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Classification Of Elements And Periodicity In Properties Class 11 MCQs Questions with Answers
The electronic configuration of halogen is
(a) ns² np6
(b) ns² np3
(c) ns² np5
(d) ns²
Answer: (c) ns² np5
The element with atomic number 35 belongs to
(a) d – Block
(b) f – Block
(c) p – Block
(d) s – Block
Answer: (c) p – Block
The correct order of first ionization potential among following elements, Be, B, C, N and O is
(a) B < Be < C < O < N
(b) B < Be < C < N < O
(c) Be < B < C < N < O
(d) Be < B < C < O < N
Answer: (a) B < Be < C < O < N
On the Pauling’s electronegativity scale the element next to F is
(a) N
(b) Cl
(c) O
(d) Ne
Answer: (c) O
The group number, number of valence electrons, and valency of an element with the atomic number 15, respectively, are:
(a) 16, 5 and 2
(b) 15, 5 and 3
(c) 16, 6 and 3
(d) 15, 6 and 2
Answer: (b) 15, 5 and 3
In the long form of the periodic table, the valence shell electronic configuration of 5s²5p4 corresponds to the element present in:
(a) Group 16 and period 6
(b) Group 17 and period 6
(c) Group 16 and period 5
(d) Group 17 and period 5
Answer: (c) Group 16 and period 5
Which of the following oxides is amphoteric in character?
(a) SnO2
(b) CO2
(c) SiO2
(d) CaO
Answer: (a) SnO2
The electronic configuration of an element is 1s², 2s² 2p6, 3s² 3p³. What is the atomic number of the element which is just below the above element in the periodic table
(a) 31
(b) 34
(c) 33
(d) 49
Answer: (c) 33
The reduction in atomic size with increase in atomic number is a characteristic of elements of-
(a) d−block
(b) f−block
(c) Radioactive series
(d) High atomic masses
Answer: (b) f−block
Increasing order of electro negativity is
(a) Bi < P < S < Cl
(b) P < Bi < S < Cl
(c) S < Bi < P < Cl
(d) Cl < S < Bi < P
Answer: (a) Bi < P < S < Cl
In the periodic table, the element with atomic number 16 will be placed in the group
(a) Third
(b) Fourth
(c) Fifth
(d) Sixth
Answer: (d) Sixth
The chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is:
(a) Both are found together in nature
(b) Both have nearly the same size
(c) Both have similar electronic configuration
(d) The ratio of their charge and size (i.e. charge density) is nearly the same
Answer: (d) The ratio of their charge and size (i.e. charge density) is nearly the same
Correct order of ionization enthalpies is
(a) Zn < Cd < Hg
(b) Cd < Hg < Zn
(c) Na > Cs > Rb
(d) Cs < Rb < Na
Answer: (d) Cs < Rb < Na
Set containing isoelectronic species is
(a) C2−2, NO+, CN–, O2+2
(b) CO, NO, O2 CN–
(c) CO2, NO2, O2, N2O
(d) CO, CO2, NO, NO2
Answer: (a) C2−2, NO+, CN–, O2+2
The d-block elements consists mostly of
(a) Monovalent metals
(b) All non-metals
(c) Elements which generally form stoichiometric metal oxide
(d) Many metals with catalytic properties
Answer: (d) Many metals with catalytic properties
The values of electronegativity of atoms A and B are 1.20 and 4.0 respectively. The percentage of ionic character of A-B bond is
(a) 50%
(b) 72.24%
(c) 55.3%
(d) 43%
Answer: (b) 72.24%
Which of the following has the highest boiling point?
(a) Ne
(b) Xe
(c) Ar
(d) Kr
Answer: (b) Xe
Consider the isoelectronic series : K+, S2-, Cl1- and Ca2+, the radii of the ions decrease as
(a) Ca2+ < K+ > Cl–, S2-
(b) Cl– > S2- > K+ > Ca2+
(c) S2- > Cl– > K+ > Ca2+
(d) K+ > Ca2+ > S2- > Cl
Answer: (c) S2- > Cl– > K+ > Ca2+
The ions O2+, F–, Na+, Mg2+ and Al3+ are isoelectronic, their ionic radii show.
(a) a significant increase from O2- to Al3+
(b) an increase from O2- to F– and then decrease from Na+ to Al3+
(c) a significant decrease from O2- to Al3+
(d) a decrease from O2- to F– and then increase from Na+ to Al3+
Answer: (c) a significant decrease from O2- to Al3+
The element californium belongs to a family of :
(a) Alkali metal family
(b) Actinide series
(c) Alkaline earth family
(d) Lanthanide series
Answer: (b) Actinide series
The ionic radii of isoelectronic species N3-, O2- and F– in Å are in the order.
