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Both the enthalpy and entropy give off energy,
Water can be sub cooled; remain a liquid below it's melting point, quite easily because of the two competing bonding states of its hydrogen bonds.
The hydrogen bonds are like binary switches
Since the polar state is denser
One can fool liquid water to maintain itself below it melting point, by flipping the hydrogen bond switch.
When ice melts, the shift from covalent to polar/covalent,
The reason is, since water expands as we heat it, the hydrogen bonding switches are being flipped more to the covalent side. The net affect is the hot water is set up better for the transition to the covalent state needed for freezing. The cold water is denser and is more polar so it resists; supercools, to maintain higher entropy.