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Zero dipole moment is present in...

Zero dipole moment is present in

A

`NH_(3)`

B

`H_(2)O`

C

cis1,2-dichloroethene

D

trans 1,2-dichloroethene

Text Solution

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The correct Answer is:
To determine which molecule has a zero dipole moment, we will analyze the given options: ammonia, water, cis-1,2-dichloroethene, and trans-1,2-dichloroethene. ### Step-by-Step Solution: 1. **Understanding Dipole Moment**: - Dipole moment is a measure of the polarity of a molecule. It occurs due to the difference in electronegativity between atoms, leading to a separation of charge. 2. **Analyzing Ammonia (NH₃)**: - Ammonia has a trigonal pyramidal shape due to the presence of a lone pair on nitrogen. - The bond dipoles (from hydrogen to nitrogen) do not cancel out because of the geometry, resulting in a net dipole moment. Thus, ammonia is a polar molecule. 3. **Analyzing Water (H₂O)**: - Water has a bent shape due to the two lone pairs on oxygen. - The bond dipoles (from hydrogen to oxygen) also do not cancel out, leading to a net dipole moment. Therefore, water is also a polar molecule. 4. **Analyzing Cis-1,2-Dichloroethene**: - In cis-1,2-dichloroethene, both chlorine atoms are on the same side of the double bond. - The bond dipoles from the carbon-chlorine bonds do not cancel out due to their arrangement, resulting in a net dipole moment. Hence, cis-1,2-dichloroethene is polar. 5. **Analyzing Trans-1,2-Dichloroethene**: - In trans-1,2-dichloroethene, the chlorine atoms are on opposite sides of the double bond. - The bond dipoles from the carbon-chlorine bonds are equal in magnitude but opposite in direction, leading to cancellation of dipole moments. Therefore, trans-1,2-dichloroethene has a net dipole moment of zero. 6. **Conclusion**: - Among the given options, only trans-1,2-dichloroethene has a zero dipole moment. ### Final Answer: The molecule with a zero dipole moment is **trans-1,2-dichloroethene**.
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a) Discuss the significance/applications of dipole moment. b) Represent diagrammatically the bond moments and the resultant dipole moment in CO_(2), NF_(3) and CHCl_(3)

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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?

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. mu of the AX_(4) type of molecule is zero. The geometry of it can be :

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. Arrange the following compounds in increasing order of dipole moments, toluene (I), o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV) :

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. A diatomic molecule has a dipole moment of 1.2D. If the bond length is 1.0times10^(-8) cm, what fraction of charge does exist each atom?

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. Arrange the following compounds in increasing order of dipole moments, toluene (I), o-dichlorobenzene (II), m-dichlorobenzene (III) and p-dichlorobenzene (IV) :

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