Edexcel International GCSE Chemistry Revision Notes on Key Topics

Free Chemistry Revision Guide

• Available on the provided website, facilitating easy tracking of revision progress through checkable sections.
• Links to teaching videos and free multiple-choice questions for further study.
• Predicted papers and video walkthroughs for this year's exams are also available.

Atomic Structure

• Atoms consist of protons, neutrons, and electrons.
• Protons: Located in the nucleus, mass of 1, charge of +1.
• Neutrons: Located in the nucleus, mass of 1, charge of 0.
• Electrons: Located in outer shells, negligible mass, charge of -1.
• The relative charge is utilized for simplicity; actual charges measured in coulombs are substantially small.
• Atomic models evolved over time from the "blob" to the current electron shell model.

Periodic Table and Isotopes

• Elements in the periodic table are arranged by increasing atomic number, not mass.
• Isotopes have the same number of protons but different numbers of neutrons, affecting their physical but not chemical properties.
• Atomic number (Z): Number of protons.
• Mass number (A): Sum of protons and neutrons, resulting in the average mass of naturally occurring isotopes.

Bonding and Structure

• Ionic bonding: Involves the transfer of electrons from metals to non-metals, forming positively and negatively charged ions.
• Covalent bonding: Involves the sharing of electron pairs between non-metals.
• Molecular shapes and angles are determined by the electron pairs around the central atom, influenced by the VSEPR theory.

Ions and Ionic Compounds

• Metals lose electrons to form positive ions; non-metals gain electrons to form negative ions.
• Ionic compounds arrange in a lattice structure, exhibiting high melting and boiling points, solubility in water, and electrical conductivity when molten or in solution.

Chemical Calculations

• Relative molecular mass and atomic mass: Reference standard is 1/12th of the mass of a carbon-12 atom.
• The mole concept: Relates the mass of substance to the quantity of matter, utilizing Avogadro's number for conversions between moles and particles.

Kinetics and Equilibria

• Reaction rates are influenced by temperature, concentration, presence of catalysts, and surface area.
• Dynamic equilibrium: Occurs in closed systems where the rates of forward and backward reactions are equal.
• Le Chatelier's principle: A system at equilibrium will adjust to counteract changes imposed on it.

Organic Chemistry Basics

• Introduction to hydrocarbons, naming conventions (alkanes, alkenes), and the importance of functional groups in determining chemical properties and reactions.

Environmental Impact of Chemistry

• Combustion reactions: Concerns over CO2 and SO2 emissions, contributing to global warming and acid rain.
• Sustainable chemistry: Emphasizes recycling, green chemistry practices, and the reduction of harmful by-products.

These summarised notes cover crucial topics within the Edexcel International GCSE Chemistry curriculum, offering foundational knowledge essential for exam preparation.