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. |
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
The correct statement about the above reaction is :
1. | Hybridization of ‘B’ changes to sp2 from sp3 while there is no change in the hybridization of 'N'. |
2. | Hybridization of ‘N’ changes to sp3 from sp2 while there is no change in the hybridization of 'B'. |
3. | Hybridization of ‘N’ changes to sp2 from sp3 while there is no change in the hybridization of 'B'. |
4. | Hybridization of ‘B’ changes to sp3 from sp2 while there is no change in the hybridization of 'N'. |
The total number of sigma and pi bonds in C2H4 is:
1. 6 sigma bonds and 1 pi-bond.
2. 3 sigma bonds and 3 pi-bonds.
3. 5 sigma bonds and 1 pi-bond.
4. 2 sigma bonds and 2 pi-bonds.
The lone pairs of electrons can be defined as:
1. | Electron pairs that participate in bonding.
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2. | Electron pairs that do not participate in bonding.
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3. | Electron pairs that are present in inner most shell.
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4. | Electron pairs that are present in valence shell of ions. |