During change of $$NO^{+}\rightarrow NO$$, the electron is added to

$$\pi \quad ^{ \ast }$$-orbital

$$\sigma \quad ^{ \ast }$$-orbital

MCQ Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 13

Which molecule has zero dipole moment?

0%
$Xe{F}_{2}$
0%
${SO}_{2}$
0%
${CH}_{4}$
0%
p-dimethoxy benzene

Which of the following molecules has unequal bond length ?

0%
BF $_3$
0%
PF $_3$
0%
PF $_5$
0%
SF $_6$

The bonds present in borazole are

0%
9 $sigma$ , 6 $pi$
0%
12 $sigma$ , 3 $pi$
0%
6 $sigma$ , 9 $pi$
0%
15 $sigma$ only

The order of O-O bond length

O_{2}, H_{2} O_{2}, O_{3}

$O_2, H_2O_2, O_3$ is

0%
$O_2 > O_3 > H_2O_2$
0%
$H_2O_2 > O_3 > O_2$
0%
$O_3 > H_2O_2 > O_2$
0%
$O_2 > H_2O_2 > O_3$

The structure of

I {C l}_{2}^{-}

$I{Cl}_{2}^{-}$ is

0%
trigonal
0%
octahedral
0%
square planar
0%
linear

Select the correct statement

0%
$(C{ H }_{ 3 }{ ) }_{ 3 }\bar { C }$ is pyramidal while $\bar { C } (CN{ ) }_{ 3 }$ is planar
0%
$\bar { C } (CN{ ) }_{ 3 }$ is Pyramidal while $\bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$ is plannar
0%
both $\bar { C } (CN{ ) }_{ 3 }$ and $\bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$ are planar
0%
both $\bar { C } (CN{ ) }_{ 3 }$ and $\bar { C } (C{ H }_{ 3 }{ ) }_{ 3 }$ are Pyramidal

Total number of electron pairs in

P C l_{5}, P C l_{4}^{+}

$PCl_{5},\ PCl_{4}^{+}$ and

P C l_{6}^{-}

$PCl_{6}^{-}$ are respectively:

0%
$20,16,24$
0%
$24,16,20$
0%
$16,20,24$
0%
$24,20,16$

Which of the following statements given below is incorrect :

0%
$ONF$ is isoelectronic with ${O_2}{N^ - }$
0%
${\rm{O}}{{\rm{F}}_2}$ is an oxide of fluorine
0%
$C{l_2}{O_7}$ is an anhydride of perchloric acid
0%
${O_3}$ molecule is bent

During change of

N O^{+} \to N O

$NO^{+}\rightarrow NO$ , the electron is added to

0%
$\sigma$ -orbital
0%
$\pi$ -orbital
0%
$\sigma \quad ^{ \ast }$ -orbital
0%
$\pi \quad ^{ \ast }$ -orbital

Hybridization of central atoms in the molecules

N (C H_{3})_{3}

$N(CH_3)_3$ and

N (S i H_{3})_{3}

$N(SiH_3)_3$ respectively are:

0%
$sp^2$ nad $sp^2$
0%
$sp^3$ and $sp^3$
0%
$sp^2$ and $sp^3$
0%
$sp^3$ and $sp^2$

Product will be:

Which of the following compound has four bond pair and one lone pair?

0%
${ NH }_{ 4 }^{ + }$
0%
${ ICI }_{ 4 }^{ - }$
0%
${ SF }_{ 4 }$
0%
${ XeF }_{ 4 }$

Explanation

S F_{4}

$SF_{4}$

Stearic No.

= \frac{6 + 4}{2} = 5

$=\cfrac{6+4}{2}=5$

Geometry

\to

$\rightarrow$ Trigonal Bipyramidal

Hybridisation

\to s p^{3} d^{2}

$\rightarrow sp^{3}d^{2}$

From the figure, we can say

No. of bond pair

= 4

$=4$

No. of lone pair

= 1

$=1$

1138902_1170638_ans_e9c3a15c780b479d973707d344551b41.png

The order of number of lone pair of xenon in following compound is.

