SSS 1

Lesson 1 · Chemistry and the Chemical Industry

• •Define Chemistry and explain its role in various professional fields in Nigeria.
• •Identify common laboratory apparatus and state their specific uses in chemical experiments.

Lesson 2 · Standard Laboratory Practices and Safety Rules

• •Explain the scientific method as an organized approach to solving chemical problems.
• •Discuss the importance of safety rules and regulations in a Chemistry laboratory.

Lesson 3 · Physical and Chemical Changes and Their Impacts

• •Distinguish between physical and chemical changes using combustion and melting as examples.
• •Evaluate the adverse effects of chemical processes on the Nigerian environment.

Lesson 4 · Careers in Chemistry and Industry Applications

• •Explain the career opportunities available to students of Chemistry in Nigeria.
• •Identify various chemical industries and their primary products.

Lesson 5 · The Bunsen Burner and Laboratory Equipment

• •Identify the basic parts of the Bunsen burner and their functions.
• •Demonstrate how to light and adjust a Bunsen burner safely.

Lesson 1 · Physical States of Matter and Kinetic Theory

• •Describe the three physical states of matter using the kinetic theory.
• •Compare the properties of solids, liquids, and gases.

Lesson 2 · Phase Changes: Melting, Boiling, and Sublimation

• •Demonstrate the process of melting and evaporation using water as a sample.
• •Explain the concept of sublimation using naphthalene or ammonium chloride.

Lesson 3 · Classification of Matter: Pure Substances and Mixtures

• •Distinguish between pure substances and mixtures with local examples like salt water.
• •Classify substances as elements, compounds, or mixtures.

Lesson 4 · Criteria for Purity in Matter

• •Explain the concept of boiling point and how impurities affect it.
• •Describe how melting point can be used to determine the purity of solids.

Lesson 5 · Heating and Cooling Curves of Matter

• •Construct a cooling curve for a pure substance to show temperature changes.
• •Interpret heating curves for different states of matter.

Lesson 1 · Evidence for Carbon Particles: Diffusion and Osmosis

• •Explain the evidence for the particulate nature of matter through diffusion.
• •Demonstrate osmosis using a local yam tuber or semi-permeable membrane.

Lesson 2 · Atoms, Molecules, and Ions as Basic Particles

• •Describe the basic structure of the atom as the smallest unit of matter.
• •Define molecules and ions as distinct types of chemical species.

Lesson 3 · The Kinetic Theory of Matter Application

• •Explain the relationship between molecular motion and temperature.
• •Describe the arrangement of particles in different states of matter.

Lesson 4 · Diffusion and Brownian Motion Demonstration

• •Calculate the rate of diffusion for different gases using Graham's Law basics.
• •Observe and explain Brownian motion using smoke particles or pollen grains.

Lesson 5 · Intermolecular Forces and Thermal Expansion

• •Explain why substances expand or contract based on particle movement.
• •Describe the forces of attraction between particles in solids and liquids.

Lesson 1 · Basic Separation: Filtration, Evaporation, and Use of Separating Funnels

• •Explain the principles of filtration and evaporation in recovering salt from sand.
• •Demonstrate the use of a separating funnel for immiscible liquids.

Lesson 2 · Distillation Processes and Industrial Applications in Nigeria

• •Describe the process of simple distillation for obtaining pure water from salt solution.
• •Explain the industrial use of fractional distillation in Nigerian oil refineries.

Lesson 3 · Chromatography: Types and Principles of Separation

• •Demonstrate paper chromatography to separate pigments in local flowers or ink.
• •Explain the principle of Rf values in identifying separated components.

Lesson 4 · Advanced Techniques: Sublimation and Magnetization

• •Describe the process of sublimation for purifying iodine or ammonium chloride.
• •Explain the use of magnetization in separating iron filings from sulphur.

Lesson 5 · Crystallization and Large-Scale Water Purification

• •Explain the steps involved in the large-scale purification of town water.
• •Demonstrate crystallization as a technique for recovering pure salt from brine.

