1.3 bonding

the electrostatic attraction between oppositely charged ions in a lattice metals + non metals

strong electrostatic forces between oppositely charged ions in a giant lattice which needs lots of energy to overcome

good because the 2 poles of water has strong forces of attraction to other charged ions, so it breaks the ionic bond by hydrogen bond formation

-can’t in solid as ions aren’t free to move in a lattice -can when molten/aqueous as ions are free to carry charge

when layers of alternating charges are distorted, like charges repel which breaks the lattice apart

shared pair of electrons between two atoms

low due to weak van der waals forces which dont need lots of energy to overcome water is simple molecular but has high MP+BP due to the presence of hydrogen bonding

poor as there are no ions to conduct electricity and electrons are localised- contains no charged particles

high due to many strong covalent bonds which need lots of energy to overcome- each atom has multiple covalent bonds

insoluble- they can’t form strong attractions with water

-when solid- diamond and sand cannot because electrons are localised, but graphite can as it has delocalised electrons free to carry charge

electrostatic attraction between a lattice of positive metal ions and delocalised electrons

high- strong electrostatic forces between positive ions and sea of delocalised electrons

layers of ions can easily slide past each other

-very strong covalent bonds -each C atom covalently bonded to 4 other C atoms -need lots of energy to overcome

a layer of graphite

layers of graphite slide over each other due to weak intermolecular forces holding them together

delocalised electrons free to carry charge through the structure

-Mg ions have greater charge -Mg has more e- -greater attraction between ions and e-