C3 - Structure And Bonding Flashcards
Ions
An atom or group of atoms with an electrical charge, either positive (+) or negative (-).
Ionic bonding
Between metals and non-metals
High melting and boiling points
Giant ionic structures
High melting and boiling points
Strong electrostatic forces
Can dissolve through H2O
Can conduct electricity when molten or dissolved in H2O as ions become free to move
Ionic lattice
When ions are closely packed with very strong electrostatic forces, between oppositely charged ions
Covalent bonding
Sharing of electrons between non-metals
Low melting and boiling points
Giant covalent structures
Bonded through strong covalent bonds
High melting and boiling points
Do not conduct electricity - not even when molten (except graphite)
Graphite
3 carbon bonds create layers that are free to slide over each other
Weak intermolecular forces between layers
Conducts heat and electricity because each carbon atom has one delocalised electron
Graphene
A single layer of graphite
Makes 3 covalent bonds and has delocalised electrons
Diamond
4 carbon bonds in a rigid structure
Hardest natural substance
Nanoscience
The study of objects on the nanometre scale
Fullerenes
3 bonds for each carbon - leaving 1 electron free to conduct electricity
They can be used to deliver drugs as they are hollow
Used as lubricants as they reduce friction
Used as catalysts
Metallic bonding
Conduct electricity due to the sea of delocalised electrons
Strong electrostatic forces
Layers of atoms can slide over each other allowing metals to be bent and shaped
Alloys
A mixture of 2 or more metals
Harder than pure metals as atoms cannot slide past each other
Pure metals
Chemical elements that consist of only one type of atom
