Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

OCR A-Level Chemistry Henry K > Chapter 6 - Shapes of Molecules and Intermolecular Forces > Flashcards

Chapter 6 - Shapes of Molecules and Intermolecular Forces Flashcards

Shapes of molecules and ions, Electronegativity and polarity, Intermolecular forces and Hydrogen bonding.

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What does molecular shape depend on?

A

Electron pairs around the central atom.

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

In what way do electron pairs interact?

A

They repel each other.

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

Which type of pair repels the most?

A

Lone pairs

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

What is the order of pair repulsion, from strongest to weakest?

A
  • Lone pair/lone pair
  • Lone pair/bonding pair
  • Bonding pair/bonding pair
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What is the name of the way to predict a molecule’s shape?

A

Electron pair repulsion theory

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

What shape name is given to a molecule with no lone pairs and 4 bonding pairs?

A

Tetrahedral

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

What is the bond angle in a tetrahedral molecule?

A

109.5

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

What shape name is given to a molecule with two bonding pairs and two lone pairs?

A

non-linear

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

What is the bond angle in a trigonal pyramidal molecule?

A

107

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

What shape name is given to a molecule with two lone pairs and two bonding pairs?

A

Non-linear

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

What is the bond angle in a non-linear molecule with two lone pairs?

A

104.5

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

What shape name is given to a molecule with 2 electron pairs around the central atom, with no lone pairs?

A

Linear

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

What is the bond angle in a linear molecule?

A

180

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

What shape name is given to a molecule with 3 electron pairs around the central atom, with no lone pairs?

A

Trigonal planar

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

What is the bond angle in a trigonal planar molecule?

A

120

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

What shape name is given to a molecule with 6 electron pairs around the central atom?

A

Octahedral

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the bond angle in an octahedral molecule?

A

90

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is electronegativity?

A

An atom’s ability to attract the electron pair in a covalent bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

How is electronegativity measured?

A

On the Pauling scale.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What does a higher Pauling value mean?

A

A higher electronegativity and thus a greater attraction for an electron pair in a covalent bond.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What makes a bond polar?

A

Two atoms with electronegativities differing by at least 0.5, the bonding electrons are pulled towards the more electronegative atom, making it polar.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What does a polar bond form?

A

A permanent dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

How is a dipole formed?

A

A difference in charge between the two atoms, caused by a shift in electron density in the bond.

24
Q

Are diatomic gases polar or non-polar, why?

A

Non-polar Because the atoms have equal electronegativities and so the electrons are equally attracted to both nuclei.

25
Q

What happens if the polar bonds are arranged symmetrically in a molecule?

A

The dipoles cancel each other out, so the molecule has no overall dipole and is non-polar.

26
Q

What happens if the polar bonds are arranged unsymmetrically in a molecule?

A

Uneven distribution of charge and the molecule will have an overall dipole.

27
Q

What can electronegativity be used to predict about bonding?

A

Whether it will be covalent or ionic bonding.

28
Q

What is the general strength of intermolecular forces?

A

Very weak

29
Q

What is the order of the intermolecular forces from strongest to weakest?

A

Hydrogen bonding Permanent dipole-dipole interactions Induced dipole-dipole

30
Q

How are induced dipole-dipole forces formed?

A
  • Movement of electrons produces a changing dipole in a molecule
  • At any instant, an instantaneous dipole will exist because there is a constant shift in the uneven distrubition of charge.
  • The instantaneous diple induces a dipole on a neigbouring molecule
  • The induced dipole induces further dipoles on neighbouring molecules, which then attract one another
31
Q

What is the effect of stronger induced dipole-dipole forces?

A

Higher boiling points

32
Q

Whats the reason for a higher boiling in a molecule

A

These molecules have a larger electron clouds, so stronger induced dipole-dipole forces. Boiling point is overcoming the intermolecular forces so stronger ones means a higher boiling point.

33
Q

How are permanent dipole-dipole interactions labelled?

A

With charges of delta+ and delta- on the atoms.

34
Q

How is hydrogen bonding formed?

A

What happens is that a weak bond is polarised between the hydrogen of one molecule and a lone pair on a neighbouring molecules, electronegative atom (for example, F, N or O.)

35
Q

What effect does hydrogen bonding have on a molecule?

A

Soluble in water. Higher boiling and freezing points than molecules of a similar size that don’t form hydrogen bonds.

36
Q

What is an interesting property of ice caused by hydrogen bonding?

A

hydrogen bonds hold water molecules apart in an open lattice structure. The water molecules in ice are held further apart than in water. As a result, solid ice is less dense than liquid water and therefore floats.

37
Q

How do intermolecular forces explain simple covalent compounds having low melting and boiling points?

A

Weak intermolecular forces to overcome.

38
Q

How do intermolecular forces explain simple covalent compounds sometimes being soluble in water?

A

Water is a polar molecule which can form hydrogen bonds with other hydrogen-based molecules.

39
Q

How do intermolecular forces explain simple covalent compounds not conducting electricity?

A

no mobile charge carriers

40
Q

what is a pure covalent bond?

A

Molecules of elements such as hydrogen and oxygen, there bonded atoms come from the same element and the electron pair is shared equally.

41
Q

Name and bond angle

A

Name: Trigonal pyramidal

Angle: 107*

42
Q

Name and bond angle

A

Non-linear & 117.5*

43
Q

Name & Bond angle

A

trigonal planar & 120*

44
Q

Name & bond angle

A

non-linear & 104.5*

45
Q

Name & bond angle

A

linear & 180*

46
Q

name & bond angle

A

tetrahedral & 109.5*

47
Q

name & bond angle

A

trigonal pyramidal & 107*

48
Q

name & bond angle

A

non-linear & 117.5*

49
Q

name & bond angle

A

non-linear & 104*

50
Q

what intermolecular forces are involved between water molecules

A

London forces

permanent dipole-dipole interactions

hydrogen bonding

51
Q

Describe in terms of the lattice structure of H20 when in solid state (ice) and when it is melting.

A

When it is ice, the water molecules in the lattice are held further apart. When it’s melting, the ice lattice collapses, and the molecules move closer together; thus increasing the density.

52
Q

state the three anomalous properties of water

A

ice less dense than water, high melting points, and boiling points

53
Q

Explain why simple molecular compounds:

a) have low melting and boiling points
b) do not usually dissolve in water
c) have poor electrical conductivity.

A

a) Weak intermolecular forces are broken by the energy present at low temperatures.
b) There are little interactions between the molecules in the lattice and the polar solvent molecules.
c) There is no mobile charged particle.

54
Q

Define dipole

A

Charge separation across a bond with one atom having a delta +ve charge and one atom a delta -ve charge.

55
Q

Define polar covalent bond

A

shared pair of electrons where the electron pair is not shared equally between the two bonded atoms.

56
Q

is water a non-polar or polar molecule?

A

polar molecule

OCR A-Level Chemistry Henry K (35 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions