Consider the isoelectronic species, Na+, Mg2+, F-, and O2-. The correct order of increasing length of their radii is

1. F-<O2-<Mg2+<Na+

2. Mg2+<Na+<F-<O2-

3. O2-<F-<Na+<Mg2+

4. O2-<F-<Mg2+<Na+

Subtopic:  Atomic Size |
 88%
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Among the following elements, the one that is not an actinoid is:

1. Curium (Z=96) 2. Californium (Z=98)
3. Uranium (Z=92) 4. Terbium (Z=65)
Subtopic:  Modern Periodic Table & Periodicity |
 85%
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The order of screening effect of electrons of s, p, d and f orbitals of a given shell of an atom on electrons in its outer shell is :

1. s > p > d > f

2. f > d > p > s

3. p < d < f < s

4. f > p > s > d

Subtopic:  Screening Effect |
 93%
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The first ionisation enthalpies of Na, Mg, Al, and Si are in the order of-

1. Na < Al < Mg < Si

2. Na > Mg > Al > Si

3. Na < Mg < Al < Si

4. Na > Mg > Al < Si

Subtopic:  Ionization Energy (IE) |
 66%
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Among halogens, the correct order of amount of energy released in electron gain (electron gain enthalpy) is-

1. F > Cl > Br > I 2. F < Cl < Br < I
3. F < Cl > Br > I 4. F < Cl < Br < I
Subtopic:  Electron Affinity (EA) |
 82%
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The period number in the long form of the periodic table is equal to : 

1. Magnetic quantum number of any element of the period.
2. Atomic number of any element of the period.
3. Maximum principal quantum number of any element of the period.
4. Maximum azimuthal quantum number of any element of the period.

Subtopic:  Modern Periodic Table & Periodicity |
 79%
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The elements in which electrons are progressively filled in 4f-orbitals are called:

1. Actinoids 2. Transition elements
3. Lanthanoids 4. Halogens
Subtopic:  Modern Periodic Table & Periodicity |
 77%
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The correct order of size of the given species is: 

1.  I > I> I+

2.  I> I> I

3.  I > I> I-

4.  I> I > I+

Subtopic:  Atomic Size |
 94%
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The formation of oxide ion O2-(g), from oxygen atom, requires first an exothermic and then an endothermic step as shown below

O(g)+e-O-(g); H=-141 kJ mol-1
O-(g)+e-O2(g); H=+780 kJ mol-1

Thus, the process of formation of O2- in the gas phase is unfavourable even though O2- is isoelectronic with neon. It is due to the fact that

1. Oxygen is more electronegative
2. Addition of electron in oxygen results in a larger size of the ion
3. Electron repulsion outweighs the stability gained by achieving noble gas configuration
4. O- ion has comparatively smaller size than oxygen atom

Subtopic:  Electron Affinity (EA) |
 84%
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The outermost electronic configuration of the last element of the p-block in the 6th period is represented by:

1. 7s27p6

2. 5f146d107s27p0

3. 4f145d106s26p6

4. 4f145d106s26p4

Subtopic:  Modern Periodic Table & Periodicity |
 77%
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