- Joined
- May 18, 2009
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I don't quite understand why HIGHER branching = HIGHER Melting Point.
Boiling Point is quite easy. Higher branching causes steric hindrance from IM forces and hence it takes less energy to rip the molecules apart.
Melting Point seems counter-intuitive. High branching causes steric hindreance from IM forces, and hence it is easier to be a compact solid?
What is going on here?
If 2 isotopes exist: one branched (MP= 20C) and one unbranched (MP= -10C)
And it is 10 degrees C,
the branched one will be a solid and the unbranched will be a liquid.
Why does it take less energy to separate the nonbranched molecules?
Boiling Point is quite easy. Higher branching causes steric hindrance from IM forces and hence it takes less energy to rip the molecules apart.
Melting Point seems counter-intuitive. High branching causes steric hindreance from IM forces, and hence it is easier to be a compact solid?
What is going on here?
If 2 isotopes exist: one branched (MP= 20C) and one unbranched (MP= -10C)
And it is 10 degrees C,
the branched one will be a solid and the unbranched will be a liquid.
Why does it take less energy to separate the nonbranched molecules?