Inorganic Chemistry

Chemical Bonding - Stability of atoms
Chemical Bonding - Valence electrons in bonding

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

- Explain why atoms bond to achieve stability
- Distinguish between stable and unstable atoms
- Relate atomic stability to noble gas uses in lighting

- Review the concept of stability of atoms
- Discuss duplet and octet configurations
- Identify stable and unstable atoms

Why do atoms form chemical bonds?

- Front Row Chemistry Grade 10 pg. 56
- Periodic table
- Diagrams of electron configurations
- Front Row Chemistry Grade 10 pg. 57
- Coloured pencils
- Periodic table

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Introduction to bond types
Chemical Bonding - Formation of ionic bonds
Chemical Bonding - Drawing ionic bond diagrams
Chemical Bonding - Structure of ionic lattice

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

- Identify different types of chemical bonds
- Classify substances by bond type
- Relate bond types to properties of common materials like salt and water

- Draw Lewis structures for various ionic compounds
- Apply electron transfer principles
- Illustrate bonding in compounds like magnesium chloride and lithium sulphide

- Discuss different types of chemical bonds
- Examine various substances and predict bond types
- Categorise materials by bonding

- Draw Lewis diagrams for magnesium chloride
- Draw Lewis diagrams for lithium sulphide
- Share diagrams with peers for review

What are the main types of chemical bonds?
How do we represent ionic bonding using diagrams?

- Front Row Chemistry Grade 10 pg. 58
- Samples of different substances
- Digital devices
- Front Row Chemistry Grade 10 pg. 59
- Exercise books
- Diagrams of ionic bonding
- Front Row Chemistry Grade 10 pg. 60
- Exercise books
- Coloured pencils
- Front Row Chemistry Grade 10 pg. 61
- Sodium chloride crystals
- Hand lens
- Watch glass

- Oral questions - Written exercises - Group discussions
- Written exercises - Peer assessment - Individual assessment

Inorganic Chemistry

Chemical Bonding - Physical properties of ionic compounds
Chemical Bonding - Formation of covalent bonds

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

- Investigate physical properties of ionic compounds
- Explain properties in terms of structure and bonding
- Relate ionic compound properties to uses in water treatment and de-icing roads

- Investigate solubility of ionic compounds
- Test electrical conductivity of ionic solutions
- Test brittleness of ionic crystals

Why do ionic compounds have high melting points and conduct electricity when dissolved?

- Front Row Chemistry Grade 10 pg. 62
- Sodium chloride
- Distilled water
- Circuit with bulb
- Front Row Chemistry Grade 10 pg. 66
- Modelling materials
- Diagrams of covalent bonding

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Single, double and triple covalent bonds

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

- Differentiate between single, double and triple covalent bonds
- Draw Lewis structures showing different bond types
- Relate bond types to gases like oxygen (double) and nitrogen (triple)

- Discuss types of covalent bonds
- Draw structures for fluorine, oxygen and nitrogen molecules
- Compare bond strengths

What is the difference between single, double and triple bonds?

- Front Row Chemistry Grade 10 pg. 67
- Exercise books
- Bond diagrams

- Written exercises - Individual assessment - Oral questions

Inorganic Chemistry

Chemical Bonding - Covalent bonding in diatomic molecules

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

- Draw Lewis structures for diatomic molecules
- Identify bonding and non-bonding electron pairs
- Relate diatomic molecules to atmospheric gases we depend on

- Draw Lewis diagrams for H₂, Cl₂, O₂, N₂
- Identify lone pairs and bonding pairs
- Practice drawing molecular structures

How do we draw covalent bonds in simple molecules?

- Front Row Chemistry Grade 10 pg. 68
- Exercise books
- Coloured pencils

- Written exercises - Peer assessment - Individual assessment

Inorganic Chemistry

Chemical Bonding - Covalent bonding in compounds
Chemical Bonding - Formation of dative (coordinate) bonds

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

- Draw Lewis structures for covalent compounds
- Apply bonding principles to multi-atom molecules
- Relate compound structures to properties of water and carbon dioxide

- Explain how dative covalent bonds form
- Draw structures showing coordinate bonds
- Apply dative bonding to understand ammonium ion formation in fertilisers

- Draw Lewis structures for HF, H₂O, NH₃, CO₂
- Discuss bonding in each compound
- Share diagrams with peers for review

- Discuss formation of dative covalent bonds
- Draw structure of ammonium ion
- Identify donor and acceptor atoms

How do we represent covalent bonding in compounds?
How is a dative bond different from a normal covalent bond?

