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# NEET Chemistry Solved Question Paper 2014

#### Multiple Choice Questions

1.

Choose the correctly paired gaseous cation and its magnetic (spin only) moment (in B.M.)

• Ti2+,3.87 B.M.

• Cr2+, 4.90 B.M.

• Co3+,3.87 B.M.

• Mn2+,4.90 B.M.

B.

Cr2+, 4.90 B.M.

Using expression, µ = $\sqrt{n\left(n+2}$ B.M. (where, n = no. of unpaired electrons)

 Ion Outer configuration n $\mu$ ${}_{22}\mathrm{Ti}^{2+}$ 3d2 2 2.84 ${}_{24}C{r}^{2+}$ 3d4 4 4.90 ${}_{27}C{o}^{3+}$ 3d6 4 4.90 ${}_{22}M{n}^{2+}$ 3d5 5 5.92

2.

The equilibrium constant for the reaction,

$\frac{1}{2}$${{\text{H}}_{2}}_{\left(g\right)}$$+$$\frac{1}{2}$${\text{I}}_{{2}_{\left(g\right)}}$$⇌$HI(g) is Kc

Equilibrium constant for the reaction 2HI(g) $⇌$H2(g) + I2(g)  will be

• 1/Kc

• 1/(Kc)2

• 2/Kc

• 2/(Kc)2

B.

1/(Kc)2

The given reaction is,

...(i)

Hence, ${\mathrm{K}}_{\mathrm{C}}=\frac{\left[\mathrm{HI}\right]}{\left[{\mathrm{H}}_{2}{\right]}^{1/2}\left[{\mathrm{I}}_{2}{\right]}^{1/2}}$    ...(ii)

Now, reverse the equaion (i) and multiple by 2, we get

Equating equations (ii) and (iii), we get

${\text{K}}_{C}^{\text{'}}=\frac{1}{\left({K}_{C}{\right)}^{2}}$

3.

What is the oxidation number of Br in KBrO?

• + 6

• + 7

• + 5

• + 8

B.

+ 7

Let the oxidation no. of Br be x.

In KBrO4, + 1 + x + 4 (-2) =0,- 7 + x = 0, x=+7

4.

Which of the following represents the correct bond order?

• ${O}_{2}^{+}<{O}_{2}^{-}>{O}_{2}^{2-}$

• ${O}_{2}^{-}>{O}_{2}^{2-}>{O}_{2}^{+}$

• ${O}_{2}^{2-}>{O}_{2}^{+}>{O}_{2}^{-}$

• ${O}_{2}^{+}>{O}_{2}^{-}>{O}_{2}^{2-}$

D.

${O}_{2}^{+}>{O}_{2}^{-}>{O}_{2}^{2-}$

Hence, the coorect Bond order is ${\text{O}}_{2}^{+}>{O}_{2}^{-}>{O}_{2}^{2-}$

 Ion Total no of electron MO configuration Bond order ${o}_{2}^{+}$ 15 2.5 ${o}_{2}^{-}$ 17 1.5 ${o}_{2}^{2-}$ 18 1.0

5.

In Omolecule, the formal charge on the central O-atom is

• 0

• -1

• -2

• +1

D.

+1

Lewis gave the structure of O, molecule as

Using the relation,
Formal charge = [Total no. of valence electrons in the free atom] - [Total no. of non-bonding (lone pair) electrons]- $\frac{1}{2}$ [Total no. of bonding (shared) electrons]
The formal charge on central O -atom i.e., no. 1

=6-2- -(6)=+1

6.

Which of the following pairs represent isotones?

• ${}_{78}{}^{195}\mathrm{Pt},{}_{76}{}^{190}\mathrm{Os}$

• ${}_{47}{}^{108}\mathrm{Ag},{}_{48}{}^{112}\mathrm{Cd}$

• ${}_{72}{}^{178}\mathrm{Hf},{}_{56}{}^{137}\mathrm{Ba}$

A.

Isotones have the same number of neutrons.
As = 77 - 33 = 44 ; Se = 78 - 34 = 44

7.

A diatomic gas at pressure P, compressed adiabatically to half of its volume, what is the final pressure?

• (2)1.4P

• P/(2)1.4

• (2)5/3P

• P/(2)5/3

A.

(2)1.4P

For adiabatic condition, ${\mathrm{PV}}^{\mathrm{\gamma }}$ = Constant

${\mathrm{P}}_{1}^{}$${\mathrm{V}}_{1}^{\mathrm{\gamma }}$ = ${\mathrm{P}}_{2}$${\mathrm{V}}_{2}^{\mathrm{\gamma }}$ ; V2$\frac{1}{2}$V1

${\mathrm{P}}_{2}$ = ${\mathrm{P}}_{1}$${\left[\frac{{\mathrm{V}}_{1}}{{\mathrm{V}}_{2}}\right]}^{\mathrm{\gamma }}$    [For diantomic gas $\mathrm{\gamma }$ = 1.4]

${\mathrm{P}}_{2}$ = ${\mathrm{P}}_{1}$

${\text{P}}_{2}$  =

8.

Which of the following is not sp2 hybridised?

• Graphite

• Graphene

• Fullerene

• Dry ice

D.

Dry ice

Solid CO2 is dry ice in which carbon atomundergoes sp-hybridisation.

9.

Which ofthe following statements is incorrect?

• Li+ has minimum degree of hydration.

• The oxidation state of K in KO2 is + 1.

• Na is used to make a Na/Pb alloy.

• MgSO4 is readily soluble in water.

A.

Li+ has minimum degree of hydration.

The hydration enthalpies of alkali metal ions decreases with increase in ionic sizes Hence, the order is Li+ > Na+> K> Rb+ > Cs+.Therefore, Li+ has maximum degree of hydration.

10.

Which is correct regarding size of atom?

• N < O

• B < Ne

• V > Ti

• Na > K

B.

B < Ne

The atomic radii of noble gases are by far the largest in their respective periods. This is due to the reason that noble gases have only van der Waals radii.