Topic #7. Dalton was wrong about all elements of the same type being identical Atoms of the same element can have different mass numbers. ISOTOPES.

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Presentation transcript:

Topic #7

Dalton was wrong about all elements of the same type being identical Atoms of the same element can have different mass numbers. ISOTOPES

How can atoms of the same element end up with a different mass? SHOULDER PARTNERS

Frederick Soddy ( ) proposed the idea of isotopes in 1912 Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons. Soddy won the Nobel Prize in Chemistry in 1921 for his work with isotopes and radioactive materials. ISOTOPES

We can also put the mass number after the name of the element: carbon-12 carbon-14 uranium-235 NAMING ISOTOPES

Isotopes are atoms of the same element having different masses, due to varying numbers of neutrons. IsotopeProtonsElectronsNeutronsNucleus Hydrogen–1 (protium) (protium)110 Hydrogen-2(deuterium)111 Hydrogen-3(tritium)112

ISOTOPES Elements occur in nature as mixtures of isotopes. Isotopes are atoms of the same element that differ in the number of neutrons.

 How heavy is an atom of oxygen?  It depends, because there are different kinds of oxygen atoms.  We are more concerned with the average atomic mass.  This is based on the abundance (percentage) of each variety of that element in nature.  We don’t use grams for this mass because the numbers would be too small. ATOMIC MASS

Instead of grams, the unit we use is the Atomic Mass Unit (amu) It is defined as one-twelfth the mass of a carbon-12 atom. Carbon-12 chosen because of its isotope purity. Each isotope has its own atomic mass, thus we determine the average from percent abundance. MEASURING ATOMIC MASS

Multiply the atomic mass of each isotope by it’s abundance (expressed as a decimal), then add the results. If not told otherwise, the mass of the isotope is expressed in atomic mass units (amu) TO CALCULATE THE AVERAGE:

ATOMIC MASSESIsotopeSymbol Composition of the nucleus % in nature Carbon C 6 protons 6 neutrons 98.89% Carbon C 6 protons 7 neutrons 1.11% Carbon C 6 protons 8 neutrons <0.01% Atomic mass is the average of all the naturally occurring isotopes of that element. Carbon =

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