Question

question 13
in the lewis structure for the of₂ molecule, the number of lone pairs of electrons around the central oxygen atom is
a 3
b 1
c 0
d 2

Explanation:

Step1: Determine valence electrons

O has 6 valence electrons, each F has 7. Total valence electrons: \(6 + 2\times7=20\).

Step2: Form bonds

O forms single bonds with two F atoms. Each bond uses 2 electrons, so \(2\times2 = 4\) electrons used in bonding.

Step3: Distribute remaining electrons

Remaining electrons: \(20 - 4=16\). These are distributed as lone pairs. Each F gets 3 lone pairs (\(2\times3\times2 = 12\) electrons for F's lone pairs). The remaining \(16-12 = 4\) electrons are on O as 2 lone pairs (\(\frac{4}{2}=2\)).

Answer:

D. 2