Paper 1

• Atomic Structure


  number of protons (or electrons in an element)
• Mass Number


  number of protons plus neutrons
• Isotope


  atoms of the same element that have different number of neutrons
• Relative Atomic Mass


  the average mass of an atom of an element relative to 1/12th of the mass of a 12C atom
• Relative Isotopic Mass


  the mass of an isotope relative to 1/12th of the mass of a 12C atom
• M/Z


  mass to charge ratio
• Avogrado


  the number of particles in one mole
• Acid


  releases H+ ions in solution
• Alkali


  releases OH ions in solution
• Strong Acid/Alkali


  fully dissociates in solution
• Weak Acid/Alkali


  partial dissociation in solution
• Neutralisation


  reaction of H+ and OHions → H2O
• Standard Solution


  a solution of accurate concentration
• Oxidising Agent 


  electron acceptor
• Reducing Agent

  electron donor
• Orbital


  a region that can hold 2 electrons of opposite spins
• Covalent Bond


  electrostatic attraction that occurs due to the sharing of two electrons between two nonmetal atoms
• Ionic Bond


  electrostatic attraction that occurs due to the electron transfer from a metal to a non-metal forming positive and negative ions
• Electronegativity


  ability of an atom to attract electrons towards itself in a covalent bond
• Ionisation Energy


  the energy required to remove 1 mole of electrons from gaseous atoms to form 1 mole of gaseous ions
• Metallic Bond


  electrostatic attraction that occurs when a positive metal ion is surrounded by a sea of delocalised electrons
• Group 7


  Disproportionation: simultaneous oxidation and reduction of a species
• Activation Energy


  minimum energy required for a reaction to occur
• Enthalpy of Combustion


  enthalpy change when one mole of a substance is completely burned in excess oxygen
• Enthalpy of Formation


  enthalpy change when one mole of a compound is formed from its elements in their standard states under standard conditions
• Enthalpy of Neutralisation


  enthalpy change when one mole of water is formed in an acid-base neutralization reaction
• Standard Conditions


  100 kPa and 298 K
• Standard States


  physical states under standard conditions
• Equilibrium


  the rate of the forwards and backwards reactions are equal
• Equilibrium


  the concentrations of reactants and products are constant
• Order


  the factor by which each reactant affects the rate
• Overall Order


  the sum of the individual orders
• Half-Life


  the time it takes for the concentration to half
• Rate-Determining Step


  the slow step in a multi-step reaction
• Bronsted-Lowry Acid


  proton donor
• Bronsted-Lowry Base


  proton acceptor
• Strong Acid/Base


  completely dissociates in water
• Weak Acid/Bae


  incomplete dissociation in water
• pH


  pH = -log10 [H+ ]
• Kw


  Kw = [H+ ][OH- ]