Properties of Chemical Bonds

High melting and boiling points because of strong attraction between oppositely charged ions in lattice require a lot of energy to overcome

Doesn't conduct because ions are fixed and cannot carry charge

Conducts electricity becayse ions are no longer fixed and can carry charge

Yes

Very low melting and boiling point because little energy needed to overcome attraction between atoms

Do not conduct in any state as electrons are bound to their atom

Insoluble in water

Low melting and boiling points because little energy needed to overcome intermolecular forces between molecules

Doesn't conduct when solid or melted because they lack free ions or electrons to carry charge

Usually insoluble in water

Very high melting and boiling points because many strong covalent bonds hold their atoms together

Doesn't conduct when solid (except graphite) or melted because have no free electrons or mobile ions to carry charge

Insoluble in water

High melting and boiling points because of strong electrostatic attraction between positive ions and delocalised electrons

Conducts when solid and melted because delocalised electrons can move freely through metal lattice and carry charge

Insoluble in water but some will react with water

KI, NaCl, CuS04, CaO

Ar, Ne, He, Xe

H2O, NH3, C6H1206, CO2

diamond, graphite, silicon, silicon dioxide

Na, Fe, Mg, Cu