If Bromine atom is available in the form of say, two isotopes `._(35)^(79)Br(49.7%)` and `._(35)^(81)Br(50.3%)` Calculate the average atomic mass of Bromine atom.

Explanation

It is given that two isotopes of Bromine are 79/35 Br(49.7%) and 81/35 Br(50.3%). Then, the average atomic mass of Bromine atom is given by
`79xx(49.7)/(100)+81xx(50.3)/(100)`
`= (3926.3)/(100)+(4074.3)/(100)`
`=(8000.6)/(100)`
`= 80.006 u`