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CS?, SO?, CH?, & CH?Cl: Are They Polar or Nonpolar Molecules?
Chapter 10, Problem 89P(choose chapter or problem)
Classify each molecule as polar or nonpolar.
(a) \(C S_{2}\)
(b) \(\mathrm{SO}_{2}\)
(c) \(\mathrm{CH}_{4}\)
(d) \(\mathrm{CH}_{3} \mathrm{Cl}\)
Questions & Answers
QUESTION:
Classify each molecule as polar or nonpolar.
(a) \(C S_{2}\)
(b) \(\mathrm{SO}_{2}\)
(c) \(\mathrm{CH}_{4}\)
(d) \(\mathrm{CH}_{3} \mathrm{Cl}\)
ANSWER:Step 1 of 3
In case of heteronuclear molecules(containing different atoms), the shared electron pair between the two atoms gets displaced more towards the more electronegative atom. The resultant covalent bond is called polar covalent bond.
As a result of polarization, the molecule possesses the dipole moment which can be defined as the product of the magnitude of the charge and the distance between the centers of positive and negative charge. Further, the dipole moment is depicted by a small arrow with tail on the positive center and head pointing towards the negative center.
On the other hand, when a covalent bond is formed between two similar atoms, for example, in \(\mathrm{H}_{2}, \mathrm{O}_{2}, \mathrm{Cl}_{2} \text { or } \mathrm{N}_{2}\), the shared pair of electrons is equally attracted by the two atoms. As a result, the electron pair is situated exactly in between the two identical nuclei. The bond so formed is called nonpolar covalent bond.
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CS?, SO?, CH?, & CH?Cl: Are They Polar or Nonpolar Molecules?
Want To Learn More? To watch the entire video and ALL of the videos in the series:
Explore the polarity of Carbon disulfide, Sulfur dioxide, Methane, and Chloromethane. Learn how molecular shape influences electron distribution. Understand which molecules possess a net dipole moment and which ones don't.