0%
$XeF_2 > XeF_4 > XeO_3 > XeO_4$
0%
${XeF_6} > XeOF_4 > XeO_3F_2$
0%
${XeO_6}^{4-} > {HXeO_4}^-$
0%
${XeF_5}^- > XeF_2 > XeO_3 > XeO_4$

X e O_{3} F_{2}

$XeO_3F_2$ the number of bond pairs on

X e

$Xe$ atom is:

0%
5
0%
2
0%
0
0%
4

The pair of species with the same bond order is:

0%
NO,CO
0%
$O_2^{2 - }{B_2}$
0%
$O_2^ + ,N{O^ + }$
0%
None of the above

The charge of an electron is

- 1.6 \times 10^{- 19} C

$-1.6 \times 10^{-19}C$ .The value free charge on

L i^{+}

$Li^+$ ion will be

0%
$3.6\times 10^{19}C$
0%
$1\times 10^{-19}C$
0%
$1.6\times 10^{-19}C$
0%
$2.6 \times 10^{-19}C$

L i H + {B - -}_{2} H_{6} \to 2 L i B - - H_{4}

$LiH + \underline {B}_2H_6 \rightarrow 2Li \underline{B}H_4$

Find the change in hybridization of the underlined atom.

0%
$sp^2 \rightarrow sp^3$
0%
$sp^3 \rightarrow sp^2$
0%
$sp \rightarrow sp^3$
0%
None

The number of right angled bonds in

{B r F}_{5}

${ BrF }_{ 5 }$ is:

0%
Six
0%
Eight
0%
Zero
0%
Four

Which has zero dipole moment

0%
cis-2-butene
0%
trans-2-butene
0%
1-butene
0%
2-methyl-1-propene

Explanation

Dipole moment,

μ = 0

$\mu=0$ due to symmetrical structure.
1632069_1193799_ans_7df436d9e9c7463ba6afce3b162c055a.png

What is the formal charge on

C l

$Cl$ in the following Lewis structure?

0%
$0$
0%
$+3$
0%
$+5$
0%
$+7$

Select the isomer given below, which have non-zero dipole moment?

0%
0%
0%
0%
all of these

For a diatomic molecule the dipole moment is 1.2 D and bond length is 1.0

\circ A

$\overset { \circ }{ A }$ then charge fraction on each atoms is:

0%
$12\%$
0%
$18\%$
0%
$25\%$
0%
$29\%$

Which of the following species is polar?

0%
$IF_7$
0%
$CIF_3$
0%
$XeF_4$
0%
$SiF_4$

Explanation

{C l F}_{3}

${ ClF }_{ 3 }$

({A B}_{3} E_{2})

$\left( { AB }_{ 3 }{ E }_{ 2 } \right)$

triagonal bipyramidol

The two axidl

C l - F

$Cl-F$ bonds, cancel their dipole moments each. The two equitorial lone pairs have a effective dipole moment in opposite direction to

C l - F

$Cl-F$ dipole moment in equitoridl plane

\Rightarrow

$\Rightarrow$

{C l F}_{3}

${ ClF }_{ 3 }$ is polar.

1092800_1200785_ans_52675e012f054ba9ae4ebb6902cf9983.jpg

Which of the following molecules has the shortest

C = C

$C=C$ bond length?

0%
$CH_2=C=CH_2$
0%
$CH_3-CH=CH_2$
0%
0%

Which of the following molecules will have polar bonds but zero dipole moment?

0%
$O_2$
0%
$CHCI_3$
0%
$CF_4$
0%
None of these

C H_{3} C H_{2} O H

$CH_3CH_2OH$ the bond that undergoes heterolytic most readily is :

0%
C-C
0%
C-H
0%
C-O
0%
O-H

How many pi (n) electrons are there in the following molecules?

0%
4
0%
6
0%
8
0%
10

In which of the following order is correct for diopole moment?

0%
$CH_3F > CH_3CI > CH_3Br > CH_3I$
0%
$CH_3CI > CH_3Br > CH_3F > CH_3I$
0%
$CH_3Br > CH_3CI > CH_3I > CH_3F$
0%
$CH_3CI > CH_3F > CH_3Br > CH_3I$

Which of the following is correct order of dipole moment.

0%
$CHC{L_3} > C{H_2}C{l_2} > C{H_3}Cl > CC{l_4}$
0%
$C{H_3}Cl > C{H_2}C{l_2} > CHC{l_3} > CC{l_4}$
0%
$C{H_2}C{l_2} > C{H_3}Cl > CHC{l_3} > CC{l_4}$
0%
$CHC{l_3} > C{H_3}Cl > C{H_2}C{l_2} > CC{l_4}$

Which of the following is incorrect order of dipole moment

0%
$N{H_3} > N{F_3} > NC{l_3}$
0%
$N{H_3} > NC{l_3} > N{F_3}$
0%
$C{H_3}Cl > C{H_3}F > C{H_3}Br$
0%
$HF > HCl > HBr$

Which of the following species has maximum dipole moment

0%
$C{H_3}F$
0%
$C{H_3}Cl$
0%
$C{H_3}Br$
0%
$C{H_3}I$

Which of the following is the correct order of dipole moment?

