Concept explainers
(a)
Interpretation:
The molecule that has greater dipole moment among
Concept introduction:
Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.
Here, B is the electronegative atom and A is the electropositive atom.
Bond polarity can be estimated by
Here, B is the electronegative atom and A is the electropositive atom.
The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.
(a)
Answer to Problem 10.58P
Explanation of Solution
Both molecules have bent shape thus greater dipole can be found on the bases of the electronegativity difference.
The formula to calculate
Substitute
The formula to calculate
Substitute
Both molecules have polar bonds and have a bent shape of
Greater the electronegativity difference between the two bonding atoms more polar will be the bond and greater will be the dipole moment.
(b)
Interpretation:
The molecule that has greater dipole moment among
Concept introduction:
Electronegativity is the tendency of an atom to attract the shared electrons in the bond towards itself. The more electronegative atom will more attract the bonding electrons towards itself than the less electronegative atom. Therefore the electrons will spend more time with the more electronegative atom than an electropositive atom. The electronegative atom will acquire the partial negative charge and the electropositive atom will acquire a partial positive charge.
Here, B is the electronegative atom and A is the electropositive atom.
Bond polarity can be estimated by
Here, B is the electronegative atom and A is the electropositive atom.
The greater electronegativity difference between the atoms induces the greater polarity in the bond thus it generates higher dipole moment.
(b)
Answer to Problem 10.58P
Explanation of Solution
The formula to calculate
Substitute
The formula to calculate
Substitute
Bond polarity and dipole moment are directly related to the electronegativity difference. Therefore,
Greater the electronegativity difference between the two bonding atoms more polar will be the bond and greater will be the dipole moment. Chlorine is more electronegative than bromine thus
(c)
Interpretation:
The molecule that has greater dipole moment among
Concept introduction:
The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.
The direction of the dipole moment is represented as follows:
The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.
(c)
Answer to Problem 10.58P
Explanation of Solution
The shape of
The dipole moment in
All the
The shape of
The dipole moment in
The individual dipole moment does not cancel each other so the value of net dipole moment is not zero and therefore
Hence,
Molecules in which individual dipole moment does not cancel each other result in net non-zero dipole moment and the overall molecule is said to be polar. In
(d)
Interpretation:
The molecule that has greater dipole moment among
Concept introduction:
The dipole moment arises when there is a separation of charges between two ions or atoms involved in the bond. The dipole moment is a vector quantity and its direction towards the most electronegative atom.
The direction of the dipole moment is represented as follows:
The polar and non-polar molecule can be identified on the basis of the net dipole moment. Polar molecules have non zero value of net dipole moment and the non polar molecules have zero net dipole moment.
(d)
Answer to Problem 10.58P
Explanation of Solution
The shape of
The dipole moment in
The individual dipole moment does not cancel each other so the value of net dipole moment is not zero and therefore
The shape of
The dipole moment in
The individual dipole moment cancels each other’s polarities so the value of net dipole moment is zero and therefore
Hence,
Molecules in which individual dipole moment does not cancel each other result in net non-zero dipole moment and the overall molecule is said to be polar. In
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Chapter 10 Solutions
Chemistry: The Molecular Nature of Matter and Change - Standalone book
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