1.8 Thermodynamics

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

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Front (Question)

Standard conditions

Back (Answer)

• 298°K • 100kPaH

Front (Question)

The strength of bonding in a lattice is given by…

Back (Answer)

Its lattice enthalpy

Front (Question)

Enthalpy of lattice dissociation

Back (Answer)

The enthalpy change to separate one mole of solid ionic compound into its gaseous ions

Front (Question)

Enthalpies of lattice dissociation Endothermic or exothermic?

Back (Answer)

Endothermic - Bonds are being broken so energy must be put in

Front (Question)

Enthalpy of lattice formation

Back (Answer)

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

Front (Question)

Enthalpies of lattice formation Endothermic or exothermic?

Back (Answer)

Exothermic - Bonds are being formed so energy is released

Front (Question)

How can lattice enthalpies be determined?

Back (Answer)

• Cannot be determined directly • Born-Haber cycles can be used

Front (Question)

Standard enthalpy of formation

Back (Answer)

The enthalpy change when one mole of a compound is formed from its constituent elements with all reactants and products in their standard states.

Front (Question)

Standard enthalpy of atomisation

Back (Answer)

The enthalpy change when one mole of gaseous atoms is formed from the element in its standard state.

#10

Front (Question)

Enthalpies of atomisation Endothermic or exothermic?

Back (Answer)

Endothermic - Gaseous atoms are formed by breaking bonds

#11

Front (Question)

Bond enthalpy

Back (Answer)

The heat energy required to break one mole of a given covalent bond in the molecules in the gaseous state

#12

Front (Question)

Bond enthalpy Endothermic or exothermic?

Back (Answer)

Endothermic - Energy required to break bonds

#13

Front (Question)

First ionisation energy

Back (Answer)

The energy required to remove one mole of electrons from one mole of atoms in the gaseous state.

#14

Front (Question)

First ionisation energy Endothermic or exothermic?

Back (Answer)

Endothermic - Energy is required to remove on electron

#15

Front (Question)

Second ionisation energy

Back (Answer)

The energy change when one mole of gaseous 2+ ions are formed from one mole of gaseous 1+ ions.

#16

Front (Question)

First electron affinity

Back (Answer)

The enthalpy change when one mole of gaseous 1- ions are formed from one mole of gaseous atoms.

#17

Front (Question)

First electron affinity Endothermic or exothermic?

Back (Answer)

Exothermic - Energy is released when the nucleus of an atom attracts an electron

#18

Front (Question)

Second electron affinity

Back (Answer)

The enthalpy change when one mole of gaseous 2- ions is formed from one mole of gaseous 1- ions

#19

Front (Question)

Second electron affinity Endothermic or exothermic?

Back (Answer)

Endothermic - Energy is required to overcome the repulsion between negative ion and negative electron

#20

Front (Question)

Perfect ionic model

Back (Answer)

Ions are perfect spheres with only electrostatic forces of attraction (no covalent character)

#21

Front (Question)

Assumption made for calculating theoretical values for lattice enthalpies

Back (Answer)

Perfect ionic model

#22

Front (Question)

What does it mean for an ionic substance to have covalent character?

Back (Answer)

Partial covalent bonding - Positive ion attracts e- in the negative ion - Ions are not spherical - Uneven distribution of charge

#23

Front (Question)

Distortion of the ions in an ionic compound

Back (Answer)

Polarisation

#24

Front (Question)

Factors that increase polarising power

Back (Answer)

Positive ions: Small and highly charged Negative ions: Large and highly charged