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Given that the percentage abundance of t...

Given that the percentage abundance of the isotope `._(10)^(20)N` is 90 % and that of the isotope `._(10)^(22)Ne` is 10 %, calculate the average atomic mass of neon.

Text Solution

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The correct Answer is:
20.2 u
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Given that the percentage abundance of the isotope ""_(10)^(20)Ne is 90% and that of the isotope ""_(10)^(22)Ne is 10%, calculate average mass of neon.

Bromine occurs in nature mainly in the form of two isotopes ._(35)^(79)Br and ._(35)(81)Br . If the abundance of ._(35)^(79)Br isotope is 49.7 ^% and that of ._(35)^(81)Br isotope is 50.3 %, calculate the average atomic mass of bromine.

Knowledge Check

  • The relative abundance of two isotopes of an element with atomic weight 85 and 87 is 75% and 25% respectively. Then calculate the average atomic weight of element

    A
    `86.0`
    B
    `85.5`
    C
    `75.5`
    D
    `40.0`

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    The relative abundance of various isotopes of silicon is as Si (28) = 92.25%, Si (29) = 4.65% and Si (30) = 3.10%. Calculate the average atomic mass of silicon.

    Natural chlorine consists of two isotopes : 75% ""_(17)^(35)Cl and 25% ""_(17)^(37)Cl . Calculate the average atomic mass of chlorine .

    The percentage abundance of two isotopes of boron in a natural sample are 80 and 20. The first isotope has 6 neutrons in the nucleus. If the actual atomic mass of boron is 11.01, calculate the mass numbers of the two isotopes.

    (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.

    Natural chlorine contains chlorine in the form of the isotope ""^(35)Cl (75.5%) and ""^(37)Cl(24.5%) . Calculate the average atomic mass of natural chlorine.

    The isotopes of an element have mass numbers, A,A+1,A+2 . The ratio of abundance of these isotopes is 3:2:4 . Calcualte the average atomic mass of the element.

    The three stable isotopes of neon: " "_(10)^(20)Ne , " "_(10)^(21)Ne and " "_(10)^(22)Ne have respective abundances of 90.51%, 0.27% and 9.22%. The atomic masses of three isotopes are 19.99 u, 20.99 u and 21.99 u, respectively. Obtain the average atomic mass of neon.

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