ionic + metallic bonding

Created by

hollie maklowicz

Cards (20)

what is an ion?
atom that has lost or gained electrons
which kinds of elements form ionic bonds?
metals and non-metals
what charge do ions from group 1 form?
1+
what charge do ions from group 2 form?
2+
what charge do ions form group 6 form?
2-
what charge do ions from group 7 form?
1-
what is the force that holds oppositely charged ions together?
electrostatic force of attraction
describe the structure of a giant ionic lattice
regular structure of alternating positive and negative ions, held together by the electrostatic force of attraction
why do ionic substances have high melting points?
electrostatic force of attraction between positive and negative ions is strong and requires lots of energy to break
why don’t ionic substances conduct electricity when solid?
ions are fixed in position so cannot move
no delocalised electrons
when can ionic substances conduct electricity? 
when they are dissolved in water or melted
why do ionic substances conduct electricity when melted or dissolved?
free ions can move and carry electric charge
describe the structure of pure metal
layers of positive metal ions surrounded by delocalised electrons
describe the bonding in a pure metal
strong electrostatic forces of attraction between metal ions and delocalised electrons
four properties of pure metals
malleable
high melting points
good electric conductor
good thermal conductor
why are pure metals malleable?
layers can slide over eachother easily
why do pure metals have high melting points?
electrostatic force of attraction between positive metal ions and delocalised electrons is strong and requires lots of energy to break
why are pure metals good conductors of heat and electric?
delocalised electrons are free to move through the metal
what is an alloy?
mixture of a metal with atoms of another element
why are alloys harder than pure metals?
different sized atoms disturb the layers, preventing them from sliding over eachother