intermolecular forces Flashcards

1
Q

define intermolecular forces

A

amount of force between neighbouring molecules

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

what are intermolecular forces caused by

A

weak attractive forces between small dipoles in different molecules

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

what are the 3 types of intermolecular forces

A

permanent dipole dipole interactions
van der waals forces
hydrogen bonding

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

define a permanent dipole dipole force

A

the weak attractive force between permanent dipoles in neighbouring polar molecules

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

if you increase the number of electrons what does this do to the strength of the van der Waals forces

A

increased number of electrons = increased strength of van der Waals forces

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

explain why electronegativity increases as you go to the right of the periodic table in terms of the size of the positive charge on the nucleus

A

number of protons increases
so increased positive charge increases
the increased attraction between the nucleus and the pair of electrons in the covalent bond
so elements on the right are more electronegative

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

explain why electronegativity increases as you go to the right of the periodic table in terms of atomic radius

A

smaller atomic radius means the closer the bonding electrons will be to the nucleus of an atom
so elements on the right as more electronegative

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

explain why electronegativity increases as you go to the right of the periodic table in terms of shielding

A

electrons in inner shells shield the electrons in the outer shells from the positive charge of the nucleus
so greater number of inner shells decreases electronegativity but as you go to the right in the same period it stays constant

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

why do atoms with more electrons have a higher boiling point

A

more electrons = stronger van der waals forces

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

what are van der waals forces caused by

A

the random movement of electrons
(every atom/molecule will experience van der waals forces)

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

if you place one atom with van der Waals forces next to another atom what will it do

A

it will induce a dipole in atom 2 with the opposite facing charges therefore both atoms now experience van der Waals forces

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

if you decrease electronegativity what happens to the strength of permanent dipole dipole forces

A

decrease electronegativity = decreased strength of permanent dipole-dipole forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

to experience a permanent dipole dipole interaction what must both molecules have?

A

a permanent dipole

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

what 2 conditions are needed for hydrogen bonding to take place

A
  1. hydrogen atom bonded to a strongly electronegative atom
  2. electronegative atom must have at least 1 lone pair of electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what atoms can bond with hydrogen and undergo hydrogen bonding

A

fluorine
oxygen
nitrogen
(all 3 are very electronegative and have at least 1 lone pair)

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

explain the bonding in hydrogen fluoride

A

fluorine has 3 lone pairs
and fluorine is the most electronegative atom so this strongly attracts the pair of electrons in the covalent bond so it is a polar molecule
hydrogen bonds form between the hydrogen on the right being attracted to the lone pairs of fluorine on the left molecule

17
Q

why is ice floating important for organisms living under water

A

insulates the water below preventing the water from freezing completely

18
Q

why does ice float

A

in ice the water molecules are further apart than in liquid water therefore it is less dense which allows it to float

19
Q

what do water molecules do at freezing point

A

arrange themselves into an ordered structure stabilised by a network of hydrogen bonds1

20
Q

in liquid water what happens in terms of hydrogen bonds

A

hydrogen bonds are constantly being being/formed due to the movement of water molecules

21
Q

why does water have a relatively high melting point

A

takes a lot of energy to break the hydrogen bonds

22
Q

iodine is non-polar what type of solvent does it dissolve in? what happens in terms of solvent molecules?

A

iodine non polar molecule so dissolves in a non polar solvent

solvent molecules move from van der Waals forces to the iodine molecules