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Standard XI
Chemistry
Bond Parameters
Question

Chemical bonding between two atoms is necessarily associated with an electrical moment arising out of the difference between in electronegativity of two atoms This means that every bonds carries with it an electrical moment called "bond moment". The dipole moment of molecule is really the vectoral sum of the individual bond moment present in it. To compute the dipole moment it is necessary to find out the values of various bond moment. In the following table dipole moment different bonds are given:
In the acetone molecule considering the normal planar structure, the observed dipole moment of acetone molecule is:

A
2.9 D
B
2.75 D
C
3 D
D
None of these
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Solution
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Correct option is A. 2.9 D

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Similar Questions
Q1
Chemical bonding between two atoms is necessarily associated with an electrical moment arising out of the difference between in electronegativity of two atoms This means that every bonds carries with it an electrical moment called "bond moment". The dipole moment of molecule is really the vectoral sum of the individual bond moment present in it. To compute the dipole moment it is necessary to find out the values of various bond moment. In the following table dipole moment different bonds are given:
In the acetone molecule considering the normal planar structure, the observed dipole moment of acetone molecule is:
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Q2
The dipole moment of molecule AB present in an electric field is 1.9 D and its dipole moment is calculated by charge and bond length is 5.7 D. Find out the nature of bond between molecules:
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Q3
Reason
It arises so, as the two ionic forms having bond moments in opposite directions contribute equally to nullify the effect.
Assertion
The ionic character exist in $$ H_2 $$ molecule but no dipole moment or bond moment exists permanently.
The ionic character exist in $$ H_2 $$ molecule but no dipole moment or bond moment exists permanently.
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Q4
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 moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of 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 molecules. Dipole moment values can be used to distinguish between cis-and trans-isomers; ortho-, meta- and para-forms of a substance, etc.

Which is a polar molecule?
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Q5
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 moment is a vector quantity. It has both magnitude and direction. Hence, dipole moment of a molecule depends upon the relative orientation of 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 molecules. Dipole moment values can be used to distinguish between cis-and trans-isomers; ortho-, meta- and para-forms of a substance, etc.

A diatomic molecule has a dipole moment of 1.2 D. If the bond length is $$1.0 \times 10^{-8} \ cm$$, what fraction of charge does exist each atom?
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