The application of dipole moment is/are :
1. | It is used to differentiate polar and non-polar bonds. |
2. | It is helpful in calculating the percentage ionic character of a molecule. |
3. | Both '1' and '2' |
4. | None of the above. |
has a net dipole moment while
\(BeF_2\) has zero dipole moment because :
1. F is more electronegative than oxygen.
2. Be is more electronegative than oxygen.
3. molecule is linear and \(BeF_2\) is bent.
4. molecule is linear and is bent.
A molecule among the following that has the maximum dipole moment is:
1. | \(\mathrm{CO_2}\) | 2. | \(\mathrm{CH_4}\) |
3. | \(\mathrm{NH_3}\) | 4. | \(\mathrm{NF_3}\) |
The correct statement among the following for a compound having a higher dipole moment is-
1. | Greater will the ionic nature. | 2. | Lesser will be the polarity. |
3. | Smaller will be the ionic nature. | 4. | None of the above. |
The correct increasing order of the polarizing power of the cationic species is:
1.
2.
3.
4.
Non-Zero dipole moment is shown by :
1.
2. p-Dichlorobenzene
3. Carbontetrachloride
4. Water.
The molecule/s that will have non zero dipole moments is /are :
1. 1,2-dichloro benzene.
2. Cis-3-hexene.
3. Trans-2-pentene.
4. All of the above.
A molecule among the following with non-zero dipole moment is:
1.
2.
3.
4.
Which of the following is a pair of polar molecules?
1.
2.
3.
4.
The correct order of increasing dipole moment is :
1. < < <
2. < < <
3. < < <
4. < < <