The shape of `XeO_2F_2` molecule is

Options

A. trigonal bipyramidal
B. square planar
C. tetrahedral
D. see-saw

Answer

To determine the shape of the molecule \(XeO_2F_2\), we can follow these steps:

### Step 1: Determine the Central Atom and Valence Electrons
- The central atom in \(XeO_2F_2\) is Xenon (Xe).
- Xenon is a noble gas and has 8 valence electrons.

**Hint:** Identify the central atom in the molecule and count its valence electrons.

### Step 2: Identify the Bonds Formed
- In \(XeO_2F_2\), Xenon forms two double bonds with two Oxygen atoms and two single bonds with two Fluorine atoms.
- Each double bond consists of one sigma bond and one pi bond, but only the sigma bonds are considered for hybridization.

**Hint:** Count the number of bonds formed by the central atom with surrounding atoms.

### Step 3: Count the Bond Pairs and Lone Pairs
- The two double bonds with Oxygen contribute 2 bond pairs (one for each double bond).
- The two single bonds with Fluorine contribute 2 more bond pairs.
- Thus, there are a total of 4 bond pairs.
- After forming these bonds, there are still 2 valence electrons left on Xenon, which will form 1 lone pair.

**Hint:** Use the formula: Total pairs = Bond pairs + Lone pairs.

### Step 4: Calculate the Steric Number
- The steric number is the sum of bond pairs and lone pairs.
- Here, we have 4 bond pairs and 1 lone pair, so the steric number is \(4 + 1 = 5\).

**Hint:** Remember that the steric number helps in determining the hybridization and geometry of the molecule.

### Step 5: Determine the Hybridization
- A steric number of 5 corresponds to \(sp^3d\) hybridization.

**Hint:** Relate the steric number to its corresponding hybridization type.

### Step 6: Identify the Geometry
- The geometry for \(sp^3d\) hybridization is trigonal bipyramidal.

**Hint:** Understand the difference between geometry and shape; geometry refers to the arrangement of all electron pairs.

### Step 7: Determine the Molecular Shape
- With one lone pair, the shape of the molecule will be based on the positions of the bond pairs.
- The lone pair will occupy an equatorial position to minimize repulsion, leading to a "T-shaped" molecular geometry.

**Hint:** Consider how lone pairs affect the overall shape of the molecule.

### Final Answer
The shape of the \(XeO_2F_2\) molecule is **T-shaped**.