Please enable JavaScript.
Coggle requires JavaScript to display documents.
Atomic structure and bonding (covalent bonding (non-metals) (giant…
Atomic structure and bonding
ionic bonding (metals + non -metals)
they have a
giant ionic lattice structure
high melting / boiling points
they have strong forces of attraction between oppositely charged ions, a large amount of energy is required to break the lattice
conduct electricity when molten/ in liquid
the ions are free to move
don't conduct electricity when solid
the ions are tightly fixed, they are not free to move
electrostatic attraction of oppositely charged ions
covalent bonding (non-metals)
simple molecular structure
low melting/ boiling points
they have weak intermolecular forces between molecules, which doesn't require much energy to break
don't conduct electricity
not charged particles free to move
giant molecular lattice structure
diamond
always bonds to 4 other atoms
doesn't conduct electricity, as no free electrons to move
high melting point (over 3500)
there are no free electrons, and lots of strong bonds that are hard to break and require a lot of energy
graphite
each bonded to 3 atoms, fourth is free to move
conducts electricity as there is one delocalised electron
high melting point (over 3600) and used as lubricant
the layers of hexagonal ring can slide over each other
silicon dioxide
shared pair of electrons which both electrons are attracted to both nuclei
metallic bonding (metals)
they have a
gaint metallic lattice structure
high melting/ boiling points
they have strong forces of attraction and a lot of energy is required to break the bonds in the lattice
conducts electricity as solids
the electrons are free to move
don't conduct electricity as molten
the atoms aren't free to move
lattice of positive ions in a sea of delocalised electrons