Chemical Periodicity Test

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Chemical Periodicity Test - 6

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Weekly Quiz Competition

Question 1
4 / -1

Which of the following doesn't decompose on heating

A
MgCO₃

B
Na₂CO₃

C
Li₂CO₃

D
Ca(HCO₃)₂

Solution

Sodium carbonate doesn't decompose on heating as it is stable to heat.
Question 2
4 / -1

Which one of the following ions has the highest value of ionic radius?

A
Li⁺

B
F⁻

C
B³⁺

D
O²⁻

Solution

O²⁻ has the highest value of ionic radius as this can be explained on the basis of whenZ/e ratio increases, the size decreases and when Z/e ratio decreases, the size increases.
Question 3
4 / -1

The unit representing atomic radii and ionic radii is

A
nm

B
cm

C
Å

D
m

Solution

Atomic radii are measured in terms of Angstrom (A^o)
Question 4
4 / -1

Arrange the elements in increasing order of atomic radius Na, Rb, K, Mg.

A
Na < K < Mg < Rb

B
K < Na < Mg < Rb

C
Mg < Na < K < Rb

D
Rb < K < Mg < Na

Solution

The increasing order of atomic radius is Mg<Na<K<Rb.

On moving down the group, the atomic radius increases. On moving from right to left in a period, the atomic radius decreases.
Question 5
4 / -1

Correct energy value order of

A
ns np nd (n−1)f

B
ns np (n−1)d (n−2)f

C
ns np (n−1)d (n−1)f

D
ns (n−1)d np (n−1)f

Solution

Energy order is followed by (n+l) rule:

l = 0 for s-orbital

l = 1 for p-orbital

l = 2 for d-orbital a

and l = 3 for f-orbital.

so correct order is ns (n−1)d np (n−1)f
Question 6
4 / -1

The ionization energy of nitrogen is more than that of oxygen because

A
Nitrogen has half filled p-orbitals

B
Nitrogen is left to the oxygen in the same period of the periodic table

C
Nitrogen contains less number of electrons

D
Nitrogen is less electronegative

Solution

The first ionization energy is the energy needed to remove the outermost, or highest energy, electron from a neutral atom in the gas phase. It is more for nitrogen than oxygen because nitrogen is more stable due to its half-filled electronic configuration.
Question 7
4 / -1

Which of the following element has the lowest ionization potential

A
Fe

B
H

C
Li

D
He

Solution

Li has lowest ionization potential because after losing an electron it will attain noble gas configuration.
Question 8
4 / -1

Ionisation energy in group 1A varies in the decreasing order as:

A
Li>Na>K>Cs

B
Na>Li>K>Cs

C
Li>Cs>K>Na

D
K>Cs>Na>Li

Solution

Atomic size increases as we move from top to down in a group, therefore, the amount of energy required for ejection of an electron from atom decreases, i.e. ionisation energy decreases. Hence, the correct order of IE₁ is Li>Na>K>Cs.
Question 9
4 / -1

Which one of the following sets of ions represent a collection of isoelectronic species?

A
K⁺,Cl⁻,Ca²⁺,Sc³⁺

B
Ba²⁺,Sr²⁺,K⁺,Ca²⁺

C
N³⁻,O²⁻,F⁻,S²⁻

D
Li⁺,Na⁺,Mg²⁺,Ca²⁺

Solution

Isoelectronic species are those which have same number of electrons.

K⁺,Cl⁻,Ca²⁺ and Sc³⁺ are isoelectronic species because each possesses 18 electrons.
Question 10
4 / -1

The electron affinity values (kJmol⁻¹) of three halogens X, Y and Z respectively are −349, −333 and −325. Then X, Y and Z respectively are :

A
F₂, Cl₂ and Br₂

B
Cl₂, F₂ and Br₂

C
Cl₂, Br₂ and F₂

D
Br₂, Cl₂ and F₂

Solution

Order of EA of halogens is Cl>F>Br.

Hence, the value of EA will be that of Cl₂, F₂, Br₂ respectively.

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Chemical Periodicity Test - 6

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Chemical Periodicity Test - 6

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Question 1

MgCO3​

Na2​CO3​

Li2​CO3​

Ca(HCO3​)2​

Solution

Question 2

Li+

F−

B3+

O2−

Solution

Question 3

nm

cm

Å

m

Solution

Question 4

Na < K < Mg < Rb

K < Na < Mg < Rb

Mg < Na < K < Rb

Rb < K < Mg < Na

Solution

Question 5

ns np nd (n−1)f

ns np (n−1)d (n−2)f

ns np (n−1)d (n−1)f

ns (n−1)d np (n−1)f

Solution

Question 6

Nitrogen has half filled p-orbitals

Nitrogen is left to the oxygen in the same period of the periodic table

Nitrogen contains less number of electrons

Nitrogen is less electronegative

Solution

Question 7

Fe

H

Li

He

Solution

Question 8

Li>Na>K>Cs

Na>Li>K>Cs

Li>Cs>K>Na

K>Cs>Na>Li

Solution

Question 9

K+,Cl−,Ca2+,Sc3+

Ba2+,Sr2+,K+,Ca2+

N3−,O2−,F−,S2−

Li+,Na+,Mg2+,Ca2+

Solution

Question 10

F2​, Cl2​ and Br2​

Cl2​, F2​ and Br2​

Cl2​, Br2​ and F2​

Br2​, Cl2​ and F2​

Solution

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MgCO₃

Na₂CO₃

Li₂CO₃

Ca(HCO₃)₂

Li⁺

F⁻

B³⁺

O²⁻

K⁺,Cl⁻,Ca²⁺,Sc³⁺

Ba²⁺,Sr²⁺,K⁺,Ca²⁺

N³⁻,O²⁻,F⁻,S²⁻

Li⁺,Na⁺,Mg²⁺,Ca²⁺

F₂, Cl₂ and Br₂

Cl₂, F₂ and Br₂

Cl₂, Br₂ and F₂

Br₂, Cl₂ and F₂