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Published on: 21/10/2025
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Questions + Answers key
Take MCQ Chemistry Test
1.
One mole of CO2 contains _______.
6.02 x 1023atoms of C
3 g of CO2
6.02 x 1023atoms of O
18.1 x 1023 molecules of CO2
2.
Which of the following has the highest mass?
1 g atom of C
\(\frac { 1 }{ 2 } \)mole of CH4
10 mL of water
3.011 x 1023atoms of oxygen
3.
The number of significant figures in 0.0101 is _______.
3
2
4
5
4.
What is the electronic configuration of the elements of group 14?
ns2 np4
ns2 np6
ns2 np2
ns2
5.
In the organic compound CH2=CH-CH2-CH2-C\(\equiv \)CH, the pair of hydridised orbitals involved in the formation of: C2 - C3 bond is _____.
sp - sp2
sp - sp3
Sp2 - Sp3
sp3 - sp3
6.
In the Lassaigne’s test for nitrogen in an organic compound, the Prussian blue colour is obtained due to the formation of: ______.
Na4[Fe(CN)6]
Fe4[Fe(CN)6]3
Fe2[Fe(CN)6]
Fe3[Fe(CN)6]4
7.
Which of the following carbocation is most stable ?
\(({ CH }_{ 3 })_{ 3 }C.\overset {+ }{ C } { H }_{ 2 }\)
\(\left( { CH }_{ 3 } \right) _{ 3 }\overset { + }{ C } \)
\({ CH }_{ 3 }{ CH }_{ 2 }\overset { +}{ C } { H }_{ 2 }\)
\({ CH }_{ 3 }\overset {+ }{ C } HC{ H }_{ 2 }{ CH }_{ 3 }\)
8.
The reaction: CH3CH2I + KOH (aq) \(\rightarrow\)CH3CH2OH + KI is classified as :________.
electrophilic substitution
nucleophilic substitution
elimination
addition
9.
The IUPAC name of ______.
1, 2-dichloropropane
3, 3-dichloropropane
1, 1-dichloropropane
dichloropropane
10.
The IUPAC name of ______.
2-methyl butanal
butan-2-aldehyde
2-ethylpropanal
3-methyl isobutraldehyde
11.
The bond that undergoes heterolytic cleavage most readily is ______.
C-C
C-O
C-H
O-H
12.
The hybridization state of a carbocation is ______.
Sp4
sp3
sp2
sp
13.
Which of the following are electrophiles?
Dimethyl sulphide
Bromides
Carbon dioxide
Ammonia
14.
Which of the following statements about a compound is incorrect?
A molecule of a compound has atoms of different elements
A compound cannot be separated into its constituent elements by physical methods of separation
A compound retains the physical properties of its constituent elements
The ratio of atoms of different elements in a compound is fIxed
15.
A student performs a titration with different burettes and finds titre values of 25.2 mL, 25.25 mL and 25.0 mL. The number of significant figures in the average titre value is _______.
1
2
3
4
16.
Which of the following statements is correct about the reaction given below?
\({ }_{4 \mathrm{Fe}}(s)+30_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(g)\)
Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass.
Total mass of reactants = total mass of product, therefore, law of multiple proportions is followed
Amount of Fe2O3 can be increased by taking anyone of the reactants (iron or oxygen) in excess
Amount of Fe2O3 produced will decrease if the amount of anyone of the reactants (iron or oxygen) is taken in excess.
17.
An organic compound containing C and H has 92.3%of carbon, its empirical formula is _______.
CH
CH3
CH2
CH4
18.
An organic compound containing C,Hand O has 49.3%carbon, 6.84% hydrogen and its vapour density is 73. Molecular formula of the compound is _______.
C3H5O2
C4H10O2
C6H10O4
C3H10O2
19.
What is the mass per cent of carbon in carbon dioxide?
0.034%
27.27%
3.4%
28.7%
20.
What will be the molality of the solution made by dissolving 10 g of NaOH in 100 g of water?
2.5 m
5 m
10 m
1.25 m
21.
X g of Ag was dissolved in HNO3 and the solution was treated with excess of NaCl, when 2.87g of AgCl was precipitated. The value of x is _______.
1.08 g
2.16 g
2.70 g
1.62g
22.
