Thomson Definitions Flashcards

1
Q

Lattice Enthalpy (delta H le)

A

The Enthalpy change that accompanies the formation of one mile of an ionic compound from its gaseous ions under standard conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Give an equation for the lattice Enthalpy of KCl

A

K+(g) + Cl- (g) ———> KCl(s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Give an equation for the lattice Enthalpy of KCl

A

K+(g) + Cl- (g) ———> KCl(s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Standard Enthalpy of formation (delta H f)

A

The Enthalpy change that occurs when one mole of a compound is formed from its constituent elements under standard conditions. All reactants and products being in their standard states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Give the equation of the Enthalpy of formation for KCl (s) (delta H f)

A

K(s) + 1/2Cl2 ———> KCl(s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Standard Enthalpy change of atomisation (delta H at)

A

The Enthalpy change that occurs when one mole of gaseous atoms form from the element on its standard state

(Making it a gas)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Give an equation for the Enthalpy change of atomisation (delta H at)

A

K(s) ———> K(g)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

First ionisation energy (Delta H ie1)

A

The Enthalpy change accompanying the removal of one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Give an equation for first ionisation energy

A

K(g) ———> K+ + e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Second ionisation Enthalpy (delta H ie2)

A

The Enthalpy change that accompanies the removal of one electron from each ion in one moles of gaseous 1+ ions to form one mole of 2+ gaseous ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Why is the second ionisation Enthalpy higher than the first

A

The outer shell of electrons is pulled in as one electron is removed. The ionic radius decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Give an equation for the second ionisation Enthalpy

A

Ca+ ———> Ca2+ +e-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Why are ionisation energies endothermic

A

Requires energy to overcome the electrostatic attraction between the negative electrons and the positive nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

First electron affinity (delta H ea1)

A

The Enthalpy change accompanying the addition of one electron to each atom in one like of gaseous atoms to form one mole of 1- ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Equation of first electron affinity

A

Cl +e- ———> Cl-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Second electron affinity (delta H ea2)

A

The Enthalpy change thag accompanies the addition of one electron to one mole of gaseous 1- ions to form one mole of gaseous 2- ions

17
Q

Equation for second electron affinity

A

O- + e- ———> O2-

18
Q

Why is the first electron affinity negative but the second positive

A

The first electron affinity is negative because the positive nucleus attracts the negative e-

The second is positive needs energy as the whole negative ion repels the electron