductivity of strong and weak acids and bases
- Set up circuits to test conductivity
- Connect conductivity to car battery technology and industrial electrochemistry

- Set up electrical circuits with bulb, dry cell and electrodes
- Test conductivity of strong and weak acids and bases
- Compare brightness of bulb in different solutions
- Record and discuss observations

Why do strong acids and bases conduct electricity better than weak ones?

- Chemistry Learner's Book Grade 10 pg. 176
- Dry cells
- Bulbs with holders
- Connecting wires
- Nails/electrodes
- Various acid and base solutions

- Practical assessment - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Uses of acids in day-to-day life

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

- 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 are acids useful in our daily lives?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers

- Oral questions - Written assignments - Project assessment

Physical Chemistry

Acids and Bases - Uses of acids in day-to-day life

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

- 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 are acids useful in our daily lives?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 178
- Digital devices
- Reference books
- Chart papers
- Markers

- 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

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

- Describe acid salts and their formation
- Identify examples of acid salts
- Relate acid salts to baking soda (sodium hydrogen carbonate) used in cooking

- 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

- Discuss characteristics of acid salts (contain replaceable hydrogen, pH less than 7)
- Write formulae of acid salts (NaHCO₃, NaHSO₄)
- Test solutions of acid salts with litmus paper
- Compare acid salts with normal salts

What is a salt and how is it formed?
How do acid salts differ from normal salts?

- 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
- Litmus paper
- pH paper
- Test tubes
- Distilled water

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

Physical Chemistry

Introduction to Salts - Basic and double salts

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

- Describe basic salts and double salts
- Identify examples of basic and double salts
- Connect double salts to alum used in water purification and dyeing

- Discuss characteristics of basic salts (contain hydroxide ions, pH greater than 7)
- Discuss double salts (two different cations or anions)
- Write formulae of double salts
- Categorise provided salt samples into types

What distinguishes basic salts and double salts from other types?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 184
- Samples of basic and double salts
- Potassium aluminium sulphate (alum)
- Litmus paper
- pH paper

- Oral questions - Written exercises - Observation