Studied by 1 person(+) ∆H
Endothermic
(-) ∆H
Exothermic
What is ∆H
Change in Enthalpy
What is ∆S
Change in Entropy (disorder)
(+) ∆S
Entropically Favorable
(-) ∆S
Entropically Unfavorable
What is ∆G when ∆H is (+) and ∆S is (+)?
At high temperatures, ∆G is spontaneous (-).
At low temperatures, ∆G is nonspontaneous (+)
What is ∆G when ∆H is (-) and ∆S is (-)?
At high temperatures, ∆G is nonspontaneous (+).
At low temperatures, ∆G is spontaneous (-)
What is ∆G when ∆H is (-) and ∆S is (+)?
∆G is spontaneous (-) at all temperatures
What is ∆G when ∆H is (+) and ∆S is (-)?
∆G is nonspontaneous (+) at all temperatures
∆G, ∆H, and ∆S are all state functions. Define state functions.
They are path independent; follow displacement, meaning the value is independent of the path chosen
Square Planar Complexes
Coordination Number: 4, d8 electron configuration
Always low-spin (fill all lower levels before moving up)
Tetrahedral Complexes
Coordination Number: 4
Always high spin (half fill all orbitals first then go back and double)
High Spin Ligand
weak crystal field splitting energy, weak field ligand
Low Spin Ligand
strong crystal field splitting energy, strong field ligand
Diamagnetic
no unpaired electrons
Paramagnetic
>0 unpaired electrons
1st law of Thermodynamics
Energy cannot be created no destroyed, only transferred
2nd law of Thermodynamics
all spontaneous chemical processes increase entropy (disorder) of universe
Note
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