Magnesium reacts with an element (X) to form an ionic compound.
If the ground state electronic configuration of (X) is ,
the simplest formula for this compound is:
1.
2.
3.
4.
1. | B < C < N < O (increasing first ionisation enthalpy) |
2. | I < Br < F < Cl (increasing negative electron gain enthalpy) |
3. | Li < Na < K < Rb (increasing metallic radius) |
4. | Al3+ < Mg2+ < Na+ <F- (increasing ionic size) |
The formation of the oxide ion O2- (g), from the oxygen atom requires first an exothermic and then an endothermic step as shown below,
Thus, the process of formation of O2- in the gas phase is unfavorable 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 a comparatively smaller size than the oxygen atom. |
3. | Oxygen is more electronegative. |
4. | Addition of electrons in oxygen results in a large size of the ion. |
The species Ar, K+ and Ca2+ contain the same number of electrons. In which order do their radii increase?
1. Ar < K+ < Ca2+
2. Ca2+ < Ar < K+
3. Ca2+ < K+ < Ar
4. K+ < Ar < Ca2+
The correct order of ionic radii is:
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2.
3.
4.
Be2+ is isoelectronic with which of the following ions?
1.
2.
3.
4.
The correct order of the decreasing ionic radii among the following isoelectronic species is:
1.
2.
3.
4.
The correct order of increasing electron affinity for the elements, O, S, F and Cl is:
1. | Cl < F < O < S | 2. | O < S < F < Cl |
3. | F < S < O < Cl | 4. | S < O < Cl < F |
Amongst the elements with the following electronic configurations, which one of them may have the highest ionisation energy?
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2.
3.
4.
1. Cr > Mn > V > Ti
2. V > Mn > Cr > Ti
3. Mn > Cr > Ti > V
4. Ti > V > Cr > Mn