Periodic Table and Periodicity

The ionic radii of O^2–, F^–, Na⁺ and Mg²⁺ are in the order :

The correct order of the ionic radii of O^2–, N^3–, F^– , Mg²⁺, Na⁺ and Al³⁺ is :

The increasing order of the atomic radii of the following elements is :- (a) C (b) O (c) F (d) Cl (e) Br

The ionic radius of Na⁺ ions is 1.02 $\mathop A\limits^o$. The ionic radii (in $\mathop A\limits^o$) of Mg²⁺ and Al³⁺, respectively, are

Given below are two statements: Statement I : Fluorine has most negative electron gain enthalpy in its group. Statement II : Oxygen has least negative electron gain enthalpy in its group. In the light of the above statements, choose the most appropriate from the options given below

The reduction in atomic size with increase in atomic number is a characteristic of elements of

Within each pair of elements F & Cl, S & Se, and Li & Na, respectively, the elements that release more energy upon and electron gain are :

The first ionization enthalpy of Na, Mg and Si, respectively, are : 496, 737 and $786 \mathrm{~kJ} \mathrm{~mol}^{-1}$. The first ionization enthalpy ($\mathrm{kJ} \,\mathrm{mol}^{-1}$) of $\mathrm{Al}$ is :

The increasing order of the ionic radii of the given isoelectronic species is :

The correct order of ionic radius is

$C{e^{ + 3}},\,\,L{a^{ + 3}},\,\,P{m^{ + 3}}\,\,$ and $Y{b^{ + 3}}\,\,$ have ionic radial in the increasing order as

Identify the elements X and Y using the ionisation energy values given below : Ionization energy (kJ/mol) 1${st}$ 2${nd}$ X 495 4563 Y 731 1450

Which one of the following ions has the highest value of ionic radius?

The set representing the correct order of ionic radius is :

The correct sequence which shows decreasing order of the ionic radii of the elements is

The ionic radii (in Å) of N^3–, O^2– and F^– are respectively:

For Na⁺, Mg²⁺, F⁻ and O²⁻; the correct order of increasing ionic radii is :

The correct order of the atomic radii of C, Cs, Al, and S is :

The ionic radii of K⁺, Na⁺, Al³⁺ and Mg²⁺ are in the order: