For each compound below, identify any polar covalent bonds and indicate the direction of the dipole moment using the symbols δ +and δ-. (a) HBr
(b) HCI
(c) H2O
(d) CH40

H-Br bond is polar, hydrogen is partly positive and bromine is partly negative

H-Cl bond is polar, hydrogen is partly positive and bromine is partly negative

O-H bond in water is polar, hydrogen is partly positive and oxygen is partly negative

C-O bond in CH40 is polar, carbon is partly positive and oxygen is partly negative

Explanation:

A molecule possess a dipole moment when there is a large difference in electro negativity between two bonding atoms in the molecule.

The presence of dipole moments introduces polarity to the molecule. In all the molecules listed in the answer, the shared electron pair of the bond is closer to the more electronegative atom causing it to be partially negative while the less electronegative atom in the bond is partially positive.

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