bond angles and polarity for

trans-PF3Cl2

Answered here.

http://ca.answers.yahoo.com/question/index?qid=20080115195956AAWiXoI

thank you !

To determine the bond angles and polarity of trans-PF3Cl2, we need to understand the molecular geometry and the polarity of each bond.

First, let's consider the molecular geometry. The molecule trans-PF3Cl2 consists of one phosphorus atom (P) bonded to three fluorine atoms (F) and two chlorine atoms (Cl). The central atom, phosphorus (P), has five electron domains: three bonding pairs (from the three F-P bonds) and two lone pairs (on the P atom).

The electronic geometry of the molecule is trigonal bipyramidal. In this geometry, the three F-P bonds lie in one plane, while the two Cl atoms are located at the axial positions. The axial positions are 180 degrees apart from each other and from the equatorial plane formed by the F-P-F bonds.

Now, let's consider the bond angles. The F-P-F bond angles in the equatorial plane are approximately 120 degrees, as they are arranged in a trigonal planar geometry. The axial F-P-Cl bond angles are approximately 90 degrees, as they are arranged in a linear geometry.

Regarding polarity, we need to look at the electronegativity difference between atoms bonded together. The electronegativity of chlorine (3.16) is higher than that of phosphorus (2.19) and fluorine (3.98). Therefore, the Cl-P bond and Cl-F bonds will have a polar covalent character, with chlorine being partially negative and phosphorus/fluorine being partially positive.

To summarize:
- The bond angles in trans-PF3Cl2 are approximately 120 degrees for F-P-F bond angles and 90 degrees for F-P-Cl bond angles.
- The molecule has a trigonal bipyramidal molecular geometry.
- The Cl-P bond and Cl-F bonds have a polar covalent character.

Remember, this explanation applied to the trans isomer of PF3Cl2. If the molecule were the cis isomer, the bond angles would differ.