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Polar covalent molecules exhibit dipole ...

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?

A

`XeF_(4)`

B

`BF_(3)`

C

`I_(2)Cl_(6)`

D

`PCl_(2)F_(3)`

Text Solution

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The correct Answer is:
To determine which of the given molecules is polar, we need to analyze the molecular geometry and the distribution of dipole moments. A polar molecule has a net dipole moment that is not equal to zero, meaning that the dipole moments of the individual bonds do not cancel each other out. ### Step-by-Step Solution: **Step 1: Analyze XeF4** - **Hybridization:** sp³d² - **Structure:** The molecule has a square planar geometry with four fluorine atoms and two lone pairs on the xenon atom. - **Dipole Moment:** The dipole moments from the four fluorine atoms cancel each other out due to symmetry. - **Conclusion:** XeF4 is a non-polar molecule (μ = 0). **Step 2: Analyze BF3** - **Hybridization:** sp² - **Structure:** The molecule has a trigonal planar geometry with three fluorine atoms. - **Dipole Moment:** The dipole moments from the three fluorine atoms cancel each other out due to symmetry. - **Conclusion:** BF3 is a non-polar molecule (μ = 0). **Step 3: Analyze I2Cl6** - **Structure:** This is a dimer of ICl3. The geometry is complex, but it can be simplified for analysis. - **Dipole Moment:** The dipole moments from the chlorine atoms cancel each other out due to symmetry, and the lone pairs on iodine also do not contribute to a net dipole moment. - **Conclusion:** I2Cl6 is a non-polar molecule (μ = 0). **Step 4: Analyze PCl2F3** - **Hybridization:** sp³d - **Structure:** The molecule has a trigonal bipyramidal geometry with two chlorine atoms and three fluorine atoms. The fluorine atoms are more electronegative and will be arranged in such a way that they create an asymmetrical distribution of charge. - **Dipole Moment:** The dipole moments from the fluorine atoms do not cancel out due to the presence of chlorine atoms in the equatorial plane. This results in a net dipole moment. - **Conclusion:** PCl2F3 is a polar molecule (μ ≠ 0). ### Final Answer: The polar molecule among the options is **PCl2F3**. ---
To determine which of the given molecules is polar, we need to analyze the molecular geometry and the distribution of dipole moments. A polar molecule has a net dipole moment that is not equal to zero, meaning that the dipole moments of the individual bonds do not cancel each other out. ### Step-by-Step Solution: **Step 1: Analyze XeF4** - **Hybridization:** sp³d² - **Structure:** The molecule has a square planar geometry with four fluorine atoms and two lone pairs on the xenon atom. - **Dipole Moment:** The dipole moments from the four fluorine atoms cancel each other out due to symmetry. ...
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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. 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) :

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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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?

The unit of dipole moment is

A molecule possessing dipole moment is

Unit of magnetic dipole moment is

Zero dipole moment is present in

Dipole moment is shown by

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