Question

Experiment shows that H₂O has a dipole moment while CO₂
has not. Point out the structures which best illustrate these
facts
O
⁄ \
(a) O = C = O ; H = H (b) O = C = O ; H – O – H
(c) C (d) O H
⫽\\ ; H - H - O ǁ ǀ
O O C = O ; O

Answer 1

O H

⫽\\ ; H - H - O ǁ ǀ

O O C = O ; O is the correct answer

Answer 2

Water has a bent structure whole carbon dioxide has a linear structure.

Explanation:

• Dipole moment is the property which determines the electric polarity of a molecule.

• Water has a dipole moment but carbon dioxide has no dipole moment.

• Water has the chemical formula of H2O.

• The central molecule i.e the oxygen has the sp3 hybridization.

The sp3 hybridization consists of 2 sigma bonds with 2 hydrogen and 2 lone pairs.

• The lone pair repulses the sigma bonds and the actual angle between the sigma bonds in water is 104.5°.

• So there remains the electric polarity in water.

• But in carbon dioxide, the central atom carbon is sp hybrid.

• This is formed by 2 sigma bonds with 2 oxygen atoms.

• So the molecule is linear with equal electronegativity on both sides.

• So carbon dioxide has no dipole moment.

For more information about dipole moment,

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Find the dimensions of (a) electric dipole moment p and (b) magnetic dipole moment M

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Dipole moment values help in predicting the shapes of covalent molecules. Explain.