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
why is nickel ductile
layers of ions can easily slide past each other
why is diamond very hard and has a high MP (3)
-very strong covalent bonds
-each C atom covalently bonded to 4 other C atoms
-need lots of energy to overcome
what is graphene
a layer of graphite
why is graphite a good lubricant
layers of graphite slide over each other due to weak intermolecular forces holding them together
why is graphite a good conductor of electricity
delocalised electrons free to carry charge through the structure
