Question

in the lewis structure for the of₂ molecule, the number of lone pairs of electrons around the central oxygen atom is
a 0
b 1
c 3
d 2

Explanation:

Step1: Determine valence electrons

Oxygen has 6 valence electrons (\(6\)), and each fluorine has 7 valence electrons (\(2\times7 = 14\)). Total valence electrons: \(6+14=20\).

Step2: Form bonds

O is the central atom. Each O - F bond uses 2 electrons. Two O - F bonds use \(2\times2 = 4\) electrons. Remaining electrons: \(20 - 4=16\).

Step3: Distribute remaining electrons

These 16 electrons are distributed as lone pairs. Each F atom gets 3 lone pairs (\(2\times3\times2 = 12\) electrons for F). The remaining \(16-12 = 4\) electrons are on O as \(4\div2=2\) lone pairs.

Answer:

D. 2