Which law states that if two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of other element, are in the ratio of small whole numbers?
Avogadro's law
Law of definite composition
Law of multiple proportions
Gay Lussac's law of gaseous volumes
23.
What will be the molarity of pure water?
18 M
50.0 M
55.6 M
100 M
24.
Which important property did Mendeleev use to classify the elements in his periodic table?
Atomic weight
Atomic number
Melting point
None of these
25.
Which of the following statements is incorrect?
Mendeleev's arranged elements in horizontal rows and vertical columns
Mendeleev's arranged elements in order of their increasing atomic number
Mendeleev's system of classifying elements was more elaborate than that of Lother Meyer
None of the above
26.
The period number in the long form of the periodic table is equal to _____.
magnetic quantum number of any element of the period
atomic number of any element of the period
maximum principal quantum number of any element of the period
maximum azimuthal quantum number of any element of the period
27.
Periodic classification of elements can be done on the basis of electronic configuration and is used to examine the _____.
periodic trends in physical properties of elements
periodic trends in chemical properties of elements
Both (a) and (b)
None of the above
28.
Predict the position of an element having the electronic configuration \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{1}\) _____.
Period 4, group 6
Period 6, group 4
Period 3, group 1
Period 4, group 5
29.
The electronic configuration of gadolinium (Atomic number 64) is _____.
[Xe] 4f3 5d5 6s2
[Xe] 4f7 5d2 6s1
[Xe] 4f7 5d1 6s2
[Xe] 4f8 5d6 6s2
30.
General outer electronic configuration of d-block elements is _____.
\((n-1) d^{1-10} n s^{3}\)
\((n+1) d^{1-10} n s^{0-2}\)
\((n-1) d^{1-10} n s^{0-2}\)
\((n-1) d^{0} n s^{0-2}\)
31.
The elements in which electrons are progressively filled in 4f-orbital are called______.
actinoids
transition elements
lanthanoids
halogens
32.
Elements are classified into four blocks like s-block, p-block, d-block and f-block on the basis of ______.
atomic number
atomic mass
atomic orbitals
All of these
33.
Out of the four blocks in which periodic table is divided, helium belongs which block?
s-block
p-block
d-block
f-block
34.
The outermost electronic configuration of p-block elements varies from ns2np 1 to ______.
\(n s^{2} n p^{5}\)
\(n s^{2} n p^{4}\)
\(n s^{2} n p^{6}\)
\(n s^{2} n p^{3}\)
35.
According to IUPAC,total number of groups and periods in the periodic table respectively are ______.
16, 9
18, 7
18, 9
13, 7
36.
Outer electronic configuration off-block elements is ______.
\((n+1) f^{1-14}(n-1) d^{0-1} n s^{2}\)
\((n-2) f^{1-14}(n+1) d^{0-1} n s^{2}\)
\((n-2) f^{1-14}(n-1) d^{0-1} n s^{2}\)
None of the above
37.
Which type of compound is shown by the following structure ______.
Alicyclic compound
Benzenoid aromatic compound
Non-benzenoid aromatic compound
Acyclic compound
38.
Correct IUPAC name for H3C ______.
2-ethyl-3-methylpentane
3, 4-dimethylhexane
2-sec-butylbutane
2, 3-dimethylbutane
39.
The structure of iso-butyl group in an organic compound is ______.
CH3-CH2-CH2-CH3
CH3-CH2-CH2-CH2-
40.
What is the correct IUPAC name of the following?
3-ethyl-1,1-dimethylcyclohexane
t-ethyl- 3,3-dimethylcyclohexane
1,1-dimethyl-3-ethylcyclohexane
None of the above
41.
Write the correct IUPAC name of the following.
1-chloro-2, 4- dinitrobenzene
6-chloro-1, 3- dinitrobenzene
1-chloro-4, 6-dinitrobenzene
2-chloro-1, 5-dinitrobenzene
42.
Which techniqaes is based on the difference in the solubilities of the compound and the impurities in a suitable solvent?
Sublimation
Crystallisation
Distillation
None of these
43.
The fragrance of flowers is due to the presence of some steam volatile organic compounds called essential oils. These are generally insoluble in water at room temperature but are miscible with water vapour in vapour phase. Asuitable method for the extraction of these oils from the flowers is ______.
distillation
crystallisation
distillation under reduced pressure
steam distillation
44.
