Electron configuration - the distribution of electrons in an atom or molecule, Spin - Electrons can have two possible states. spin up and spin down. in an orbital, each electron will be in a different spin state., orbitals - regions where there is a 95% probability of locating an electron, ionic bonding - electrostatic attraction between two oppositely charged ions, electrostatic attraction - the force experienced by oppositely charged particles. it holds the particles strongly together., giant ionic lattice - a regular arrangement of positive and negative ions, e.g NaCl, Lone pair - a non-binding pair of electrons, Organic compound - a compound that contains one or more carbons in a carbon chain, Delocalised electrons - electrons that are free to move. They are present in metals and are not associated with a single atom or covalent bond, Electronegativity - the tendency of an atom to attract a bonding pair of electrons, Intermolecular forces - the attraction or repulsion between neighbouring molecules, dipole - separation of charges within a covalent molecule, hydrogen bonding - the strongest form of intermolecular force involving a bond between a hydrogen adn either a fluorine, oxygen or nitrogen atom., Mole - Amount of a substance equivalent to the number of atoms in 12g of carbon-12., Molar mass - the mass of one mole of a substance, titration - a method of volumetric analysis used to calculate the concentration of a solution, solution - a liquid mixture where a solute is dissolved in a solvent, Standard solution - a solution of known concentration used in volumetric analysis, solute - the substance dissolved in a solvent to form a solution, solvent - a liquid which dissolves another substance, Stoichiometry - the relationship between reactants and products to work out how much product can be produced from given amounts of reactants, Theoretical mass - the expected amount of product from a reaction calculated from a balanced equation, reversible reaction - A reaction where the reactants react to form products and the products simultaneously react to re-form reactants, percentage yield - the actual amount of mass worked out as a percentage of the theoretical mass, Atomic number - the number of protons in an atom, Cation - ions with a positive charge, Anion - ions with a negative charge, isoelectronic - having the same number of electrons, first ionisation energy - the energy needed to remove one mole of electrons from one mole of a gaseous atom, periodicity - the repeating pattern seen by the elements in the periodic table, electron affinity - the change in energy when one mole of a gaseous atom gains one mole of electrons to form one mole of negative ions, malleable - can be hammered into shape without breaking, ductile - can be hammered or stretched thin into wires without breaking, alkali solution - solution with a pH above 7, oxidation - loss of electrons from an atom/ion, allotropes - two or more physical forms that an element can exist in. e.g. graphite and diamond are allotropes of carbon, amphoteric - substance that can act as both an acid and a base, Redox - the transfer of electrons during chemical reactions, reduction - when an atom/ion gains electrons, oxidation state - the number assigned to an element in a chemical compound due to how many electrons the element has gained/lost,

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