crystal bonding

explain the boiling and melting points of ionic

high (smaller the ion=higher melting point), because lots of energy needed to break strong electrostatic forces of attraction

why can’t solid iconic not conduct electricity?

the ions can’t move around and carry charge

why is ionic (molten/dissolved) a good conductor of electricity?

the ions are free to move and can carry around charge

why is ionic highly soluble?

water is a polar molecule and those charges attract the ions causing the lattice to separate

why are the melting and boiling points high for metallic?

lots of attraction between positive metal ions and delocalised electrons

why is metallic a good electricity conductor?

they have free delocalised electrons

why is metallic so malleable (easily shaped)?

has layers which can slide over each other

why is metallic insoluble?

the water cannot break the metallic lattice

why does giant covalent have high mp and bp (including graphite and graphene)?

lots of energy needed to break strong covalent bonds

if giant covalent doesn’t have mobile charged particles. what does this mean?

not a good conductor of electricity

why is giant covalent very strong(including graphene)?

has a rigid structure and many strong bonds

why is giant covalent insoluble (including graphite and graphene)?

it is non polar

why is graphite and graphene good conductors of electricity?

they have free delocalised electrons

why is graphite soft?

there are only weak forces between layers, which can slide

why doesn’t simple molecular melt?

it sublimes (solid →gas) at a low temp, weak intermolecular forces which require little energy to overcome

does simple molecular conduct electricity?

no