Grade 10 Chemistry Scheme of Work

Chemistry Scheme of Work

• This document outlines the first term's chemistry syllabus for Grade 10 students at Princeton College, Lagos.
• The scheme covers topics from Introduction to Chemistry to Examination, spread across 13 weeks.

Weekly Topics

• Week 1: Introduction to Chemistry (defining chemistry, branches, careers, relevance)
• Week 2: Familiarization of Apparatus in the Chemistry Laboratory
• Week 3: Physical and Chemical Changes
• Week 4: Elements, Atoms, and Molecules
• Week 5: Relative Atomic Mass (defining relative atomic mass and isotopes)
• Week 6: Compounds
• Week 7: (Missing week 7 information)
• Week 8: Nomenclature of compounds (rules for assigning oxidation numbers, naming inorganic compounds)
• Week 9: Mixtures (defining mixtures, types, examples of homogenous and heterogeneous mixtures including colloids and suspensions)
• Week 10: Separation Techniques (filtration, evaporation, simple distillation, fractional distillation, chromatography)
• Weeks 11-12 (Missing week information)
• Week 13: Examination

Introduction to Chemistry (Week 1)

• Chemistry is the study of the composition, properties, structures, uses, physical and chemical changes in matter.
• Chemistry is a science because it uses the scientific method (observation, hypothesis, testing).
• Branches of chemistry: Analytical, Biochemistry, Industrial, Nuclear (Radioactive), Physical, Organic.
• Careers related to Chemistry: Education (teachers, lecturers, lab assistants), Manufacturing (industrial chemists), Agriculture (agricultural chemists), Healthcare (pharmacists, doctors, nurses, medical biochemists), Petroleum (chemical engineers, petrochemical engineers, research chemists ), Food processing (food technologists).

Laboratory Apparatus (Week 2)

• Laboratory apparatus are made of glass, porcelain, plastic or metal.
• Glassware is used for storing reagents and boiling or collecting chemicals.
• Porcelain is used for experiments requiring prolonged heating.
• Plastics are used for apparatus not affected by dilute acids or alkalis.
• Specific examples of apparatus: test tubes, test tube racks, test tube holders, reagent bottles, beakers, Bunsen burners, stands and clamps, measuring cylinders, crucibles, droppers, evaporating dishes, flat bottomed flasks, mortar and pestles, spatulas, filter funnels, safety glasses, round bottomed flasks, tripods, etc.

Physical and Chemical Changes (Week 3)

• Physical changes alter the physical state of a substance but not its composition (e.g., melting, dissolving).
• Chemical changes result in the formation of new substances due to a change in composition (e.g., burning, rusting).
• Matter exists in three states (solid, liquid, gas, plasma)

Elements, Atoms, and Molecules (Week 4)

• An element is a substance that cannot be broken down into simpler substances.
• Examples: Hydrogen, Oxygen, Nitrogen, Carbon, Calcium, Iron
• An atom is the smallest unit of an element that can participate in a chemical reaction.
• Atoms are made of subatomic particles (protons, neutrons, electrons).
• A molecule is a group of atoms bonded together.
• Elements can exist as molecules (diatomic, or monoatomic).

Relative Atomic Mass and Isotopes (Week 5)

• Relative atomic mass (Ar): The mass of an atom compared to the mass of an arbitrary reference atom.
• Isotopes: Atoms of the same element with different mass numbers (different number of neutrons) but the same atomic number.
• Relative atomic mass is calculated using isotopic abundance and mass numbers.

Compounds (Week 6)

• A compound is a substance formed by the chemical combination of two or more different elements.
• Examples of compounds include water (H₂O), sodium chloride (NaCl), glucose (C₆H₁₂O₆).
• Compounds are represented by chemical formulas that show the elements and their ratios.

Nomenclature of Compounds (Week 8)

• Rules for naming compounds: use IUPAC guidelines
• Rules for oxidation numbers (important for naming compounds)
• Rules for binary (2-element) and oxy-compounds.

Mixtures (Week 9)

• A mixture is a combination of two or more substances physically combined.
• Mixtures can be homogeneous (uniform composition) or heterogeneous (non-uniform composition).
• Examples of mixtures: saltwater (homogeneous), sand and water (heterogeneous)
• Types of mixtures include: suspensions, colloids, solutions

Separation Techniques (Week 10)

• Techniques used to separate mixtures: filtration, evaporation, simple distillation, fractional distillation, chromatography.
• Techniques are based on differences in physical properties (boiling points, solubility etc) of the components in a mixture.