Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 10

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Weekly Quiz Competition

Question 1
1 / -0

The elements in which electrons are progressively filled in 4f-orbital are called

A
Actinoids

B
Transition elements

C
Lanthanoids

D
Halogens

Solution

The sixth period (n = 6) contains 32 elements and successive electrons enter 6s, 4f, 5d and 6p orbitals, in the order of filling up of the 4f orbitals begins with cerium (Z = 58) and ends at lutetium (Z = 71) to give the 4f-inner transition series which is called the lanthanoid series.
Question 2
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Which of the following statements are correct?

(i) Helium has the highest first ionisation enthalpy in the periodic table.

(ii) Chlorine has less negative electron gain enthalpy than fluorine.

(iii) Mercury and bromine are liquids at room temperature.

(iv) In any period, atomic radius of alkali metal is the highest.

A
(i),(ii),(iii)

B
(i),(ii),(iv)

C
(i),(iii),(iv)

D
(ii),(iii),(iv)

Solution

Helium being the smallest noble gas has the highest ionisation enthalpy.
Question 3
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Which of the following is the correct order of size of the given species:

A
\( I > I^-> I^+\)

B
\(I^+> I^-> I\)

C

\(I > I^+> I^- \)

D

\(I^-> I > I^+ \)

Solution

A cation is smaller than its parent atom because it has fewer electrons while its nuclear charge remains the same. The size of an anion will be larger than that of the parent atom because the addition of one or more electrons would result in increased repulsion among the electrons and a decrease in effective nuclear charge.
Question 4
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Which of the following sets contain only isoelectronic ions?

(i) \(Zn ^{2+},\, Ca ^{2+},\, Ga ^{3+},\, Al ^{3+}\)

(ii) \(K^ +,\, Ca ^{2+},\, Sc ^{3+},\, Cl^- \)

(iii) \(P ^{3-},\, S ^{2-},\, Cl ^-,\, K ^+\)

(iv) \(Ti ^{4+},\, Ar,\, Cr ^{3+} ,\, V ^{5+}\)

A
(i),(ii)

B
(ii),(iii)

C
(iii),(iv)

D
(i),(iv)

Solution

When we find some atoms and ions which contain the same number of electrons, we call them isoelectronic species. For example, \(O ^{2-}\), \(F ^-\), \(Na ^+\) and \(Mg ^{2+}\) have the same number of electrons (10).
Question 5
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In which of the following options order of arrangement does not agree with the variation of property indicated against it?

(i) \(Al ^{3+}\) < \(Mg ^{2+}\) < \(Na ^+\) < \(F ^-\) (increasing ionic size)

(ii) B < C < N < O (increasing first ionisation enthalpy)

(iii) I < Br < Cl < F (increasing electron gain enthalpy)

(iv) Li < Na < K < Rb (increasing metallic radius)

A
(i),(iv)

B
(iii),(iv)

C
(ii),(iii)

D
(i),(ii)

Solution

The ionisation enthalpy of N is higher than that of O due to greater stability of half-filled electronic configuration.

Again in option (iii), the electron gain enthalpy of F is lower than that of Cl due to small size of F.
Question 6
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Which of the following have no unit?

(i) Electronegativity

(ii) Electron gain enthalpy

(iii) Ionisation enthalpy

(iv) Metallic character

A
(i),(ii)

B
(ii),(iii)

C
(iii),(iv)

D
(i),(iv)

Solution

A qualitative measure of the ability of an atom in a chemical compound to attract shared electrons to itself is called electronegativity. Unlike ionization enthalpy and electron gain enthalpy, it is not a measureable quantity.
Question 7
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In the following questions a statement of Assertion (A) followed by a statement of reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): Boron has a smaller first ionisation enthalpy than beryllium.

Reason (R): The penetration of a 2s electron to the nucleus is more than the 2p electron hence 2p electron is more shielded by the inner core of electrons than the 2s electrons.

