The correct order for electron affinity of halogens is :
1. Br > F
2. F > Cl
3. Br > Cl
4. F > I
Element/Ion that has the highest electron affinity is :
1. | F- | 2. | O- |
3. | O | 4. | Na |
Values of electronegativity like 3.0, 2.8, 2.5 are related to :-
(1) Elements having low IP in the periodic table
(2) Elements having high EA in the periodic table
(3) Chalcogens
(4) None of the above
The pair of which addition of 2nd electron in both the atoms are endothermic :-
(1) N, Ne
(2) Be, F
(3) B, C
(4) All of the above
The incorrect match among the following is:
1. B < C < N < O (increasing first ionisation enthalpy)
2. I < Br < F < Cl (increasing electron gain enthalpy)
3. Li < Na < K < Rb (increasing metallic radius)
4. Al3+ < Mg2+ < Na+ <F- (increasing ionic size)
Which one of the following orders is correct for the bond dissociation enthalpy of halogen molecules?
1. Cl2 > Br2 > F2 > I2
2. Br2 > I2 > F2 > Cl2
3. F2 > Cl2 > Br2 > I2
4. I2 > Br2 > Cl2 > F2
The formation of the oxide ion O2-(g), from oxygen atom requires first an exothermic and
then an endothermic step as shown below,
Thus, process of formation of O2- in gas phase is unfavourable even though O2- is
isoelectronic with neon. It is due to the fact that
1. electron repulsion outweighs the stability gained by achieving noble gas configuration
2. O- ion has comparatively smaller size than oxygen atom
3. Oxygen is more electronegative
4. addition of electron in oxygen result in large size of the ion
The correct order of increasing electron gain enthalpy with a negative sign for the elements O, S, F, and Cl is :
1. Cl < F < S < O
2. O < S < F < Cl
3. F < S < O < Cl
4. S < O < Cl < F
Which of the following transformation least energy is required?
(1)
(2)
(3)
(4)
Which of the following represents correct order of electron affinity?
(1) Cl>F>S>O
(2) F>O>S>Cl
(3) F>Cl>S>O
(4) Cl>S>O>F