Chapter 2, Problem 2.113SP

Interpretation Introduction

(a)

Interpretation:

The grams present in 1 unified atomic mass unit should be determined.

Concept introduction:

Atomic weight of the element represents weighted average of mass of isotopes that naturally occurs in nature. For example, carbon has two major naturally occurring isotopes ${}_6^{12}\text{C}$ and ${}_6^{13}\text{C}$. Therefore, the atomic weight can be represent as follows:

$\text{Atomic weight of C}=\left(\begin{array}{l}\left({\text{Mass of }}_6^{12}\text{C}\right)\left({\text{Abundance of }}_6^{12}\text{C}\right)\\ +\left({\text{Mass of }}_6^{13}\text{C}\right)\left({\text{Abundance of }}_6^{13}\text{C}\right)\end{array}\right)$

Interpretation Introduction

(b)

Interpretation:

Total number of atoms equivalent to a mole should be determined.

Concept introduction:

Periodic table represents a systematic arrangement according to element’s physical as well as chemical properties. Here, elements are represented as a two-letter symbol and are arranged in increasing order of atomic number. First letter of symbol is always represented in capital letters and second letter is always represented as small letter.