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Periodic properties - JEE MCQ


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20 Questions MCQ Test - Periodic properties

Periodic properties for JEE 2024 is part of JEE preparation. The Periodic properties questions and answers have been prepared according to the JEE exam syllabus.The Periodic properties MCQs are made for JEE 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises, MCQs and online tests for Periodic properties below.
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Periodic properties - Question 1

The increasing order of the atomic radius of is

Detailed Solution for Periodic properties - Question 1
As we move from left to right in a period, effective nuclear charge increases. Due to this atomic radius decreases. Thus, correct order of atomic radii of period elements is
Periodic properties - Question 2

Which is not the correct order for the stated property.

Detailed Solution for Periodic properties - Question 2

On moving along the period, ionization enthalpy increases. In second period, the order of ionization enthalpy should be as follows:
F > O > N
But N has half-filled structure, therefore, it is more stable than O. That is why its ionization enthalpy is higher than O. Thus, the correct order of IE is
F > N > O

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Periodic properties - Question 3

The electronic configuration which is associated with highest first ionisation enthalpy is:

Detailed Solution for Periodic properties - Question 3
Half-filled or completely filled orbitals attain extra stability due to symmetrical distribution of electrons and high exchange energy.
Periodic properties - Question 4

Identify the correct order of the size of the following:

Detailed Solution for Periodic properties - Question 4

For isoelectronic species, size of anion increases as negative charge increases whereas size of cation decreases with increase in positive charge. Further ionic radii of anions is more than that of cations. Thus the correct order is 

Periodic properties - Question 5

atoms of are converted into X+(g) by energy atoms of are converted into by energy . , then ionization potential and electron affinity of  respectively are

Detailed Solution for Periodic properties - Question 5


for atoms
atoms of have been ionized, by energy
Thus, ionization energy per atom

for atoms
Thus, electron affinity of is per atom.

Periodic properties - Question 6
Which of the following elements represents highly electropositive as well as highly electronegative character in its period?
Detailed Solution for Periodic properties - Question 6
First period has and He only out of which He is inert, hence, H behaves as a highly electropositive as well as electronegative.
Periodic properties - Question 7

Match Column-I with Column-II and select the correct answer by the given codes.

Detailed Solution for Periodic properties - Question 7

Helium (He) → Highest ionisation energy due to noble gas in nature.
Fluorine (F) High electronegativity in nature due to small size and -1 oxidation state.
Rubidium (Rb) → Most electropositive element due to large atomic size.
Lithium (Li) → Strongest reducing agent due to small size and positive oxidation state (+1)

Periodic properties - Question 8
and are isoelectronic. The order of their ionic size is
Detailed Solution for Periodic properties - Question 8
Among the isoelectronic species, the cation having more positive charge would be the smaller in size.
Periodic properties - Question 9

The set of three elements having successive atomic numbers and having the ionization energies of 2372, 520 and per mol is

Detailed Solution for Periodic properties - Question 9

He (Z = 2) is a noble gas and has highest I.E. The I.E. of Be(Z = 4) is more than that of Li(Z = 3)

Periodic properties - Question 10

In a given energy level, the order of penetration effect of different orbitals is

Detailed Solution for Periodic properties - Question 10

Penetration effect order is s > p > d > f.

Periodic properties - Question 11

What is the order of ionisation energies of the coinage metal

Detailed Solution for Periodic properties - Question 11


In all the above given cases, unpaired -electron has to be removed. In the case of , a electron is to be removed which is closer to the nucleus than the electron of .
So, of of Ag.
However, in case of Au, due to imperfect screening effect of of orbitals, the nuclear charge increases and therefore 5s of is more tightly held. Thus, the order of IE1 is Cu > Ag < Au.

Periodic properties - Question 12
What is the correct order of electronegativity?
Detailed Solution for Periodic properties - Question 12
Higher the positive charge the greater is the EN and higher the negative charge the lesser is the EN. So, EN order is
Periodic properties - Question 13
In which of the following process highest energy is absorbed?
Detailed Solution for Periodic properties - Question 13
has completely filled -orbital, so highest energy is absorbed when it converts to ion.
Periodic properties - Question 14
In lanthanides, with increase in atomic number atomic radius decreases, except for the element . What is ?
Detailed Solution for Periodic properties - Question 14
Lanthanides show decrease in atomic radius with increase in atomic number since electrons are filled in the -subshell. Since, the -subshell after poor shielding, the atomic size will decrease as the nuclear charge increases.
Eu electronic configuration is with half-filled outermost shell so nuclear pull is less and it does not show lanthanide contraction.
Periodic properties - Question 15
Which of the following processes requires maximum energy
Detailed Solution for Periodic properties - Question 15
has stable electronic configuration (1s2,2s22p6). If remove extra electrone that is present in inner shell, so need more energy to remove it.(insufficient amount of energy)
Periodic properties - Question 16

The electronic contigurations of four elements are given below. Arrange these elements in the correct order of magnitude of their electron affinity
(i)
(ii)
(iii)
(iv)
Select the correct answer using the codes

Detailed Solution for Periodic properties - Question 16

Electron affinity increases with the decrease in the size and it also depends on the electronic configuration

Periodic properties - Question 17
What was the main drawback of Mendeleev's periodic table?
Detailed Solution for Periodic properties - Question 17

Mendeleev's arranged all the known elements in increasing order of their atomic masses and gave the periodic law.

According to Mendeleev's Periodic law, The physical and chemical properties of the elements are the periodic function of their atomic masses.

Mendeleev designed a periodic table and arranged all the elements in increasing order of their atomic masses but not included the isotpes. As isotopes also have the different atomic masses. It is the major limitation of the Mendeleev's periodic table.

Periodic properties - Question 18

Higher second ionisation enthalpies than expected are observed for

Detailed Solution for Periodic properties - Question 18

The electronic configuration of is and that of is . Their second ionisation enthalpies are higher than expected because after removal of one electron chromium gets a half-filled electronic configuration and get a fully-filled electronic configuration. These configuration are more stable than the partial-filled electronic configuration. So, it is very difficult to remove the second electron in both cases.
Thus, option (d) is correct.

Periodic properties - Question 19

In second period of the long form of the periodic table, an element X has second lowest first ionization enthalpy and element Y has second highest first ionization enthalpy values. What are X and Y ?

Detailed Solution for Periodic properties - Question 19

The order of ionization enthalpy of elements of 2nd period in long form of periodic table is Li < B < Be < C < O < N < F < Ne.
Generally, on going left to right in a period, ionization energy increases, but there are some exceptions to this. For example, Be has more ionization energy than B, due to fulfilled s-orbital. And N has more ionization energy than O due to half filled p-subshell.
So,In second period of the long form of the periodic table, the element B has second lowest first ionization enthalpy and element F has second highest first ionization enthalpy values.

Periodic properties - Question 20

Which among the following elements of 3nd period shows maximum tendency of forming dπ − pπ bond ?

Detailed Solution for Periodic properties - Question 20

Among the given elements Cl has maximum tendency of dπ − pπ bonding On moving across period, nuclear charge increases and more s, p-electrons are added. Due to incomplete shielding of nuclear charge, the atomic size and so the size of 3 d-orbitals
decreaxes from Si < P < S < Cl
Decrease in size of 3 d-orbitals leads to stronger dπ−pπ overlap.

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