Inorganic Chemistry

Electron arrangement - Writing s and p notation I
Electron arrangement - Writing s and p notation II
Electron arrangement - Practical activity
Historical development of the periodic table I

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

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

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

- 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 do you write the electron arrangement of an element using s and p notation?
How can we demonstrate electron arrangement using locally available materials?

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

- Written exercises - Oral questions - Observation
- 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

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

Transition elements
Stability of atoms

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

- 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

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

Where are transition elements located in the periodic table?

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Cations and anions
Valency and oxidation number I
Valency and oxidation number II

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

- Identify elements with variable oxidation numbers
- Write oxidation numbers of transition elements
- Apply Roman numerals to represent variable oxidation states

- 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

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

How do atoms form ions?
Why do some elements have more than one oxidation number?

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

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

- Oral questions - Written exercises - Practical drawings
- 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

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

- Oral questions - Written exercises - 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
Chemical Bonding - Role of valence electrons in bonding

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

- 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

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

- 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 balance a chemical equation?
How does electron arrangement determine the organization of the periodic table?

- Access and Learn Chemistry Learner's Book pg. 65
- Digital devices
- Practice worksheets
- Access and Learn Chemistry Learner's Book pg. 66
- 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
Chemical Bonding - Ionic bonding in sodium chloride and magnesium oxide

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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Periodic table

- Oral questions - Group discussions - Written assignments

Inorganic Chemistry

Chemical Bonding - Giant ionic structures and lattice
Chemical Bonding - Solubility of ionic compounds
Chemical Bonding - Thermal conductivity, melting and boiling points of ionic compounds

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

- Describe giant ionic structures
- Model a 3-dimensional ionic lattice structure
- Link crystal structures to materials like gemstones and minerals

- Model a 3-dimensional sodium chloride ionic structure using locally available materials
- Discuss the arrangement of ions in a crystal lattice
- Compare models with diagrams of giant ionic lattices

How does the arrangement of ions affect the properties of ionic compounds?

- 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

- Project work - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Electrical conductivity in molten and aqueous ionic compounds
Chemical Bonding - Uses of ionic compounds

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

- 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

Why do ionic compounds conduct electricity only when molten or in solution?

- 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

- Practical report - Observation - Oral questions

Inorganic Chemistry

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:

- 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

- 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

How do non-metal atoms bond with each other?

- 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 exercises - Observation - 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
Chemical Bonding - Melting, boiling points and conductivity of molecular substances

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

- 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 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⁺)

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

How is a dative covalent bond different from an ordinary covalent bond?
Why do molecular substances have low melting and boiling points?

- 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

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

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

Inorganic Chemistry

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

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

- 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 some molecular substances dissolve in organic solvents but not in water?

- 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

- Practical report - Written assignments - 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
Chemical Bonding - Metallic bonding and delocalised electrons

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

- Written assignments - Group presentations - Oral questions

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

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

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

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

Why are metals malleable and ductile?
How does metallic bonding make metals suitable for electrical wiring?

- 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

- Practical observation - Written exercises - Oral questions
- 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
Periodicity - Melting, boiling points and electrical conductivity of group I elements

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

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Periodicity - Reactions of group I elements with oxygen
Periodicity - Reactions of group I elements with chlorine and cold water
Periodicity - Applications of group I elements
Periodicity - Appearance, atomic and ionic radii of group II elements

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

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

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

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 112
- Gas jar of oxygen
- Deflagrating spoon
- Bunsen burner
- Lithium and sodium metals
- Litmus paper
- Access & Learn Chemistry Learner's Book Grade 10 pg. 114
- Chlorine gas
- Cold water
- Beakers
- Access & Learn Chemistry Learner's Book Grade 10 pg. 117
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 118
- Magnesium ribbon
- Calcium metal
- Sandpaper
- Periodic table

- Practical report - Written exercises - Observation

Inorganic Chemistry

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

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
Periodicity - Applications of group II elements

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

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

- 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

- 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

Why does magnesium react slowly with cold water but vigorously with steam?
How is calcium used in the construction industry?

- 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

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

- Practical report - Written exercises - Observation
- 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

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

- Practical report - Observation - Written exercises

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

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

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

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

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 148
- Periodic table
- Digital devices
- Reference materials
- Access & Learn Chemistry Learner's Book Grade 10 pg. 151
- Graph paper
- Periodic table
- Data tables
- Access & Learn Chemistry Learner's Book Grade 10 pg. 155
- Sodium, magnesium, sulphur
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Distilled water

- Written exercises - Oral questions - Group discussions
- 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