Chapter 11.4, Problem 4RQ

(a)

Interpretation Introduction

Interpretation: The position on the periodic table and the valence shell electron configuration of the element tungsten needs to be determined.

Concept Introduction : Valence electrons are the electrons which occupy the outermost shell and core electrons are the electrons occupying the innermost shell.

Answer to Problem 4RQ

  $\text{Tungsten}\text{is}\text{[Xe]}{\text{6s}}^{\text{2}}{\text{4f}}^{\text{14}}{\text{5d}}^4$

Position in periodic table is group-6B

Explanation of Solution

Tungsten, W has $\text{z}=7\text{4}$

Nearest noble gas is Xe with 54 electrons. So, remaining 20 electrons are to be filled.

Therefore, the valence electron configuration is $\text{[Xe]}{\text{6s}}^{\text{2}}{\text{4f}}^{\text{14}}{\text{5d}}^4$ and it position is d-block element, group 6B.

(b)

Interpretation Introduction

Interpretation: The position on the periodic table and the valence shell electron configuration of the element Cesium needs to be determined.

Concept Introduction : Valence electrons are the electrons that occupy the outermost shell(highest energy level) and core electrons are the electrons occupying the innermost shell(lowest energy level).

Answer to Problem 4RQ

  $\text{Cesium}\text{is}{\text{[Xe]6s}}^1$

Position in periodic table is group-1A

Explanation of Solution

Cesium, Ce has $\text{z}=\text{55}$

Nearest noble gas is Xe with 54 electrons. So, remaining 1 electron are to be filled.

Therefore, the valence electron configuration is ${\text{[Xe]6s}}^1$ and it position is s-block element, group 1A.

(c)

Interpretation Introduction

Interpretation: The position on the periodic table and the valence shell electron configuration of the element arsenic needs to be determined.

Concept Introduction : Valence electrons are the electrons that occupy the outermost shell(highest energy level) and core electrons are the electrons occupying the innermost shell(lowest energy level).

Answer to Problem 4RQ

  $\text{Arsenic}\text{is}\text{[Ar]}3{\text{d}}^{\text{10}}4{\text{s}}^{\text{2}}4{\text{p}}^{\text{3}}$

Position in periodic table is group-5A

Explanation of Solution

Arsenic, As have $\text{z}=33$

Nearest noble gas is Ar with 18 electrons. So, remaining 15 electrons are to be filled.

Therefore, the valence electron configuration is $\text{[Ar]}3{\text{d}}^{\text{10}}4{\text{s}}^{\text{2}}4{\text{p}}^{\text{3}}$ and it position is p-block element, group 5A.

(d)

Interpretation Introduction

Interpretation:The position on the periodic table and the valence shell electron configuration of the element polonium needs to be determined.

Concept Introduction : Valence electrons are the electrons that occupy the outermost shell(highest energy level) and core electrons are the electrons occupying the innermost shell(lowest energy level).

Answer to Problem 4RQ

  $\text{Polonium}\text{is}{\text{[Xe]6s}}^2{\text{4f}}^{\text{14}}{\text{5d}}^{\text{10}}{\text{6p}}^4$

Position in periodic table is group-6A

Explanation of Solution

Polonium, Po has $\text{z}=84$

Nearest noble gas is Xe with 54 electrons. So, remaining 30 electron are to be filled.

Therefore, the valence electron configuration is ${\text{[Xe]6s}}^2{\text{4f}}^{\text{14}}{\text{5d}}^{\text{10}}{\text{6p}}^4$ and it position is s-block element, group 6A.