2.3.1 metallic bonding and uses

what is the structure of metlas

positive metal ions in regular layers to form laatic structure surrounded by a sea of delocalised electrons

what is the metallic bond

electrostatic atrtraction between the positive metal ions and negative delocalised electrons

why are metals malleable

layers can slide over each other because regular sized

where are the attractive forces between metal ions and electrons

in all directions

what does this mean for the malleability

layers can slide and metallic bonds are reformed

why are metals strong and hard

because of strong attractive forces between metal ions and delocalised electrons

when and why can metals conduct electricity

conduce in solid or liquid because the delocalised electrons are free to move and carry a charge through the structure

why are metals good conductors of heat

cations in metal lattice vibrate and bumb into surrounding metal ions, conducting heat

vibrating cations transfers kinetic energy to electrons and these electrons can move about and transfer heat through the substance

why do metals have high melting and boiling points

due to strong electrostatic forces of attraction betwencations and free electronsw

how does the greater charge of cation affect m and b point

greater charge, greater electrostatic attraction so high m and b point

how does ionic radius affect m and b point

smaller ionic radius greater electrostatic attraction so higher m and b points