Related Problems with Solutions
Problem 10 : Explain the concept of a dipole moment in polar covalent bonds. Calculate the dipole moment for hydrogen fluoride (HF) and carbon dioxide (CO₂) molecules.
Solution :
A dipole moment occurs in polar covalent bonds when there is an unequal sharing of electrons, creating a partial positive and partial negative end. It is measured in Debye units (D).
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Hydrogen fluoride (HF) has a polar covalent bond. The dipole moment (μ) is calculated as the product of the bond length (d) and the bond charge (Q), where Q is the product of the charges on the atoms and the electron charge (e): μ(HF) = d(HF) * Q(H) * Q(F) μ(HF) = d(HF) * (1e) * (7e) = d(HF) * 7e
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Carbon dioxide (CO₂) has polar bonds but is a linear molecule, resulting in no net dipole moment. The dipole moments of the two C-O bonds cancel each other out.
So, HF has a dipole moment, while CO₂ does not have a net dipole moment.
