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physical chemistry > 3.1.3.7 Forces between molecules > Flashcards

3.1.3.7 Forces between molecules Flashcards

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1
Q

the strongest type of interaction that occurs between molecules of hydrogen peroxide and water

A

Hydrogen bond(ing) / H bonding / H bonds

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2
Q

in terms of electronegativity, why the boiling point of H2S2 is lower than H2O2

A

Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules

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3
Q

the strongest attractive force between two ammonia molecules

A

Hydrogen bonds / H bonds

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4
Q

the strongest type of intermolecular force in how the strongest type of intermolecular force in liquid HF arises (CH4)

A

Van der Waals/ vdw/London/ temporary (induced) dipole/ dispersion forces

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5
Q

the strongest type of intermolecular force in Ammonia (NH3)

A

Hydrogen bonds/H bonds

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6
Q

strongest type of intermolecular force present in Liquid F2

A

van der Waals’ / induced/temporary dipole-dipole / dispersion / London forces

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7
Q

strongest type of intermolecular force present in Liquid CH3F

A

dipole-dipole

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8
Q

strongest type of intermolecular force present in Liquid CH3F

A

hydrogen bonding

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9
Q

how the strongest type of intermolecular force in liquid HF arises

A

large difference in electronegativity between H and F / F most/very/much more electronegative
δ+H-Fδ- dipole created or dipole clearly implied
attraction/bond formed between δ+H and lone pair on F

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10
Q

the trend in the boiling points of the hydrogen halides from HCl to HI

A

van der Waals’ / induced/temporary dipole-dipole / dispersion / London forces / attractions
increase with the increasing Mr / size / mass / N 0 of e- / size of e- cloud (in the hydrogen halides)

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11
Q

reason why the boiling point of HF is higher than that of all the other hydrogen halides

A

hydrogen bonding stronger than van der Waals’ attraction/forces

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12
Q

why the boiling point of methanol is much higher than that of oxygen

A

van der Waals’ forces between oxygen molecules
Hydrogen bonding between methanol molecules
H-B stronger than van der Waals’ OR stronger IMF in methanol

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13
Q

in terms of the intermolecular forces present in each compound, why HF has a higher boiling point than HCl

A

HF = hydrogen bonding
HCl = (permanent) dipole-dipole bonding or even van de Waals’
Hydrogen bonding stronger / is the strongest IMF

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14
Q

the strongest type of intermolecular force between hydrogen fluoride molecules

A

Hydrogen bonds/hydrogen bonding/H bonds/H bonding

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15
Q

why the boiling point of fluorine is very low

A

vdw / van der Waals forces between molecules

IMF are weak / need little energy to break IMF / easy to overcome IMF

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16
Q

the structure of and bonding in graphite and explain why the melting point of graphite is very high

A

Layers of (C atoms)
Connected by covalent bonds within each layer
Van der Waals forces/IMF between layers/weak forces between layers
Many/strong covalent bonds need to be broken

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17
Q

why iodine vaporises when heated gently

A

Van der Waals forces are weak or easily broken

Van der Waals between molecules (or implied)

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18
Q

the strongest type of intermolecular force in water

A

Hydrogen/H bonds

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19
Q

the strongest type of intermolecular force in hydrogen sulfide (H2S)

A

van der Waals/vdw/dipole-dipole/London/temporarily induced dipole/dispersion forces

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20
Q

why the boiling point of water is much higher than the boiling point of hydrogen sulfide

A

Hydrogen bonds/IMF (in water) stronger
OR IMF/VDW/dipole-dipole forces (in H2S) are weaker
OR H bonding is the strongest IMF

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21
Q

why the boiling points increase from H2S to H2Te

A

Atoms/molecules get larger/more shells/more electrons/more surface area
therefore increased Van der Waals/IMF forces

22
Q

three types of intermolecular force

A

Van der Waals’
dipole – dipole
hydrogen bonding

23
Q

Why hydrogen fluoride requires more heat energy for melting than does hydrogen chloride

A

H-Bonding in HF
(dipole-) dipole/V dW in HCl
H-bonding is stronger than dipole-dipole or V.dW

24
Q

Why hydrogen iodide requires more heat energy for melting than does hydrogen chloride

A

HI bigger molecule than HCl

Therefore the forces between HI molecules are stronger

25
Q

why diamond and iodine (solid) have different melting points

A

Iodine Weak van der Waals’ forces / induced dipole-induced dipole
Diamond Covalent bonds would need to be broken
Many / strong covalent bonds OR much energy needed

