Inorganic Chemistry

Electron arrangement - Energy levels and sub-levels

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

- 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

How are electrons organized within energy levels?

- Access and Learn Chemistry Learner's Book pg. 32
- Digital devices
- Charts showing energy levels

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Electron arrangement - Types of orbitals

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

- Describe the shapes of s and p orbitals
- Identify the number of orbitals in each sub-level
- Visualize orbital shapes as regions where electrons are likely found

- Search for information on types of orbitals
- Study diagrams showing shapes of s and p orbitals
- Watch videos showing electrons in various orbitals

What do s and p orbitals look like?

- Access and Learn Chemistry Learner's Book pg. 34
- Digital devices
- Charts showing orbital shapes

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Electron arrangement - Aufbau's principle
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:

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

- 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

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

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

In what order do electrons fill the orbitals in an atom?
How do you write the electron arrangement of an element using s and p notation?

- Access and Learn Chemistry Learner's Book pg. 36
- Digital devices
- Aufbau diagram
- Access and Learn Chemistry Learner's Book pg. 38
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 39

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

Inorganic Chemistry

Electron arrangement - Practical activity

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

- Practical assessment - Observation - Written exercises

Inorganic Chemistry

Historical development of the periodic table I
Historical development of the periodic table II

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

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

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

How did scientists first attempt to organize the elements?

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

- Oral questions - Group discussions - Written exercises

Inorganic Chemistry

Groups and periods I
Groups and periods II

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

- 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

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

What are groups and periods in the periodic table?

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

- Oral questions - Written exercises - Observation

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

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Valency and oxidation number II

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Radicals
Electron arrangement of ions using s and p notation

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

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

- 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

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

What are radicals and how are they used in Chemistry?
How does the electron arrangement of an ion differ from that of its atom?

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

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

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

Inorganic Chemistry

Deriving formulae of compounds I
Deriving formulae of compounds II

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

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

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

How do you write the formula of a compound?

- Access and Learn Chemistry Learner's Book pg. 63
- Valency tables
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 64

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Writing balanced chemical equations I

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Writing balanced chemical equations II

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

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

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

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

- 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

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

- 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 do you write balanced equations for reactions involving acids?
How does electron arrangement determine the organization of the periodic table?

- Access and Learn Chemistry Learner's Book pg. 66
- Digital devices
- Practice worksheets
- Access and Learn Chemistry Learner's Book pg. 67
- Manila paper or carton box
- Coloured pencils
- Flashcards
- Access & Learn Chemistry Learner's Book Grade 10 pg. 70
- Digital devices
- Modelling clay or plasticine
- Wooden splints

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

Inorganic Chemistry

Chemical Bonding - Types of chemical bonds
Chemical Bonding - The ionic chemical bond

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

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

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

What determines the type of bond formed between atoms?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Digital devices
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices

- Oral questions - Group discussions - Written assignments

Inorganic Chemistry

Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide
Chemical Bonding - Giant ionic structures and lattice

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

- 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

- Written assignments - Practical observation - Oral questions

Inorganic Chemistry

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:

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

- 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

Why do ionic compounds dissolve in water but not in organic solvents?

- 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

- Practical report - Observation - Written exercises

Inorganic Chemistry

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

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

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

- 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

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

Why do ionic compounds conduct electricity only when molten or in solution?
How do non-metal atoms bond with each other?

- 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

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

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

- Written exercises - Observation - 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

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

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

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

Why do molecular substances have low melting and boiling points?
Why do some molecular substances dissolve in organic solvents but not in water?

- 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
- Practical report - Written assignments - Oral questions

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

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

- Model assessment - Written exercises - Group discussions

Inorganic Chemistry

Chemical Bonding - Uses of diamond, graphite and silicon (IV) oxide

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

- 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

How do the structures of diamond and graphite determine their uses?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 96
- Digital devices
- Charts showing applications

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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

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

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

- Describe physical properties of metallic structures
- Investigate thermal conductivity of metals
- Connect metallic properties to uses in cooking utensils and electrical wires

- 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

- 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

Why are metals good conductors of electricity and heat?
Why are metals malleable and ductile?

- 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

- Written exercises - Oral questions - Observation
- Practical observation - Written exercises - Oral questions

Inorganic Chemistry

Chemical Bonding - Uses of metallic structures related to properties
Periodicity - Introduction to periodic properties
Periodicity - Physical appearance and density of group I elements

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

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

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

How does metallic bonding make metals suitable for electrical wiring?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 101
- Digital devices
- Samples of metal products
- Access & Learn Chemistry Learner's Book Grade 10 pg. 104
- Periodic table charts
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 106
- Sodium metal
- Scalpel blade
- Petri dish

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Gradation in size of atoms and ions of group I elements
Periodicity - Ionisation energy and electronegativity of group I elements

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

- Describe the trend in atomic and ionic radii of group I elements
- Draw electron arrangements of group I atoms and ions
- Relate atomic size to the number of energy levels in atoms

- Draw dot (.) and cross (x) structures of lithium, sodium and potassium atoms and ions
- Compare atomic and ionic radii of group I elements
- Analyse data on atomic and ionic radii trends

Why is the ionic radius of sodium smaller than its atomic radius?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 107
- Periodic table
- Graph paper
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 108
- Data tables

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

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 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 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 do melting points decrease down group I elements?

- 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

- Practical report - Written exercises - Observation

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
Periodicity - Ionisation energy, melting and boiling points 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

- 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

- 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

- 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 does sodium react more vigorously with water than lithium?
Why do group II elements have two ionisation energies?

- 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

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

- Practical report - Written exercises - Observation
- 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 - Applications of group II 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

- 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

How is calcium used in the construction industry?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 129
- Digital devices
- Reference materials

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

Periodicity - Preparation of chlorine and physical properties of group VII elements
Periodicity - Melting, boiling points and gradation in size of group VII elements

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

- 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

- 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

- 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 chlorine collected by downward delivery?
Why is iodine a solid while chlorine is a gas at room temperature?

- 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 - Observation - Written exercises
- 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 - Displacement reactions and bleaching action of chlorine
Periodicity - Applications of group VII elements

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

- Practical report - Written exercises - Observation

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 - 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

- 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

- Data analysis - Written exercises - Oral questions
- 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