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,B-11. The average atomic mass of boron is found to be 10.80u. Calculate the percentage abundance of B^(10) isotope :-

B has two isotopes 10B (19%) and 11B( 81%) . What is the atomic mass of B .

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 :

(a) What are radioactive isotopes ? Give two examples of radioactive isotopes (b) Give any two uses of ratioactive isotopes (c) An element Z contains two naturally occuring isotopes ._(17)^(35) Z and ._(17)^(37)Z . If the average atomic mass of this element be 35.5 u, calculate the percentage of two isotopes.

Nuturally occurring boron consists of two isotopes whese atomic weight are 10.01 and 11.01 The atomic weight of nurons is 10.81 Calculate the percentage of each isotope is natural boron

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