Question

Based on this Lewis structure of an oxygen molecule, which statement is true?

A) The two oxygen atoms are sharing two valence electrons between them.
B) The two oxygen atoms are sharing six valence electrons between them.
C) The two oxygen atoms are sharing four valence electrons between them.
D) The two oxygen atoms are sharing eight valence electrons between them.

Answer 1

The oxygen molecule forms a double covalent bond by sharing two pairs (four) of electrons, which means six electrons are shared in total between the two oxygen atoms.

Step-by-step explanation:

The oxygen molecule (O2) is composed of two oxygen atoms, each with six electrons in its valence shell. These two oxygen atoms achieve stability by forming a double covalent bond, where they share two pairs of electrons between them. This sharing fills each oxygen atom's valence shell, bringing them to a stable state. A double covalent bond is represented in Lewis structures with two lines, indicating two pairs of shared electrons.

Therefore, the correct statement regarding the oxygen molecule's Lewis structure is: B) The two oxygen atoms are sharing six valence electrons between them.

Answer 2

The correct statement is that the two oxygen atoms in an oxygen molecule are sharing four valence electrons between them, as they form a double covalent bond.

Step-by-step explanation:

Based on the Lewis structure of an oxygen molecule, the statement that is true is C) The two oxygen atoms are sharing four valence electrons between them. An oxygen atom typically has six electrons in its valence shell and needs two more electrons to achieve a stable octet configuration. In an oxygen molecule (O₂), each oxygen atom shares two pairs of electrons with the other, forming a double covalent bond. This means there are a total of four electrons being shared between the two oxygen atoms.