Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment? a)CO2b)HIc)H2Od)SO2Correct answer is 'C'. Can you explain this answer?

Question

Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment? ​a)CO2b)HIc)H2Od)SO2Correct answer is 'C'. Can you explain this answer?

Answer

Lp in si is sp2 hybrised  lp of sp2 hubrised will be more than h2o

Answer

Among these four It's maximum in HI Bec. it's dipole is not cancelled by any other electronegative element as in case if rest three..!

Answer

In case of HI the electronegativity difference between the typ atoms is very prominent and as iodine has 3 lone pairs lone pair moment also.contributes towards the high dipole moment

Answer

Electronegativity and Dipole Moment

The dipole moment of a molecule is a measure of its polarity, which is the separation of positive and negative charges within the molecule. It is determined by the electronegativity difference between the constituent atoms and the molecular shape.

Electronegativity
Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond. It depends on factors like atomic size, nuclear charge, and electron configuration.

Dipole Moment
The dipole moment of a molecule is a vector quantity that points from the positive to the negative charge. It is determined by the magnitude of the charge separation (which depends on electronegativity) and the distance between the charges.

Effect of Electronegativity and Shape on Dipole Moment
- Electronegativity Difference: The larger the difference in electronegativity between the atoms in a bond, the more polar the bond will be. This leads to a larger dipole moment.
- Molecular Shape: In molecules with polar bonds, the overall dipole moment also depends on the molecular shape. If the polar bonds are symmetrically arranged, their dipole moments can cancel each other out, resulting in a nonpolar molecule. However, if the polar bonds are asymmetrically arranged, their dipole moments do not cancel out, resulting in a polar molecule.

Comparison of the Given Molecules
a) CO2:
- Carbon and oxygen have a significant electronegativity difference, making the carbon-oxygen bonds polar.
- However, the molecule has a linear shape with the carbon atom in the center and the two oxygen atoms on either side.
- The dipole moments of the carbon-oxygen bonds cancel each other out due to the symmetric arrangement, resulting in a net dipole moment of zero. Therefore, CO2 is a nonpolar molecule with a low dipole moment.

b) HI:
- Hydrogen and iodine have a significant electronegativity difference, making the hydrogen-iodine bond polar.
- The molecule is linear, and the dipole moment does not cancel out.
- HI is a polar molecule with a dipole moment.

c) H2O:
- Oxygen is more electronegative than hydrogen, creating polar bonds.
- The molecule has a bent shape with the oxygen atom in the center and the two hydrogen atoms at an angle.
- The dipole moments of the oxygen-hydrogen bonds do not cancel out due to the asymmetric arrangement, resulting in a net dipole moment.
- H2O is a polar molecule with a dipole moment.

d) SO2:
- Sulfur and oxygen have a significant electronegativity difference, making the sulfur-oxygen bonds polar.
- The molecule has a bent shape with the sulfur atom in the center and the two oxygen atoms at an angle.
- The dipole moments of the sulfur-oxygen bonds do not cancel out due to the asymmetric arrangement, resulting in a net dipole moment.
- SO2 is a polar molecule with a dipole moment.

Conclusion
Among the given molecules, H2O (option c) has the highest dipole moment. This is because it has polar bonds and an asymmetric molecular shape, which results in a net dipole moment.

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