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chemistry ocr a a level > 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.

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1
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.

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2
Q

What does molecular shape depend on?

A

Electron pairs around the central atom.

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3
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.

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4
Q

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

A

Trigonal planar

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5
Q

name & bond angle

A

non-linear & 104*

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6
Q

Name & Bond angle

A

trigonal planar & 120*

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7
Q

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

A

Electron pair repulsion theory

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8
Q

How is electronegativity measured?

A

On the Pauling scale.

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9
Q

What does a polar bond form?

A

A permanent dipole

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10
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.

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11
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.

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12
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.)

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13
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.

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14
Q

what intermolecular forces are involved between water molecules

A

London forces

permanent dipole-dipole interactions

hydrogen bonding

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15
Q

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

A

Higher boiling points

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16
Q

Name and bond angle

A

Name: Trigonal pyramidal

Angle: 107*

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17
Q

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

A

Weak intermolecular forces to overcome.

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18
Q

Define dipole

A

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

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19
Q

Name & bond angle

A

linear & 180*

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20
Q

name & bond angle

A

non-linear & 117.5*

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21
Q

What can electronegativity be used to predict about bonding?

A

Whether it will be covalent or ionic bonding.

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22
Q

name & bond angle

A

tetrahedral & 109.5*

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23
Q

Name & bond angle

A

non-linear & 104.5*

24
Q

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

A

104.5

25
Q

What is the general strength of intermolecular forces?

A

Very weak

26
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
27
Q

Define polar covalent bond

A

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

28
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.

29
Q

How are permanent dipole-dipole interactions labelled?

A

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

30
Q

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

A

Non-linear

31
Q

Which type of pair repels the most?

A

Lone pairs

32
Q

In what way do electron pairs interact?

A

They repel each other.

33
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.

34
Q

Name and bond angle

A

Non-linear & 117.5*

35
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.

36
Q

What is the bond angle in a tetrahedral molecule?

A

109.5

37
Q

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

A

no mobile charge carriers

38
Q

What is the bond angle in a trigonal planar molecule?

A

120

39
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.

40
Q

What is the bond angle in a linear molecule?

A

180

41
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.

42
Q

is water a non-polar or polar molecule?

A

polar molecule

43
Q

state the three anomalous properties of water

A

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

44
Q

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

A

Tetrahedral

45
Q

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

A

non-linear

46
Q

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

A

Octahedral

47
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.

48
Q

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

A

Hydrogen bonding

Permanent dipole-dipole interactions

Induced dipole-dipole

49
Q

name & bond angle

A

trigonal pyramidal & 107*

50
Q

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

A

Linear

51
Q

What is the bond angle in an octahedral molecule?

A

90

52
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.

53
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
54
Q

What is the bond angle in a trigonal pyramidal molecule?

A

107

55
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.

56
Q

What is electronegativity?

A

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

chemistry ocr a a level (35 decks)

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