Question

Draw the Lewis structures for SeO₂, PCl₃, NNO, COS, and PF₃. Which of the compounds are polar? Which of the compounds exhibit at least one bond angle that is approximately 120 degrees? Which of the compounds exhibit hybridization by the central atom? Which of the compounds have a linear molecular structure?

Short answer

Lewis dot structure will represent the presence of lone pairs and bonds formed by the central molecule, through which we can also determine the hybridization. The compounds which will have a net dipole moment not equal to zero will be considered as polar molecules.

Step-by-step solution

Lewis structure of SeO2, PCl3, NNO, COS, and PF3.

The Lewis structure shows the lone pair of electrons and bonds formed in a molecule.

Polar compounds

When an electronegative atom bonds with an electropositive element, they attract the electrons and this causes the production of negative and positive charges on an atom, which eventually gives the polar character to a molecule. All 5 molecules are polar compounds because they result in a net dipole moment.

Bond angle

Only SeO₂ has a 120-degree bond angle, because it has a bent shape due to the presence of one lone pair and forms 120 degrees. Whereas PCl₃ and PF₃have different bond angles that is 103 degree and 96 degrees. Whereas NNO and COS are linear molecules.

Hybridisation of central atom

In PCl₃and PF₃, the central atom that is phosphorus forms a three-sigma bond and has one lone pair, so it exhibits sp³hybridization. Whereas in , SeO₂ shows sp²hybridization. In OCS and NNO, carbon and nitrogen show both sp hybridization.

Linear molecule

Among the given compounds, only NNO and COS has linear structure because they present at 180 degrees from each other.