Naturally occurring gallium consists of two isotopes. one of those isotopes is 71ga with an isotopic mass of 70.9247050 amu and an abundance of 39.892%. what is the mass number of the other isotope?

The answer is 69.

Relative atomic mass of an element is a sum of the products of each isotopic mass and its abundance. We first need to calculate the isotopic mass of the second isotope to find out its mass number.

So,
- the isotopic mass of the first isotope: Ar1 = 70.9247050 amu
- the abundance of the first isotope: a1 = 39.892% = 0.39892
- the abundance of the second isotope a2 = 100% - a1 = 100% - 39.892% = 60.108% = 0.60108
- the isotopic mass of the second isotope is unknown: Ar2 = ?

Thus, using the formula:
Ar(Ga) = Ar1 * a1 + Ar2 * a2
69.723 = 70.9247050 * 0.39892 + Ar2 * 0.60108
69.723 = 28.2932833186 + 0.60108 Ar2
0.60108 Ar2 = 69.723 - 29.2832833186 = 41.4297166814
Ar2 = 41.4297166814 / 0.60108 = 68.92546197078592 amu ≈ 69 amu

Since the isotopic mass of the second isotope is ≈ 69 amu, the mass number of the isotope is 69.

☆ionisation energy increases across a period from na -> ar☆ionisation energy decreases down a group from li -> fr☆ionic radius decreases across a period from na -> cl☆ionic radius increases down a groupfrom f -> ii hope it clarifies your doubts