- Front Row Chemistry Grade 10 pg. 69
- Exercise books
- Molecular diagrams

- Front Row Chemistry Grade 10 pg. 71
- Exercise books
- Diagrams of dative bonding

- Written exercises - Individual assessment - Observation
- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Chemical Bonding - Properties of simple molecular substances

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

- Describe simple molecular structures
- Investigate properties of molecular substances
- Relate molecular properties to everyday substances like sugar and wax

- Investigate properties of molecular substances
- Compare melting points of molecular compounds
- Discuss intermolecular forces

Why do molecular substances have low melting points?

- Front Row Chemistry Grade 10 pg. 72
- Samples of molecular substances
- Bunsen burner

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Chemical Bonding - Van der Waals forces and hydrogen bonding

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

- Distinguish between Van der Waals forces and hydrogen bonds
- Explain the effect of intermolecular forces on properties
- Relate hydrogen bonding to water's unique properties essential for life

- Visualise hydrogen bonding in water
- Compare substances with different intermolecular forces
- Discuss effect on boiling points

Why does water have a higher boiling point than expected?

- Front Row Chemistry Grade 10 pg. 74
- Diagrams of hydrogen bonding
- Digital devices

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Chemical Bonding - Structure and properties of diamond

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

- Describe the structure of diamond
- Explain properties of diamond in terms of structure
- Relate diamond's hardness to its use in cutting tools and jewellery

- Understand physical properties of giant covalent structures
- Build models of diamond structure
- Discuss uses of diamond

Why is diamond the hardest naturally occurring substance?

- Front Row Chemistry Grade 10 pg. 76
- Models of diamond structure
- Modelling materials

- Observation - Written exercises - Project work

Inorganic Chemistry

Chemical Bonding - Structure and properties of graphite and silicon dioxide
Periodicity - Physical properties of alkali metals (atomic and ionic radii)
Periodicity - Physical properties of alkali metals (appearance and hardness)

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

- Describe structures of graphite and silicon dioxide
- Compare properties of different giant covalent structures
- Relate graphite conductivity to pencil writing and lubricant uses

- Describe trends in atomic and ionic radii of alkali metals
- Explain reasons for observed trends
- Relate atomic size to reactivity of sodium in sodium vapour lamps

- Build models of graphite structure
- Compare graphite and diamond properties
- Discuss structure and uses of silicon dioxide

- Discuss trends in physical properties of Group I elements
- Complete tables showing atomic and ionic radii
- Explain trends down the group

Why can graphite conduct electricity while diamond cannot?
How do atomic and ionic sizes change down Group I?

- Front Row Chemistry Grade 10 pg. 77
- Modelling materials
- Sand samples
- Front Row Chemistry Grade 10 pg. 85
- Periodic table
- Data tables
- Front Row Chemistry Grade 10 pg. 87
- Lithium, sodium, potassium samples
- Scalpel
- White tile

- Written exercises - Project work - Observation
- Oral questions - Written exercises - Observation

Inorganic Chemistry

Periodicity - Physical properties of alkali metals (conductivity, melting and boiling points)
Periodicity - Ionisation energy of alkali metals

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

- Test electrical conductivity of alkali metals
- Describe trends in melting and boiling points
- Relate conductivity to use of sodium in heat transfer systems

- Test conductivity using simple circuit
- Study data on melting and boiling points
- Explain trends in terms of metallic bonding

Why do melting points decrease down Group I?

- Front Row Chemistry Grade 10 pg. 89
- Circuit with bulb
- Alkali metal samples
- Data tables
- Front Row Chemistry Grade 10 pg. 90
- Data tables
- Digital devices

- Practical assessment - Written exercises - Oral questions

Inorganic Chemistry

Periodicity - Reaction of alkali metals with air/oxygen
Periodicity - Reaction of alkali metals with water

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

- Investigate reaction of alkali metals with oxygen
- Write balanced equations for the reactions
- Relate oxidation of sodium to its storage under oil

- Carry out experiments on reaction with air
- Observe flame colours and products
- Write word and chemical equations

What happens when alkali metals burn in air?

