Atomic Radii, Ionic Radii and Vanderwall Radii

The metallic radius is half the internuclear distance separating the non-metal cores in the metallic crystal.

Explain the variation of atomic radius in the first transition series.

Covalent radius has a higher value than Van der Waals radius.

The atomic radius increases with increase in number of shells.

Screening factor calculated by using the formula, ${\mathrm{Z}}_{\mathrm{eff}}={\mathrm{Z}}_{\mathrm{actual}}-\mathrm{\sigma }$ is known as _____.

State the Slater's rule for calculating the screening factor.

On moving from left to right across a period of the periodic table, the atomic size

Name the element having the largest atomic size among the elements carbon, nitrogen and oxygen. 

Name the smallest atom in the third period. (Chlorine/ Sodium)

What is effective nuclear charge? How it changes in a group and a period? 

Cation is smaller than neutral atom and anion a bigger than neutral atom. Why? 

Van der Waals radius is _____ than covalent radius.

Which of the following species have correct order of size?

Along the period $(⟶)$ atomic/ionic radii and metallic character decreases while $IE,EN,$non-metallic character and oxiding power increases. Down the group $(\downarrow ),$ atomic/ionic radii, metallic character and reducing character increases while $IE$ and $EN$ decrease. However, ${{∆}_e}_g{H}^{⊝}$ becomes less negative down a group but more negative along a period.

In which of the following pairs, both species have nearly  the same size?

Along the period $(⟶)$ atomic/ionic radii and metallic character decreases while $IE,EN,$non-metallic character and oxiding power increases. Down the group $(\downarrow ),$ atomic/ionic radii, metallic character and reducing character increases while $IE$ and $EN$ decrease. However, ${{∆}_e}_g{H}^{⊝}$ becomes less negative down a group but more negative along a period.

If the ionic radii of ${\mathrm{M}}^{\oplus }$ and ${\mathrm{X}}^{⊝}$ are about $135 \mathrm{pm},$then expected values of metallic radii of $\mathrm{M}$and $\mathrm{X}$ should be respectively.

Arrange the following as per the instruction given in the bracket.
$\mathrm{N}\mathrm{a}, \mathrm{K}, \mathrm{L}\mathrm{i}$ (Increasing atomic size).

Arrange the following as per the instruction given in the bracket.

$\mathrm{H}\mathrm{e}, \mathrm{A}\mathrm{r}, \mathrm{N}\mathrm{e}$ (Increasing order of the number of electron shells).

How does the following property vary in the periodic table?
Atomic radius.

Explain the following.
Atomic size of the elements on moving from left to right in a period decrease.

The three elements $\mathrm{X},\mathrm{Y}$ and $\mathrm{Z}$ have ionic radii $1.33\stackrel{\text{o}}{\text{A}},0.95\stackrel{\text{o}}{\text{A}}$ and $0.60\stackrel{\text{o}}{\text{A}},$ respectively. Arrange them in increasing order of atomic numbers.