C3 (Bonding) Flashcards
1
Q
Ionic
A
- electrostatic forces of attractions between oppositely charged ions
- full amount of electrons in outer most shell (like noble gas)
- creates a giant lattice structure which is very strong
- between non metal and metal
2
Q
Properties of Ionic
A
- high melting and boiling points
- brittle
- colourless
- cannot conduct electricity in solid state as ions cant move
- opposite in liquids as ions can movw
3
Q
Simple molecular
A
- simple molecules joined by weak intermolecular forces of attraction
- forces of attraction strong inside the molecule
- creates low melting and boiling points
- do not conduct as held in a covalent bond (two non-metals)
- examples: Water + Hydrogen Chloride
4
Q
Metallic
A
- electrostatic force between delocalised electrons and positive ions
- delocalised electrons create a sea of electrons
- good conductors because of the free electrons
- high melting and boiling points because harder to break electrostatic force
- two metals
5
Q
Covalent
A
- two non metals sharing electrons
- arranged in strong latices with strong structures
- high melting and boiling points
- drawn through dot and cross diagrams
6
Q
Diamond (properties ext)
A
- high melting point
- hard
- not conductive, non metal
- carbon bonded to 4 other strongly
- no free electrons
- used for jewellery and drills
7
Q
Graphite (properties ext)
A
- high melting point
- soft because weak intermolecular forces of attraction
- free electrons meaning conductive
- grey non metal
- giant covalent bonded with 3 others
- free electrons form a ‘cloud of electrons’
- used for lubricant and pencils
8
Q
Monatomic
A
- noble gas
- full electrons in outer most shell meaning strong electrostatic forces of attraction
9
Q
What are the 3 giant covalent bonds
A
Silicon dioxide, diamond, graphite
10
Q
Why does giant covalent have high melting/ boiling points?
A
- strong covalent bonds
- lots of energy required to brake down the bonds
11
Q
Why is diamond not conductive and graphite is
A
- diamond uses all delocalised electrons as it is bonded to 4 carbon atoms and outer shell of carbon is 4
- graphite only bonds to 3, meaning it has that free electron
12
Q
Why are metals malleable and how can it be changed?
A
- layers slide as the atoms are the same size
- mix metals to become alloys
