Course Overview

This chemistry paper focuses on three core areas that'll give you a solid foundation for understanding how matter works. You'll explore particles and their behaviour, learn about elements and compounds, and discover how chemical reactions actually happen.

The course also includes practical skills that you'll use in lab work and exams. These hands-on techniques are just as important as the theory because they show you how chemistry works in the real world.

Quick tip: Each section builds on the previous one, so make sure you understand particles before moving on to compounds and reactions.

States of Matter and Atomic Structure

States of matter behave differently because of how their particles move and attract each other. In solids, particles vibrate in fixed positions with strong attractions. Liquids have particles that move freely but stay close together, while gases have particles zooming around in straight lines with no attractions at all.

An atom is incredibly tiny - about 1×10⁻¹⁰m across! Inside each atom, you'll find protons (positive charge, mass of 1), neutrons (no charge, mass of 1), and electrons (negative charge, almost no mass). The number of protons always equals the number of electrons in a neutral atom.

Scientists like Democritos, Dalton, Thomson, Rutherford, and Bohr gradually discovered atomic structure over time. Bohr's model shows us that electrons live in shells around the nucleus, and they can only move in fixed orbits - they can't just exist anywhere they fancy.

Remember: Mass number = protons + neutrons, whilst atomic number = just the protons (which also equals electrons).

Chemical Bonding and the Periodic Table

The periodic table is brilliantly organised - groups (vertical columns) tell you how many electrons are in the outer shell, whilst periods (horizontal rows) show how many electron shells an atom has. The first shell holds 2 electrons, and the second and third shells each hold 8.

Ionic bonding happens between metals and non-metals when electrons transfer from one atom to another. For example, sodium (2.8.1) gives its outer electron to chlorine (2.8.7), creating charged ions that attract each other. This typically occurs between groups 1-2 and groups 6-7.

Covalent bonds form when non-metals share electrons to complete their outer shells. Hydrogen gas (H₂) is a perfect example - two hydrogen atoms each contribute one electron to share. Metallic bonds give metals their high melting points and electrical conductivity, though pure metals are often mixed with other elements to create stronger alloys.

Key insight: The type of bonding determines the properties - ionic and metallic compounds have high melting points, whilst simple covalent compounds have low melting points.

Separation Techniques

Distillation separates liquid mixtures by using different boiling points. Simple distillation works for liquids with very different boiling points (like separating water from salt), whilst fractional distillation handles liquids with similar boiling points by using a fractionating column.

The process is straightforward: heat the mixture, collect the vapour in a condenser cooled by cold water, then gather the pure liquid in a beaker. The substance with the lowest boiling point evaporates first, leaving behind anything with higher boiling points.

Pure substances have specific melting and boiling points, which is how you can identify them. If you've got a mixture of more than one compound, these temperatures will be different from the pure substance values.

Lab tip: Always run cold water through the condenser to ensure proper condensation - hot water won't cool the vapour effectively.

More Separation Methods and Chemical Formulas

Filtration separates insoluble solids from liquids using filter paper in a funnel - the liquid passes through whilst the solid residue stays behind. Crystallisation gets soluble solids out of solutions by gently heating until crystals start forming, then cooling to let more crystals grow.

Chromatography separates mixtures by how far different substances travel up paper with a solvent. You calculate the Rf value using: distance travelled by solute ÷ distance travelled by solvent. Always draw your starting line in pencil (it won't dissolve) and don't let the solvent touch your sample spot directly.

Chemical formulas show the actual number of atoms in molecules (like CH₄ for methane), whilst empirical formulas give the simplest ratio of atoms. For example, C₄H₈Cl₂ has the empirical formula C₂H₄Cl.

Chromatography hack: Different substances travel different distances because they have varying attractions to the paper and solvent.

Chemical Reactions and Calculations

Conservation of mass means no matter disappears or appears during chemical reactions. If the mass seems to change, it's usually because gases are involved - mass increases when gas reactants from air join in, and decreases when gas products escape.

Moles help you count particles (6.022×10²³ particles = 1 mole). Calculate moles using: mass in grams ÷ Mr (relative molecular mass). You can also work out concentration using: mass of solute ÷ volume of solution, or moles ÷ volume.

Remember that diatomic molecules like H₂, Cl₂, and O₂ always exist as pairs in nature. Chemical equations show reactants turning into products, and you'll need to balance them properly whilst using state symbols: $s$ solid, $l$ liquid, $g$ gas, (aq) dissolved in water.

Limiting reactants: Reactions stop when one reactant runs out - this is your limiting reactant, whilst leftovers are called excess reactants.