Covalent Bonding Flashcards
1
Q
Covalent bonding is between what atoms?
A
non metals
2
Q
How do covalent bonds hold electrons together?
A
The electrostatic attraction between the (shared) pairs of electrons and the positive nuclei involved in the bond
3
Q
Atom
A
Smallest part of an element that can exist
4
Q
Molecule
A
A collection of two or more atoms held together by covalent bonding
5
Q
Simple molecules
A
- Strong covalent bond between atoms, weak intermolecular force between molecules
- They have low boiling points because little energy is needed to break weak intermolecular force
- Do not conduct electricity because no
electrons are free to move
6
Q
Covalent bonded structures
A
Giant covalent lattice and simple molecules
7
Q
Giant covalent
A
- arranged in giant lattices
- High melting and boiling points because a lot of energy is needed to break strong covalent bonds
- Most giant covalents do not conduct electricity but Graphite does
8
Q
Allotropes
A
Different structures of the same element
9
Q
Graphite
A
- Form of carbon
- Carbon atoms form layers that can slide over each other
- weak intermolecular forces between layers
- Conduct electricity
- Softer than diamond
-Joined to 3 carbon atoms
10
Q
Diamond
A
- Every carbon atom joined to four other carbon atoms
- Doesn’t conduct electricity
- Very hard 😉
11
Q
Silicone dioxide
A
- Contains silicone and oxygen
- Similar structure to diamond
- very hard
12
Q
C60 Fullerenes
A
- Molecules are spherical
- Slippery
- Lower melting and boiling points that graphite and diamond because of weak intermolecular forces
