Question

Among the following, the molecule with the lowest dipole moment is
A \[\text{CHC}{{\text{l}}_{\text{3}}}\]​
B \[\text{C}{{\text{H}}_{3}}\text{Cl}\]
C \[\text{C}{{\text{H}}_{2}}\text{C}{{\text{l}}_{2}}\]
D \[\text{CC}{{\text{l}}_{\text{4}}}\]​

Answer 1

Hint: In any system where there is a charge separation, a dipole moment develops. Therefore, they can occur in both covalent and ionic bonds. The difference in electronegativity between two atoms that are chemically linked causes dipole moments.

Complete step-by-step answer:The polarity of a chemical bond between two atoms in a molecule is gauged by the bond dipole moment. It involves the idea of an electric dipole moment, which is a gauge of how far apart a system's positive and negative charges are from one another. Since the bond dipole moment has both a magnitude and a direction, it is a vector quantity. Note that the two electric charges that form in a molecule and have equal magnitudes but opposite signs are denoted by the letters ${{\delta }^{+}}$ and ${{\delta }^{-}}$. They are separated by a predetermined distance, often represented by the letter "d."

The bond dipole moment, which is distinct from the molecule's overall dipole moment, is the dipole moment of a single bond in a polyatomic molecule.
It is a vector quantity, meaning it has a specific magnitude and direction.

Being a vector quantity, it is also possible for it to equal zero because the two bond dipoles can cancel one another out.

A little arrow with its head on the positive centre and tail on the negative centre is typically used to represent it.

The dipole moment in chemistry is denoted by a modest modification of the arrow sign. On the positive centre and the negative centre, there is a cross to indicate it.
The lowest (zero) dipole moment is in \[\text{CC}{{\text{l}}_{\text{4}}}\]. Its symmetrical tetrahedral structure is the reason for this. Due to this, the opposite dipole moment of the other three bonds cancels out the dipole moment of one bond.

Option ‘D’ is correct

Note: Another vector quantity with a direction parallel to the bond axis is the bond dipole moment ($\mu $). The arrows used to depict dipole moments in chemistry start at the positive charge and stop at the negative charge.
The electrons usually shift from their initial positions to get closer to the more electronegative atom when two atoms with different electronegativities contact. The bond dipole moment can be used to visualise this electron motion.