MCQ Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 15

VSEPR theory suggest a small departure from

$109^0 28'$ for

$NH_3$ molecule. The H-N-H bond angle has been found to be

$107^0$ what kind of hybrid orbital will be occupied by the non -bonding pair of electron?

0%
$sp^3$
0%
$sp^{3.4}$
0%
$sp^{2.13}$
0%
$sp^2$

Which of the following has -O-O- linkage ?

0%
$H_2S_2O_6$
0%
$H_2S_2O_8$
0%
$H_2S_2O_3$
0%
$H_2S_4O_6$

Which species has the maximum number of lone pair of electrons on the central atom ?

0%
$[ ClO^-_3]$
0%
$XeF_4$
0%
$SF_4$
0%
$[ I^-_3]$

Which of the following sets of molecule(s) is/are having a linear shape but different hybridization?

0%
$I^-_3$ and $CO_2$
0%
$HgCl_2$ and $ICl^-_2$
0%
$XeF_2$ and $C_2H_2$
0%
$XeF_2$ and $OCl^-$

Explanation

A) $I_{3}^{-}$ and $CO_{2}$ are linear in shape. $I_{3}^{-}$ undergoes $sp^{3}$ hybridization and $CO_{2}$ undergoes $sp$ hybridization.

B) $HgCl_{2}$ and $ICl_{2}^{-}$ are linear in shape. $HgCl_{2}$ undergoes $sp$ hybridization and $ICl_{2}^{-}$ undergoes $sp^{3}d$ hybridization .

C) $XeF_{2}$ and $C_{2}H_{2}$ are linear in shape. $XeF_{2}$ undergoes $sp^{3}d^{2}$ and $C_{2}H_{2}$ undergoes $sp$ hybridization.

D) $XeF_{2}$ and $OCl^{-}$ are linear in shape. $XeF_{2}$ undergoes $sp^{3}d^{2}$ and $OCl^{-}$ undergoes $sp^{3}$ hybridization .

Hence, options A, B, C, and D all are correct.

$OF_2$ number of bond pairs and lone pairs of electrons are:

0%
2, 6
0%
2, 8
0%
2, 10
0%
1, 9

Explanation

$OF_2$ molecule, the total number of bond pairs and lone pairs of electrons present is 2 and 8. There are two bond pairs of electrons which form two

$O-F$ pairs.

$O$ atom has two lone pairs of an electron. Each

$F$ atom has 3 lone pairs of electrons. Thus in total, there are 8 lone pairs of electrons.

Hence the correct answer is option B.

A diatomic molecule has a dipole moment of

$1.2 D$ if its bond distance is

$1.0 \mathring{A}$ . What fraction of an electronic charge 'e' (i.e. charge on an electron) exists on each atom?

0%
$20\%$ of e
0%
$21\%$ of e
0%
$19\%$ of e
0%
$25\%$ of e

Which of the following molecule/species is having minimum number of lone pair on its central atom?

0%
$BrF_3$
0%
${BrF_4}^-$
0%
${XeF_5}^+$
0%
${I_3}^-$

Which of the following statement is/are correct ?

0%
All carbon to carbon bonds contains a sigma bond and one or more $\pi$ -bonds
0%
All carbon to carbon bonds are sigma bonds
0%
All oxygen to hydrogen bonds are hydrogen bonds
0%
All carbon to hydrogen bonds are sigma bonds

$NO_3^-$ ion, number of bond pairs and lone pairs of electrons on nitrogen atom are -

0%
2, 2
0%
3, 1
0%
1, 3
0%
4, 0

Explanation

$NO_3^-$ ion, due to the presence of one negative charge, number of valence electrons

$=5+1=6$

One

$O-$ atom forms two bonds and two

$O-$ atom are shared with two electrons of

$N-$ atom

Thus,

$3$

$O-$ atoms are shared with

$8$ electrons of

$N-$ atom.

Number of bond pairs (or shared pairs)

$=4$

Number of lone pairs

$=0$

Hence correct answer is option D.

1560987_1725931_ans_645de7b7bcdc436899ac71e8a15e9582.jpg

$OF_2$ , the number of bond pairs and lone pairs of electrons is, respectively:

0%
$2, 6$
0%
$2, 8$
0%
$2, 10$
0%
$2, 9$

The formula charges on three oxygen atoms of ozone molecule are respectively:

0%
+1, 0 , + 1
0%
0, 0 , 0
0%
+1, 0 , -1
0%
-1 , +1 , -1

Explanation

According to the electron-dot structure, there are 12 number of bonding electrons and 6 number of non-bonding electrons.

Now we have to calculate the formal charges of each oxygen atom.

