Multiple Choice QuestionsThe ions N3-, O2-, F-, Na+, Mg2+ are isoelectronic. Their ionic radii show
an increase from N3- to F- and then decrease from N+ to Mg2+
a decrease from N3- to F- and then increase from Na+ to Mg2+
a significant increase from N3- to Mg2+
a significant decrease from N3- to Mg2+
Which of the following pairs of ions cannot be separated by H2S in dilute HCl?
Bi3+, Sn4+
Al3+, Hg2+
Cu2+, Zn2+
Ni2+, Cu2+
The radius of H-atom in its ground state is 0.58Å .The radius of, 3Li2+ ithe similar state is
0.1777 Å
0.706 Å
1.06 Å
0.058 Å
The correct order of ionization energies is
Cu > Ag > Au
Cu > Au > Ag
Au > Cu > Ag
Ag > Au > Cu
The set representing the correct order of ionic radius is
Li+ > Be2+ > Na+ > Mg2+
Na+ > Li+ > Mg2+ > Be2+
Li+ > Na+ > Mg2+ > Be2+
Mg2+ > Be2+ > Li+ > Na+
Which of the following is the correct decreasing order of oxidation state of nitrogen?
HNO3 > NO > NH4Cl > N2
HNO3 > NO > N2 > NH4Cl
HNO3 > NH4Cl > NO > N2
NO > HNO3 > NH4Cl > N2
Which of the following has highest electron affinity?
N
O
F
Cl
D.
Cl
The electron affinities of some of the elements of second period ( i.e. N, O, F, etc) are however, lower than the corresponding elements ( i.e P, S, Cl, etc) of the third period. This is due to the reason that the elements of second period have the smallest atomic sizes amongst the elements in their respective groups. As a result, there are considerable electron-electron repulsion with the atom itself and hence, the additional electron is not accepted with the same case as compared to the remaining elements in the same group.
Ionisation energy in group 1A varies in the decreasing order as
Li > Na > K > Cs
Na > Li > K > Cs
Li > Cs > K Na
K > Cs > Na > Li
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