Summary
Summary Physical Chemistry Complete Definitions
A complete collection of all the physical chemistry definitions you will need to know, including equations.
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Standardconditi
Pressure 100hPa
ENTHALPY :÷:÷ ::* .
State Physical state of a substance under
standard conditions
-
Enthalpy change of a reaction or Hit
The that accompanies reaction in the lattice enthalpy 4etF
enthalpy change a
shown in a chemical equation under standard The that accompanies the formation of mole of
molar quantities enthalpy change one
conditions with ,
all reactants and products in their standard an ionic compound from its gaseous ions under standard conditions
↳
states it is a measure of the
strength of ionic bonding in a lattice
Mg 1st
t
I 0,191 →
My 0151 Or H? -
602kt mot
"
ktcg) t (I
-
(g) → KC1 Is ) OLEH ? -711 KTMOI
- '
Or H°=
'
1M quit 2 1204 ktmot
0,1g) →
Mgocsl
-
Exothermic
Exothermic or endothermic
Enthalpy change of solution Osoi Htt
Enthalpy
D-
change of formation Of H
The when one mole of a
enthalpy change that takes place
Enthalpy change that takes place when one mole of a compound solute dissolves in a solvent
is formed from its elements under standard conditions with all reactants ,
wastes , tag → Natcaq) CI
-
Oso , Htt +4kt mot
"
t
caq) :
and products in their standard states
Exothermic or endothermic
I MG0 Of Htt
"
0 -602 KJMOI
Mg 1st t (9) → a) =
,
Exothermic or endothermic Enthalpy change of hydration 0nydH°
Of Hoot an element = 0 The enthalpy change that accompanies the dissolving of gaseous ions in
water to form one mole of aqueous ions .
Enthalpy change of combustion 0cH°
Natcaq) Onyd H0
'
Nate g) taq → = -
406kt moi
The change that takes place when one mole of a substance
enthalpy Exothermic
reacts completely with oxygen under standard conditions , with all reactants
and products in their standard states
first ionisation energy 0
, #
Ht
C4H , (g) t 6 I0 , G) → 410 , loft 5thOH1 0CH ? -2877kt mot
'
The enthalpy change required to remove one electron from each
Exothermic atom in one mole of gaseous atoms to
form one mole of gaseous
It ions .
Enthalpy change of neutralisation One at H0
Endothermic
The enthalpy change that accompanies the reaction of an acid by
Naia, → rateg) + e- 0
,
HI t 496kt moi
"
a base to
form one mole of H , 0 IN Under standard conditions wait , g) I 2nd
,
Nat , g) → + e- ionisation energy is bigger than the first 4£ HI ,
+4561
.
'
KTMOI
with all reactants and products standard states
in their .
Energy to lose electrons
'
Htcaq )
-
t OH can → H , 0 4) One at H -
57kt mot
-
'
HE -57kt moi first Hit
HC1 1AQ ) NA0H can O neut
affinity Of .az
'
t H , 01Mt Nathan electron
.
→
The value of Oneutttis the same for all reactions The enthalpy change that takes place when one electron is added
to each atom in one mole of gaseous atoms to form one mole of gaseous
Enthalpy change of atomisation Oath t
-
ions .
The enthalpy change that takes place for the formation of one 1st electron exothermic however 2nd 3rd endothermic
affinity is
,
,
etc are
µY⑧µ
mole of gaseous atoms from the element in its standard state under 041 t e
-
→ 0
-
4) OEAIH ! -
141kt mot
"
standard conditions 04g ) 0.ca , Ho
am
-
O
-
'
eg) te
→ 790kt moi
-
. -
- t
" " '
Na Is) → Na 191 Oath t 107 KTMOI '
Energy
:
to gain electrons
I C1 2CG ) → C1 1GI 0 at
H°= t 12 I KTMOI
"
Endothermic (bonds are broken )
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