Lesson 1 · Sub-atomic Particles: Protons, Neutrons, and Electrons

• •Identify the three sub-atomic particles and their locations in the atom.
• •Describe the properties of protons, neutrons, and electrons (mass and charge).

Lesson 2 · Atomic Number and Mass Number Calculations

• •Define atomic number and mass number of an element.
• •Calculate the number of neutrons in an atom given mass and atomic numbers.

Lesson 3 · Isotopes and Relative Atomic Mass Calculation

• •Explain the concept of isotopes using Carbon and Chlorine as examples.
• •Calculate the relative atomic mass of elements with multiple isotopes.

Lesson 4 · Development of the Atomic Theory and Models

• •Describe Dalton’s atomic theory and its modern modifications.
• •Explain the contribution of Rutherford and Bohr to atomic models.

Lesson 5 · Atomic Structure and Nuclear Composition

• •Define nucleons and their relevance to atomic mass.
• •Draw simple atomic diagrams showing the nucleus and electron shells.

Lesson 1 · Energy Levels and Shell Notation (K, L, M)

• •Explain the K, L, M, and N shell arrangement for electrons.
• •Write the electronic configuration of the first 20 elements using shell notation.

Lesson 2 · Atomic Orbitals: S, P, D, F Sub-levels

• •Identify the shapes of s and p orbitals in an atom.
• •Describe the maximum capacity of s, p, d, and f sub-levels.

Lesson 3 · Aufbau Principle and Sub-shell Configuration

• •Apply the Aufbau principle to write configurations for the first 30 elements.
• •Explain Pauli’s exclusion principle and Hund’s rule of maximum multiplicity.

Lesson 4 · Electronic Configuration and the Periodic Table Relationship

• •Determine the group and period of an element from its electronic configuration.
• •Identify valence electrons and their significance in chemical reactions.

Lesson 5 · Orbital Diagrams and Sub-shell Stability

• •Illustrate orbital diagrams using boxes and arrows for nitrogen and oxygen.
• •Explain the stability of half-filled and completely filled sub-shells.

Lesson 1 · History and Structure of the Periodic Table

• •Describe the historical development of the periodic table by Mendeleev and Moseley.
• •Explain the arrangement of elements in groups and periods.

Lesson 2 · Periodic Trends: Atomic Radius and Electronegativity

• •Explain the trend of atomic radius across a period and down a group.
• •Compare the electronegativity of elements across the periodic table.

Lesson 3 · Ionization Energy and Electron Affinity Trends

• •Define ionization energy and explain its variation across periods.
• •Describe the trend of electron affinity within the periodic table.

Lesson 4 · Properties of Chemical Families and Groups

• •Identify the chemical properties of Group 1 (Alkali Metals) and Group 2.
• •Describe the characteristics of transition elements and noble gases.

Lesson 5 · Reactivity Patterns in the Periodic Table

• •Predict the reactivity of metals and non-metals based on their periodic position.
• •Compare the diagonal relationship between certain elements in the second and third periods.

Lesson 1 · Electrovalent (Ionic) Bonding and Properties

• •Explain the formation of electrovalent (ionic) bonds through electron transfer.
• •Describe the properties of ionic compounds using sodium chloride as an example.

Lesson 2 · Covalent Bonding: Shared Electron Pairs

• •Explain the formation of covalent bonds through shared pairs of electrons.
• •Distinguish between single, double, and triple covalent bonds with examples.

Lesson 3 · Coordinate Covalent and Metallic Bonding

• •Describe the formation of coordinate (dative) covalent bonds.
• •Illustrate dative bonding using the ammonium ion ($NH_4^+$) as a case study.

Lesson 4 · Intermolecular Forces: Hydrogen Bonding and Van der Waals

• •Explain the nature of hydrogen bonding and its effect on boiling points.
• •Identify substances that exhibit Van der Waals forces.

Lesson 5 · Predicting Bond Types and Lewis Structures

• •Predict the type of bond formed between two elements using electronegativity differences.
• •Draw Lewis dot structures for simple molecules like $H_2O$ and $CO_2$.

