Inorganic Chemistry

Structure of the atom - Rutherford's atomic model

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

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

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

What did Rutherford's gold foil experiment reveal about the atom?

- Access and Learn Chemistry Learner's Book pg. 18
- Digital devices
- Internet access

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Structure of the atom - Bohr's atomic model
Structure of the atom - Comparing atomic models

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

- Describe the structure of the atom using Bohr's model
- Explain the concept of energy levels in an atom
- Relate Bohr's model to how electrons orbit the nucleus like planets around the sun

- Search for information on Bohr's atomic model
- Watch animations on atomic models
- Draw and label Bohr's atomic model

How did Bohr improve on Rutherford's atomic model?

- Access and Learn Chemistry Learner's Book pg. 20
- Digital devices
- Charts showing Bohr's model
- Access and Learn Chemistry Learner's Book pg. 21
- Manila papers

- Oral questions - Observation - Written exercises

Inorganic Chemistry

Structure of the atom - Modelling project
Relative Atomic Mass - Atomic number and mass number
Relative Atomic Mass - Meaning of isotopes

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

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

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

How can we represent the structure of an atom using locally available materials?

- Access and Learn Chemistry Learner's Book pg. 22
- Locally available materials
- Scissors, glue
- Access and Learn Chemistry Learner's Book pg. 24
- Periodic table
- Digital devices
- Digital devices
- Charts showing isotopes

- Project assessment - Peer evaluation - Observation

Inorganic Chemistry

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

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

- Define Relative Atomic Mass (R.A.M)
- Explain the concept of isotopic abundance
- Connect R.A.M to the values shown on the periodic table

- Search for information on Relative Atomic Mass
- Discuss with peers the meaning of isotopic abundance
- Study the relationship between R.A.M and isotopes

What is Relative Atomic Mass and why is it not always a whole number?

- Access and Learn Chemistry Learner's Book pg. 27
- Digital devices
- Periodic table
- Scientific calculators
- Digital devices

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Relative Atomic Mass - Calculations from isotopic abundances II

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

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

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

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

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Relative Atomic Mass - Determining relative abundance

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

- Calculate relative abundance of isotopes given R.A.M
- Solve reverse problems on isotopic abundances
- Apply mathematical skills to determine isotope compositions

- Study worked examples on determining relative abundance
- Calculate relative abundances from given R.A.M values
- Practise solving reverse problems

How can you determine the relative abundance of isotopes if you know the R.A.M?

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Relative Atomic Mass - Practical activity with dice
Electron arrangement - Energy levels and sub-levels

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

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

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

How can we use a simulation to understand isotopic abundances?

- Access and Learn Chemistry Learner's Book pg. 30
- Coloured dice
- Flashcards
- Access and Learn Chemistry Learner's Book pg. 32
- Digital devices
- Charts showing energy levels

- Practical assessment - 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

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

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

In what order do electrons fill the orbitals in an atom?

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

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

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

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

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

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

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

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Electron arrangement - Practical activity

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
Groups and periods I

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

- Oral questions - Group discussions - Written exercises

Inorganic Chemistry

Groups and periods II
Position of an element and electron arrangement

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

- Arrange the first 20 elements into groups and periods
- Relate electron arrangement to group and period number
- Use electron configuration to predict an element's position in the periodic table

- Copy and complete the table for the first 20 elements
- Identify elements belonging to each group and period
- Discuss how electron arrangement changes across periods

How does electron arrangement determine an element's position in the periodic table?

- Access and Learn Chemistry Learner's Book pg. 49
- Periodic table
- Digital devices
- Access and Learn Chemistry Learner's Book pg. 51
- Manila paper
- Graph paper
- Scissors

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical families - Alkali metals and Alkaline earth metals
Chemical families - Halogens and Noble gases
Transition elements

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

- Identify members of alkali metals and alkaline earth metals
- Describe common features of Group I and Group II elements
- Recognize everyday applications of these elements like sodium in salt and calcium in bones

- Identify elements in Group I and Group II
- Discuss with peers common features of alkali metals
- Search for information on properties of alkaline earth metals

What are the characteristics of alkali metals and alkaline earth metals?

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

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Stability of atoms

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

- Explain the stability of noble gas atoms
- Describe how atoms gain stability through electron loss or gain
- Relate atomic stability to the octet rule and full outer shells

- Draw atomic structures of helium, neon and argon
- Discuss with peers the meaning of stability of an atom
- Identify what makes noble gases stable

Why are noble gases stable?

