Question

Halogens form a variety of covalent compounds with each other. For example, chlorine and fluorine form the compounds${\text{ClF,ClF}}_{\text{3}}$, and${\text{ClF}}_{\text{5}}$. Predict the molecular structure (including bond angles) for each of these three compounds. Would you expect${\text{FCl}}_{\text{3}}$to be a stable compound? Explain.

Short answer

The molecule are square pyramidal, T-shaped, and linear.

They have ${\text{<90}}^{°}{\text{and90}}^{\circ }\text{anglesrespectively.}$

We wouldn't anticipate $FC{l}_3$ to be stable because the fluorine atom lacks the third electron and is unable to accept further electrons.

Step-by-step solution

Definition of Bond angle

The angle produced between two covalent bonds that originate from the same atom is known as the bond angle.

Molecular structure

The first molecule (CIF) is straight and has no angles (only 2 atoms).

${\text{ClF}}_{\text{3}}$ is the second molecule. $T$ is the shape of this molecule. Because of electron

repulsion between two lone electron pairs, its angles are near 90 degrees, but

somewhat less.

${\text{ClF}}_{\text{5}}$ is the last molecule. It is shaped like a square pyramid. Because every bond is perpendicular to the ones next to it, the angles are exactly 90 degrees.

Because the fluorine atom has just two electron shells and no d atomic orbital, we would anticipate ${\text{FCl}}_{\text{3}}$ to be unstable. To break the octet rule and accept

electrons from chlorine atoms, it must create the third shell and the d orbital.

Draw the structure

Therefore, the structure of the molecule are square pyramidal, T-shaped, and

linear. They have ${\text{<90}}^{°}$and $90°$ angles, respectively. We wouldn't anticipate

${\text{FCl}}_{\text{3}}$to be stable because the fluorine atom lacks the third electron and is unable to accept further electrons.