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A-Level Chemistry > Lattice enthalpy > Flashcards

Lattice enthalpy Flashcards

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1
Q

What is lattice enthalpy?

A

The enthalpy change that accompanies the formation of one mole of an ionic lattice compound from its gaseous ions under standard conditions

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2
Q

What is lattice enthalpy a measure of?

A

Strength of ionic bonding in a giant ionic lattice

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3
Q

What type of enthalpy change is lattice enthalpy always?

A

Exothermic - it always has a negative value

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4
Q

What is a Born-Haber cycle?

A

An energy cycle used to determine lattice enthalpy

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5
Q

What is standard enthalpy change of atomisation?

A

The enthalpy change that takes place for the formation of one mole of gaseous atoms from the element in the standard state, under standard conditions

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6
Q

What is first ionisation energy?

A

The enthalpy change required to remove one electron from each atom in mole of gaseous atoms to form one mole of gaseous +1 ions

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7
Q

Are ionisation energies endothermic or exothermic?

A

Endothermic

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8
Q

What is the first electron affinity?

A

The enthalpy change that takes place when one electron is added to each atom in mole of gaseous atoms to form one mole of gaseous 1- ions

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9
Q

Are first electron affinities exothermic or endothermic?

A

Exothermic

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10
Q

What is required if an anion has a greater charge than -1, such as O 2-?

A

Successive electron affinities are required

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11
Q

Are second electron affinities endothermic or exothermic?

A

Endothermic

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12
Q

What is the Born-Haber cycle for magnesium oxide?

A
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13
Q

What are the calculations you’d for the magnesium oxides Born-Haber cycle?

A
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14
Q

Why may enthalpy values need to be halved or doubled in lattice enthalpy calculations?

A

Depending on the moles of elements in the ionic solid involved

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15
Q

What is enthalpy change of solution?

A

The enthalpy change that takes place when one mole of an ionic substance dissolves in sufficient water to form an infinitely dilute solution

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16
Q

Is enthalpy change of solution endothermic or exothermic?

A

Either

17
Q

What is enthalpy change of hydration?

A

The enthalpy change when 1 mole of a specified gaseous ion dissolves in sufficient water to form an infinitely dilute solution

18
Q

Are hydration enthalpies endothermic or exothermic?

A

Exothermic

19
Q

What 2 processes take place when a solid ionic compound dissolves in water?

A
  • The ionic lattice is broken up forming separate gaseous ions (opposite of lattice enthalpy)
  • The separate gaseous ions interact with polar water molecules to form hydrated aqueous ions. The energy change involved is the enthalpy change of hydration
20
Q

What is the equation for enthalpy of solution?

A

Enthalpy of solution = reverse lattice enthalpy + hydartion enthalpy

21
Q

What is the equation for enthalpy of solution?

A

Enthalpy of solution = reverse lattice enthalpy + hydration enthalpy

22
Q

What is the energy cycle between gaseous ions, aqueous ions and an ionic lattice?

A
23
Q

How do you find the total Δhyd H?

A

Add together the Δhyd H values of both anions and cations together

24
Q

What are the effects of ionic charge on lattice enthalpy?

A
  • Ionic charge increases
  • Attraction between ions increases
  • Lattice energy becomes more negative
  • Melting point increases - lattice enthalpy incdreases
25
Q

What are the effects of ionic size on lattice enthalpy?

A
  • Ionic radius increases
  • Attraction between ions decreases
  • Lattice enthalpy less negative
  • Melting point decreases - lattice enthalpy decreases
26
Q

What are the affects of ionic charge on hydration?

A
  • Ionic charge increases
  • Attraction with water molecules increases
  • Hydration energy becomes more negative
27
Q

What are the effects of ionic size on hydration?

A
  • Ionic radius increases
  • Attraction between ion and water molecules decreases
  • Hydration energy less negative

A-Level Chemistry (42 decks)

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