V K Sally and R Goel Solutions for Chapter: Structure of Atom, Exercise 2: EXERCISE 4B

${}_1{}^1\mathrm{H}$,  ${}_1{}^2\mathrm{H}$ and  ${}_1{}^3\mathrm{H}$  are the isotopes of hydrogen. Explain:
(i) Why do these isotopes have similar chemical properties?
(ii) Why are these isotopes electrically neutral?
 

The ratio of isotopes of  ${}_{17}{}^{37}\mathrm{Cl}$, and  ${}_{17}{}^{35}\mathrm{Cl}$ in natural chlorine is 1:3. Calculate the fractional atomic mass of chlorine. 

Find out the valency of the atoms represented by the Fig. (i) and (ii).
 
 

Why do helium, neon and argon have a zero valency?

1.  ${}_{10}{}^{20}\mathrm{Ne}$,  ${}_{10}{}^{21}\mathrm{Ne}$ and  ${}_{10}{}^{22}\mathrm{Ne}$ are the isotopes of neon.
(i) What do the subscripts and superscripts represent?
(ii) What is the cause of change in superscripts?
(iii) Give the geometric diagram of  ${}_{10}{}^{22}\mathrm{Ne}$.

What information do you get from the figure given about the atomic number, mass number and valency of atoms X, Y, and Z?. Give your answer in a tabular form.

An element E is available in the form of two isotopes  ${}_{15}{}^{31}\mathrm{E}$(75.8%) and  ${}_{15}{}^{33}\mathrm{E}$ (24.2%) Calculate the average atomic mass of element E.

The average atomic mass of a sample of an element X is 23.04 m. What are the percentage of isotopes ${}_{11}{}^{23}\mathrm{X} \mathrm{and} {}_{11}{}^{24}\mathrm{X}$ in the sample?