Inorganic Chemistry

Structure of the atom - Dalton's atomic model

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

- Describe the structure of the atom using Dalton's model
- Explain the key postulates of Dalton's atomic theory
- Relate Dalton's model to the concept of matter being made of small particles

- Review with peers the concept of the structure of the atom
- Search for information on Dalton's atomic model
- Draw a representation of Dalton's atomic model

How did Dalton describe the structure of atoms?

- Access and Learn Chemistry Learner's Book pg. 17
- Digital devices
- Charts showing atomic models

- Oral questions - Observation - Written exercises

Inorganic Chemistry

Structure of the atom - Rutherford's atomic model
Structure of the atom - Bohr's atomic model
Structure of the atom - Comparing atomic models
Structure of the atom - Modelling project
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:

- Describe the structure of the atom using Rutherford's model
- Explain the gold foil experiment and its findings
- Connect Rutherford's discoveries to our understanding of nuclear structure

- Construct a model of an atom using locally available materials
- Label the nucleus, protons, neutrons and electrons on the model
- Apply creative skills to represent abstract scientific concepts physically

- Watch simulation on the Rutherford Gold Foil experiment
- Discuss with peers the observations and conclusions of the experiment
- Draw a representation of Rutherford's atomic model

- Use locally available materials to model the structure of the atom
- Label the parts of the atomic model
- Display the constructed model for peer assessment

What did Rutherford's gold foil experiment reveal about the atom?
How can we represent the structure of an atom using locally available materials?

- Access and Learn Chemistry Learner's Book pg. 18
- Digital devices
- Internet access
- Access and Learn Chemistry Learner's Book pg. 20
- Charts showing Bohr's model
- Access and Learn Chemistry Learner's Book pg. 21
- Manila papers
- Access and Learn Chemistry Learner's Book pg. 22
- Locally available materials
- Scissors, glue
- Access and Learn Chemistry Learner's Book pg. 24
- Periodic table
- Digital devices
- Digital devices
- Charts showing isotopes

- Oral questions - Written exercises - Group discussions
- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

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

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Relative Atomic Mass - Calculations from isotopic abundances II
Relative Atomic Mass - Determining relative abundance

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

- Calculate R.A.M for elements with three or more isotopes
- Solve complex problems involving isotopic abundances
- Apply R.A.M calculations to real-world chemistry problems

- Study worked examples on R.A.M calculations for multiple isotopes
- Calculate R.A.M for elements with three isotopes
- Solve practice problems on isotopic abundances

How do you calculate R.A.M for elements with multiple isotopes?

- Access and Learn Chemistry Learner's Book pg. 28
- Scientific calculators
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 29

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Relative Atomic Mass - Practical activity with dice

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

- Simulate isotopic abundances using dice
- Calculate R.A.M from simulated data
- Connect hands-on activities to abstract chemical concepts

- Carry out activities using dice to simulate isotopic abundances
- Record and calculate R.A.M from simulated data
- Compare results with actual R.A.M values

How can we use a simulation to understand isotopic abundances?

- Access and Learn Chemistry Learner's Book pg. 30
- Coloured dice
- Flashcards

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Electron arrangement - Energy levels and sub-levels
Electron arrangement - Types of orbitals
Electron arrangement - Aufbau's principle

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Electron arrangement - Writing s and p notation I
Electron arrangement - Writing s and p notation II

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

- Write electron arrangement of elements 1-10 using s and p notation
- Follow the steps for writing electron arrangements
- Apply the rules for filling electrons in s and p orbitals

- Study worked examples on writing s and p notation
- Draw electron arrangements for elements 1-10
- Practise writing s and p notation independently

How do you write the electron arrangement of an element using s and p notation?

- Access and Learn Chemistry Learner's Book pg. 38
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 39

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Electron arrangement - Practical activity
Historical development of the periodic table I

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

- Demonstrate electron filling using plastic beakers
- Model electron configurations using locally available materials
- Visualize abstract electron arrangements through hands-on activities

- Carry out activities to illustrate the order of filling electrons using labelled plastic beakers
- Use beads or pebbles to represent electrons
- Discuss the relationship between energy levels and orbitals

How can we demonstrate electron arrangement using locally available materials?

- Access and Learn Chemistry Learner's Book pg. 40
- Plastic beakers
- Beads or pebbles
- Labels
- Access and Learn Chemistry Learner's Book pg. 45
- Digital devices
- Timeline charts

- Practical assessment - Observation - Written exercises

Inorganic Chemistry

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:

- Explain Mendeleev's contribution to the periodic table
- Describe Moseley's work on atomic numbers
- Recognize Mendeleev as the father of the periodic table

- Search for information on Mendeleev's and Moseley's contributions
- Discuss why Mendeleev is called the father of the periodic table
- Compare Mendeleev's table with the modern periodic table

Why is Mendeleev called the father of the periodic table?

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

- Oral questions - Written exercises - Group discussions

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

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

- Identify the position of transition elements in the periodic table
- Describe general characteristics of transition elements
- Recognize transition metals in everyday items like iron in construction and copper in wiring

- 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

- Identify transition elements in the periodic table
- Discuss with peers the characteristics of transition elements
- Colour-code elements in the periodic table

How can you predict an element's position in the periodic table from its electron arrangement?
Where are transition elements located in the periodic table?