(a) 1.36, 1.40, 1.71
(b) 1.36, 1.71, 1.40
(c) 1.71, 1.40, 1.36
(d) 1.71, 1.36, 1.40
Answer: (c) 1.71, 1.40, 1.36
Pick out the isoelectronic structures from the following
(I) CH+3 (II) H3O+ (III) NH3 (IV) CH−3
(a) I and II
(b) III and IV
(c) I and III
(d) II, III and IV
Answer: (d) II, III and IV
The most electronegative element of the periodic table is
(a) Iodine
(b) Sulphur
(c) Oxygen
(d) Fluorine
Answer: (d) Fluorine
Which of the following represents most electropositive element?
(a) [He]2s1
(b) [He]2s²
(c) [Xe]6s1
(d) [Xe]6s²
Answer: (c) [Xe]6s1
Eka-alurninium and Eka-silicon are known as
(a) Gallian and germanium
(b) Aluminium and silicon
(c) Iron and sulphur
(d) Neutron and magnesium
Answer: (a) Gallian and germanium
An element with atomic number 106 has been discovereq recently. Which of the following electronic configuration will it have
(a) [Rn]5f146d47s²
(b) [Rn]5f146d57s1
(c) [Rn]5f14 6d67s0
(d) 5f146d7s²7p³
Answer: (a) [Rn]5f146d47s²
If the ionic radii of K+ and F– are about 1.34 Å each, then the expected values of atomic radii of K and F should be respectively
(a) 2.31 and.0.64 Å
(b) 2.31 and 1.34 Å
(c) 0.64 and 2.31 Å
(d) 1.34 and 1,34 Å
Answer: (a) 2.31 and.0.64 Å
Which pair of elements belongs to same group?
(a) Elements with atomic no. 17 and 38
(b) Elements with atomic no. 20 and 40
(c) Elements with atomic no. 17 and 53
(d) Elements with atomic no. 11 and 33
Answer: (c) Elements with atomic no. 17 and 53
The first ionisation energy for Li is 5.4 eV and electron affinity of Cl is 3.61 eV. The ∆H (in k] mol-1) for the reaction.
Li (g) + Cl (g) → Li+ (g) + Cl– (g) if the resultant ions do not combine with each other is [1eV = 1.6 × 10-19 J]
(a) 70
(b) 100
(c) 170
(d) 270
Answer: (c) 170
Element with atomic number 56 belongs to which block?
(a) s
(b) p
(c) d
(d) f
Answer: (a) s
The first ionisation energy will be maximum for
(a) Uranium
(b) Hydrogen
(c) Lithium
(d) Iron
Answer: (b) Hydrogen
Which of the following forms the most stable gaseous negative ion?
(a) F
(b) Cl
(c) Br
(d) I
Answer: (b) Cl
Which of the following elements are found in pitch blende?
(a) Actinium and protoactinium
(b) Neptunium and plutonium
(c) Actinium only
(d) Both (a) and (b)
Answer: (d) Both (a) and (b)
Which one of the following is the correct order of size?
(d) I > I– > I+
(b) I > I+ > I–
(c) I+ > I– > 1
(d) I– > I > I+
Answer: (d) I– > I > I+
The ionic radius of Cr is minimum in which of the following compounds?
(a) K2CrO4
(b) CrF3
(c) CrO2
(d) CrCl3
Answer: (a) K2CrO4
The general outer electronic configuration of transition elements is
(a) ns²nd1-10
(b) ns²np1(n – 1)d1-10
(c) ns²np6(n – 1)d1-10
(d) ns0-2 (n – 1)d1-10
Answer: (d) ns0-2 (n – 1)d1-10
According to the periodic law of elements the variation in properties of elements is related to their
(a) nuclear neutron-proton number ratio
(b) atomic masses
(c) nuclear masses
(d) atomic numbers
Answer: (d) atomic numbers
In the long form of the periodic table, the valence shell electronic configuration of 5s²5p4 corresponds to the element present in:
(a) Group 16 and period 6
(b) Group 17 and period 6
(c) Group 16 and period 5
(d) Group 17 and period 5
Answer: (c) Group 16 and period 5
The band length in LiF will be
(a) Less than that of NaF
(b) Equal to that of KF
(c) More than that of KF
(d) Equal to that of NaF
Answer: (a) Less than that of NaF
The correct order of electron affinities is
(a) 0 > S > Se
(b) 0 < S < Se
(c) 0 < Se < S
(d) S < Se < 0
Answer: (c) 0 < Se < S
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