The order of electronegativity of carbon in sp, ${\mathrm{sp}}^2 \mathrm{and} {\mathrm{sp}}^3$ hybridized states follows

1. $\mathrm{sp}>{\mathrm{sp}}^2>{\mathrm{sp}}^3$

2. ${\mathrm{sp}}^3>{\mathrm{sp}}^2>\mathrm{sp}$

3. $\mathrm{sp}>{\mathrm{sp}}^3>{\mathrm{sp}}^2$

4. ${\mathrm{sp}}^2>\mathrm{sp}>{\mathrm{sp}}^3$

 

In which of the dimerization process, the achievement of the octet is not the driving force.

1.  $2AlC{l}_3 \to A{l}_{2}C{l}_6$

2.  $BeC{l}_2\to BeC{l}_2 \left(solid\right)$

3.  $2lC{l}_3 \to l_{2}C{l}_6$

4.  $2B{H}_3 \to B_2{H}_6$

Anhydrous $AlC{l}_3$ is covalent. If the lattice energy for${\mathrm{AlCl}}_3 = 5137 \mathrm{kJ} {\mathrm{mol}}^{-1},$${∆}_{hydration}$ for ${\mathrm{Al}}^{3+} = -4665 \mathrm{kJ} {\mathrm{mol}}^{-1} \mathrm{and} {∆}_{\mathrm{Hydration}} \mathrm{for} {\mathrm{Cl}}^{-} = -381 \mathrm{kJ} {\mathrm{mol}}^{-1}$, will it remain covalent or become ionic in aqueous solution?

1.  It will remain covalent

2.  It will remain ionic

3.  It may or may not become ionic

4.  Being ionic or covalent of any molecule is independent of ionisation energy

The melting point of $Al{F}_3$ is $104°C$ and that of $Si{F}_4$ is $-77°C$ (it sublimes) because:

1.  There is a very large difference in the ionic character of the Al - F and Si - F bonds

2.  In $Al{F}_3, A{l}^{3+}$ interacts very strongly with the neighboring $F^{-}$ ions to give a three-dimensional structure but in $Si{F}_4$ no such interaction is possible

3.  The silicon ion in the tetrahedral $Si{F}_4$ is not shielded effectively from the fluoride ions whereas in $Al{F}_3, the A{l}^{+3}$ ion is shielded on all sides

4.  The attractive forces between the $Si{F}_4$ molecules are strong whereas those between the $Al{F}_3$ molecule are weak

In the series ethane, ethylene and acetylene, the C - H bond energy is

1.  The same in all the three compounds

2.  Greatest in ethane

3.  Greatest in ethylene

4.  Greatest in acetylene

The bond order depends on the number of electrons in the bonding and antibonding orbitals. Which of the following statements are correct about bond order?

1.  Bond order can have a negative value.

2.  It always has an integral value.

3.  It is a nonzero quantity

4.  It can assume any value-positive or integral or fractional, including zero upto four.

What is the best description of the geometry of the nitrogen atoms in dimethylnitrosamine, ${\left({\mathrm{CH}}_3\right)}_2\mathrm{NNO}$?

         N bounded to $C{H}_3$ groups                       N bonded to O

1.  Trigonal planar                                         Linear

2.  Trigonal planar                                         Bent

3.  Trigonal pyramidal                                   Linear

4.  Trigonal pyramidal                                   Bent

The following diagram is sometimes used to illustrates the structure of benzene $C_6{H}_6$

Which of the statements concerning the structure of benzene is false?

1.  The double bonds oscillate rapidly back and forth between adjacent pairs of carbon atoms

2.  The $\mathrm{H} -\mathrm{C} -\mathrm{C} \mathrm{angles} \mathrm{are} 120°$

3.  The carbon atoms form a flat hexagonal ring

4.  Above structures are resonance structures

The diamagnetic species is

1. NO

2. ${\mathrm{NO}}_2$

3. ${\mathrm{O}}_2$

4. ${\mathrm{CO}}_2$

Consider the Lewis structure given below for the $C{H}_{3}CCH$ molecule

What is the maximum number of atoms that can lie in the same plane?

1.  Three

2.  Four

3.  Five

4.  Six