Formal charge $=$ Valence electrons $-$ Non-bonding electrons $-\dfrac{Bonding\,\,electrons}{2}$

Formal charge on $O_1=6-2-\dfrac 62=+1$

Formal charge on $O_2=6-4-\dfrac 42=0$

Formal charge on $O_3=6-6-\dfrac 22=-1$

Hence the correct answer is option C.

1561020_1725924_ans_894fb0212f4e42ffaff8f8e392174f12.jpg

Covalency is favoured in the following cases:

0%
a smaller cation
0%
a larger anion
0%
large charges on cation and anion
0%
a cation without noble gas configuration

$C-C$ bond length is maximum in:

0%
diamond
0%
graphite
0%
naphthalene
0%
fullerene

Identify the correct sequence of increasing number of

$\pi-$ bonds in structures of the following molecules.
(i)

$H_{2}S_{2}O_{6}$
(ii)

$H_{2}SO_{3}$
(iii)

$H_{2}S_{2}O_{5}$

0%
$I, II, III$
0%
$II, III, I$
0%
$II, I, III$
0%
$I, III, II$

The number of

$P-O-P$ bonds in cyclic metaphosphoric acid is:

0%
zero
0%
two
0%
three
0%
four

Compound

$X$ is anhydride of sulphuric acid. The number of sigma bonds and

$\pi$ - bonds present in

$X$ are respectively:

0%
$6$ and $6.95$
0%
$5$ and $5.95$
0%
$3$ and $3$
0%
$4$ and $5.92$

The bond length of the species

$O_2, O_2^+,and\ O_2^-$ are in the order of:

0%
$O_2^+ >O_2 >O_2^-$
0%
$O_2^+ >O_2^- >O_2$
0%
$O_2 >O_2 ^+>O_2^-$
0%
$O_2^->O_2 >O_2^+$

Explanation

As bond order increases bond length decreases the bond order of species are:

$\dfrac {Number \, of \, bonding \, electron- Number \, of a.b. \, electron}{2}$

For

$O_2=\dfrac {10-6}{2}=2$

$O_2^+=\dfrac {10-5}{2}=2.5$

$O_2^-=\dfrac {10-7}{2}=1.5$

so bond order

$O_2^+ >O_2 >O_2^-$ and bond length are

$O_2^- >O_2 >O_2^+$

Option D is correct.

Which species has the maximum number of lone pairs of electrons on the central atom?

0%
$ClO_3^-$
0%
$XeO_4$
0%
$I_3^-$
0%
$SF_4$

The bond strength increase:

0%
with increasing bond order
0%
with increasing extent of overlapping of orbitals
0%
with decreasing in bond length
0%
from a single bond to triple bond

In which pair(s) is/are the stronger bond found in the first species?

0%
${O_{2}}^{-}, O_{2}$
0%
$N_{2}, {N_{2}}^{+}$
0%
${NO}^{+}, {NO}^{-}$
0%
$CO,{O_{2}}^{2+}$

Number of sigma bonds in

$P_4O_{10}$ is:

0%
6
0%
7
0%
17
0%
16

Explanation

Number of sigma bonds in

$P_4O_{10}$ is

$(d)$

$16$ .

1671707_1752273_ans_6d94f3d2a5a54122b3dc875cdf0e1a10.PNG

In which case the bond length is minimum between carbon and nitrogen?

0%
$CH_3NH_2$
0%
$C_6H_5CH=NOH$
0%
$CH_3CONH_2$
0%
$CH_3CN$

Explanation

$CH_3CN$ bond order between C and N is 3 so its bond length is minimum.

There is triple bond between C and N in

$CH_3CN$

Option D is correct.

How many bonding electron pairs are there in white phosphorous?

0%
6
0%
12
0%
4
0%
8

The number of

$P-O-P$ bonds in cyclic meta phosphoric acid is:

0%
one
0%
two
0%
three
0%
four

Explanation

The number of

$P-O-P$ bond in cyclic metaphosphoric acid is three.
1562116_1733883_ans_d2c21c97386242329e248c511d9aa253.PNG

In benzene the total number of

$\sigma$ bonds is

0%
$3$
0%
$6$
0%
$9$
0%
$12$

Explanation

$C-C\ \sigma$ bonds

$=6$

$C-H\ \sigma$ bonds

$=6$

__________

Total sigma bond

$=12$

1677609_1761229_ans_255dc85702df44a993e1399560cc63b3.png

Which of the following statements are correct about

$CO_{3}^{2-}$ ?

0%
The hybridisation of central atom is $sp^{3}$ .
0%
Its resonance structure has one $C-O$ single bond and two $C=O$ double bonds.
0%
The average formal charge on each oxygen atom is $0.67$ units.
0%
All $C-O$ bond lengths are equal.

