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 d2sphybridization.

Subtopic:  Hybridisation |
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 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 

Subtopic:  Polarity |
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The shapes of sp, sp2, sp3 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

Subtopic:  Hybridisation |
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BF3+NH3F3B.NH3

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'.

Subtopic:  Hybridisation |
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The total number of sigma and pi bonds in C2His

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.

Subtopic:  Hybridisation |
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The lone pairs of electrons can be defined as -

1. Electron pairs that participate in bonding.

2. Electron pairs  that do not participate in bonding.

3. Electron pairs that are present in inner most shell.

4.Electron pairs that are present in valence shell of ions.

Subtopic:  Octate, Isoelectronic Species, Lewis Structure & Formal Charge |
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Be2 molecule does not exist. The best explanation to explain this on the basis of the molecular orbital theory is -

1. The bond order of Be2 is one.

2. The bond order of Be2 is negative.

3. The bond order of Be2 is zero.

4. The bond order of Be2 is two.

Subtopic:  M.O.T |
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The axial bonds are longer as compared to equatorial bonds in PCl5 because -

1. Axial bond pairs suffer more repulsion from the equatorial bond pairs

2. Equatorial bond pairs suffer more repulsion from the axial bond pairs

3. Both 1, and 2

4. None of the above

Subtopic:  Hybridisation |
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The relation between hydrogen bond and the van der Waals forces is -

1. Both the bonds have equal strength

2. Hydrogen bonds are weaker than van der Waals forces

3. Hydrogen bonds are stronger than van der Waals forces

4. None of the above

Subtopic:  Types of Chemical Bond |
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The significance of the octet rule is:

1. To determine the stability of atoms.

2. To find the hybridization of elements.

3. To calculate the number of lone pairs.

4. None of the above.

Subtopic:  Octate, Isoelectronic Species, Lewis Structure & Formal Charge |
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