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The molecule which does not exhibit net ...

The molecule which does not exhibit net dipole moment is

A

`NH_3`

B

`CHCl_3`

C

`H_2 O`

D

`C Cl_4`

Text Solution

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The correct Answer is:
To determine which molecule does not exhibit a net dipole moment among the given options (ammonia, CHCl3, water, or CCl4), we will analyze the molecular geometry and the polarity of the bonds in each molecule. ### Step-by-Step Solution: 1. **Understanding Dipole Moment**: - A dipole moment occurs when there is a separation of charge due to differences in electronegativity between atoms in a bond. A net dipole moment exists when the individual bond dipoles do not cancel each other out. 2. **Analyzing Ammonia (NH3)**: - Ammonia has a pyramidal shape due to the presence of a lone pair on nitrogen. - The nitrogen atom is more electronegative than hydrogen, leading to bond dipoles pointing towards nitrogen. - The lone pair also contributes to the dipole moment, resulting in a net dipole moment that is not zero. 3. **Analyzing CHCl3 (Chloroform)**: - Chloroform has a tetrahedral geometry. - The chlorine atoms are more electronegative than carbon and hydrogen, creating dipoles that point towards the chlorine atoms. - Since the dipoles do not cancel out completely due to the asymmetrical arrangement, CHCl3 has a non-zero dipole moment. 4. **Analyzing Water (H2O)**: - Water has a bent shape due to the two lone pairs on oxygen. - The oxygen atom is more electronegative than hydrogen, resulting in dipoles directed towards the oxygen. - The bent shape means that the dipoles do not cancel out, leading to a net dipole moment that is also non-zero. 5. **Analyzing CCl4 (Carbon Tetrachloride)**: - CCl4 has a symmetrical tetrahedral shape. - Each C-Cl bond has a dipole moment pointing towards the chlorine atoms. - Because of the symmetrical arrangement, the dipoles cancel each other out completely, resulting in a net dipole moment of zero. 6. **Conclusion**: - Among the options provided, CCl4 is the only molecule that does not exhibit a net dipole moment due to its symmetrical structure and equal bond dipoles that cancel each other out. ### Final Answer: The molecule which does not exhibit a net dipole moment is **CCl4**.
To determine which molecule does not exhibit a net dipole moment among the given options (ammonia, CHCl3, water, or CCl4), we will analyze the molecular geometry and the polarity of the bonds in each molecule. ### Step-by-Step Solution: 1. **Understanding Dipole Moment**: - A dipole moment occurs when there is a separation of charge due to differences in electronegativity between atoms in a bond. A net dipole moment exists when the individual bond dipoles do not cancel each other out. 2. **Analyzing Ammonia (NH3)**: ...
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Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which is a polar molecule?

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Polar covalent molecules exhibit dipole moment. Dipole moment is equal to the product of charge separation , q and the bond length d for the bond. Unit of dipole moment is debye. One debye is equal to 10^(-18) esu cm. Dipole moments is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of the bond dipoles, but not on the polarity of bonds alone. A symmetrical structure shows zero dipole moment. Thus, dipole moment helps to predict the geometry of a molecules. Dipole moment values can be distinguish between cis- and trans- isomers, ortho, meta and pare-forms of a substance, etc. Q. Which of the following statement is correct regarding C_(2)H_(2)F_(2) molecule?

All molecules with polar bonds have dipole moment.

All molecules with polar bonds have dipole moment.

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