- 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
- Periodic table
- Coloured pencils
- Access and Learn Chemistry Learner's Book pg. 55
- Digital devices

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

Inorganic Chemistry

Cations and anions

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

- Oral questions - Written exercises - Practical drawings

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

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

- 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

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations I
Writing balanced chemical equations II

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

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

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

What are the parts of a chemical equation?

- 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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Writing balanced chemical equations III

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

- 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

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

- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

Chemical Bonding - The ionic chemical bond
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
Chemical Bonding - Electrical conductivity in molten and aqueous ionic compounds

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

- Describe the formation of ionic bonds
- Illustrate electron transfer using dot and cross diagrams
- Relate ionic bonding to common substances like table salt

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

- Discuss the formation of ionic bonds between metals and non-metals
- Draw dot (.) and cross (x) diagrams to show ionic bonding
- Identify examples of ionic compounds

- 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

How do metals and non-metals combine to form ionic compounds?
Why do ionic compounds dissolve in water but not in organic solvents?

- 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
- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 79
- Dry cells
- Bulb/ammeter
- Connecting wires
- Carbon rods
- Lead (II) bromide

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

Inorganic Chemistry

Chemical Bonding - Uses of ionic compounds
Chemical Bonding - The covalent chemical bond

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

- Outline uses of ionic compounds
- Relate properties of ionic compounds to their uses
- Identify ionic compounds in everyday products like fertilizers and antacids

- Search for information on uses of ionic compounds using print or digital materials
- Discuss uses of sodium chloride, calcium carbonate and potassium nitrate
- Relate uses to specific properties

How are the properties of ionic compounds useful in everyday life?

- 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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Chemical Bonding - Double and triple covalent bonds

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

- Illustrate double and triple covalent bonds
- Draw Lewis structures for oxygen and nitrogen molecules
- Relate multiple bonds to atmospheric gases we breathe

- 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 some molecules have double or triple bonds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 83
- Modelling materials
- Charts of molecular structures

- Written exercises - Model assessment - 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
Chemical Bonding - Solubility and uses 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

- 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

- 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

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

Why does water have a relatively high boiling point compared to other small molecules?
Why do molecular substances have low melting and boiling points?

- 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol

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

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of diamond

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

- Model assessment - Written exercises - Oral questions

Inorganic Chemistry

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:

- 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

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

Why can graphite conduct electricity while diamond cannot?

- 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

- Model assessment - Written exercises - Group discussions

Inorganic Chemistry

Chemical Bonding - Metallic bonding and delocalised electrons

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Physical properties of giant metallic structures
Chemical Bonding - Uses of metallic structures related to properties
Periodicity - Introduction to periodic properties
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 physical properties of metallic structures
- Investigate thermal conductivity of metals
- Connect metallic properties to uses in cooking utensils and electrical wires

- 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

- 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

- 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

Why are metals malleable and ductile?
What causes the repeating pattern of properties in the periodic table?

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

- Practical observation - Written exercises - Oral questions
- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

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

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

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

Why does lithium have a higher ionisation energy than sodium?

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

- Written exercises - Data analysis - Oral questions

Inorganic Chemistry

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 group I elements with chlorine and cold water
- Write balanced equations for the reactions
- Connect vigorous reactions to safety precautions in laboratories and industries

- 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 does sodium react more vigorously with water than lithium?

- 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

- Practical report - Written exercises - Observation

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
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 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 127
- Dilute acids
- 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 - Melting, boiling points and gradation in size of group VII elements
Periodicity - Reactions of group VII elements with water and metals

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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 139
- Chlorine gas
- Bromine water
- Iodine crystals
- Iron wool
- Litmus paper

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Displacement reactions and bleaching action of chlorine

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

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

- 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 can chlorine displace bromine and iodine from their compounds?

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

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

- 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

- 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

- 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 does atomic radius decrease across period 3?
Why are metallic oxides basic while non-metallic oxides are acidic?

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

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

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

- 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⁺)

How do acids behave when dissolved 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
- Blue litmus paper

- Observation - Oral questions - Written exercises

Physical Chemistry

Acids and Bases - Properties of bases
Acids and Bases - Reaction of dilute acids with metals
Acids and Bases - Confirmatory test for hydrogen gas

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
- 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

- Practical assessment - Oral questions - Written exercises

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

- 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

What gas is produced when acids react with carbonates?

- 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
- pH paper
- Beakers
- Bunsen burner

- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Reaction of acids with metal hydroxides
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:

- Describe reactions of acids with metal hydroxides
- Demonstrate neutralisation using indicators
- Connect neutralisation to antacid medication for treating stomach acidity

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

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

- 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

How do indicators show the end point of neutralisation?
What does the pH scale measure?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 173
- Sodium hydroxide solution
- Dilute sulphuric (VI) acid
- Phenolphthalein indicator
- Beakers
- Measuring cylinders
- 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 - Oral questions - Written assignments
- Practical assessment - Observation - Written exercises

Physical Chemistry

Acids and Bases - Strong and weak 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

- Practical assessment - Observation - Written assignments

Physical Chemistry

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:

- 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
- 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 - Oral questions - Written exercises