C3- Structure and Bonding
Ionic Bonding
Metallic bonding
Covalent bonding
States of matter
Simple
Giant
Fullerenes
loses/gains electrons
metal & non-metal
High m.p and b.p.
+ions & -ions
(transferring of electrons)
don't conduct when solid, but when molten/ dissolved
e.g. NaCl
giant ionic structure
between metals
+ions in a sea of electrons
high m.p and b.p.
conduct electricity
Giant structure
low m.p. and b.p.
doesn't conduct
Carbon nanotubes
Graphene
between non-metals
Diamond
Graphite
doesn't conduct
conducts
high m.p. and b.p.
solid
liquid
gas
particles are tightly-packed- they can't move, only vibrate
Particles are very close to each other- they can flow over each other, but movement is restricted
Particles are very far apart and randomly arranged- they move around very fast in all directions
Ions are arranged in a regular way- the electrostatic attraction forms the ionic bonds
You need to break all the ionic bonds throughout the structure which are strong and need lots of energy to break
When solid, the ions are in fixed positions. When molten or dissolved, the ions are free the move, and can carry a charge
There are millions of atoms, and so millions of bonds, that need a lot of energy to break them
soft
layers have weak FOA between them, so they're easier to lose, hence why they're soft
hard
Atoms are linked very tightly in a lattice structure (that's perfect & symmetrical) so hard to move
Pencil
Layers separate easily and transfer on the paper when writing
Only 3 bonds are used with other carbon atoms, so the fourth is with a free delocalised electron that can carry a charge through the structure
Industrial diamond
Used on the edge of cutting tools, as its hard and has a high m.p.
All 4 bonds are used with other carbon atoms, so there are no free, delocalised electrons or ions to carry a charge
Lubricant
light and layers mean it can slide over each other
Reflective
Perfect, symmetrical lattice
shared pair of electrons
Free, delocalised electrons can carry a charge though the metal