Brainscape's Knowledge GenomeTM

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


See full index

A Level Chemistry Year 2 > Enthalpy, Entropy and Free Energy > Flashcards

Enthalpy, Entropy and Free Energy Flashcards

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

What is enthalpy change?

A

The heat energy transferred in a reaction at constant pressure

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

What are the units of enthalpy change, ΔH?

A

kJ mol^-1

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

What are standard conditions?

A

1 atm (1000 kPa) of pressure and 298K (25°C)

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

Is -ve ΔH endothermic or exothermic?

A

Exothermic

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

Is +ve ΔH endothermic or exothermic?

A

Endothermic

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

Why is the ΔH value a negative number for exothermic?

A

Because heat energy is given out (the chemicals lose energy)

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

Why is the ΔH value a positive number for endothermic?

A

Because heat energy is absorbed (the chemicals gain energy)

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

What is enthalpy change of formation?

A

The enthalpy change when 1 mole of a compound is formed from its elements

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

What is enthalpy change of atomisation of an element?

A

The enthalpy change when 1 mole of gaseous atoms is formed from an element

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

Give an example of a reaction that has enthalpy change of formation

A

Cl2 (g) + Ca (s) —> CaCl2 (s)

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

Give an example of a reaction that has enthalpy change of atomisation of an element

A

1/2Cl2 (g) —> Cl (g)

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

What is enthalpy change of atomisation of a compound?

A

The enthalpy change when 1 mole of a compound is converted to gaseous atoms

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

Give an example of a reaction that has enthalpy change of atomisation of a compound

A

NaCl (s) —> Na (g) + Cl (g)

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

What is the first ionisation energy?

A

The energy needed to change 1 mole of gaseous atoms into 1 mole of gaseous 1+ ions

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

Write an equation representing the first ionisation energy of Mg

A

Mg (g) —> Mg+ (g) + e-

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

What is the second ionisation energy?

A

The energy needed to change 1 mole of gaseous 1+ ions into 1 mole of gaseous 2+ ions

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

Write an equation representing the second ionisation energy of Mg

A

Mg+ (g) —> Mg2+ (g) + e-

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

What is the first electron affinity?

A

The energy needed to change 1 mole of gaseous atoms into 1 mole of gaseous 1- ions

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

Write an equation for the first electron affinity of O

A

O (g) + e- —> O-

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

What is the second electron affinity?

A

The energy needed to change 1 mole of gaseous 1- ions into 1 mole of gaseous 2- ions

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

Write an equation for the second electron affinity of O

A

O- + e- —> O 2-

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

What is lattice enthalpy?

A

The enthalpy change when 1 mole of a solid ionic compound is formed from its gaseous ions

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

Write the reaction of Na+ and Cl- that has lattice enthalpy

A

Na+ (g) + Cl- (g) —> NaCl (s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is enthalpy change of hydration?

A

The enthalpy change when 1 mole of gaseous ions is dissolved in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Write the reaction of Na+ that has enthalpy change of hydration

A

Na+ (g) —> Na+ (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is enthalpy change of solution?

A

The enthalpy change when 1 mole of solute is dissolved in a solvent (e.g. water)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Write the reaction of NaCl that has enthalpy change of solution

A

NaCl (s) —> NaCl (aq)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What do ionic compounds form?

A

Regular structures called giant ionic lattices

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is a giant ionic lattice?

A

Where oppositely charged ions are held together by electrostatic attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is lattice enthalpy a measure of?

A

Ionic bond strength

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What happens when gaseous ions combine to make a solid ionic lattice?

A

Energy is given out - called the lattice enthalpy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

The more negative the lattice enthalpy, the…?

A

…stronger the ionic bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

What 2 factors affect the lattice enthalpy?

A

Ionic charge

Ionic radius

34
Q

How does ionic charge affect lattice enthalpy?

A

The higher the charges on the ions, the stronger the electrostatic attraction between ions, so the more energy is released when an ionic lattice forms, so the lattice enthalpy will be more negative

35
Q

How does ionic radius affect the lattice enthalpy?

A

The smaller the ionic radii of the ions involved, the higher the charge density of the ion. This means the electrostatic force of attraction between the ions is greater so the lattice enthalpy is more negative

36
Q

What is the trend in ionic radius down a group?

A

Ionic radius increases down the group

37
Q

Why does the ionic radius increase down a group?

A

Ionic radii increase down a group as more shells are added (per period)

38
Q

What is the direct route to form an ionic lattice from elements in their standard states?

A

Converting the elements in their standard states directly into an ionic lattice

39
Q

What is the indirect route to form an ionic lattice from elements in their standard states?

A

Forming gaseous atoms and converting them into gaseous ions, them form the ionic lattice

40
Q

What are the 4 stages to form an ionic lattice from atoms in their standard states by the indirect route, and state what the energy change is called for each one?

A
  • Gaseous atoms form (enthalpy change of atomisation)
  • Atoms of one element lose electrons to form a positive ion (first ionisation energy)
  • Atoms of one element gain electrons to form a negative ion (first electron affinity)
  • Positive and negative ions form a solid ionic lattice (lattice enthalpy)
41
Q

What is a Born-Haber cycle?

A

An enthalpy cycle that allows you to calculate the lattice enthalpy for a system

42
Q

What is Hess’s Law?

A

The total enthalpy change of a reaction is always the same, no matter which route is taken

43
Q

How do you find the lattice enthalpy?

A

It can’t be measured directly, so if you know all the other enthalpy changes, use Hess’s Law and the Born-Haber cycle to work out the lattice enthalpy

44
Q

What are the 3 differences on a Born-Haber cycle for a Group 2 element compared to other compounds?