- Front Row Chemistry Grade 10 pg. 91
- Sodium metal
- Deflagrating spoon
- Gas jar of oxygen
- Front Row Chemistry Grade 10 pg. 93
- Sodium, potassium
- Trough with water
- Phenolphthalein

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of alkali metals with chlorine and dilute acids
Periodicity - Applications of alkali metals

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

- Describe reactions of alkali metals with chlorine
- Explain reactions with dilute acids
- Relate sodium chloride formation to table salt production

- Investigate reaction of sodium with chlorine
- Discuss reactions with dilute acids (video)
- Write balanced equations

Why are reactions of alkali metals with acids dangerous?

- Front Row Chemistry Grade 10 pg. 94
- Gas jar of chlorine
- Deflagrating spoon
- Digital devices
- Front Row Chemistry Grade 10 pg. 96
- Digital devices
- Pictures of applications

- Written exercises - Observation - Oral questions

Inorganic Chemistry

Periodicity - Physical properties of alkaline earth metals (atomic and ionic radii)
Periodicity - Physical properties of alkaline earth metals (appearance, hardness, conductivity)

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

- Describe trends in atomic and ionic radii of Group II elements
- Compare trends with Group I
- Relate atomic size to reactivity of calcium in bone formation

- Observe appearance of alkaline earth metals
- Test hardness and conductivity
- Connect magnesium's light weight to its use in aircraft alloys

- Observe trends in atomic and ionic radii
- Complete tables showing radii data
- Compare with Group I trends

- Observe appearance of magnesium and calcium
- Test hardness and ductility
- Test electrical conductivity

How do atomic sizes of Group II elements compare with Group I?
Why are alkaline earth metals harder than alkali metals?

- Front Row Chemistry Grade 10 pg. 98
- Periodic table
- Data tables

- Front Row Chemistry Grade 10 pg. 99
- Magnesium ribbon
- Calcium metal
- Circuit with bulb

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

Inorganic Chemistry

Periodicity - Physical properties of alkaline earth metals (melting points and ionisation energy)

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

- Describe trends in melting points and ionisation energy
- Compare first and second ionisation energies
- Relate ionisation energy to element reactivity in fireworks

- Study data on melting and boiling points
- Investigate ionisation energy trends
- Discuss factors affecting ionisation energy

Why do alkaline earth metals have higher ionisation energies than alkali metals?

- Front Row Chemistry Grade 10 pg. 102
- Data tables
- Digital devices

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Reaction of alkaline earth metals with air/oxygen

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

- Investigate reactions of Group II metals with oxygen
- Write balanced equations for the reactions
- Relate magnesium burning to its use in flares and fireworks

- Burn magnesium and calcium in air
- Observe products formed
- Write word and chemical equations

What products form when alkaline earth metals burn in air?

- Front Row Chemistry Grade 10 pg. 106
- Magnesium ribbon
- Calcium metal
- Bunsen burner

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of alkaline earth metals with water and steam

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

- Investigate reactions with water and steam
- Compare reactivity of magnesium and calcium
- Relate calcium hydroxide formation to lime water used in construction

- React magnesium and calcium with cold water
- React magnesium with steam
- Test gas produced and write equations

Why does magnesium react slowly with cold water but vigorously with steam?

- Front Row Chemistry Grade 10 pg. 107
- Magnesium, calcium
- Trough
- Steam apparatus

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of alkaline earth metals with chlorine and dilute acids
Periodicity - Applications of alkaline earth metals

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

- Describe reactions with chlorine gas
- Investigate reactions with dilute acids
- Relate magnesium chloride formation to uses in dust control on roads

- Identify uses of alkaline earth metals
- Relate properties to applications
- Connect calcium carbonate to cement production and antacid tablets

- React magnesium with chlorine gas
- React magnesium and calcium with dilute acids
- Write balanced equations

- Search for information on uses of alkaline earth metals
- Discuss applications of magnesium, calcium and barium
- Present findings to class

What products form when alkaline earth metals react with chlorine and acids?
How are alkaline earth metals used in medicine and industry?

