Chapter 40, Problem 1P

(a)

To determine

The symbols for other two isotopes of Nitrogen.

Explanation of Solution

Introduction:

Isotopes are the element having same atomic number with different atomic weight or mass number.

An Isotope is another form of same element having same number of protons but different number of neutrons. Therefore, different isotopes of different elements have different atomic mass. Isotopes are either stable or radioactive in nature.

The element Nitrogen $\left(\text{N}\right)$ has atomic number $7$ , atomic weight $14\text{a}\text{.m}\text{.u}\text{.}$ present in group $15$ and period $2$ of the periodic table. Nitrogen can have one more or one less neutron in its nucleus therefore there are two other Nitrogen with mass number $13$ and 14.

Write the symbols of the other two isotopes of Nitrogen.

  ${}^{13}\text{N}$ and ${}^{15}\text{N}$

Conclusion:

Thus, the other two Isotopes of Nitrogen are ${}^{13}\text{N}$ and ${}^{15}\text{N}$ .

(b)

To determine

The symbols for other two isotopes of Iron.

Explanation of Solution

Introduction:

Isotopes are the element having same atomic number with different atomic weight or mass number.

An Isotope is another form of same element having same number of protons but different number of neutrons. Therefore, different isotopes of different elements have different atomic mass. Isotopes are either stable or radioactive in nature.

The element Iron $\left(\text{Fe}\right)$ has atomic number $26$ , atomic weight $56\text{a}\text{.m}\text{.u}\text{.}$ present in group $8$ and period $4$ of the periodic table. Iron can have two less neutrons in its nucleus therefore, there are two other Iron with mass number $54$ and $55$ .

Write the symbols of the other two isotopes of Iron.

  ${}^{54}\text{Fe}$ and ${}^{55}\text{Fe}$

Conclusion:

Thus, the other two Isotopes of Iron are ${}^{54}\text{Fe}$ and ${}^{55}\text{Fe}$ .

(c)

To determine

The symbols for other two isotopes of Tin.

Explanation of Solution

Introduction:

Isotopes are the element having same atomic number with different atomic weight or mass number.

An Isotope is another form of same element having same number of protons but different number of neutrons. Therefore, different isotopes of different elements have different atomic mass. Isotopes are either stable or radioactive in nature.

The element Tin $\left(\text{Sn}\right)$ has atomic number $50$ , atomic weight $118\text{ a}\text{.m}\text{.u}\text{.}$ present in group $14$ and period $5$ of the periodic table. Tin can have one less and one more neutrons in its nucleus therefore, there are two other Tin with mass number $117$ and $118$ .

Write the symbols of the other two isotopes of Tin.

  ${}^{117}\text{Sn}$ and ${}^{118}\text{Sn}$

Conclusion:

Thus, the other two Isotopes of Tin are ${}^{117}\text{Sn}$ and ${}^{118}\text{Sn}$ .