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Magazine Chapter 2: Problem 223
Non-zero dipole moment is shown by :
(a) \(\mathrm{CCl}_{4}\)
\(\square\) (b) \(\mathrm{CO}_{2}\)
(c) \(\mathrm{H}_{2} \mathrm{O}\)
\(\square\) (d)
Short Answer
Expert verified
(c) \( \mathrm{H}_{2} \mathrm{O} \) and chlorobenzene have non-zero dipole moments.
Step by step solution
01
Understanding Dipole Moment
A dipole moment occurs in a molecule when there is a separation of charge due to differences in electronegativity between atoms, leading to an overall molecular dipole. Molecules with nonzero dipole moments are often polar.
02
Analyzing Options
Each option represents a different molecule: (a) \( \mathrm{CCl}_4 \), (b) \( \mathrm{CO}_2 \), (c) \( \mathrm{H}_2 \mathrm{O} \), and (d) chlorobenzene. We need to assess each for its symmetry and charge distribution to find the one with a nonzero dipole moment.
03
Option A: \( \mathrm{CCl}_4 \)
This molecule is tetrahedral with four \( \mathrm{C-Cl} \) bonds evenly distributed around the central carbon atom. Its symmetrical structure causes the dipole moments of the bonds to cancel each other, resulting in a net dipole moment of zero.
04
Option B: \( \mathrm{CO}_2 \)
This molecule is linear, with oxygen atoms placed symmetrically on either side of the carbon. The linear geometry causes the dipole moments from the \( \mathrm{C=O} \) bonds to cancel out, resulting in a zero net dipole moment.
05
Option C: \( \mathrm{H}_2 \mathrm{O} \)
Water has an angular or bent geometry due to the two lone pairs on the oxygen, making it a polar molecule. The bond dipoles do not cancel each other out, resulting in a nonzero dipole moment.
06
Option D: Chlorobenzene
Chlorobenzene is a planar molecule with a chlorine atom substituting one hydrogen in benzene. The presence of a highly electronegative chlorine causes a dipole, and due to the lack of perfect symmetry as in options A and B, it results in a nonzero dipole moment.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
CCl4 structure
The molecular structure of carbon tetrachloride ( \( \mathrm{CCl}_4 \)) is a perfect example of a molecule that is symmetrical, leading to an interesting outcome regarding its dipole moment. The molecule is tetrahedral, meaning it forms a four-cornered shape like a pyramid. Every corner represents a chlorine atom, while the carbon atom sits in the center.
- Each \( \mathrm{C-Cl} \) bond in \( \mathrm{CCl}_4 \) is polar due to the difference in electronegativity between carbon and chlorine.
- The symmetrical arrangement in a tetrahedral geometry causes the individual bond dipoles to cancel each other out.
- This mutual cancellation results in a molecule with no net dipole moment, making \( \mathrm{CCl}_4 \) non-polar.
CO2 linear geometry
Carbon dioxide ( \( \mathrm{CO}_2 \)) is another interesting molecule to study regarding molecular geometry and dipole moments. The structure of \( \mathrm{CO}_2 \) is linear, with carbon at the center and two oxygen atoms symmetrically placed at each end.
- Each \( \mathrm{C=O} \) bond is polar because of the substantial electronegativity difference between carbon and oxygen.
- However, because \( \mathrm{CO}_2 \) is linear, these dipole moments are equal and opposite direction, resulting in a cancellation.
- Thus, the net dipole moment of \( \mathrm{CO}_2 \) is zero, making it a non-polar molecule.
H2O polarity
Water ( \( \mathrm{H}_2 \mathrm{O} \)) is a classic example of a polar molecule due to its unique molecular geometry. The shape of water is described as a bent or angular form owing to the two lone electron pairs on the oxygen atom.
- The \( \mathrm{H-O} \) bonds are polar, caused by the significant electronegativity difference.
- Due to its bent shape, these polar bonds do not exactly cancel out as they do in linear structures.
- This results in a net dipole moment, making water a polar molecule, which explains its extensive solvent capabilities.
Chlorobenzene dipole
Chlorobenzene is an aromatic compound where one hydrogen of a benzene ring is replaced by a chlorine atom. This modification results in a molecular structure that is not fully symmetrical, which leads to a nonzero dipole moment.
- The benzene ring is planar and usually non-polar, but the presence of chlorine, which is highly electronegative, affects this balance.
- Chlorine attracts the shared electrons more strongly, creating a polar \( \mathrm{C-Cl} \) bond.
- Because the systematic symmetry seen in molecules like \( \mathrm{CCl}_4 \) and \( \mathrm{CO}_2 \) is disrupted, chlorobenzene has a net dipole moment.