- Front Row Chemistry Grade 10 pg. 110
- Magnesium ribbon
- Chlorine gas
- Dilute HCl and H₂SO₄

- Front Row Chemistry Grade 10 pg. 112
- Digital devices
- Pictures of applications

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

Inorganic Chemistry

Periodicity - Introduction to halogens

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

- Identify elements in the halogen family
- Describe electron configuration of halogens
- Relate halogen reactivity to their use in water treatment and disinfectants

- Determine chemical family of chlorine and fluorine
- Write electron configurations
- List other halogens

Why are halogens called "salt formers"?

- Front Row Chemistry Grade 10 pg. 114
- Periodic table
- Digital devices

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Periodicity - Laboratory preparation of chlorine gas

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

- Prepare chlorine gas in the laboratory
- Describe properties of chlorine gas
- Relate chlorine properties to its use in bleach and water purification

- Prepare chlorine gas from HCl and MnO₂
- Collect chlorine gas
- Observe properties of chlorine

How is chlorine gas prepared and collected safely?

- Front Row Chemistry Grade 10 pg. 115
- MnO₂, conc. HCl
- Round bottomed flask
- Gas jars

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Trends in physical properties of halogens (atomic radii, melting and boiling points)

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

- Describe trends in atomic radii of halogens
- Explain trends in melting and boiling points
- Relate physical state changes to molecular size and intermolecular forces

- Review atomic structure of halogens
- Study trends in physical properties
- Explain trends using intermolecular forces

Why do halogens change from gas to solid down the group?

- Front Row Chemistry Grade 10 pg. 117
- Data tables
- Periodic table

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Periodicity - Trends in physical properties of halogens (atomic radii, melting and boiling points)
Periodicity - Appearance, physical state and solubility of halogens

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

- Describe trends in atomic radii of halogens
- Explain trends in melting and boiling points
- Relate physical state changes to molecular size and intermolecular forces

- Describe appearance and physical states of halogens
- Investigate solubility in water and organic solvents
- Relate iodine's colour to its use as antiseptic in wound treatment

- Review atomic structure of halogens
- Study trends in physical properties
- Explain trends using intermolecular forces

- Observe appearance of chlorine, bromine and iodine
- Test solubility in water
- Compare solubility of halogens

Why do halogens change from gas to solid down the group?
Why do halogens have different colours and physical states?

- Front Row Chemistry Grade 10 pg. 117
- Data tables
- Periodic table

- Front Row Chemistry Grade 10 pg. 118
- Bromine, iodine samples
- Distilled water
- Test tubes

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

Inorganic Chemistry

Periodicity - Electrical conductivity of halogens

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

- Investigate electrical conductivity of halogens
- Explain why halogens do not conduct electricity
- Contrast halogen non-conductivity with metal conductivity in wiring

- Test electrical conductivity of iodine crystals
- Discuss results in terms of structure
- Compare with ionic and metallic substances

Why don't halogens conduct electricity?

- Front Row Chemistry Grade 10 pg. 120
- Iodine crystals
- Circuit with bulb
- Beaker

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Electron affinity and ion formation of halogens

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

- Define electron affinity
- Explain trends in electron affinity down Group VII
- Relate electron affinity to halogen reactivity in forming salts

- Understand how halogen atoms form ions
- Discuss electron affinity values
- Explain trend down the group

Why does electron affinity decrease down Group VII?

- Front Row Chemistry Grade 10 pg. 121
- Data tables
- Digital devices

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Reaction of halogens with metals

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

- Investigate reactions of halogens with metals
- Write balanced equations for the reactions
- Relate iron chloride formation to industrial rust prevention

- React chlorine with iron and zinc
- Observe products formed
- Write balanced equations

What happens when halogens react with metals?

- Front Row Chemistry Grade 10 pg. 122
- Iron filings
- Chlorine gas
- Combustion tube

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of chlorine with water
Periodicity - Displacement reactions of halogens

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

- Investigate reaction of chlorine with water
- Describe bleaching action of chlorine water
- Relate chlorine water to swimming pool disinfection

- Investigate displacement reactions of halogens
- Explain order of reactivity of halogens
- Apply displacement reactions to understand water purification processes

- Prepare chlorine water
- Test with litmus paper
- Investigate decomposition in sunlight

- Add chlorine water to potassium bromide and iodide solutions
- Observe colour changes
- Write ionic equations

How does chlorine react with water and why is it used as a bleach?
Why can chlorine displace bromine and iodine from their salts?

