chemistry - key concepts in chemistry: ionic bonding (1.21 - 1.27)

1.21 how are ionic bonds formed?

electrons transferred between metal & non-metal atoms

strong ionic bond - strong electrostatic forces of attraction between oppositely charged ions

metal atoms lose electrons - form cations (+ve ions)

non-metal atoms gain electrons - form anions (-ve ions)

1.21 dot & cross diagrams

1.22 ion definition

atom/group of atoms with positive/negative charge

1.23 calculate numbers of protons, neutrons & electrons in simple ions given atomic number & mass number

1.24 formation of ions - groups 1, 2, 6 & 7

1.25 endings -ide & -ate (names of compounds)

-ide: contains 2 elements; e.g. iron (II) sulfide

-ate: contains 3/more elements, 1 is oxygen; e.g. iron (II) sulfate

1.26 ionic formulae - oxide, hydroxide, halide, nitrate, carbonate, sulfate

oxide = O^2-

hydroxide = OH^-

halide = (group 7)^-

nitrate = NO₃^-

carbonate = CO₃^2-

sulfate = SO₄^2-

1.26 deduce formula of ionic compounds given formula of ions

e.g. Na⁺ + Cl^- → NaCl

e.g. Na⁺ + CO₃^2- → Na₂CO₃

1.27 structure of ionic compound

lattice structure

regular arrangement of ions

held together by strong electrostatic forces of attraction (ionic bonds) between oppositely charged ions