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.

The important condition/s required for the linear combination of atomic orbitals to form molecular orbitals is:

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.

The axial bonds are longer as compared to equatorial bonds in PCl₅ because:

The relation between hydrogen bond and the van der Waals forces is:

If the main axis of a diatomic molecule is z, then the molecular orbital p_x and p_y overlap to form which of the following orbital:

1.  $\mathrm{\pi }$ molecular orbtial
2.  σ molecular orbital
3.  δ molecular orbtial
4.  No bond will form

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.

The incorrect statement among the following is:

The correct Lewis structure of acetic acid is:

1.		2.
3.		4.	None of the above.

H₂ molecule on the basis of valence bond theory is formed due to:

1. Attractive forces being more than the repulsive forces.

2. Attractive forces being less than the repulsive forces.

3. No force of attraction.

4. Only repulsive force.