Inorganic Chemistry

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

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

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

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

- 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

- 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

How did scientists first attempt to organize the elements?
Why is Mendeleev called the father of the periodic table?

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

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

Inorganic Chemistry

Position of an element and electron arrangement
Chemical families - Alkali metals and Alkaline earth metals

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

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

- 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

How can you predict an element's position in the periodic table from its electron arrangement?

- 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

- Practical assessment - Oral questions - Observation

Inorganic Chemistry

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

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

- Identify members of halogens and noble gases
- Describe common features of Group VII and Group VIII elements
- Connect halogens to uses like chlorine in water treatment and noble gases in lighting

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

Why are noble gases called inert gases?

- Access and Learn Chemistry Learner's Book pg. 53
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 54
- Coloured pencils
- Access and Learn Chemistry Learner's Book pg. 55

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Cations and anions

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
Radicals

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

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

- 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

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

What is the difference between valency and oxidation number?
What are radicals and how are they used in Chemistry?

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

- 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

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

- 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

How does the electron arrangement of an ion differ from that of its atom?

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

- 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
Writing balanced chemical equations III
Role of electron arrangement in the periodic table - Project

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

- 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

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

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

How do you balance a chemical equation?
How do you write balanced equations for reactions involving acids?

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Role of valence electrons in bonding
Chemical Bonding - Types of chemical bonds
Chemical Bonding - The ionic chemical bond

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

- Explain the role of valence electrons in bonding
- Identify the octet and duplet rule in bond formation
- Relate chemical bonding to everyday materials like plastics and metals

- Review the concept of stability of atoms (gaining and/or losing electrons)
- Discuss in groups the role of valence electrons in bonding (octet/duplet noble gas configuration)
- Use digital devices to watch animations on atomic stability

Why do atoms form bonds with other atoms?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 70
- Digital devices
- Modelling clay or plasticine
- Wooden splints
- Access & Learn Chemistry Learner's Book Grade 10 pg. 71
- Charts showing bond types
- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices

- Oral questions - Observation - Written exercises

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
Chemical Bonding - Electrical conductivity in molten and aqueous 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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 79
- Dry cells
- Bulb/ammeter
- Connecting wires
- Carbon rods
- Lead (II) bromide

- Practical report - Observation - Written exercises

Inorganic Chemistry

Chemical Bonding - Uses of ionic compounds
Chemical Bonding - The covalent chemical bond
Chemical Bonding - Double and triple covalent bonds

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

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

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

- 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

- 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

How are the properties of ionic compounds useful in everyday life?
Why do some molecules have double or triple bonds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 81
- Digital devices
- Samples of ionic compounds
- Access & Learn Chemistry Learner's Book Grade 10 pg. 82
- Modelling clay
- Wooden splints
- Charts showing covalent bonds

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

- Written assignments - Group presentations - Oral questions
- 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

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

- Investigate melting and boiling points of molecular substances
- Explain why molecular substances have low melting points
- Relate molecular properties to everyday substances like sugar and wax

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

Why do molecular substances have low melting and boiling points?

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Solubility and uses of molecular substances
Chemical Bonding - Giant atomic structure of diamond
Chemical Bonding - Giant atomic structure of graphite

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

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

- 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

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

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

Why do some molecular substances dissolve in organic solvents but not in water?
Why is diamond the hardest natural substance?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 92
- Sulphur powder
- Sugar crystals
- Distilled water
- Ethanol
- Access & Learn Chemistry Learner's Book Grade 10 pg. 93
- Modelling clay
- Toothpicks
- Charts of diamond structure
- Access & Learn Chemistry Learner's Book Grade 10 pg. 94
- Charts of graphite structure

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

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

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

Why are metals good conductors of electricity and heat?

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Uses of metallic structures related to properties

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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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
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:

- 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

- 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

- 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

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

What causes the repeating pattern of properties in the periodic table?
Why does lithium have a higher ionisation energy than sodium?

- 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
- 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

- Oral questions - Written exercises - Group discussions
- 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

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

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

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

- 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

- 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

Why does chlorine turn moist blue litmus paper red and then white?
How is chlorine used to make drinking water safe?

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

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

- Practical report - Written exercises - Observation
- 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 - Atomic size, ionisation energy and electronegativity across period 3
Periodicity - Reactions of period 3 elements with oxygen and water

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

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

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

Why does atomic radius decrease across period 3?

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

- Data analysis - Written exercises - Oral questions

Inorganic Chemistry

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