Question

29
in the lewis structure for the of2 molecule, the number of lone pairs of electrons around the
central oxygen atom is * (0.5 points)
2
3
0
4
1

Explanation:

Step1: Determine valence electrons

Oxygen has 6 valence electrons (\(6e^-\)), and each fluorine has 7 valence electrons (\(2\times7e^-\)). Total valence electrons \(=6 + 2\times7=20e^-\).

Step2: Form bonds

Oxygen forms single bonds with two fluorine atoms (\(2\times2e^-\) used in bonding). Remaining electrons \(=20 - 4 = 16e^-\).

Step3: Distribute remaining electrons

These 16 electrons are distributed as lone pairs. Each fluorine gets 3 lone pairs (\(2\times3\times2e^-\)), using \(12e^-\). The remaining \(16 - 12 = 4e^-\) are on oxygen as 2 lone pairs (\(\frac{4e^-}{2e^-\text{ per pair}} = 2\) pairs).

Answer:

2