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 option 'B'. 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? &#8203;a)CO2b)HIc)H2Od)SO2Correct answer is option 'B'. Can you explain this answer?

Answer

Answer b

Answer

yaaa it is correct ans... dipole moment of CO2 ,H2O ,&SO2 is zero

Answer

H₂O will have highest dipole moment due to maximum difference in electronegativity of H and O atoms.

Answer

Polarity and Dipole Moment

Polarity in a molecule refers to the distribution of electron density within the molecule. It occurs when there is an uneven distribution of electrons, resulting in a separation of charge. The dipole moment, represented by the symbol μ, is a measure of the magnitude and direction of the polarity in a molecule.

Factors Affecting Polarity and Dipole Moment

The polarity and dipole moment of a molecule depend primarily on two factors:
1. Electronegativity of the constituent atoms: Electronegativity is the ability of an atom to attract electrons towards itself in a chemical bond. The greater the difference in electronegativity between atoms, the more polar the bond and the molecule will be.
2. Shape of the molecule: The spatial arrangement of atoms in a molecule determines its shape, which in turn affects its dipole moment. If the molecule is symmetrical, the dipole moments of individual bonds cancel out, resulting in a nonpolar molecule. On the other hand, if the molecule is asymmetrical, the dipole moments do not cancel out, leading to a polar molecule.

Analysis of the Options

a) CO2 (Carbon Dioxide):
- Carbon and oxygen have different electronegativities (2.55 for carbon and 3.44 for oxygen).
- However, the molecule has a linear shape, which leads to a symmetrical distribution of the bonding electrons.
- As a result, the dipole moments of the two carbon-oxygen bonds cancel out, making the molecule nonpolar.

b) HI (Hydrogen Iodide):
- Hydrogen and iodine have different electronegativities (2.20 for hydrogen and 2.66 for iodine).
- The molecule has a linear shape, similar to CO2.
- However, the larger difference in electronegativity between hydrogen and iodine results in a polar bond.
- Since there are only two atoms in the molecule, the dipole moment is not canceled out, making it a polar molecule.
- Thus, HI has the highest dipole moment among the given options.

c) H2O (Water):
- Hydrogen and oxygen have different electronegativities (2.20 for hydrogen and 3.44 for oxygen).
- The molecule has a bent or V-shaped geometry, which is asymmetrical.
- This asymmetry leads to a net dipole moment, making water a polar molecule.
- However, the dipole moment is lower than that of HI due to the smaller difference in electronegativity.

d) SO2 (Sulfur Dioxide):
- Sulfur and oxygen have different electronegativities (2.58 for sulfur and 3.44 for oxygen).
- The molecule has a bent or V-shaped geometry, similar to H2O.
- The dipole moments of the two sulfur-oxygen bonds do not cancel out, resulting in a net dipole moment and a polar molecule.
- However, the dipole moment is lower than that of HI due to the smaller difference in electronegativity.

Conclusion
Among the given options, HI (Hydrogen Iodide) has the highest dipole moment. This is because hydrogen and iodine have the highest difference in electronegativity, and the linear shape of HI does not cancel out the dipole moments of the

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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?