How does hydrogen bonding affect the melting point?

Let's get them all into K, simple 0k is -273°C so 273k is 0°C as both are linear in growth, just different start points. so 273 + 1064 is the...

You often see in the literature the phrase, $"recrystallized to constant melting point"$; i.e. a material is successively recrystallized until a consistent melting point is achieved. Often, after repeat recrystallizations,...

I would guess, $H_2Te$ $>$ $H_2Se$ $>$ $H_2S$ $"<<"$ $H_2O$ with respect to melting point. But as a chemist, as a physical scientist, you are required to interpret data,...

Hydrogen is a strong bond, therefore, it produces a lower evaporation rate and thus, a lower vapor pressure.

Hydrogen Bonding is a type of dipole-dipole interaction. This means that there are permanent partial charges on hydrogen and oxygen in water, so they attract each other from separate molecules....

Consider water, $OH_2$. This is a very low molecular weight material that has quite an elevated normal boiling point. The strength and persistence of intermolecular hydrogen bonding is responsible for...

Hydrogen bonding occurs where HYDROGEN is bound to a strongly electronegative element, i.e. hydrogen is bound to fluorine, nitrogen, or oxygen. In $"fluoroform"$, the hydrogen is bound to carbon not...

The melting points (and undoubtedly also the boiling points) of the nitro phenols reflect the degree of intermolecular hydrogen bonding. For $"orthonitrophenol"$, hydrogen bonding would be intramolecular, i.e. confined to...

The normal melting point of methanol is $-97.6$ $""^@C$. But here, clearly, we compare apples and oranges, by comparing a melting point, a transition from solid to liquid, to...

Well, let's take the average using absolute temperature: $((54+265.7)*K)/2$ $=$ $159.9*K$ $=-113$ $""^@C$. The literature melting point of chlorine is $-101.5$ $""^@C$, so this estimate is a good first approximation....