- Front Row Chemistry Grade 10 pg. 124
- Chlorine gas
- Distilled water
- Litmus paper

- Front Row Chemistry Grade 10 pg. 125
- Chlorine, bromine water
- KBr, KI solutions
- Test tubes

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Applications of halogens

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

- Identify uses of halogens
- Relate properties to applications
- Connect fluoride in toothpaste to dental health protection

- Search for information on uses of halogens
- Discuss applications of F, Cl, Br and I
- Present findings to class

How are halogens used in water treatment, medicine and industry?

- Front Row Chemistry Grade 10 pg. 127
- Digital devices
- Product samples

- Oral questions - Written exercises - Group presentations

Inorganic Chemistry

Periodicity - Introduction to noble gases

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

- Identify noble gases and their electron configurations
- Explain why noble gases are chemically inert
- Relate noble gas stability to their use in light bulbs and balloons

- Determine electronic configuration of noble gases
- Discuss stability of full electron shells
- List noble gas elements

Why are noble gases unreactive?

- Front Row Chemistry Grade 10 pg. 128
- Periodic table
- Digital devices

- Oral questions - Written exercises - Observation

Inorganic Chemistry

Periodicity - Trends in physical properties of noble gases

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

- Describe trends in physical properties of noble gases
- Explain trends in ionisation energy
- Relate noble gas properties to neon signs and helium balloons

- Review atomic structure of noble gases
- Study trends in atomic radii and ionisation energy
- Discuss reactivity based on electron configuration

Why do noble gases have very high ionisation energies?

- Front Row Chemistry Grade 10 pg. 129
- Data tables
- Periodic table

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Periodicity - Applications of noble gases
Periodicity - Introduction to Period 3 elements

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

- Identify uses of noble gases
- Relate properties to applications
- Connect argon's inertness to its use in welding and light bulbs

- Identify Period 3 elements and their properties
- Classify elements as metals, metalloids or non-metals
- Relate Period 3 elements to common materials like aluminium foil and silicon chips

- Search for information on uses of noble gases
- Discuss applications of He, Ne and Ar
- Present findings to class

- List Period 3 elements from Na to Ar
- Discuss bonding and structure of each element
- Classify elements by type

How are noble gases used despite being unreactive?
What elements are found in Period 3 and how do their properties vary?

- Front Row Chemistry Grade 10 pg. 131
- Digital devices
- Pictures of applications

- Front Row Chemistry Grade 10 pg. 131
- Periodic table
- Element samples

- Oral questions - Written exercises - Group presentations
- Oral questions - Written exercises - Observation

Inorganic Chemistry

Periodicity - Trends in atomic radii across Period 3

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

- Describe trends in atomic radii across Period 3
- Explain reasons for the observed trend
- Relate atomic size to element reactivity in sodium vs chlorine

- Study data on atomic radii of Period 3 elements
- Plot graph of atomic radius vs atomic number
- Explain trend using nuclear charge

Why does atomic radius decrease across Period 3?

- Front Row Chemistry Grade 10 pg. 132
- Data tables
- Graph paper

- Written exercises - Graphical work - Oral questions

Inorganic Chemistry

Periodicity - Trends in ionisation energy across Period 3

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

- Describe trends in ionisation energy across Period 3
- Explain factors affecting ionisation energy
- Relate ionisation energy to metallic character of sodium vs non-metallic chlorine

- Study ionisation energy data for Period 3
- Discuss trend and anomalies
- Explain using atomic structure

Why does ionisation energy generally increase across Period 3?

- Front Row Chemistry Grade 10 pg. 133
- Data tables
- Digital devices

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Trends in melting and boiling points across Period 3

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

- Describe trends in melting and boiling points across Period 3
- Explain trends using structure and bonding
- Relate silicon's high melting point to its use in computer chips

- Study data on melting and boiling points
- Relate trends to bonding and structure
- Explain anomalies

Why does silicon have the highest melting point in Period 3?

