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Assertion : The dipole moment helps to ...

Assertion : The dipole moment helps to predict whether a molecule is polar or non- polar.
Reason : The dipole moment helps to predict geometry of molecule.

A

If both `(A)` and `(R )` are correct and `(R )` is the correct explanation of `(A)`

B

If both `(A)` and `(R )` are correct and `(R )` is the correct explanation of `(A)`

C

If `(A)` is correct but `(R )` is incorrect

D

If `(A)` is incorrect but `(R )` is correct

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question regarding the assertion and reason provided, we will analyze each statement step by step. ### Step 1: Analyze the Assertion **Assertion:** The dipole moment helps to predict whether a molecule is polar or non-polar. - **Explanation:** The dipole moment is a vector quantity that indicates the separation of positive and negative charges in a molecule. If a molecule has a net dipole moment (not equal to zero), it is considered polar. Conversely, if the dipole moment is zero, the molecule is non-polar. For example, in the case of BF3, the dipole moment is zero due to its symmetrical trigonal planar shape, indicating that it is non-polar. ### Step 2: Analyze the Reason **Reason:** The dipole moment helps to predict the geometry of the molecule. - **Explanation:** The dipole moment can provide insights into the molecular geometry. For example, in CO2, the dipole moment is also zero, which suggests that the molecule has a linear geometry. The symmetry in the arrangement of atoms leads to the cancellation of dipole moments, allowing us to infer the shape of the molecule. ### Step 3: Correlation Between Assertion and Reason - The assertion states that dipole moments can help determine if a molecule is polar or non-polar, while the reason states that dipole moments can help predict molecular geometry. Both statements are true and are interconnected. The geometry of a molecule influences its dipole moment, and the dipole moment can give information about the geometry. ### Conclusion - Both the assertion and the reason are correct, and the reason provides a correct explanation for the assertion. Therefore, the correct answer is that both the assertion and reason are true, and the reason correctly explains the assertion. ### Final Answer **Both the assertion and reason are correct, and the reason is the correct explanation for the assertion.** ---
To solve the question regarding the assertion and reason provided, we will analyze each statement step by step. ### Step 1: Analyze the Assertion **Assertion:** The dipole moment helps to predict whether a molecule is polar or non-polar. - **Explanation:** The dipole moment is a vector quantity that indicates the separation of positive and negative charges in a molecule. If a molecule has a net dipole moment (not equal to zero), it is considered polar. Conversely, if the dipole moment is zero, the molecule is non-polar. For example, in the case of BF3, the dipole moment is zero due to its symmetrical trigonal planar shape, indicating that it is non-polar. ### Step 2: Analyze the Reason ...
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Which of the following molecule is polar and non-planar

The dipole moments of the given molecules are such that :

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. 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. 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. Which of the following statement is correct regarding C_(2)H_(2)F_(2) 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. 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) :

All molecules with polar bonds have dipole moment.

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