Bonding Flashcards

1
Q

Anion

A

Negatively charged ion formed when an atom gains electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Cation

A

Positively charged ion formed when an atom loses electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Ionic bond

A

The electrostatic force of attraction between oppositely charged ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Lattice

A

Ionic bond that are in a 3D arrangement, made up of repeating unit cells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Covalent bonding

A

The electrostatic forces of attraction between a par of electrons shared between two atoms and the positively charged nuclei of those atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Dative or coordinate covalent bond

A

One where both electrons in the covalent bond come from one atom or group of atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Ionic character

A

It is hard to say if a bond is 100% ionic/ covalent. Instead we talk about the ionic character of a bond and we have an arbitrary cut-off between ionic + covalent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Sigma bonds

A

Single bonds formed from the overlap of:
2 s-orbitals
s+p-orbitals head on
2 p-orbitals head on

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Pi bond

A

2 p-orbitals overlap sideways head on

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Double bond

A

sigma and then a pi bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Triple bond

A

Sigma and then 2 pi bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Valence Shell Electron Pair Repulsion Theory

A
  1. Electron occurs in pairs (bonding pairs and lone pairs)
  2. Electron pair repel
  3. Not all electron pair repulsion are the same
    LP:LP>LP:BP>BP:BP
  4. For the sake of shapes of molecules, double and triple bonds are counted as one bonding pair
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Tetrahedral

A

4 BP : 0 LP
E.g. CH4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Pyramidal

A

3 BP : 1 LP
E.g. NH3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Planar V shaped

A

2 BP : 2 LP
E.g. H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Trigonal Planar

A

3 BP : 0 LP
E.g. BH3

17
Q

Linear

A

2 BP / 1 BP

18
Q

Polar molecule

A

Relates to molecules with covalent and not ionic or metallic bonds
It is a dipole

19
Q

Dipole

A

A molecule with positive and negative ends

20
Q

2 things to get polar covalent bond

A
  1. Have polar covalent bonds. Without polar covalent bonds there is no charge
  2. The symmetry of the molecule must allow for different centres of positive and negative charge
21
Q

Intermolecular forces

A

Forces between molecules

22
Q

Dipole-Dipole attraction

A

Force of attraction between the opposite ends of permanent dipoles on neighbouring molecules

23
Q

Van der Waals forces (London dispersion force)

A

Force of attraction between temporary instantaneous dipoles induced on neighbouring non-polar molecules
Random movement of electron in an atom results in a temporary formation of a dipole

24
Q

Hydrogen bonding

A

Force of attraction between a hydrogen atom, which is covalently bonded to a small highly electronegative atom and a lone pair of electrons on another small highly electronegative atom