The pair of electrons in the given carbanion, CH₃C≡C^-, is present in which of the following orbitals?

1.	sp3	2.	sp2
3.	sp	4.	2p

Which of the following species contains equal number of $\mathrm{\sigma }$ and $\mathrm{\pi }$ bonds?

1. ${\mathrm{HCO}}_3^{-}$                                   

2. XeO₄

3. (CN)₂                                     

4. CH₂(CN)₂

The correct bond order in the following species is

1. ${\mathrm{O}}_2^{2+}>{\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{-}$

2. ${\mathrm{O}}_2^{2+}<{\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{+}$

3. ${\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{2+}$

4. ${\mathrm{O}}_2^{-}<{\mathrm{O}}_2^{+}>{\mathrm{O}}_2^{2+}$

XeF₂ is isostructural with : 

1. TeF₂

2. ICI₂^-

3. SbCl₃

4. BCl₃

A polar molecule among the following is -

1. BF₃

2. SF₄

3. SiF₄

4. XeF₄

Which one of he following pairs is isostructural (i.e., having the same shape and

hybridization)?

1. [BCl₃ and BrCl₃]

2. [NH₃ and ${\mathrm{NO}}_3^{-}$]

3. [NF₃ and BF₃]

4. [${\mathrm{BF}}_4^{-}$ and ${\mathrm{NH}}_4^{+}$]

Bond order of 1.5 is shown by

1. ${\mathrm{O}}_2^{+}$     

2. ${\mathrm{O}}_2^{-}$       

3. ${\mathrm{O}}_2^{2-}$     

4. O₂

What is the dominant intermolecular force on bond that must be overcome in converting

liquid CH₃OH to a gas?

1. Hydrogen bonding

2. Dipole-dipole interaction

3. Covalent bonds

4. London dispersion force

The correct order of electronegativity of hybrid orbitals of carbon is:

(1) sp>sp²<sp³             

(2) sp>sp²>sp³

(3) sp<sp²>sp³             

(4) sp<sp²<sp³

$H_{2}O$ has a net dipole moment while Be$F_2$ has zero dipole moment because :

(1) F is more electronegativity than oxygen 

(2) Be is more electronegativity than oxygen 

(3) $H_{2}O<mspace\; width="1em"></mspace>$ molecule is linear and Be$F_2$ is bent 

(4) $Be{F}_2$ molecule is linear and $H_{2}O$ is bent