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 A exist in two isotopic forms A^15 and A^16 . If the average atomic mass of A was found to be 15.24, then the % relative abundance of A^15 will be

An element exist in nature in two isotopic forms: X^(30)(90%) and X^(32)(10%) . What is the average atomic mass of element?

Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.

Boron has two isotopes, B-10 and B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage of abundance of these isotopes.

(i) How would you define the terms atomic mass and molecular mass ? (ii) Nitrogen occurs in nature in the form of two isotopes with atomic masses 14 and 15 respectively. If the average atomic mass of nitrogen is 14.0067, what is the percent abundance of the two isotopes ?

Nitrogen occurs in nature in the form of two isotopes with atomic mass 14 and 15 respectively. If average atomic mass of nitrogen is 14.0067, what is the % abundabce of the two isotopes ?

Why are the atomic masses of most of the elements not whole numbers ?

Atomic mass of an element is not neccessurity a whole number because

Carbon found nature as a mixture of C-12 and C-13. The average atomic mass of carbon is 12.011u. What is the percentage abundance of carbon-12 in nature ?

Carbon found nature as a mixture of C-12 and C-13. The average atomic mass of carbon is 12.011u. What is the percentage abundance of carbon-12 in nature ?