Which of the following chemical structures can form hydrogen bonds with water? methane (ch4), molecular oxygen (o2), hydrogen sulfide. explain.

Molecular oxygen and Hydrogen fluoride.

Explanation:

Definition:

Hydrogen bonding:

It is a type of dipole-dipole attraction between the hydrogen atom and more electronegative atoms.

In hydrogen bonding mostly the highly electronegative atoms are fluorine, nitrogen and oxygen.

Explanation:

In given compound such as methane CH₄ the electronegativity of carbon is 2.55 while that of hydrogen is 2.2 so there is smaller electronegativity difference that's why it can not form hydrogen bond.

In case of molecular oxygen the electronegativite atom oxygen is present. It can form hydrogen bonds with water. its electronegativity is 3.44.

In case of hydrogen fluoride the electronegativity atom fluorine is present. It will form hydrogen bonds with water. Its electronegativity is 3.98. So it is more likely to take part in hydrogen bonding.

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

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