Explain what is wrong with the following structure. An upper H is single-bonded to a H to the right, which is single bonded to an upper O with pairs of dots above, to the left, and below.

The structure does not obey the valence rule. From the structure, it is impossible for the hydrogen atom to bond to more than one atom.

The valence rule posits that an atomic element has the ability to gain or lose the maximum number of electrons in its outermost shell.

From the information, the hydrogen is bonded to a hydrogen atom and singly bonded to another oxygen atom.

This does not conform to the rule of valence electrons and therefore affects the stability of the hydrogen atom because the hydrogen has the ability to bond to only one atom and not two different atoms.

Therefore, we can conclude that the structure does not obey the valence rule and hydrogen can only bond to one atom at a time.

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The middle Hydrogen atom is bonded to two instead of one atom

Oxygen is bonded to one instead of two atoms

Oxygen has three instead of two lone pairs of electron.

Explanation:

If we look at the structure, we will notice that it does not satisfy the basic principles of valency.

Hydrogen has a valency of 1. However, the middle hydrogen atom is bonded to two atoms instead of only one atom - the other atom of hydrogen and an atom of oxygen.

Secondly, oxygen has three lone pairs instead of two lone pairs, hence it is bonded to only one instead of two atoms. This does not correspond to the known valency of oxygen.