thermodynamics Flashcards

1
Q

standard enthalpy of formation

A

the enthalpy change when one mole of compound is formed from its elements, under standard conditions, all reactants and products in their standard states

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

first ionisation enthalpy

A

the standard enthalpy change when one mole of electrons is removed from one mole of gaseous atoms to give one mole of gaseous ions with a single positive charge

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

atomisation

A

enthalpy change when one mole of gaseous atoms are formed from an element in its standard state

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

mean bond enthalpy

A

-enthalpy change when one mole of gaseous molecules each break a covalent bond to form 2 free radicals
-over an average number of compounds

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

first electron affinity

A

standard enthalpy change when one mole of gaseous atoms is converted into one mole of gaseous ions each with a negative charge under standard conditions

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

lattice formation enthalpy

A

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

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

lattice dissociation enthalpy

A

standard enthalpy change when one mole of solid ionic compound dissociates into its gaseous ions

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

standard enthalpy of hydration

A

standard enthalpy change when one mole of gaseous ions is converted into one mole of aqueous ions

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

standard enthalpy of solution

A

standard enthalpy change when one mole of solute dissolves to form its aqueous ions

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

what 2 factors determine how exothermic a lattice enthalpy will be

A

-charge of ions
-size of ions

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

CRAM

A

-charge
-radius
-attraction
-more exothermic/endothermic

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

size of ions

A

smaller the ion, the greater the attraction to an oppositely charged ion

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

charge on ions

A

greater the charge, stronger the attraction to an oppositely charge ion

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

what is covalent character

A

ionic attraction between:
small positively charged ion
big negatively charged ion

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

theoretical model

A

PERFECT IONIC MODEL
- perfect spheres/point charges
-purely ionic bonding

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

experimental model

A

BORN HABER CYCLE
-polarisable ions
-ionic bonding plus some covalent character

17
Q

how to dissolve an ionic compound

A

-break ionic bonds
-form bonds between the water molecules and the ions

18
Q

entropy

A

-the amount of disorder within a system
-always a positive number
-entropy change is either a positive or negative value
- jk-1 mol-1

19
Q

calculating entropy changes

A

sum of products - sum of reactants

20
Q

gibbs

A

^G = ^H - (T x ^S)

21
Q

bond enthalpy

A

value of atomisation X2