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Report (any type)/Brief report
22/09/2021
Water’s liquid state at room temperature and is probably attributable to hydrogen .
Water is a molecule of fairly negligible mass: ##18.01*g*mol^-1##. This is less than ammonia, or dioxygen, or dinitrogen, a little more than methane, but still less than ethane, and propane. And yet all these other molecules are GASES at room temperature, and have normal boiling points below that of water.
We know, or should know, that as atoms, and molecules get bigger, there should be a greater degree of dispersion forces that operate between particles, yet it seems that the boiling point of water is anomalously high. And so in fact it is.
The difference between water and these other molecules that another intermolecular force operates, and that is hydrogen bonding. Oxygen is electronegative with respect to hydrogen, and tends to polarize electron towards itself. The result is that we may represent the water molecule as ##””^(delta+)H-^(delta-)O^(delta-)-H^(delta+)##, i.e. as a dipole in which charge is strongly separated.
Given the strength of this dipole, and the small size of the water molecule, this interaction between the dipoles of adjacent molecules acts as a potent intermolecular force that elevates water’s boiling point.
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I want to thank your team (Jeff) for finding a new writer when you were unable to reach my existing writer to revise my paper. I appreciate your professionalism and efforts. Thanks
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