Naturally occurring copper exists in two isotopic forms: 63cu and 65cu. the atomic mass of copper is 63.55 amu. what is the approximate natural abundance of 63cu?

To calculate the average atomic weight, each exact atomic weight is multiplied by its percent abundance, then, add the results together.  If the natural abundance of 63Cu is assigned x, the natural abundance of 65Cu is 1-x (the two abundance always add up to 1). So the solution is: (63)(x)+(65)(1-x) = 63.55, 63x+65-65x=63.55, x=0.725=72.5%. The natural abundance of 63Cu is 72.5%, that of 65Cu is 1-72.5%=27.5%.

Is there a diagram/picture you can provide? it seems this question goes along with a

The closer the atoms are to becoming ionic the more highly dense the negatively charged side gets.