A
Assertion and reason both are correct statements but reason is not correct explanation for assertion

B
Assertion is correct statement but reason is wrong statement

C
Assertion and reason both are correct statements and reason is correct explanation for assertion

D
Assertion and reason both are wrong statements

Solution

In beryllium, the electron removed during the ionization is an s-electron whereas the electron removed during ionization of boron is a p-electron. The penetration of a 2s-electron to the nucleus is more than that of a 2p-electron; hence the 2p electron of boron is more shielded from the nucleus by the inner core of electrons than the 2s electrons of beryllium. Therefore, it is easier to remove the 2p-electron from boron compared to the removal of a 2s-electron from beryllium. Thus, boron has a smaller first ionization enthalpy than beryllium.

Question 8

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Electronic configuration of some elements is given in Column I and their electron gain enthalpies are given in Column II. Match the electronic configuration with electron gain enthalpy.

Column (I)	Column (II)
(i) \(1s^2\,2s^2\,sp^6\)	(a) -53
(ii) \(1s^2\,2s^2\,2p^6\, 3s^1\)	(b) -328
(iii) \(1s^2\,2s^2\,2p^5\)	(c) -141
(iv) \(1s^2\,2s^2\,2p^4\)	(d) +48

(i) → (c) (ii) → (b) (iii) → (a) (iv) → (d)

(i) → (d) (ii) → (a) (iii) → (c) (iv) → (b)

(i) → (d) (ii) → (c) (iii) → (b) (iv) → (a)

(i) → (d) (ii) → (a) (iii) → (b) (iv) → (c)

Question 9
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The formation of the oxide ion, \(O^{2- }\)(g), from oxygen atom requires first an exothermic and then an endothermic step as shown below:

O (g) + \(e^-\) → \(O^-\) (g) ; \(\Delta H^{\ominus}\) = -141 kJ \(mol^{-1}\)

\(O^-\)(g) + \(e^-\) → \(O^{2- }\)(g); \(\Delta H^{\ominus}\) = +780 kJ \(mol^{-1}\)

Thus process of formation of \(O^{2- }\) in gas phase is unfavourable even though \(O^{2- }\) is isoelectronic with neon. It is due to the fact that,

A
Oxygen is more electronegative

B
Addition of electron in oxygen results in larger size of the ion

C
Electron repulsion outweighs the stability gained by achieving noble gas configuration

D
\(O^-\) ion has comparatively smaller size than oxygen atom

Solution

When an electron is added to O atom to form \(O^-\) ion, energy is released. Thus, the first electron gain enthalpy of O is negative. On the other hand, when an electron is added to \(O^-\) ion to form \(O^{2- }\) ion, energy has to be given out in order to overcome the strong electronic repulsions. Thus the second electron gain enthalpy of O is positive.
Question 10
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In the following questions a statement of Assertion (A) followed by a statement of reason (R) is given. Choose the correct option out of the choices given below each question.

Assertion (A): Electron gain enthalpy becomes less negative as we go down a group.

Reason (R): Size of the atom increases on going down the group and the added electron would be farther from the nucleus.

A
Assertion and reason both are correct statements but reason is not correct explanation for assertion

B
Assertion and reason both are correct statements and reason is correct explanation for assertion

C
Assertion and reason both are wrong statements

D
Assertion is wrong statement but reason is correct statement

Solution

The electron gain enthalpy decreases from top to bottom in a group.
Question 11
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Ionic radii vary in

(i) inverse proportion to the effective nuclear charge.

(ii) inverse proportion to the square of effective nuclear charge.

(iii) direct proportion to the screening effect.

(iv) direct proportion to the square of screening effect.

A
(i),(ii)

B
(i),(iii)

C
(ii),(iii)

D
(ii),(iv)

Solution

The cation with the greater positive charge will have a smaller radius because of the greater attraction of the electrons to the nucleus. Anion with the greater negative charge will have the larger radius. In this case, the net repulsion of the electrons will outweigh the nuclear charge and the ion will expand in size so the ionic radii vary in inverse proportion to the effective nuclear charge and direct proportion to the screening effect.
Question 12
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An element belongs to \(3 ^{rd}\) period and group-13 of the periodic table. Which of the following properties will be shown by the element?

