Isotopes. Let’s Review ProtonsNeutronsElectrons Charge +1 0 Mass 1 amu 0 Location nucleus Electron cloud.

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Presentation transcript:

Isotopes

Let’s Review ProtonsNeutronsElectrons Charge +1 0 Mass 1 amu 0 Location nucleus Electron cloud

Isotopes Atoms that have the same number of protons, but have different numbers of neutrons Examples Hydrogen (Protium)Hydrogen (Deuterium)Hydrogen (Tritium) Notice that each of these atoms have one proton; therefore they are all types of hydrogen. They just have a different mass number (# of neutrons).

Isotopes of Hydrogen Hydrogen (Protium) Protons = 1 Neutrons = 0 Electrons = 1 Hydrogen (Deuterium) Protons = 1 Neutrons = 1 Electrons = 1 Hydrogen (Tritium) Protons = 1 Neutrons = 2 Electrons = 1 What is the mass number for each of these isotopes? REMEMBER: Mass Number = protons + neutrons Mass = 1 amu Mass = 2 amuMass = 3 amu

Isotopes of Hydrogen H Hydrogen H Hydrogen H Hydrogen - 3 Using Hyphen Notation the number represents the mass number of the isotope. Mass = 1 amu Mass = 2 amuMass = 3 amu

Isotopes of Carbon

Average Atomic Mass The weighted average of the masses of all the naturally occurring isotopes of an element The average considers the percent abundance of each isotope in nature This is the decimal number found on the periodic table of elements

Average Atomic Mass Hydrogen (Protium) Mass # = 1 amu Hydrogen (Deuterium) Mass # = 2 amu Hydrogen (Tritium) Mass # = 3 amu If you simply average the three, 2 amu (1 amu + 2 amu + 3 amu/3) would be the atomic mass, but since 99.9% of the Hydrogen is Protium, the atomic mass is around 1 amu (.999 x 1 amu) What would be the atomic mass (≈) of Hydrogen if these three isotopes were found in the following percentages (99.9, 0.015, 0) respectively?

Average Atomic Mass Example: Lithium-6 is 4% abundant and lithium-7 is 96% abundant. What is the average mass of lithium? 6 * *.96 = 6.91