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

Which of the following compound have the same no. of lone pair with their central atom?

(i)$<mspace\; width="1em"></mspace>{\mathrm{XeF}}_5^{-<mspace\; width="1em"></mspace>}$             

(ii) ${\mathrm{BrF}}_3$                 

(iii) ${\mathrm{XeF}}_2$                     

(iv) ${\mathrm{H}}_3{\mathrm{S}}^{+}$               

(v) Triple Methylene     

options are as follows :        

(1) (iv) and (v)                                     

(2) (i) and (iii) 

(3) (i) and (ii)                                     

(4) (ii) (iv), (v)

In which of the following species central atom is NOT surrounded by exactly 8 valence electrons?

(a) $B{F_4}^{-}$

(b) $NC{l}_3$

(c) PC${l_4}^{+}$

(d) $S{F}_4$

The least polar bond is present in which of the following?

Which set contains only covalently bonded molecules?

(1) $BC{l}_{3<mspace\; width="1em"></mspace>},<mspace\; width="1em"></mspace>SiC{l}_4<mspace\; width="1em"></mspace>,PC{l}_3$

(2) $N{H}_{4}Br<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>N_2{H}_4,HBr$

(3) $I_{2<mspace\; width="1em"></mspace>,}{H}_{2}S<mspace\; width="1em"></mspace>,<mspace\; width="1em"></mspace>NAI$

(4) $A{l}_2,O_{3<mspace\; width="1em"></mspace>},<mspace\; width="1em"></mspace>A{S}_4$

Bond order of 1.5 is shown by

1. ${\mathrm{O}}_2^{+}$     

2. ${\mathrm{O}}_2^{-}$       

3. ${\mathrm{O}}_2^{2-}$     

4. O₂

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 ${\mathrm{NH}}_4^{+}$]

A polar molecule among the following is -

1. BF₃

2. SF₄

3. SiF₄

4. XeF₄