1.3 bonding Flashcards
definition of ionic bonding
the electrostatic attraction between oppositely charged ions in a lattice
metals + non metals
ionic properties- MP+BP
strong electrostatic forces between oppositely charged ions in a giant lattice which needs lots of energy to overcome
ionic properties- solubility in water
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
ionic properties- conductivity
-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
ionic properties- brittleness
when layers of alternating charges are distorted, like charges repel which breaks the lattice apart
definition of covalent bonding
shared pair of electrons between two atoms
simple molecular properties- MP+BP
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
simple molecular properties- conductivity
poor as there are no ions to conduct electricity and electrons are localised- contains no charged particles
macromolecular structure properties- MP+BP
high due to many strong covalent bonds which need lots of energy to overcome- each atom has multiple covalent bonds
macromolecular structure properties- solubility in water
insoluble- they can’t form strong attractions with water
macromolecular structure properties- conductivity
-when solid- diamond and sand cannot because electrons are localised, but graphite can as it has delocalised electrons free to carry charge
definition of metallic bonding
electrostatic attraction between a lattice of positive metal ions and delocalised electrons
metallic bonding properties- MP+BP
high- strong electrostatic forces between positive ions and sea of delocalised electrons
