Essential Chemistry Concepts for A-Level Success
Periodic table trends follow predictable patterns that make chemistry much easier to understand. As you move across a period, covalent radius decreases because more protons create stronger nuclear charge, pulling electrons closer. Moving down a group increases radius due to additional electron shells.
Ionisation energy and electronegativity both increase across periods moreprotons=strongerpull but decrease down groups (more shielding from inner electrons). This pattern explains why Group 7 elements are excellent oxidising agents - they desperately want to gain electrons.
Activation energy determines reaction speed - it's the minimum kinetic energy particles need to react successfully. Lower activation energy means faster reactions, which is why catalysts are so useful in industry.
Bonding types depend on electronegativity differences. Non-polar covalent bonds form between identical atoms, whilst polar covalent bonds create slight charges due to unequal electron sharing. These differences affect everything from boiling points to solubility.
Quick Tip: Remember that intermolecular forces are the weak attractions between molecules - they're what you're breaking when substances melt or boil, not the actual chemical bonds!
Enthalpy changes show energy differences between reactants and products. Exothermic reactions have negative values (energy released), whilst endothermic reactions are positive (energy absorbed). The activated complex represents the unstable transition state at an energy diagram's peak.
Chromatography separates mixtures based on solubility differences. In paper chromatography, compounds that travel furthest are most soluble in the mobile phase. Gas-liquid chromatography uses retention time instead - peak height indicates concentration.
Redox reactions involve electron transfer. Oxidising agents gain electrons (get reduced), whilst reducing agents lose electrons (get oxidised). Common examples include hydrogen peroxide for disinfection and carbon monoxide in metal extraction.