Lesson 1 · The Mole Concept and Molar Mass Calculation

• •Define the mole as a unit of measurement for amount of substance.
• •Calculate the molar mass of simple compounds like $CaCO_3$ and $NaCl$.

Lesson 2 · Avogadro’s Number and Particle Conversions

• •Apply Avogadro’s constant to determine the number of particles in a sample.
• •Solve problems involving the conversion between mass, moles, and number of particles.

Lesson 3 · Empirical and Molecular Formula Calculations

• •Determine the empirical formula of a compound from percentage composition data.
• •Calculate the molecular formula given the empirical formula and relative molecular mass.

Lesson 4 · Percentage Composition and Molar Volume of Gases

• •Calculate the percentage by mass of an element within a compound.
• •Solve problems involving molar volume of gases at S.T.P. and R.T.P.

Lesson 5 · Molar Concentration and Solution Dilution

• •Calculate the concentration of solutions in $mol/dm^3$ and $g/dm^3$.
• •Solve dilution problems to determine the final concentration of a solution.

Lesson 1 · Symbols, Formulas, and Word Equations

• •Identify the symbols used in chemical equations (s, l, g, aq).
• •Write word equations and convert them into symbols and formulas.

Lesson 2 · Balancing Chemical Equations: Inspection Method

• •Apply the Law of Conservation of Mass to balance chemical equations.
• •Balance complex redox and non-redox equations using the inspection method.

Lesson 3 · Stoichiometry of Reacting Masses

• •Interpret chemical equations in terms of moles, mass, and gas volume.
• •Calculate reacting masses of reactants and products in a chemical reaction.

Lesson 4 · Stoichiometry of Reacting Volumes and Limiting Reactants

• •Solve problems involving gas volumes in reactions using molar volume constants.
• •Identify the limiting reactant in a chemical reaction through stoichiometric calculations.

Lesson 5 · Percentage Yield and Chemical Efficiency

• •Calculate the percentage yield and theoretical yield of a chemical process.
• •Explain the importance of atom economy in Nigerian industrial production.

Lesson 1 · Boyle’s Law: Pressure and Volume Relationship

• •Explain the relationship between volume and pressure using Boyle’s Law.
• •Solve mathematical problems involving Boyle’s Law with pressure-volume units.

Lesson 2 · Charles’s Law: Temperature and Volume Relationship

• •State Charles’s Law and explain the effect of temperature on gas volume.
• •Calculate gas volumes at different temperatures using the Kelvin scale.

Lesson 3 · The General Gas Law Calculations

• •Derive and apply the General Gas Law equation for changing conditions.
• •Solve problems involving pressure, volume, and temperature simultaneously.

Lesson 4 · Ideal Gas Law and the Gas Constant R

• •State the Ideal Gas Law ($PV = nRT$) and define the gas constant.
• •Calculate the number of moles or pressure of an ideal gas.

Lesson 5 · Graham’s and Dalton’s Laws of Gases

• •State Graham's Law of diffusion and Dalton's Law of partial pressures.
• •Calculate the partial pressure of a gas in a mixture of gases.

Lesson 1 · Definitions and Properties of Acids and Bases

• •Define acids and bases according to Arrhenius and Bronsted-Lowry theories.
• •Distinguish between strong and weak acids using local examples like lime juice.

Lesson 2 · The pH Scale and Chemical Properties of Acids

• •Describe the physical and chemical properties of acids, including reactions with metals.
• •Explain the pH scale and its use in measuring acidity and alkalinity.

Lesson 3 · Classification of Oxides and Properties of Bases

• •Identify various types of oxides (acidic, basic, amphoteric, neutral).
• •Explain the preparation and properties of common bases like NaOH and $Ca(OH)_2$.

Lesson 4 · Preparation and Classification of Salts

• •Define a salt and list the methods of preparing soluble salts.
• •Describe the preparation of insoluble salts by double decomposition (precipitation).

Lesson 5 · Neutralization Reactions and Applications of Salts

• •Explain the process of neutralization and its application in treating soil acidity.
• •Identify the uses of common salts in Nigerian domestic and industrial sectors.