Question

Draw lewis structure for Pf3, CSF2, BF3, XeF4

1. which of the molecules are polar
2. which of the molecules violate the octet
3. which of the molecules above contain no lone pair
4. which of the molecules have sp3 hybridization

Answer 1

The Lewis structures for Pf3, CSF2, BF3, and XeF41 are provided along with information on their polarity, violation of the octet rule, presence of lone pairs, and hybridization.

Step-by-step explanation:

The Lewis structures for the given molecules are as follows:

• Pf3: F:P:F
• CSF2: F-S-F-C
• BF3: F-B-F-F
• XeF41: Xe-F-F-F-F

The molecules Pf3, CSF2, and BF3 all have polar bonds, but the molecule XeF41 does not. A molecule is polar if it has a dipole moment due to the unequal distribution of electron density.

Molecules that violate the octet rule are those that have more or less than eight valence electrons around the central atom. None of the given molecules violate the octet rule as they all have eight valence electrons around the central atom.

None of the given molecules above contain lone pairs as all the atoms are bonded to other atoms.

The molecules Pf3, CSF2, and BF3 have sp3 hybridization. In these molecules, the central atom is surrounded by four electron pairs and adopts a tetrahedral shape, which corresponds to sp3 hybridization.