- Front Row Chemistry Grade 10 pg. 134
- Data tables
- Charts

- Written exercises - Oral questions - Observation

Inorganic Chemistry

Periodicity - Electron affinity and electronegativity across Period 3

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

- Define electron affinity and electronegativity
- Describe trends across Period 3
- Relate electronegativity to bond polarity in water molecules

- Discuss electron affinity trends
- Study electronegativity values across Period 3
- Explain factors affecting these properties

Why does electronegativity increase across Period 3?

- Front Row Chemistry Grade 10 pg. 135
- Data tables
- Digital devices

- Written exercises - Oral questions - Individual assessment

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with oxygen (Na, Mg, Al)

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

- Investigate reactions of Na, Mg and Al with oxygen
- Write balanced equations for the reactions
- Relate magnesium oxide formation to its use in antacids and refractory materials

- Burn sodium, magnesium and aluminium in air
- Observe products formed
- Write word and chemical equations

What products form when Period 3 metals burn in oxygen?

- Front Row Chemistry Grade 10 pg. 136
- Na, Mg, Al samples
- Bunsen burner
- Deflagrating spoon

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with oxygen (Si, P, S)

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

- Describe reactions of Si, P and S with oxygen
- Write balanced equations for the reactions
- Relate sulphur dioxide formation to air pollution and acid rain

- Discuss reactions of silicon and phosphorus with oxygen
- Burn sulphur in oxygen
- Write balanced equations

What products form when Period 3 non-metals burn in oxygen?

- Front Row Chemistry Grade 10 pg. 136
- Sulphur powder
- Gas jar of oxygen
- Deflagrating spoon

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with chlorine (Na, Mg, Al)

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

- Investigate reactions of Period 3 metals with chlorine
- Write balanced equations for the reactions
- Relate aluminium chloride to its use as catalyst in industry

- React sodium, magnesium and aluminium with chlorine
- Observe products formed
- Write balanced equations

What happens when Period 3 metals react with chlorine?

- Front Row Chemistry Grade 10 pg. 137
- Na, Mg samples
- Chlorine gas
- Deflagrating spoon

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with chlorine (Si, P)
Periodicity - Reaction of Period 3 elements with water (Na, Mg)

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

- Describe reactions of Si and P with chlorine
- Write balanced equations for the reactions
- Relate silicon tetrachloride to semiconductor manufacturing

- Investigate reactions of sodium and magnesium with water
- Compare reactivity of the two metals
- Relate sodium hydroxide formation to soap making

- Discuss reactions of silicon and phosphorus with chlorine
- Write balanced equations
- Compare metal and non-metal chlorides

- React sodium and magnesium with cold water
- React magnesium with steam
- Write balanced equations

What are the products when Period 3 non-metals react with chlorine?
Why does sodium react more vigorously with water than magnesium?

- Front Row Chemistry Grade 10 pg. 138
- Reference materials
- Digital devices

- Front Row Chemistry Grade 10 pg. 140
- Sodium, magnesium
- Trough with water
- Phenolphthalein

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

Inorganic Chemistry

Periodicity - Reaction of Period 3 elements with dilute acids

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

- Investigate reactions of Period 3 metals with dilute acids
- Write balanced equations for the reactions
- Relate hydrogen gas production to laboratory gas collection techniques

- React magnesium and aluminium with dilute HCl and H₂SO₄
- Test gas produced
- Write balanced equations

What products form when Period 3 metals react with dilute acids?

- Front Row Chemistry Grade 10 pg. 139
- Mg ribbon
- Dilute HCl, H₂SO₄
- Test tubes

- Practical assessment - Written exercises - Observation

Inorganic Chemistry

Periodicity - Comparison of trends across Period 3 and down groups

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

- Compare periodic trends across periods and down groups
- Summarise factors affecting periodic properties
- Apply periodic trends to predict element behaviour in new materials

- Compare trends across Period 3 with trends down groups
- Create summary tables of periodic trends
- Discuss patterns and exceptions

How do trends across a period differ from trends down a group?

- Front Row Chemistry Grade 10 pg. 141
- Summary charts
- Periodic table

- Written exercises - Oral questions - Individual assessment