Explanation

The hybridisation of central atom is $sp^2$
Since a net charge of ${-}2$ is shared over 3 $Oxygen$ atoms, hence formal charge = $0.67$ units
In resonating structures bonds are not fixed and therefore, all bond lengths are equal.

hence options

$(C)$ and

$(D)$ are correct.

The bond in

$K_{4}[Fe(CN)_{6}]$ are

0%
all ionic
0%
all covalent
0%
ionic and covalent
0%
ionic, covalent and co-ordinate covalent

Explanation

The bond in

$K_{4}[Fe(CN)_{6}]$ are ionic, covalent and co-ordinate covalent.

Ionic bond between cation and anion, covalent bond between C and N atom in the ligand and coordinate bond between ligand and central metal atom.

1672772_1760693_ans_f669014b44c4414bb3e4452420057d73.png

Which of the following has no net dipole moment?

Number of bonds in benzene

0%
$6\sigma$ and $3\pi$
0%
$12\sigma$ and $3\pi$
0%
$3\sigma$ and $12\pi$
0%
$6\sigma$ and $6\pi$

Explanation

The number of bonds in benzene is

$12\sigma$ and

$3\pi$ bonds.

Number of

$\sigma$ bonds in

0%
$6$
0%
$15$
0%
$10$
0%
$12$

Explanation

There are

$15\ \sigma$ and

$3\ \pi$ bonds in the given molecule. Each double bond contain

$1\ \sigma$ and

$1\ \pi$ and single bond form is always a sigma bond.

Which of the following statements is wrong?

0%
Single $N-N$ bond is stronger than the single $P-P$ bond.
0%
$PH_{3}$ can act as a ligand in the formation of coordination compound with transition elements.
0%
$NO_{2}$ is paramagnetic in nature.
0%
Covalency of nitrogen in $N_{2}O_{5}$ is four.

In a compound the number of sigma and pi bonds respectively are :

0%
19, 11
0%
19, 5
0%
13, 11
0%
7, 3

Which of the following compounds have the same no. of lone pairs with their central atom?

(I)

$XeF_5^-$ (II)

$BrF_3$ (III)

$XeF_2$ (IV)

$H_3S^+$ (V) Triple Methylene

0%
IV and V
0%
I and III
0%
I and II
0%
II, IV and V

Explanation

$XeF_5^-$ : 2 lone pairs : pentagonal planar

$BrF_3$ : 2 lone pairs : Bent-T-shape

$XeF_2$ : 3 lone pairs : Linear

$H_3S^+$ : 1 lone pairs : Pyramidal Linear

Triple Methylene : 1 lone pair : V-shape

Correct set of species with zero dipole moment is :
(i)

$CO_{2}$ (ii)

$COCl_{2}$ (iii)

$CH_{2}Cl_{2}$ (iv)

$BCl_{3}$

0%
(i) and (iv)
0%
(ii) and (iv)
0%
(iii) and (iv)
0%
(i), (iii) and (iv)

Which of the following combination of orbitals does not form covalent bond (x-axis is inter nuclear axis) :

0%
$s + p_{y}$
0%
$p_{y} + p_{y}$
0%
$d_{yz} + d_{yz}$
0%
$d_{xy} + d_{xy}$

Covalency favoured in the following case :

0%
smaller cation
0%
larger anion
0%
large charge on cation and anions
0%
all of these

Consider the following compounds and select the incorrect statement from the following :

$NH_{3}, PH_{3}, H_{2}S, SO_{2}, SO_{3}, BF_{3}, PCl_{3}, IF_{7}, P_{4}, H_{2}$

0%
Six molecules out of given compound involves hybridisation
0%
Three molecules are hypervalent compounds
0%
Six molecules out of above compounds are non-planar in structure
0%
Two molecules out of given compounds involves $(d \pi- p \pi)$ bonding as well as also involves $(p \pi - p \pi)$ bonding

The incorrect statement(s) regarding

$\overset .{C} X_3$ species is :

0%
If electronegativity of surrounding element $'X'$ is less than $2.5$ , then central carbon atom used almost $33 \%$ s-character in their hybrid bonding orbitals.
0%
If electronegativity of surrounding element $'X'$ is greater than $2.5$ , then central carbon atom used almost $25 \%$ s-character in their hybrid bonding orbitals.
0%
If $'X'$ is $'F'$ , then species should be polar and pyramidal
0%
If $'X'$ is $H$ , then species should be polar and planar

Number of lone pairs present on central atom of

$I_{3}^{-}$ are:

0%
$9$
0%
$1$
0%
$6$
0%
$3$

Explanation

${I_{3}}^{-}$ has a linear structure. The number of lone pairs on central atom is

$3$ .

2113376_2005418_ans_0a80f9dbb0ce432cb94a5ef77c365e85.png

CBSE Questions for Class 11 Medical Chemistry Chemical Bonding And Molecular Structure Quiz 15 - 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 15 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

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