Question

For $OF _2$ molecule consider the following : A Number of lone pairs on oxygen is 2 B FOF angle is less than $1045^{\circ}$ C Oxidation state of $O$ is $-2$ D Molecule is bent ' $V$ ' shaped E Molecular geometry is linear correct options are:

• A. A, C, D only
• B. C, D, E only
• C. B, E, A only
• D. A, B, D only

Answer 1

The Correct Option is D

The question involves determining the correct statements about the molecule \(OF_2\) (Oxygen Difluoride). Let's analyze each option one by one to determine which are correct:

1. Number of lone pairs on oxygen is 2: In the \(OF_2\) molecule, the oxygen atom is bonded to two fluorine atoms and also has two lone pairs of electrons. This gives a total of 4 electron regions (2 bonds + 2 lone pairs) around the oxygen. Hence, option A is correct.
2. FOF angle is less than \(104.5^{\circ}\): The geometry of \(OF_2\) is bent due to the lone pairs' repulsion being greater than that of the bonded pairs. This repulsion slightly decreases the angle from the tetrahedral angle of \(109.5^{\circ}\) to a smaller angle. Thus, the \(FOF\) angle is indeed less than \(104.5^{\circ}\). Option B is correct.
3. Oxidation state of \(O\) is \(-2\): Typically, oxygen has an oxidation state of \(-2\). However, in \(OF_2\), oxygen is less electronegative than fluorine. Hence, fluorine takes a charge of \(-1\), making oxygen's oxidation state \(+2\). Therefore, option C is incorrect.
4. Molecule is bent 'V' shaped: Due to the presence of two lone pairs on oxygen, which causes greater repulsion and reduces the bond angle, the molecular shape of \(OF_2\) is bent or 'V'-shaped. Therefore, option D is correct.
5. Molecular geometry is linear: The presence of lone pairs on the oxygen atom causes the geometry to be bent rather than linear. Therefore, option E is incorrect.

Based on the analysis, the correct options are: A, B, D only.