Science Exam Preparation

Write shell electron configurations for neutral atoms among the first 20 elements.

Determine the number of valence electrons from an element’s shell electron configuration.

Use electron configuration to determine an element’s period and main-group family.

Predict the charge and electron configuration of a common monatomic ion formed by a Group 1, Group 2, Group 6, or Group 7 element.

Explain why Group 1 metals become more reactive down the group using electron-shell structure.

Explain why Group 7 non-metals become less reactive down the group using electron-shell structure.

Predict the outcome of a Group 7 displacement reaction from the halogen reactivity pattern.

Determine the charges of common monatomic ions from their periodic-table groups.

Use the swap method and simplify charge ratios to construct a neutral ionic formula.

Derive the formula of a binary ionic compound from its name.

Name a binary ionic compound from its formula.

Balance a simple chemical equation by changing coefficients without changing chemical formulas.

Explain ionic bond formation as electron transfer followed by electrostatic attraction between oppositely charged ions.

Draw an electron-transfer diagram for a simple ionic compound.

Relate the giant ionic lattice to an ionic compound’s melting point and electrical conductivity when solid or molten.

Explain covalent bond formation as the sharing of electron pairs between non-metal atoms.

Draw electron-sharing diagrams for simple covalent molecules.

Name binary molecular compounds using numerical prefixes and derive their formulas from their names.

Relate the particle structure of a simple molecular substance to its typical melting point and electrical conductivity.

Explain the hardness and high melting point of diamond from its giant covalent structure.

Explain graphite’s electrical conductivity and softness from its bonding and layered structure.

Distinguish simple molecular, giant covalent, ionic, and metallic structures using property data.

Explain metallic bonding using a lattice of positive ions and delocalised electrons, and use it to account for conductivity, malleability, and ductility.

Use particle theory to compare the arrangement and movement of particles in solids, liquids, and gases.

Define reaction rate in terms of a measurable change in reactant or product quantity over time.

Explain the occurrence of a reaction using collision frequency and successful collisions.

Calculate and compare average reaction rates from experimental measurements.

Interpret a reaction-progress graph to compare rates and identify when a reaction is complete.

Explain why increasing a solid reactant’s surface area increases reaction rate using collision theory.

Explain how a catalyst increases reaction rate and remains chemically unchanged.

Plan a fair investigation of the effect of surface area or a catalyst on reaction rate by identifying variables and suitable measurements.

Arrange selected metals in a reactivity series using observations from reactions with water, acids, or metal-ion solutions.

Predict whether a selected metal will react with water or dilute acid using its position in the reactivity series.

Predict and explain whether a metal-displacement reaction will occur.

Write and balance symbol equations for simple metal reactions with oxygen, acids, or metal compounds.

Choose whether a metal is found native, extracted by carbon reduction, or extracted by electrolysis based on its reactivity.

Explain the extraction of a metal below carbon in the reactivity series as reduction of its oxide by carbon.

Explain why metals above carbon in the reactivity series require electrolysis for extraction.

Write the thermal decomposition equation for calcium carbonate and use its products to explain observed mass change and a positive carbon-dioxide test.

Interpret the demands of the command words identify, describe, explain, compare, predict, and justify in chemistry questions.

Construct a full-mark short response that links chemical observations to particle-level or electron-level reasoning.

Apply atomic structure, bonding, rates, and reactivity knowledge to unfamiliar tables, graphs, and experimental scenarios.

Complete a timed mixed-format practice set covering the full topic list.

Classify errors from practice questions as knowledge, calculation, interpretation, or exam-technique errors and select a correction strategy.