26
Q

the strongest type of intermolecular force between hydrogen fluoride molecules

A

Hydrogen bonding

27
Q

Why HI molecules don’t have hydrogen bonding like HF molecules

A

Fluorine more/very electronegative or iodine less electronegative or electronegativity difference too small in HI
HI dipole weaker or bonding e– more equally shared

28
Q

the strongest attractive force between two ammonia molecules

A

Hydrogen bonds / H bonds

29
Q

why iodine has a higher melting point than fluorine

A

Iodine has more electrons / iodine is bigger (atom or molecule) / iodine has bigger Mr / bigger surface area
Stronger / more van der Waals forces / vdw / London / temporarily induced dipole / dispersion forces between molecules

30
Q

the strongest type of intermolecular force in a sample of NHF2

A

Hydrogen bonds

31
Q

Although phosphine molecules contain hydrogen atoms, there is no hydrogen bonding between phosphine molecules. Suggest an explanation for this.

A

Difference in electronegativity between P and H is too small

32
Q

the strongest type of intermolecular force holding the water molecules together in the ice crystal

A

Hydrogen bonding

33
Q

the strongest type of intermolecular force in methane

A

Van der Waals’/VdW

34
Q

reason why the melting point of ice is higher than the melting point of methane

A

Hydrogen bonding is stronger (than van der Waals forces)/IMF in ice stronger (than IMF in methane)/H bonds take more energy to break

35
Q

the strongest type of intermolecular force between CCl2F2 molecules

A

Dipole – dipole

36
Q

why the boiling point of water is much higher than the boiling point of hydrogen sulfide

A

Hydrogen bonds/IMF (in water) stronger
IMF/VDW/dipole-dipole forces (in H2S) are weaker
H bonding is the strongest IMF

37
Q

why the boiling points increase from H2S to H2Te

A

Atoms/molecules get larger/more shells/more electrons/more surface area
therefore increased Van der Waals/IMF forces

38
Q

the strongest type of intermolecular force in Methane (CH4)

A

Van der Waals/ vdw/London/ temporary (induced) dipole/ dispersion forces

39
Q

the strongest type of intermolecular force in Ammonia (NH3)

A

Hydrogen bonds/H bonds

40
Q

how the strongest type of intermolecular force arises between two molecules of ammonia

A

(Large) electronegativity difference between N + H/ N very electronegative;
Forms N δ– / H δ+ or dipole explained in words
Lone pair on N attracts/forms weak bonds with H (δ+)

41
Q

why HF has a higher boiling point than HCl

A

HF = hydrogen bonding
HCl = (permanent) dipole-dipole bonding or even van de Waals’
Hydrogen bonding stronger / is the strongest IMF

42
Q

the strongest type of interaction that occurs between molecules of hydrogen peroxide and water

A

Hydrogen bond(ing) / H bonding / H bonds

43
Q

why the boiling point of H2S2 is lower than H2O

A

Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules

44
Q

the strongest attractive force between two ammonia molecules

A

Hydrogen bonds / H bonds

45
Q

the strongest type of intermolecular force between hydrogen fluoride molecules

A

Hydrogen bonds/hydrogen bonding/H bonds/H bonding

46
Q

the strongest type of interaction between polymer chains of Kevlar

A

Hydrogen bond(ing)

47
Q

the strongest type of intermolecular force between one molecule of ammonia and one molecule of water

A

Hydrogen bonding / hydrogen bonds / H-bonding / H-Bonds

48
Q

Phosphine (PH3) has a structure similar to ammonia. In terms of intermolecular forces, suggest the main reason why phosphine is almost insoluble in water.

A

(Phosphine) does not form hydrogen bonds (with water)

49
Q

why iodine has a higher melting point than fluorine

A

Iodine has more electrons / iodine is bigger (atom or molecule) / iodine has bigger Mr / bigger surface area
Stronger / more van der Waals forces / vdw / London / temporarily induced dipole / dispersion forces between molecules

50
Q

the strongest type of intermolecular force in a sample of NHF2

A

Hydrogen bonds

51
Q

why the boiling point of methanol is much higher than that of oxygen

A

van der Waals’ forces between oxygen molecules;
Hydrogen bonding between methanol molecules;
H-B stronger than van der Waals’ OR stronger IMF in methanol;

52
Q

why the boiling point of H2S2 is lower than H2O2

A

Electronegativity of S lower than O or electronegativity difference between H and S is lower
No hydrogen bonding between H2S2 molecules Or only van der Waals / only dipole-dipole forces between H2S2 molecules

physical chemistry (18 decks)

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