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Isotopes. Atoms with the same number of protons but different numbers of neutrons Ex) Carbon 12 vs. Carbon 14 These atoms have a different mass Chemically alike because still have the same number of protons. Isotopes of Hydrogen. Hydrogen -1 simply called hydrogen

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isotopes
Isotopes
  • Atoms with the same number of protons but different numbers of neutrons
  • Ex) Carbon 12 vs. Carbon 14
  • These atoms have a different mass
  • Chemically alike because still have the same number of protons
isotopes of hydrogen
Isotopes of Hydrogen
  • Hydrogen -1 simply called hydrogen
  • Hydrogen - 2 called deuterium
  • Hydrogen - 3 called tritium
development of amus
Development of AMUs
  • Atomic Mass Units (AMUs)
  • Protons have a mass of 1 amu
  • Neutrona have a mass of 1 amu
  • Electrons have a mass of 0 amu
atomic mass
Atomic Mass
  • The weighted average mass of the isotopes in a naturally occurring sample of the element
  • Don’t confuse with “mass number”
  • To calculate atomic mass you need 3 pieces of information
  • 1. The number of stable isotopes
  • 2.The mass of each isotope
  • 3.The natural percent abundance of each isotope
atomic mass1
Atomic Mass
  • Example Problem - Calculate the atomic mass for element X. One isotope has a mass of 10 amus (10X) and is 20% abundant. The other has a mass number of 11 amus (11X) and an abundance of 80%.
  • To solve: Multiply the mass number times the abundance than add them together.
atomic mass2
Atomic Mass
  • 10 x 0.20 = 2.0
  • 11 x 0.80 = 8.8
  • Add 2.0 + 8.8 = 10.8
    • The atomic mass of element X is 10.8 amus
atomic mass3
Atomic Mass
  • Your turn. Solve:
    • What is the atomic mass of Element Z? The isotopes are 16Z, 17Z, 18Z; with percent abundances of 99.759, 0.037, 0.204.
atomic mass4
Atomic Mass
  • Answer
    • 16 x 0.99759 = 15.961
    • 17 x 0.00037 = 0.0063
    • 18 x 0.00204 = 0.0367
  • 15.961 + 0.0063 + 0.0367 = 16.004
  • Tha atomic mass of element Z is 16.004 amus
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