Chapter 3, Problem 3.119MP

(a)

Interpretation Introduction

Interpretation:

The ionization energy of rubidium when light of given wavelength ejects electrons at velocity of $\text{2}\text{.450 }\times {\text{ 10}}^{\text{6}}\text{ m/s}$ has to be calculated

Concept introduction:

Ionization energy:

In a gaseous state isolated neutral atom, the amount of energy required to eject an electron from outermost shell is known as ionization energy. Ionization energy increases from left to right across periods due to increase of effective nuclear charge. Ionization energy decreases down the group due to addition of electrons enters into new orbital which is far from nucleus.

(b)

Interpretation Introduction

Interpretation:

The ionization energy of potassium when light of given wavelength ejects electrons at velocity of $\text{1}\text{.240 }\times {\text{ 10}}^{\text{6}}\text{ m/s}$ has to be calculated.

Concept introduction:

Ionization energy:

In a gaseous state isolated neutral atom, the amount of energy required to eject an electron from outermost shell is known as ionization energy. Ionization energy increases from left to right across periods due to increase of effective nuclear charge. Ionization energy decreases down the group due to addition of electrons enters into new orbital which is far from nucleus.