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A Level Chemistry > Chapter 17: Thermodynamics > Flashcards

Chapter 17: Thermodynamics Flashcards

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1
Q

Bond Dissociation Enthalpy

A

The enthalpy change for breaking 1 mole of bonds in 1 mole of gaseous molecules.

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2
Q

What type of process is bond dissociation enthalpy?

A

Endothermic

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3
Q

Example of bond dissociation enthalpy reaction

A

Cl2 (g) -> Cl (g) + Cl (g)

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4
Q

Standard Enthalpy of Formation

A

Enthalpy change when 1 mole of a substance is formed from its elements under standard conditions (298K and 100kPa), with all substances being in their standard states.

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5
Q

What type of process is standard enthalpy of formation?

A

Exothermic

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6
Q

Example of standard enthalpy of formation reaction

A

C (s, graphite) + 2H2 (g) -> CH4 (g)

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7
Q

Enthalpy of Atomization

A

Enthalpy change when 1 mole of gaseous atoms of a substance are formed from the substance in its standard state under standard conditions (298K and 100kPa).

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8
Q

What type of process is enthalpy of atomization?

A

Endothermic

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9
Q

Example of enthalpy of atomization reaction

A

1/2 Cl2 (g) -> Cl (g)

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10
Q

Ionization Enthalpy

A

Enthalpy change for the conversion of 1 mole of gaseous atoms to 1 mole of gaseous cations, each atom losing an electron.

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11
Q

What type of process is ionization enthalpy?

A

Endothermic

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12
Q

Example of ionization enthalpy reaction

A

Na (g) -> Na+ (g) + e-

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13
Q

Second Ionization Enthalpy

A

Involves the removal of a second electron from the gaseous cation.

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14
Q

What type of process is second ionization enthalpy?

A

Endothermic

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15
Q

Example of second ionization enthalpy reaction

A

Na+ (g) -> Na2+ (g) + e-

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16
Q

Enthalpy of Electron Affinity

A

Enthalpy change for the conversion of 1 mole of gaseous atoms into 1 mole of gaseous anions, each atom gaining an electron.

17
Q

What type of process is enthalpy of electron affinity?

A

Exothermic

18
Q

Example of enthalpy of electron affinity reaction

A

Cl (g) + e- -> Cl- (g)

19
Q

Second Electron Affinity

A

Enthalpy change for the conversion of 1 mole of gaseous 1- ions to 1 mole of gaseous 2- ions by gaining one electron.

20
Q

What type of process is second electron affinity?

A

Endothermic

21
Q

Example of second electron affinity reaction

A

O- (g) + e- -> O2- (g)

22
Q

Lattice Formation Enthalpy

A

Enthalpy change for the formation of 1 mole of solid ionic compound from its constituent gaseous ions.

23
Q

What type of reaction is lattice formation enthalpy?

A

Exothermic

24
Q

Example of lattice formation enthalpy reaction

A

Na+ (g) + Cl- (g) -> NaCl (s)

25
Q

Lattice Dissociation Enthalpy

A

Enthalpy change when 1 mole of an ionic lattice dissociates into isolated gaseous ions.

26
Q

What type of process is lattice dissociation enthalpy?

A

Endothermic

27
Q

Example of lattice dissociation enthalpy reaction

A

NaCl (s) -> Na+ (g) + Cl- (g)

28
Q

Enthalpy of Solution

A

Enthalpy change when 1 mole of an ionic compound is dissolved in water to produce aqueous ions in its standard state under standard conditions.

29
Q

Stage 1 of Enthalpy of Solution

A

Separating the ions in the crystal- lattice dissociation enthalpy

30
Q

What type of process is stage 1 of enthalpy of solution?

A

Endothermic because energy is required to overcome attractive forces between the ions.

31
Q

Stage 2 of Enthalpy of Solution

A

Hydration of ions- the ions form bonds with the H2O molecules

32
Q

Standard Enthalpy of Hydration

A

Enthalpy change when 1 mole of gaseous ions is converted to 1 mole of aqueous ions in its standard state under standard conditions.

33
Q

What type of reaction is standard enthalpy of hydration?

A

Exothermic

34
Q

Example of standard enthalpy of hydration reaction

A

Na+ (g) -> Na+ (aq)

35
Q

Mean Bond Enthalpy

A

Average enthalpy change for breaking 1 mole of a particular bond in a range of different compounds in the gas phase.

36
Q

What type of process is mean bond enthalpy?

A

Endothermic

37
Q

Steps of Constructing a Born-Haber Cycle

A 
Step 1: atomisation of the metal
Step 2: atomisation of the non-metal
Step 3: ionisation of the metal
Step 4: electron affinity of the non-metal
Step 5: formation of the lattice

A Level Chemistry (5 decks)

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