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Cations and anions
Valency and oxidation number I

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

- Oral questions - Written exercises - Practical drawings

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

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

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

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

What are radicals and how are they used in Chemistry?

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

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Electron arrangement of ions using s and p notation

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

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

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

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

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

How do you write balanced equations for reactions involving acids?

- Access and Learn Chemistry Learner's Book pg. 66
- Digital devices
- Practice worksheets
- 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

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

- Oral questions - Observation - Written exercises

Inorganic Chemistry

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

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

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

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

How do metals and non-metals combine to form ionic compounds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 72
- Charts showing ionic bond formation
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 73
- Digital devices
- Periodic table
- Access & Learn Chemistry Learner's Book Grade 10 pg. 76
- Modelling materials (clay, toothpicks)
- Charts of ionic lattices

- Written exercises - 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

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

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

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Chemical Bonding - Double and triple covalent bonds
Chemical Bonding - Covalent bonding in ammonia and hydrogen chloride

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
- Access & Learn Chemistry Learner's Book Grade 10 pg. 84
- Charts showing molecular structures
- Digital devices

- Written exercises - Model assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Dative covalent (coordinate) bonding

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

Chemical Bonding - Hydrogen bonding and Van der Waals forces

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

- Differentiate between intermolecular and intramolecular forces
- Illustrate hydrogen bonding and Van der Waals forces
- Connect intermolecular forces to properties of water like surface tension

- Discuss types of intermolecular forces using print or digital materials
- Illustrate hydrogen bonding in water molecules using models
- Draw diagrams showing Van der Waals forces

Why does water have a relatively high boiling point compared to other small molecules?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 86
- Modelling materials
- Digital devices

- Written exercises - Model assessment - Oral questions

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

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of diamond

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

- Describe the giant atomic structure of diamond
- Model the structure of diamond using locally available materials
- Connect diamond's structure to its use in cutting tools and jewelry

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

Why is diamond the hardest natural substance?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 93
- Modelling clay
- Toothpicks
- Charts of diamond structure

- Model assessment - Written exercises - Oral questions

Inorganic Chemistry

Chemical Bonding - Giant atomic structure of graphite

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

- 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

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

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

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

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

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

- Oral questions - Written exercises - Group discussions

Inorganic Chemistry

Periodicity - Ionisation energy and electronegativity of group I elements
Periodicity - Melting, boiling points and electrical conductivity of group I elements

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

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

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

Why does lithium have a higher ionisation energy than sodium?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 108
- Data tables
- Graph paper
- Digital devices
- Access & Learn Chemistry Learner's Book Grade 10 pg. 110
- Connecting wires
- Dry cells
- Bulb
- Sodium metal
- Lithium metal

- Written exercises - Data analysis - Oral questions

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

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

- Practical report - Written exercises - Observation

Inorganic Chemistry

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

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

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

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

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

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

- Observation - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Ionisation energy, melting and boiling points of group II elements
Periodicity - Reactions of group II elements with water, steam and oxygen

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

- Data analysis - Written exercises - Oral questions

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

- 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

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

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

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

Why can chlorine displace bromine and iodine from their compounds?

- Access & Learn Chemistry Learner's Book Grade 10 pg. 142
- Potassium bromide solution
- Potassium iodide solution
- Chlorine gas
- Coloured cloth
- Flower petals

- Practical report - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of group VII elements

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

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

- Search for information on applications of halogens
- Discuss uses of chlorine in water treatment, bromine in photography, iodine in medicine
- Create presentations on halogen applications

How is chlorine used to make drinking water safe?

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

- Written assignments - Group presentations - Oral questions

Inorganic Chemistry

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

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

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

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

- Written exercises - Oral questions - Group discussions

Inorganic Chemistry

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

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

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

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

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

- Access & Learn Chemistry Learner's Book Grade 10 pg. 155
- Sodium, magnesium, sulphur
- Gas jar of oxygen
- Bunsen burner
- Litmus paper
- Distilled water
- Access & Learn Chemistry Learner's Book Grade 10 pg. 158
- Chlorine gas
- Dilute acids
- Sodium, magnesium
- Test tubes
- Bunsen burner

- Practical report - Written exercises - Observation