(i) Good conductor of electricity

(ii) Liquid, metallic

(iii) Solid, metallic

(iv) Solid, non metallic

A
(ii),(iv)

B
(ii),(iii)

C
(i),(iii)

D
(i),(iv)

Solution

Group-13 third period element is Aluminum which is a metal. It is solid, metallic and a good conductor of electricity.
Question 13
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Electronic configurations of four elements A, B, C and D are given below :

(A) \(1s ^2\, 2s ^2\, 2p ^6\)

(B) \(1s ^2\, 2s ^2\, 2p ^4\)

(C) \(1s ^2\, 2s ^2\, 2p ^6\,3s^1\)

(D) \(1s ^2\, 2s ^2\, 2p ^5\)

Which of the following is the correct order of increasing tendency to gain electron:

A
A < C < B < D

B
A < B < C < D

C
D < B < C < A

D
D < A < B < C

Solution

Electron Gain Enthalpy: The electron gain enthalpy is the molar enthalpy \((\Delta_{eg} H)\) change when an isolated gaseous atom or ion in its ground state adds an electron to form the corresponding anion.
Question 14
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For the second period elements the correct increasing order of first ionisation enthalpy is

A
Li < B < Be < C < O < N < F < Ne

B
Li < B < Be < C < N < O < F < Ne

C
Li < Be < B < C < O < N < F < Ne

D
Li < Be < B < C < N < O < F < Ne

Solution

‘Be’ and ‘N’ have comparatively more stable valence sub-shell than ‘B’ and ‘O’.

\(\therefore\) Correct order of first ionisation enthalpy is:

Li < B < Be < C < O < N < F < Ne
Question 15
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The element Z = 114 has been discovered recently. It will belong to which of the following family/group and electronic configuration?

A
\(Nitrogen\, family,[Rn]\ 5f^{14}6d^{10}7s^2 7p^6\)

B
\(Halogen\, family, [Rn]\ 5f^{14} 6d^{10} 7s^2 7p^5\)

C
\(Carbon\, family, [Rn]\ 5f^{14} 6d^{10} 7s^2 7p^2\)

D
\(Oxygen\, family, [Rn]\ 5f^{14} 6d^{10} 7s^2 7p^4\)

Solution

Z = 114

\(Z_{114}= [Rn]\, 5f^{14} 6d^{10} 7s^2 7p^2\)

valence configuration is \(ns^2 np^2\, so\, Z_{114}\) belong to carbon family.

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Classification of Elements and Periodicity in Properties Test - 10

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Question 1

Actinoids

Transition elements

Lanthanoids

Halogens

Solution

Question 2

(i),(ii),(iii)

(i),(ii),(iv)

(i),(iii),(iv)

(ii),(iii),(iv)

Solution

Question 3

\( I > I^-> I^+\)

\(I^+> I^-> I\)

\(I > I^+> I^- \)

\(I^-> I > I^+ \)

Solution

Question 4

(i),(ii)

(ii),(iii)

(iii),(iv)

(i),(iv)

Solution

Question 5

(i),(iv)

(iii),(iv)

(ii),(iii)

(i),(ii)

Solution

Question 6

(i),(ii)

(ii),(iii)

(iii),(iv)

(i),(iv)

Solution

Question 7

Assertion and reason both are correct statements but reason is not correct explanation for assertion

Assertion is correct statement but reason is wrong statement

Assertion and reason both are correct statements and reason is correct explanation for assertion

Assertion and reason both are wrong statements

Solution

Question 8

(i) → (c) (ii) → (b) (iii) → (a) (iv) → (d)

(i) → (d) (ii) → (a) (iii) → (c) (iv) → (b)

(i) → (d) (ii) → (c) (iii) → (b) (iv) → (a)

(i) → (d) (ii) → (a) (iii) → (b) (iv) → (c)

Question 9

Oxygen is more electronegative

Addition of electron in oxygen results in larger size of the ion

Electron repulsion outweighs the stability gained by achieving noble gas configuration

\(O^-\) ion has comparatively smaller size than oxygen atom

Solution

Question 10

Assertion and reason both are correct statements but reason is not correct explanation for assertion

Assertion and reason both are correct statements and reason is correct explanation for assertion

Assertion and reason both are wrong statements

Assertion is wrong statement but reason is correct statement

Solution

Question 11

(i),(ii)

(i),(iii)

(ii),(iii)

(ii),(iv)

Solution

Question 12

(ii),(iv)

(ii),(iii)

(i),(iii)

(i),(iv)

Solution

Question 13