Question

Draw Lewis dot structures for each hypothetical molecule shown below, using the correct number of valence electrons for each atom. Determine which molecules make sense because each atom has a complete valence shell, and each bond has the correct number of electrons. Explain what makes the other molecule nonsensical, considering the number of bonds each type of atom can make.

Short answer

Lewis's structure of the given structure a and b is illustrated and explained in the following description in which part a is the correct structure and part b is an incorrect structure.

This is because the hydrogen in part ‘(b)’ is sharing two electrons with two different carbons, which is not possible.

Step-by-step solution

Definition of Lewis structure, the valence electron, and valence shell

The dot structure representing the lone pairs of electrons and the bonding between the molecules is known as the Lewis structure.

A valence electron is an electron that is present in the outermost shell of the atom. It donates to the other atom that lacks the electrons.

A valence shell is an orbit in which the valence electron revolves around the nucleus of an atom.

Explanation of part ‘(a)’

The Lewis structure of part ‘a’ is illustrated as above. In this structure, the valence structure in the molecule given is complete. The bonds between each atom in the structure share the exact and correct number of electrons.

Explanation of part ‘(b)’

The Lewis structure of part ‘b’ is illustrated as above. In this structure, the representation of the hydrogen atom is wrong since the hydrogen atom can donate one electron to the other atom. In this structure, the hydrogen atom bonds with two different atoms, which can never happen.