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Question: Which of the following is a polar molecule? A. \(B{{F}_{3}}\) B. \(S{{F}_{4}}\) C. \(Si{{F}_{4...

Which of the following is a polar molecule?
A. BF3B{{F}_{3}}
B. SF4S{{F}_{4}}
C. SiF4Si{{F}_{4}}
D. XeF4Xe{{F}_{4}}

Explanation

Solution

Hint: It has an unsymmetrical see-saw structure. It is a colorless corrosive gas that releases dangerous HF upon exposure to water or moisture. Despite these unwelcome characteristics, this compound is a useful reagent for the preparation of organofluorine compounds, some of which are important in the pharmaceutical as specialty chemical industries.

Complete step by step answer:
A polar molecule is one where some of the atoms are more electronegative, that is they attract electrons more than the other atoms. As a result, the electrons in the molecule are dragged closer to one side of the molecule, making a positively charged side and a negatively charged side. The most famous polar molecule is water.

The most important polar molecule on Earth is water. Water is a polar molecule due to the strong electronegativity of the oxygen atom. This forces most of the electrons to the side of the molecule where oxygen is present, creating a highly negative area. The other side of the molecule becomes more positive, due to the protons of the hydrogen atom. Because water is a polar molecule which can interact with other water molecules therefore, it creates a more stable structure.

Now, let’s see why SF4S{{F}_{4}}is a polar molecule!
SF4S{{F}_{4}}Is a polar molecule as the individual bond dipoles do not cancel each other. It contains 4 bond pairs of electrons and 1 lone pair of electrons. S atom undergoes sp3ds{{p}^{3}}d hybridization which results in distorted tetrahedral geometry. Here, SF4S{{F}_{4}} bond angles are around 102 degrees in the equatorial plane and around 173 degrees between the axial and equatorial positions.

Therefore, SF4S{{F}_{4}} is a polar molecule.

Note: Bonding electron pairs have lesser repulsions as compared to lone pair electrons. Sulfur Tetrafluoride does not follow the octet rule. It will hold more than 8 electrons. Sulfur having valence electrons in the 3rd energy level, will also have access to the 3rd sublevel, thus following for more than 8 electrons.