Test: Periodic Properties- 2 - Chemistry MCQ

La³⁺ > Gd³⁺ > Eu³⁺ > Lu³⁺

V²⁺ > V³⁺ > V⁴⁺ > V⁵⁺

Tl⁺ > In⁺ > Sn²⁺ > Sb³⁺

K⁺ > Sc³⁺ > V⁵⁺ > Mn⁷⁺

It has maximum ionic character

It has minimum ionic character

It has associated molecules

It has least molecular weight

1 + 3 + 4

2 – 1 + 3

1 + 5

5 – 3

F > O > N > C

C > N > O > F

O > N > F > C

O > F > N > C

F^– > F > Cl^– > Cl

F > Cl > Cl^– > F^–

F^– > Cl^– > Cl > F

F^– > Cl^– > F > Cl

The second ionization energy of sulphur is greater than that of chlorine

The third ionization energy of phosphorus is greater than that of aluminium

The first ionization energy of aluminium is approximately the same as that of gallium

The second ionization energy of boron is greater than that of carbon.

Lead

Carbon

Silicon

Tin

The first ionization potential of Al is less than the first ionization potential of Mg

The second ionization potential of Mg is greater than the second ionization potential of Na

The first ionization potential of Na is less than the first ionization potential of Mg

The third ionization of potential Mg is greater than the third ionization potential of Al

786, 1012, 999, 1256

1012, 786, 999, 1256

786, 1012, 1256, 999

786, 999, 1012, 1256

Nitrogen

Phosphorus

Aluminium

Boron 

E₁ < E_2 ​

E₁ = E₂ 

E₁ > E_2 ​

E₁ ≥ E_2​

The second ionization energy of Se is greater than that of second ionization energy of As

The first ionizat ion energy of C²⁺ ion is greater than that of first ionizat ion energy of N²⁺ ion.

The third ionizat ion energy of F is greater than that of third ionization energy of O

Helogens have highest I.E. in respective period

Q: Alkaline earth metal

P: Alkali metals

R: s-block element

They belong to same period

| I.E. of process (II) | = | E.A. of process (I) |

| I.E. of process (III) | = | I.E. of process (II) |

| I.E. of process (IV) | = | E.A. of process (I) |

| I.E. of process (IV) | = | I.E. of process (III) |

O < S < F < Cl

O < S < Cl < F

S < O < F < Cl

S < O < Cl < F

–780, + 590

–590, + 780

+590, + 780

+780, +590

The magnitude of the second electron affinity of sulphur is greater than that of oxygen

The magnitude of the second electron affinity of sulphur is less than that of oxygen

The first electron affinities of bromine and iodine are approximately the same

The first electron affinit ies of fluorine is greater than that of chlorine

Greater is the nuclear charge, greater is the electron gain enthalpy

Nitrogen has almost zero electron gain enthalpy

Electron gain enthalpy decreases from fluorine to iodine in the group

Chlorine has highest electron gain enthalpy

O^– ion has comparat ively larger size than oxygen atom

Oxygen has high electron affinity

O^– ion will tend to resist the addition of another electron

Oxygen is more electronegative

Ca, Sr, Ba        

Cu, Au, Ag        

N,P, As        

Cl, Br, I

Cl > O > N > C

Cl > O > C > N  

Cl > N > C > O

Cl > C > O > N

Increasing size: Al³⁺ < Mg²⁺ < Na⁺ < F^–

Increasing I.E.₁: B < C < N < O

Increasing E.A₁: I < Br < F < Cl

Increasing metallic radius: Li < Na < K < Rb

Van der Waals radius of iodine is more than its covalent radius

All isoelectronic ions belong to same period of the periodic table

I.E₁ of N is higher than that of O while I.E₂ of O is higher than that of N

The electron affinity N is almost zero while that of P is 74.3 kJ mol^–1

ΔH₃ is more negative than ΔH₁ and ΔH₂

ΔH₁ is less negative than ΔH₂

ΔH₁, ΔH₂ and ΔH₃ are negative whereas ΔH₄ is positive

ΔH₁, and ΔH₃ are negative whereas ΔH₂ and ΔH₄ are positive

WZ does not conduct electricity in solid and fused state

YZ conducts electricity in fused as well as solution state

XZ conducts electricity only in solution state

WX conducts electricity only in fused state

Δ (E.N.) of M and O < Δ (E.N.) of O and H

Δ (E.N.) of M and O = Δ (E.N.) of O and H

Δ (E.N.) of M and O > Δ (E.N.) of O and H

Cannot be predicted according Δ (E.N.) data

Be (4)        

Ne (10)        

N(7)        

O (8)

3.16

0.0

 2.8

4.16

I alone

II alone

I and II

II and III

S^2– > Cl^– > K⁺ > Ca²⁺ (Ionization energy)

C < N < F < O (2^nd Ionization energy)

B > Al > Ga > In > Tl (Electronegativity)

Na⁺ > Li⁺ > Mg²⁺ > Be²⁺ > Al³⁺ (Ionicradius)