What is the technological applications of fractional distillation?
To separate different fractions of crude oil in petroleum industry
To separate different fractions of volatile and non-volatile solvents
To separate mixture of amino acids
No technological application of fractional distillation
45.
What is mass silicon in 100 g of sodium silicate, Na2SiO3? [Na = 23, Si = 28, O = 16u]
16.7%
23.0%
28.0%
82.0%
46.
One mole of oxygen gas at STP is equal to _________
6.022 x 1023 molecules of oxygen
6.022 x 1023 atoms of oxygen
16 g of oxygen
32 g of oxygen
47.
The general electronic configuration of d-block elements is ______.
\((n-1) d^{1 \text { to } 10} n s^{2}\)
\((n-1) d^{1-10} n s^{0-2}\)
\((n-1) d^{1 \text { to } 10} n s^{1-2}\)
\((n-1) d^{1-9} n s^{0-2}\)
48.
Which of the following statements related to the modern periodic table is incorrect?
The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in a p-shell.
The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.
Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
The block indicates value of azimuthal quantum number (l) for the last subshell that received electrons in building up the electronic configuration.
49.
Which of the following statements related to the modern periodic table is incorrect?
The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in a p-shell.
The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.
Each block contains a number of columns equal to the number of electrons that can occupy that subshell.
The block indicates value of azimuthal quantum number (l) for the last subshell that received electrons in building up the electronic configuration
50.
Anything that influences the valence electrons will affect the chemistry of the element. Which one of the following factors does not affect the valence shell?
Valence principal quantum number (n)
Nuclear charge (Z)
Nuclear mass
Number of core electrons
1.
(a)
6.02 x 1023atoms of C
2.
(a)
1 g atom of C
3.
(a)
3
4.
(c)
ns2 np2
5.
(c)
Sp2 - Sp3
6.
(b)
Fe4[Fe(CN)6]3
7.
(b)
\(\left( { CH }_{ 3 } \right) _{ 3 }\overset { + }{ C } \)
8.
(b)
nucleophilic substitution
9.
(c)
1, 1-dichloropropane
10.
(c)
2-ethylpropanal
11.
(d)
O-H
12.
(c)
sp2
13.
(a)
Dimethyl sulphide
14.
(c)
A compound retains the physical properties of its constituent elements
15.
(c)
3
16.
(a)
Total mass of iron and oxygen in reactants = total mass of iron and oxygen in product therefore it follows law of conservation of mass.
17.
(a)
CH
18.
(c)
C6H10O4
19.
(b)
27.27%
20.
(a)
2.5 m
21.
(b)
2.16 g
22.
(c)
Law of multiple proportions
23.
(c)
55.6 M
24.
(a)
Atomic weight
25.
(b)
Mendeleev's arranged elements in order of their increasing atomic number
26.
(c)
maximum principal quantum number of any element of the period
27.
(c)
Both (a) and (b)
28.
(a)
Period 4, group 6
29.
(c)
[Xe] 4f7 5d1 6s2
30.
(c)
\((n-1) d^{1-10} n s^{0-2}\)
31.
(c)
lanthanoids
32.
(c)
atomic orbitals
33.
(b)
p-block
34.
(c)
\(n s^{2} n p^{6}\)
35.
(b)
18, 7
36.
(c)
\((n-2) f^{1-14}(n-1) d^{0-1} n s^{2}\)
37.
(b)
Benzenoid aromatic compound
38.
(b)
3, 4-dimethylhexane
39.
(a)
40.
(a)
3-ethyl-1,1-dimethylcyclohexane
41.
(a)
1-chloro-2, 4- dinitrobenzene
42.
(b)
Crystallisation
43.
(d)
steam distillation
44.
(a)
To separate different fractions of crude oil in petroleum industry
45.
(d)
82.0%
46.
(a)
6.022 x 1023 molecules of oxygen
47.
(b)
\((n-1) d^{1-10} n s^{0-2}\)
48.
Statement (b) is incorrect.
The d-block has 10 columns because a maximum of 10 electrons can occupy all the orbitals in a d subshell.
49.
(b)
The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in a d-subshell.
50.
(c)
Nuclear mass
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