Question

Question #f965b

Answer 1

Different boiling points!

Explanation:

Water and nitrogen both have very different boiling points.

Pure water has a boiling point of `100^@C`. In that state, it turns into a gas. Below `100^@C` and above `0^@C`, water is a liquid.

Nitrogen, on the other hand, has a very low boiling point, which is `-195.8^@C`. So, if the temperature is above `-195.8^@C`, then it will exist as a gas.

Therefore, at room temperature, which is around `25^@C`, water exists as a liquid, while nitrogen exists as a gas.

Answer 2

They have different condensation points, affecting their covalent bonds and the intensity of compounds in an area.

Explanation:

Compared to Nitrogen, Water has a much higher condensation point of 0-100 degrees celsius, nitrogen at-195.8.

Therefore, when water is still in liquid state, the nitrogen will be in the state gas. This is due to the difference in condensation point, which affects the covalent bonds between the compounds, affecting the state of matter of the compound directly.

When there is a stronger covalent bond, the force of attraction between compounds are stronger, therefore causing the compounds to be more densely packed, changing its state. (stronger covalent bonds -> more densely packed -> solid
weaker covalent bonds -> less dense -> gas)

Due to the difference in condensation points, both covalent compounds may not be able to be in the same state of matter under the same temperature.

Answer 3

Consider the degree of `"intermolecular force"` that operates between each set of molecules....

Explanation:

For the dinitrogen molecule, the `"intramolecular force"`, the force between atoms, is strong. So strong that the `N-=N` triple bond is one of the strongest bonds known. However, the intermolecular force is relatively weak...only dispersion forces operate between molecules, which depend on the transient polarizability of only a few electrons...there are NO molecular dipoles that could operate between molecules.

On the other hand, in the water molecule, while the `H-O` bond is certainly weaker than the intramolecular bond in the dinitrogen molecule, the INTERMOLECULAR force is relatively strong. And this is a consequence of hydrogen-bonding, where hydrogen is bound to a strongly electronegative element, such as oxygen or nitrogen or fluorine....

....the heteroatom polarizes electron density towards itself to give `stackrel(delta+)H-stackrel(delta-)O-H`, `stackrel(delta+)H-stackrel(delta-)F` or `stackrel(delta+)H-stackrel(delta-)NH_2` dipoles, and these dipoles interact with each other in the bullk solution, andcin aggregate this constitutes a POTENT INTERMOLECULAR force.

The result? Water has a normal boiling point of `100` `""^@C`, the which is absurdly high for such a small molecule. The boiling points of ammonia, `-33.3` `""^@C`, and hydrogen fluoride, `+19.5` `""^@C`, are also high. Compare the hydrides of the lower group members, `HCl`, `H_2S`, `PH_3` etc. (you will have to look these up), the which, although bigger, heavier molecules, with more electrons, have reduced volatilities with respect to the first-row hydrides, because their hydrogen-bonding interaction is not so strong.