Classification of Elements and Periodicity in Properties Set-2

Q1. How is the covalent radius of a non-metallic element like Chlorine calculated?

Q2. The metallic radius of Copper ($\text{Cu}$) is assigned a value of $128\text{ pm}$. This is based on the internuclear distance of $256\text{ pm}$ between adjacent $\text{Cu}$ atoms in the solid crystal, where the metallic radius is:

Q3. Why does atomic size generally decrease across a period (left to right)?

Q4. Why does the atomic radius increase as we descend a group?

Q5. When comparing the size of an anion ($\text{X}^-$) to its parent atom ($\text{X}$), the anion is:

Q6. An atom ($\text{X}$) forms a cation ($\text{X}^+$). Which statement correctly describes the relationship between their sizes?

Q7. Consider the isoelectronic species $\text{O}^{2-}, \text{F}^{-}, \text{Na}^{+}, \text{Mg}^{2+}$. Which ion has the largest radius?

Q8. Which isoelectronic species will have the smallest radius among $\text{N}^{3-}, \text{O}^{2-}, \text{F}^{-}$?

Q9. Arrange the following isoelectronic species in the order of increasing ionic radii: $\text{Mg}^{2+}, \text{Na}^{+}, \text{F}^{-}$.

Q10. Why are the atomic radii of noble gases not typically compared with the covalent radii of other elements?