Question

Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? A. There is a single bond, a double bond, and six lone pairs. B. There is a single bond and four lone pairs. C. There is a single bond and six lone pairs. D. There is a double bond and six lone pairs.

Answer 1

Answer:

None of these

Explanation:

$O_2$:-

Valence electrons of oxygen = 6

The total number of the valence electrons  = 2(6) = 12

The Lewis structure is drawn in such a way that the octet of each atom and duet for the hydrogen in the molecule is complete. So, The Lewis structure is shown in image below.

Formula for formal charge :

$\text{Formal charge}=\text{Valence electrons}-\text{Non-bonding electrons}-\frac{\text{Bonding electrons}}{2}$

Formal charge for oxygen:

$\text{Formal charge}=6-4-\frac{4}{2}=0$

From the structure,

Number of bond pairs = 4 (Double bond)

Number of lone pairs = 4

Hence, the correct option is:-   None of these

Answer 2

The structure is the representation of the sharing and the transfer of electrons between the atoms to form the bond. The Lewis structure of oxygen has one single bond and four lone pairs.

What is Lewis dot structure?

The Lewis dot structure is the representation of the valence electron in the form of dot, and the sharing of electrons between the atoms.

The oxygen atom has been consisted of 6 valence electrons. The oxygen atom requires 2 electrons to complete the octet. Thus, the 2 electrons are shared between two oxygen atoms, forming the bond and stabilizing the atom.

The Lewis dot structure is given in the image attached. It can be described as the there is the presence of a single bond, and four lone pairs are available in the structure.

Thus, option B is correct.

Learn more about the Lewis structure, here:

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