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Naturally occuring boron has two isotope...

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`.

Text Solution

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Let x be the fraction of `""^10B` isotope and `(1-x)` that of `""^11B` isotope, then, `(x)10+(1-x)11=10.2`
Fraction of `""^10B` isotope, `x=0.8 (" or "80%)` and fraction of `"^11B` isotope, `(1-x)=0.2(" or "20%)`.
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  • Isotopes are the atoms of same element: they have same atomic number but different mass numbers. Isoto have different number of neutrons in their nucleus. If an element exists in two isotopes having atomic mas 'a' and 'b' in the ratio m:n, then average atomic mass will be ( m xx a + n xx b)/( m + n) Different isotopes of same element have same position in the periodic table. The elements which have sin isotope are called monoisotropic elements. Greater is the percentage composition of an isotope, more wiki be its abundance in nature. Atomic mass of boron is 10.81. It has two isotopes namely ""_(5) ^(11)B and ""_(5) ^(x) B with their relative abundance of 8 and 20% respectively. The value of x is

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  • Isotopes are the atoms of same element: they have same atomic number but different mass numbers. Isoto have different number of neutrons in their nucleus. If an element exists in two isotopes having atomic mas 'a' and 'b' in the ratio m:n, then average atomic mass will be ( m xx a + n xx b)/( m + n) Different isotopes of same element have same position in the periodic table. The elements which have sin isotope are called monoisotropic elements. Greater is the percentage composition of an isotope, more wiki be its abundance in nature. An element, X has the following isotopic.composition. ""^(2)X:90%,""^(109)X,8% ""(202)X,2%. The weight average atomic mass of the naturally occurring element 'X' is closest to:

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