An element of atomic weight Z consists of two isotopes of mass number (Z-1) and (Z+2). Calculate the % of higher isotope.

An elements of atomic mass "m" consists of two isotopes of mass numbers (m-1) and (m+2). The percentage abundance of lighter isotope is

An element is found in nature in two isotopic forms with mass numbers (A-1) and (A+3). If the average atomic mass of the element is found to be A, then the relative abundance of the heavier isotope in the nature will be :

An element is found in nature in two isotopic forms with mass numbers (A-1) and (A+3). If the average atomic mass of the element is found to be A, then the relative abundance of the heavier isotope in the nature will be :

The element, boron has two isotopes ( ""^(10)B and ""^(11)B ). Calculate the natural abundance o the isotopes of boron if the atomic mass of the element be 10.8.

Naturally occuring boron has two isotopes of masses 10 amu and 11 amu. Calculate the percentage of each isotope if the average atomic mass of boron is 10.2 .

Atomic weight of chlorine is 35.5 . It has two isotopes of atomic weight 35 and 37 . What is the percentage of the heavier isotope in the sample ?

Atomic weight of chlorine is 35.5 . It has two isotopes of atomic weight 35 and 37 . What is the percentage of the heavier isotope in the sample ?