Question

Experiment shows that \[{{\rm{H}}_{\rm{2}}}{\rm{O}}\] has a dipole moment while \[{\rm{C}}{{\rm{O}}_{\rm{2}}}\] has not. Point out the structures which best illustrate these facts
A)

B)

C)

D)

Answer 1

Hint: To find out the hybridization of the Ag atom in the given complex, first we have to calculate the oxidation state of the silver (Ag) atom. Then, we have to find its hybridization using the valence bond theory.

Complete Step by Step Answer:
The diagram of the \[{\rm{C}}{{\rm{O}}_{\rm{2}}}\] molecule is,

Image: \[{\rm{C}}{{\rm{O}}_{\rm{2}}}\] molecule
So, we see that the shape of the molecule is linear, having the oxygen atom on either end of the carbon atom. The nature of the C=O is polar because of the more electronegative oxygen than carbon. The polarity of the two C=O bonds point exactly opposite to one another, so the individual bond dipoles get cancelled. Therefore, the carbon dioxide molecule has a dipole moment of zero.

The water molecule is as follows:

Image: Water molecule

In the water molecule, the two polar bonds of O-H are present. And they point in the same direction which is towards the central atom O. Therefore, the dipole moments of the two bonds are not getting cancelled but added. So, the water molecule has some dipole moment.

Therefore, option A depicts the correct diagram of water and carbon dioxide, that is the linear structure of \[{\rm{C}}{{\rm{O}}_{\rm{2}}}\] and bent structure of water.

Note: The dipole moment's magnitude helps us to identify the nature of the polar bond. The increase of the dipole moment's magnitude tells us the bond's polar nature. Molecules possessing zero dipole moment are non-polar molecules.