What is the correct Lewis structure for O2? A) O-O B) :-: C) = D) : O ≡ O : E) none of the above
The Correct Answer and Explanation is :
The correct Lewis structure for dioxygen (O₂) is option C) =, which represents a double bond between the two oxygen atoms.
Explanation:
- Understanding the Basics: Oxygen (O) is in Group 16 of the periodic table and has six valence electrons. To form a stable molecule, oxygen atoms tend to share electrons. The goal of drawing a Lewis structure is to illustrate how the atoms are bonded and how the electrons are distributed.
- Valence Electrons: Each oxygen atom contributes six valence electrons, giving a total of 12 electrons for the O₂ molecule. The Lewis structure should account for all these electrons.
- Bonding: Oxygen typically forms two bonds to achieve a full outer shell (octet rule), which consists of eight electrons in total.
- Single Bond: A single bond (represented by a single line, as in A) would result in each oxygen atom sharing only two electrons, leading to only four electrons total around each atom, which is insufficient for stability.
- Double Bond: A double bond (represented by two lines, as in C) allows each oxygen atom to share four electrons (two pairs), fulfilling the octet requirement. In this case, each oxygen atom would have eight electrons around it, making the molecule stable.
- Other Options:
- A) O-O: This represents a single bond, which is incorrect.
- B) :-:: This suggests lone pairs, but doesn’t convey the bonding accurately.
- D) : O ≡ O :: This indicates a triple bond, which is not applicable since oxygen typically does not form a triple bond with itself in O₂.
- Conclusion: Therefore, the correct representation of the Lewis structure for O₂, demonstrating the two oxygen atoms bonded by a double bond, is C) =. This structure indicates that the molecule is stable, with each oxygen atom having a complete octet, fulfilling the chemical bonding requirements for diatomic oxygen.