Embibe Experts Solutions for Chapter: Classification of Elements and Periodicity in Properties, Exercise 3: EXERCISE-3

Compounds that formally contain ${\mathrm{Pb}}^{4+}$ are easily reduced to ${\mathrm{Pb}}^{2+}.$ The stability of the lower oxidation state is due to _____ effect.

For an element the successive ionisation energy values (in eV/atom), are given below.

$14.534, 29.601, 47.448, 77.472, 97.888, 552.057, 667.029$

Find the number of valence shell electrons in that element.

How many following properties is higher for fluorine as compared to chlorine.

Atomic mass, Covalent radius, Ionic radius $\left({\mathrm{X}}^{-}\right)$, Ionization energy, Electron affinity, Electronegativity, Hydration energy of uninegative ion $\left({\mathrm{X}}^{-}\right)$,

How many orders are CORRECT

(a) Acidic strength $\Rightarrow \mathrm{ClOH}<\mathrm{BrOH}<\mathrm{IOH}$

(b) Basic strength $\Rightarrow \mathrm{MgO}<\mathrm{CaO}<\mathrm{SrO}<\mathrm{BeO}$

(c) Electronegativity $\Rightarrow \mathrm{Mg}<\mathrm{Na}<\mathrm{Si}<\mathrm{S}<\mathrm{Cl}$

(d) Electron affinity $\Rightarrow \mathrm{Mg}<\mathrm{Na}<\mathrm{Si}<\mathrm{S}<\mathrm{Cl}$

(e) $\%$ Ionic character $\Rightarrow \mathrm{NaF}<\mathrm{KF}<\mathrm{RbF}$

Write the number of pairs in which size of first element or ion is higher as compared to ${\mathrm{II}}^{\mathrm{nd}}$ out of following eight pairs.

$\left(\mathrm{O}, \mathrm{S}\right), \left(\mathrm{He}, \mathrm{Ne}\right), \left(\mathrm{Kr}, \mathrm{Ne}\right), \left(\mathrm{Na}, {\mathrm{Na}}^{+}\right), \left(\mathrm{Cl}, {\mathrm{Cl}}^{-}\right), \left({\mathrm{I}}^{-}, {\mathrm{Cl}}^{-}\right), \left(\mathrm{Li}, \mathrm{Na}\right), \left({\mathrm{Li}}^{+}, {\mathrm{Na}}^{+}\right)$

Total number of enthalpy(s) (out of given eight) of $\mathrm{A}\left(\mathrm{g}\right)$ which is/are not associated with conversion of ${\mathrm{A}}_{\left(\mathrm{g}\right)}^{-}\to {\mathrm{A}}_{\left(\mathrm{g}\right)}^{+4}$ :

${\mathrm{IE}}_1, {\mathrm{IE}}_2, {\mathrm{IE}}_3, {\mathrm{IE}}_4, {\mathrm{IE}}_5, {\mathrm{IE}}_6, {\mathrm{EGE}}_1, {\mathrm{EGE}}_2$

($\mathrm{IE}=$ ionization energy, $\mathrm{EGE}=$ electron gain enthalpy)

Calculate $\mathrm{E}.\mathrm{N}$. of chlorine atom on Pauling scale if $\mathrm{I}.\mathrm{E}$. of ${\mathrm{Cl}}^{-}$ is $4\mathrm{eV}$ & $\mathrm{E}.\mathrm{A}$. of ${\mathrm{Cl}}^{+}$ is $+13.0 \mathrm{eV}$.

Upto argon find the number of elements which have lower ${\mathrm{IE}}_1$ as compared to $\mathrm{He}$?