Identify the correct order of dipole moment in the following:

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$HF > HCl > HBr$

${CH}_{3} F > {CH}_{3} Cl > {CH}_{3} Br$

${BF}_{3} > {BCl}_{3} > {BBr}_{3}$

$F_{2} > {Cl}_{2} > {Br}_{2}$

answer is A.

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Detailed Solution

The dipole moment is a measure of bond polarity, which is affected by the electronegativity of the atoms in the chemical bond. The dipole moment increases as the electronegativity of an atom increases.
Fluorine has the greatest electronigativity. As a result, it attracts more electrons than other atoms. Electronegativity decreases from top to bottom in the periodic table. As a result, fluorine is the most electronegative element and iodine is the least electronegative. As a result, charge polarisation is greatest in HF and least in HI, and HF has the greatest dipole moment of any element.

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