Question

How many protons, electrons, and neutrons does the following isotope contain? 79Br+

Answer 1

The number of protons = atomic number in Periodic table, so 35

The number of neutrons = mass number - number of protons = 79-35=44

The number of electrons = atomic number - 1 = 35-1 =34

Answer 2

Explanation:

Atomic mass of a substance means the sum of total number of protons and neutrons present in an atom.

Whereas atomic number means the total number of protons present in an atom.

For example, in $^{79}Br^{+}$ atomic mass is 79 and it is known that atomic number of Br is 35.

Hence, total number of protons, electrons and neutrons present in $^{79}Br^{+}$ are as follows.

                Atomic mass = No. of protons + No. of neutrons

                         79  = 35 + No. of neutrons

               No. of neutrons = 79 - 35 = 44

When an atom is neutral then number of protons equal number of electrons. And, a positive charge means loss of an electrons.

So, number of electrons present in $^{79}Br^{+}$ is 35 - 1 = 34.

Thus, we can conclude that in $^{79}Br^{+}$ number of protons are 35, number of neutrons are 44 and number of electrons are 34.