Which of the following best explains how two oxygen atoms, each with six valence electrons, can bond with each other?

• A. They share two pairs of electrons to form a double covalent bond.
• B. They form a metallic bond by pooling their valence electrons.
• C. They share one pair of electrons to form a single covalent bond.
• D. One oxygen atom transfers two electrons to the other, forming an ionic bond.

Answer: (A)

Verified step by step guidance

1. Step 1: Understand the valence electron configuration of oxygen atoms. Each oxygen atom has six valence electrons, needing two more electrons to complete its octet (8 electrons in the valence shell).
2. Step 2: Recognize the types of chemical bonds: ionic bonds involve transfer of electrons, covalent bonds involve sharing electrons, and metallic bonds involve pooling electrons in a 'sea' of electrons.
3. Step 3: Analyze the bonding possibilities between two oxygen atoms. Since both have similar electronegativities and need electrons to complete their octets, they are more likely to share electrons rather than transfer them.
4. Step 4: Determine how many electron pairs must be shared. Each oxygen needs two electrons to complete its octet, so they share two pairs of electrons, forming a double covalent bond.
5. Step 5: Conclude that the best explanation is that the two oxygen atoms share two pairs of electrons to form a double covalent bond, which satisfies the octet rule for both atoms.