A
  • There is an extra ionisation energy (2nd ionisation energy) to form a 2+ ion
  • You need to multiply the atomisation enthalpy of the non-Group 2 element by the number of moles of the element there are in 1 mole of ionic lattice
  • You need to multiply the first electron affinity of negative ion by the number of moles of ions formed
45
Q

What 2 things happen when a solid ionic lattice dissolves in water?

A
  • The bonds between the ions break to give gaseous ions

- Bonds between the ions and water are formed

46
Q

When a solid ionic lattice dissolves in water, the bonds between the ions break to give gaseous ions. Is this an exothermic or endothermic process?

A

Endothermic

47
Q

What is the enthalpy change equal to when the bonds between the ions in a solid ionic lattice break to give gaseous ions?

A

Negative lattice enthalpy

48
Q

When a solid ionic lattice is dissolved in water, bonds form between the ions and the water. Is this process endothermic or exothermic?

A

Exothermic

49
Q

When a solid ionic lattice is dissolved in water, bonds form between the ions and the water. What is this type of enthalpy change called?

A

Enthalpy change of hydration

50
Q

What is enthalpy change of hydration?

A

The enthalpy change when 1 mole of gaseous ions is dissolved in water

51
Q

Give an example of an equation for the enthalpy change of hydration?

A

Na+ (g) —> Na+ (aq)

52
Q

Why does water form bonds with ions?

A

Water is a polar molecule, where the oxygen is more electronegative than the hydrogen, so it has a dipole. The positive ions then form weak bonds with the partial negative charge on the oxygen and the negative ions form weak bonds with the partial positive charge on the Hydrogen

53
Q

What is the enthalpy change of solution?

A

The enthalpy change when 1 mole of solute is dissolved in a solvent

54
Q

Substances generally only dissolve if the energy…?

A

released is the same, or greater than, the energy taken in

55
Q

A reaction or state change is more likely when there is a… entropy change?

A

positive

56
Q

What effect on entropy does dissolving have?

A

Normally causes an increase in entropy

57
Q

Why does dissolving small, highly charged ions normally causes a decrease in entropy?

A

When water molecules surround the ions, there become more organised and orderly

58
Q

What are the 3 steps for drawing an enthalpy cycle to work out the enthalpy change of solution?

A
  • Put the ionic lattice and dissolved ions at the top and connect them with a line for enthalpy change of solution (direct route)
  • Connect the ionic lattice to the gaseous ions with a line for negative lattice enthalpy
  • Connect the gaseous ions to the dissolved ions with a line for hydration enthalpies of each ion
59
Q

What extra do you have to do when drawing an enthalpy cycle for 2+ or 2- ions?

A

You need to multiply the enthalpies of hydration by the number of moles of the ions that are reacting

60
Q

What 2 factors affect the enthalpy of hydration?

A

Ionic radius

Ionic charge

61
Q

Why do ions with a greater charge have a greater enthalpy of hydration?

A

Ions with a higher charge are better at attracting water molecules than ions with lower charge, so more energy is released when the bonds are made, so they have a more exothermic enthalpy of hydration

62
Q

Why do smaller ions (smaller ionic radius) have a greater enthalpy of hydration?

A

Smaller ions have a greater charge density than bigger ions. They attract water molecules better, so have a more exothermic enthalpy of hydration

63
Q

What is entropy?

A

A measure of dispersal of energy in a system (number of ways particles can be arranged)

64
Q

Which has a higher entropy, a gas or a solid?

A

Gas has a higher entropy because it’s more disordered

65
Q

What 3 factors affect entropy?

A

Physical state
Dissolution
Number of gaseous particles

66
Q

How does physical state affect the entropy?

A

Particles in a solid are fixed in a regular pattern, so they are very ordered, so have a low entropy. Gas particles are not fixed at all, so they can go wherever they want, do they’re very disordered so has a high entropy

67
Q

Why does dissolving a solid increase entropy?

A

Dissolved particles can move freely as they’re no longer fixed in one place

68
Q

How does the number of gaseous particles affect the entropy?

A

The greater the number of gas particles, the higher the entropy

69
Q

Why does a greater number of gaseous particles mean a greater entropy?

A

The more particles there are, the more combinations of ways that their energies can be arranged so a higher entropy

70
Q

Why is there an increase in entropy when water evaporates?

A

Because there is a state change from liquid to gas

71
Q

What is the equation to calculate entropy change, ΔS?

A

ΔS = S products - S reactants

72
Q

What are the units of entropy change?

A

J K^-1 mol^-1

73
Q

What is free energy change, ΔG?

A

A measure used to predict whether a reaction is feasible

74
Q

What is a feasible reaction?

A

A reaction that, once started, will carry on to completion, without any energy being supplied to it

75
Q

Is a reaction feasible if the ΔG (free energy change) value is negative or zero?

A

The reaction is theoretically feasible

76
Q

What is the equation for free energy, ΔG?

A

ΔG = ΔH - TΔS

ΔG: Free energy change
ΔH: Enthalpy change
T: Temperature
ΔS: Entropy change

77
Q

Even if the value of ΔG is negative or zero, why might a reaction not happen?

A

It might have a very high activation energy or very slow rate so that it’s not noticeable

78
Q

Why is an exothermic (-ve ΔH) reaction with a positive entropy change always feasible?

A

Because ΔG is always negative because ΔG = ΔH-TΔS

79
Q

Why is an endothermic (+ve ΔH) reaction with a negative entropy change not feasible?

A

Because ΔG would be positive because ΔG = ΔH-TΔS

80
Q

If a reaction is exothermic (-ve ΔH) and has a negative entropy change, will the reaction be feasible?

A

It’ll be feasible below a certain temperature where ΔG is zero or negative

A Level Chemistry Year 2 (7 decks)

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