Q. No.The correct relationship between bond strength and bond order is :
1.
Bond strength is directly proportional to the bond order.
2.
Bond strength is inversely proportional to the bond order.
3.
There is no relationship between these two terms.
4.
None of the above.
The bond length can be defined as:
| 1. | The equilibrium distance between the nuclei of two bonded atoms in a molecule. |
| 2. | The farthest distance between the nuclei of two bonded atoms in a molecule. |
| 3. | The shortest distance between the nuclei of two bonded atoms in a molecule. |
| 4. | None of the above. |
\(\text{H}_3\text{PO}_3\) can be represented by structures 1 and 2 shown below.
However, these two structures cannot be considered as canonical forms of a resonance hybrid because:
| 1. | The positions of the atoms are different in each structure.
|
| 2. | The positions of the atoms remain unchanged.
|
| 3. | \(\text{H}_3\text{PO}_3\) does not show resonance.
|
| 4. | Two hydrogen atoms are missing. |
The shape of molecule is bent while that of is linear. The correct explanation for this fact is that dipole moment of:
| 1. | carbon dioxide is 3.84 D and that of water is zero. |
| 2. | water is zero and that of carbon dioxide is 1.84 D. |
| 3. | carbon dioxide is zero and that of water is 1.84 D. |
| 4. | carbon dioxide is 3.84 D and that of water is 1.84 D. |
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. |
The difference between electronegativity and electron gain enthalpy is:
| 1. | An element has a constant value of the electron gain enthalpy but not of electronegativity. |
| 2. | There is no difference between these two terms. |
| 3. | An element has a constant value of electronegativity but not of electron gain enthalpy. |
| 4. | None of the above. |
The correct order of increasing ionic character in the molecules: LiF, K2O, and ClF3 is:
1.
2.
3.
4.
CH4 does not exhibit square planar geometry because:
| 1. | For square planar geometry, 5 bonds are required. |
| 2. | Carbon does not have d-orbitals to undergo dsp2 hybridization. |
| 3. | Due to steric hindrance CH4 does not exhibit square planar geometry. |
| 4. | Carbon does not have d-orbitals to undergo d2sp3 hybridization. |
BeH2 molecule has a zero dipole moment because -
| 1. |
Dipole moments of each H–Be bond are unequal and are in opposite directions. |
| 2. | Dipole moments of each H–Be bond are equal and are in opposite directions. |
| 3. | Dipole moments of each H–Be bond are equal and are in same directions. |
| 4. | Dipole moments of each H–Be bond are unequal and are in same directions. |
Among and , _____ has higher dipole moment because -
1. NF3 ; the resultant bond moment of the N–H bonds add up with the lone pair while N – F bonds partly cancels the moment of the lone pair.
2. NH3 ; the resultant bond moment of the N–F bonds add up with lone pair while N - H bonds partly cancels the moment of the lone pair.
3. NF3 ; the resultant bond moment of the N–F bonds add up with the lone pair while N – H bonds partly cancels the moment of the lone pair.
4. NH3 ; the resultant bond moment of the N–H bonds add up with lone pair while N – F bonds partly cancels the moment of the lone pair.
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