Consider the isoelectronic species, ${\mathrm{Na}}^{+}, {\mathrm{Mg}}^{2+}, {\mathrm{F}}^{-}, \mathrm{and} {\mathrm{O}}^{2-}$. The correct order of increasing length of their radii is :

1. ${\mathrm{F}}^{-}<{\mathrm{O}}^{2-}<{\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}$

2. ${\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}<{\mathrm{F}}^{-}<{\mathrm{O}}^{2-}$

3. ${\mathrm{O}}^{2-}<{\mathrm{F}}^{-}<{\mathrm{Na}}^{+}<{\mathrm{Mg}}^{2+}$

4. ${\mathrm{O}}^{2-}<{\mathrm{F}}^{-}<{\mathrm{Mg}}^{2+}<{\mathrm{Na}}^{+}$

The correct order of size of the given species is: 

Match the correct atomic radius with the corresponding element.

Codes :

Given are the following sets of species:

(a) ${\mathrm{Zn}}^{2+}, {\mathrm{Ca}}^{2+}, {\mathrm{Ga}}^{3+}, {\mathrm{Al}}^{3+}$

(b) ${\mathrm{K}}^{+},\hspace{0.17em}{\mathrm{Ca}}^{2+}, {\mathrm{Sc}}^{3+},\hspace{0.17em}{\mathrm{Cl}}^{-}$

(c) ${\mathrm{P}}^{3-}, {\mathrm{S}}^{2-}, {\mathrm{Cl}}^{-}, {\mathrm{K}}^{+}$

(d) ${\mathrm{Ti}}^{4+}, \mathrm{Ar}, {\mathrm{Cr}}^{3+}, {\mathrm{V}}^{5+}$

The sets containing only isoelectronic ions among the above are:

1. (a), (d)

2. (b), (c)

3. (c), (d)

4. (b), (d)

In which following options of arrangement does not agree with the variation of the property indicated against it?

Choose the correct option

The ionic radii vary in :

Choose the correct option :

1. (a), (c)

2. (b), (c)

3. (c), (d)

4. (b), (d)