3.1.8 Thermodynamics Flashcards

1
Q

3.1.8.1 Born-Haber cycles

Define enthalpy of formation.

A

The enthalpy change when one mole of a compound is formed from its constituent elements in their standard states under standard conditions.

Exothermic (-ve) for most substances

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2
Q

3.1.8.1 Born-Haber cycles

Define first ionisation energy.

A

Enthalpy change when each atom in 1 mole of gaseous atoms loses 1 electron to form 1 mole of gaseous 1+ ions.

Endothermic (+ve)

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3
Q

3.1.8.1 Born-Haber cycles

Define second ionisation energy.

A

Enthalpy change when each ion in 1 mole of gaseous 1+ ions loses 1 electron to form 1 mole of gaseous 2+ ions.

Endothermic (+ve)

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4
Q

3.1.8.1 Born-Haber cycles

Define enthalpy of atomisation.

A

Enthalpy change when 1 mole of gaseous atoms is produced from an element in its standard state.

Endothermic (+ve) → 1/2 I2 (s)→I (g)

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5
Q

3.1.8.1 Born-Haber cycles

Outline an example of enthalpy of atomisation.

A

½ I (s) →I (g)

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6
Q

3.1.8.1 Born-Haber cycles

Define bond enthalpy.

A

Enthalpy change when 1 mole of covalent bonds is broken in the gaseous state.

Endothermic (+ve)

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7
Q

3.1.8.1 Born-Haber cycles

Outline an example of enthalpy of formation.

A

2Na(s) + 1/2O2(g) →Na2O(s)

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8
Q

3.1.8.1 Born-Haber cycles

Outline an example for the first ionisation energy.

A

Mg(g) →Mg+ + e-

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9
Q

3.1.8.1 Born-Haber cycles

Outline an example for the second ionisation energy.

A

Mg+(g) →Mg2+(g) + e-

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10
Q

3.1.8.1 Born-Haber cycles

Outline an example of bond enthalpy.

A

I2 (g) →2I (g)

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11
Q

3.1.8.1 Born-Haber cycles

Define the first electron affinity.

A

When each atom in 1 mole of a gaseous atoms gains 1 electron to form 1 mole of gaseous 1- ions.

Exothermic (-ve) for many metals.

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12
Q

3.1.8.1 Born-Haber cycles

Outline an example for the first electron affinity.

A

O (g) + e- → O-(g)

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13
Q

3.1.8.1 Born-Haber cycles

Define the second electron affinity.

A

Enthalpy change when each ion in one mole of gaseous 1- ions gains 1 electron to form one mole of gaseous 2- ions.

Endothermic (+ve) as adding -ve electron to a -ve ion = +

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14
Q

3.1.8.1 Born-Haber cycles

Outline an example for the second electron affinity.

A

O- (g) + e- →O2- (g)

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15
Q

3.1.8.1 Born-Haber cycles

Define lattice enthalpy.

A

can be defined as either enthalpy of lattive dissociation or enthalpy of lattice formation.

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16
Q

3.1.8.1 Born-Haber cycles

Define lattice enthalpy of formation.

A

Enthalpy change when 1 mole of a solid ionic compound is formed into its consituent ions in gas phase.

Exothermic (-ve)

17
Q

3.1.8.1 Born-Haber cycles

Outline an example of lattice enthalpy of formation.

A

Mg2+ (g) + 2Cl- (g)→MgCl2 (s)

18
Q

3.1.8.1 Born-Haber cycles

Define lattice enthalpy of dissociation.

A

Enthalpy change when 1 mole of a solid ionic compound is broken up into its consituent ions in gas phase.

Endothermic (+ve)

19
Q

3.1.8.1 Born-Haber cycles

Outline an example of lattice enthalpy of dissociation.

A

MgCl2 (s) →Mg2+ (g) + 2Cl- (g)

20
Q

3.1.8.1 Born-Haber cycles

Define the enthalpy of hydration.

A

Enthalpy change when 1 mole of gaseous ions become aqueous ions / hydrated.

Exothermic (-ve), gives out energy as bonds are made between ion and H2O

21
Q

3.1.8.1 Born-Haber cycles

Outline an example of enthalpy of hydration.

A

Mg2+ (g) + aq→Mg2+(aq)

22
Q

3.1.8.1 Born-Haber cycles

Define enthalpy of solution.

A

Standard enthalpy change when one mole of an ionic solid dissolves in a large enough amount of water to ensure that the dissolved ions are well separated and do not interact with one another.

23
Q

3.1.8.1 Born-Haber cycles

Outline an example of enthalpy of solution.

A

MgCl2 (s)