Periodic Properties of Elements Test

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Periodic Properties of Elements Test - 2

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Weekly Quiz Competition

Question 1
1 / -0

Arrange S, P and As in order of increasing ionisation energy.

A
S < P < As

B
P < S < As

C
As < S < P

D
As < P < S

Solution

P and As belongs to the same group i.e. 15, whereas S belongs to group 16. Also S and P belong to the same period . As P has exactly half filled orbitals, therefore, As < S < P.
Question 2
1 / -0

What is the correct order of the size of the species?

A
Cl > Cl⁺ > Cl^-

B
Cl⁺ > Cl^-> Cl

C
Cl^-> Cl⁺ > Cl

D
Cl^-> Cl > Cl ⁺

Solution

Size of anion is larger and cation is smaller than the neutral atom.
Question 3
1 / -0

Which of the following is the correct order of increasing ionic radii?

A
K⁺, Ca²⁺, S^2-

B
Be²⁺, Mg²⁺, Na⁺

C
O^2-, F ^-, N^3-

D
S^2-, O^2-, As^3-

Solution

This is the correct order. Be²⁺is from period 2, so its size is smaller. Also, Na⁺is from group 1, so it is larger in size.
Question 4
1 / -0

The electronic configuration of elements of group 18 is represented by :

A
ns²

B
ns² np⁵

C
ns² np⁶

D
(n-1)d⁸ n²

Solution

Completely filled s and p orbitals is the representation of group 18 , noble gases.
Question 5
1 / -0

General configuration of elements of group 9 of transition metals belonging to d block is

A
(n-1)d⁶ ns²

B
nd⁷ ns²

C
(n-1)d²ns²np⁶

D
(n-1)d⁷ns²

Solution

This represents the group 9 as 7 + 2= 9.
Question 6
1 / -0

In transition elements, the incoming electron occupies (1-n)d subshell in preference to

A
np level

B
ns level

C
(n-1)p level

D
(n-1)s level

Solution

The filling of the orbitals is in the order: ns, (n-1)d, np, so (n-1)d orbitals are filled before np orbital in transition elements.
Question 7
1 / -0

Which of the following configurations represents the most electropositive element?

A
[He] 2s¹

B
[Xe] 6s¹

C
[He] 2s²

D
[Xe] 2s²

Solution

Single electron of s orbital is easily removed, also it has 6 shells, so there is sheilding effect due to which the electron is easily removed.
Question 8
1 / -0

What information about the chemical nature of the element is given by the configuration 1s² 2s² 2p⁶ 3s²?

A
It is a metal

B
It is a non metal

C
It is a transition metal

D
It is a noble gas

Solution

It is an alkaline earth metal belonging to group 2 and period 3.
Question 9
1 / -0

Which of the following ions does not have the configuration of argon?

A
Cl^-

B
K⁺

C
Ca²⁺

D
I^-

Solution

After addition of an electron, the configuration of iodine becomes equal to that of xenon.
Question 10
1 / -0

The general electronic configuration of transition elements is

A
(n-1) d ^1-10 . ns^0-2

B
(n-1) d ^1-10 . ns¹

C
(n-1) d ^1-10 . ns^1-2

D
(n-1) d ^1-10 . ns² . np⁶

Solution

The electrons may occupy d block of penultimate shell or the s block or ultimate shell.
Question 11
1 / -0

The anion O^2- is isoelectric with

A
F⁺

B
N^2-

C
F^-

D
N³⁺

Solution

It is isoelectric with O^2-

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Periodic Properties of Elements Test - 2

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Periodic Properties of Elements Test - 2

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Question 1

S < P < As

P < S < As

As < S < P

As < P < S

Solution

Question 2

Cl > Cl+ > Cl -

Cl+ > Cl - > Cl

Cl - > Cl+ > Cl

Cl - > Cl > Cl +

Solution

Question 3

K+, Ca2+, S2-

Be2+, Mg2+, Na+

O2-, F -, N3-

S2-, O2-, As3-

Solution

Question 4

ns2

ns2 np5

ns2 np6

(n-1)d8 n2

Solution

Question 5

(n-1)d6 ns2

nd7 ns2

(n-1)d2 ns2 np6

(n-1)d7 ns2

Solution

Question 6

np level

ns level

(n-1)p level

(n-1)s level

Solution

Question 7

[He] 2s1

[Xe] 6s1

[He] 2s2

[Xe] 2s2

Solution

Question 8

It is a metal

It is a non metal

It is a transition metal

It is a noble gas

Solution

Question 9

Cl-

K+

Ca2+

I-

Solution

Question 10

(n-1) d 1-10 . ns0-2

(n-1) d 1-10 . ns1

(n-1) d 1-10 . ns1-2

(n-1) d 1-10 . ns2 . np6

Solution

Question 11

F+

N2-

F-

N3+

Solution

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Question Analysis

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Cl > Cl⁺ > Cl^-

Cl⁺ > Cl^-> Cl

Cl^-> Cl⁺ > Cl

Cl^-> Cl > Cl ⁺

K⁺, Ca²⁺, S^2-

Be²⁺, Mg²⁺, Na⁺

O^2-, F ^-, N^3-

S^2-, O^2-, As^3-

ns²

ns² np⁵

ns² np⁶

(n-1)d⁸ n²

(n-1)d⁶ ns²

nd⁷ ns²

(n-1)d²ns²np⁶

(n-1)d⁷ns²

[He] 2s¹

[Xe] 6s¹

[He] 2s²

[Xe] 2s²

Cl^-

K⁺

Ca²⁺

I^-

(n-1) d ^1-10 . ns^0-2

(n-1) d ^1-10 . ns¹

(n-1) d ^1-10 . ns^1-2

(n-1) d ^1-10 . ns² . np⁶

F⁺

N^2-

F^-

N³⁺