Energetics 2 Flashcards

1
Q

Lattice energy

A

The energy change when one mole of an ionic solid is formed from its gaseous ions

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2
Q

Atomisation energy

A

The energy change for the formation of one mole of gaseous atoms from an element in its standard state at 298K and 100kPa
Eg 1/2Br2(l)=>Br-(g)

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3
Q

Electron affinity

A

First electron affinity is the energy change for the addition of one electron for each mole of atoms in the gas phase

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4
Q

Second electron affinity

A

Energy change for the addition of one electron for each mole of ions with a negative charge in the gas phase

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5
Q

Lattice energy provides a measure of

A

Ionic bond strength

Always exothermic as is the energy of bonds being made

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6
Q

Experimental lattice energy value is

A

From a born-Haber cycle

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7
Q

Theoretical lattice energy value is

A

Obtained from electrostatic theory
Based on: ionic charges and ionic radii
Assumes perfect ionic bonding

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8
Q

Comparing experimental and theoretical lattice energy values indicates

A

The degree of covalent bonding

Possible covalent character?

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9
Q

Polarising power

A

Based on the strength of the pull of cations on the electrons and how much the anion allows the electrons to be pulled

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10
Q

Factors that increase polarisation in ionic compound are

A
  • increased charge on anion or cation
  • increased size of anion
  • decreased size of cation
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11
Q

The greater the polarisation effect on covalent character

A

The greater the covalent character

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12
Q

Hydration of ions

A

When ionic substances in water, polar water highly attracted to ions
The process of water molecules linking to ions
Water molecules are vibrating, s as they bond to the ions they the ions free from the lattice

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13
Q

Enthalpy of hydration

A

Heat energy change when one mole of gaseous ions dissolve in an excess of water to form an infinitely dilute solution under standard conditions

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14
Q

Enthalpy of solution

A

Heat energy change when one mole of ionic solid dissolved in excess water in standard conditions

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15
Q

Enthalpy of hydration is affected by

A

Ionic radii
Ionic charges
Greater attraction more energy released

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16
Q

Entropy

A

Measure of the disorder of a system and that the natural direction of change is increasing total entropy

17
Q

Entropy change of a system =

A

Entropy change of products - entropy change of reactants

18
Q

Entropy change of surroundings =

A
  • enthalpy / temperature
19
Q

Total Entropy change =

A

Entropy change of systems + entropy change of surroundings

20
Q

2nd law of thermodynamics

A

For a reaction to be feasible at a given temperature total entropy change > 0

21
Q

Entropy changes occur during

A
  • changes of state
  • dissolving of a solid ionic lattice
  • reactions where there is a change in the number of moles from reactants to products
22
Q

Gibbs free energy change

A

Enthalpy - (temperature x entropy change of system) < 0 to be feasible

23
Q

Gibbs at equilibrium =

A

-R x T x lnK