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. |
can be represented by structures 1 and 2 shown below.
These two structures cannot be taken as the canonical forms of the resonance hybrid, because :
1. | The positions of the atoms have changed.
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2. | The positions of the atoms are constant.
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3. | H3PO3 does not show resonance.
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4. | Two hydrogen atoms are missing. |
The shape of molecule is bent while that of is linear. The correct explanation is:
1. | The dipole moment of carbon dioxide is 3.84 D and water is zero. |
2. | The dipole moment of water is zero and carbon dioxide is 1.84 D. |
3. | The dipole moment of carbon dioxide is zero and water is 1.84 D. |
4. | The dipole moment of carbon dioxide is 3.84 D and 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. |
The shapes of sp, , orbitals formed due to hybridization of atomic orbitals would be respectively:
1. Trigonal planar, linear, tetrahedral
2. Linear, trigonal planar, tetrahedral
3. Linear, tetrahedral, trigonal planar
4. Tetrahedral, trigonal planar, linear