0%
$P(CF_3)_3(CH_3)_2 > P(CH_3)_3(CF_3)_2$
0%
$CH_3F > CH_3 Cl$
0%
$CH_2 Cl_2 > CH_3Cl$
0%

Which of the following species is non polar?

0%
$SO_{2}$
0%
$NO_{2}^{\ominus}$
0%
$XeOF_{2}$
0%
$PCl_{3}F_{2}$

Which of the following have largest dipole moment ?

Find the total number of sigma bonds in

H_{n} P_{n} O_{3 n}

$H_nP_nO_{3n}$ where n > 2.

0%
3n
0%
4n
0%
5n
0%
3 (n-1)

Which of the following compounds will show highest dipole moment

The dipole moment of the ammonia molecule is

1.48 D

$1.48D$ . The length of the dipole is

0%
$3.08\times 10^{-13}\ m$
0%
$5\times 10^{2}\ m$
0%
$308\ m$
0%
$None of these$

Which of the following fluoride of xenon has zero dipole moment?

0%
$XeF_2$
0%
$XeF_3$
0%
$XeF_4$
0%
$XeF_6$

The enthalpy of combination of

H_{2} (g)

$H_2(g)$ at

298 K

$298\,K$ to given

H_{2} O

$H_2O$ is

- 298 k J m o l^{- 1}

$-298\,kJ\,mol^{-1}$ and bond enthapies of

H - H

$H-H$ and

O = O

$O=O$ are

433 k J m o l^{- 1}

$433\,kJ\,mol^{-1}$ and

492 k J m o l^{- 1}

$492 kJ\,mol^{-1}$ , respectively.The mean bond enthalpy of

$O-H$ is:

$(\Delta H_{vap}$ of

$H_2O=40.65\,kJ/mol)$

0%
$464\,kJ\,mol^{-1}$
0%
$488.5\,kJ\,mol^{-1}$
0%
$232\,kJ\,mol^{-1}$
0%
$-232\,kJ\,mol^{-1}$

How many sigma

$s-sp^3$ bonds are there in ethane?

0%
7
0%
5
0%
6
0%
3

In which pair, the stronger bond found in the first species
a)

$O_{2}^{-}, O_{2}$ b)

$\mathbf{N}_{2} \cdot \mathbf{N}_{2}^{+}$ c)

$\mathrm{NO}^{+}, \mathrm{NO}^{-}$

0%
a only
0%
b only
0%
a and c only
0%
b and c only

Among the species

$C{O_2}C{H_3}CO{O^ - },CO,C{O_3}^{2 - }$ HCHO which has the weakest carbon oxygen bond

0%
$C{O_2}$
0%
$C{H_3}CO{O^ - }$
0%
$CO$
0%
$C{O_3}^{2 - }$

The interaction energy between two temporary dipoles is proportional to (where r is the distance between the two particles)

0%
$1/r^4$
0%
$1/r^2$
0%
$1/r^5$
0%
$1/r^6$

Carbon - halogen bond is most susceptible to cleave in

0%
Benzyl bromide
0%
Bromobenzene
0%
Vinyl bromide
0%
Benzyl chloride

The X -X bond lenght is

$1.00$

$\mathop A\limits^ \circ$ and C - C bond length is

$1.54$

$\mathop A\limits^ \circ$ . If electronegativities of

$X$ and

$C$ are

$3.0$ and

$2.0$ respestively the C - X bond length is likely to be :-

0%
$1.27\,\mathop A\limits^ \circ$
0%
$1.18\,\mathop A\limits^ \circ$
0%
$1.08\,\mathop A\limits^ \circ$
0%
$1.28\,\mathop A\limits^ \circ$

Which of the following has non-zero dipole moment?

0%
0%
0%
Trans-2-butene
0%
Boron trichloride

Which of the following combinations is not allowed (assumed z-axis is internuclear axis).

0%
$2s$ and $2s$
0%
$2p_{x}$ and $2p_{x}$
0%
$2s$ and $2p_{x}$
0%
$2p_{x}$ and $2p_{y}$

The compound with lowest dipole moment is.

0%
$C{H_3}F$
0%
$C{H_3}CI$
0%
$C{H_3}Br$
0%
$CH{Cl}_3$

Which of the following compounds has the largest
dipole moment?

0%
$CH_3-Cl$
0%
$CH_2-Cl_2$
0%
$CH-Cl_3$
0%
$C-Cl_4$

$\rm{O-H}$ bond length is

$1 \mathop {\text{A}}\limits^ \circ$ and it's dipole moment is

$1.5D$ . So the fraction of the charge on oxygen is

0%
$0.3125$
0%
$0.4$
0%
$0.5$
0%
$0.246$

CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 13 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 13 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

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