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Atomic Masses

Atomic Masses

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Atomic Masses

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  1. Atomic Masses Test Friday!

  2. Atomic Mass is an average (decimal) • An average of known isotopes for an element • The atomic mass of an element is closest to the most common isotope found in nature • So, since Carbon’s atomic mass is closest to 12, Carbon-12 would be the most common isotope found in nature

  3. 19 K 39.0983 Isotopes and atomic mass • Potassium • How many protons? • How many neutrons? 19 20 potassium atoms: 93.25% will have 20 neutrons, 6.7302% will have 22 neutrons, 0.0117% will have 21 neutrons

  4. How is that weight calculated? potassium atoms: 93.25% will have 20 neutrons, 6.7302% will have 22 neutrons, 0.0117% will have 21 neutrons All will have 19 protons, so…. (.9325*20) + (.067302*22) + (.000117*21) = 39.0983 amu a weighted average 93.25% will weigh 39 amu 6.7302% will weigh 41 amu 0.0117% will weigh 40 amu

  5. Remember! 100% in decimal form = 1 50% = .5 35% = .35 10 = .1 1% = .01 .1% = .001 If in doubt, divide the percentage by 100!

  6. Approximately 75% of the chlorine atoms found innature have a mass of 35. The other 25% have a massof 37. What should we report as the atomic weight forchlorine? • [(.75)(35)] + [(.25)(37)] • = 26.25 + 9.25 • = 35.5 • The KEY is to convert the percentages to decimals correctly!

  7. 1. Suppose that there were two isotopes of Sodium.28% of the naturally occurring sodium atoms had amass of 22, and 72% atoms had a mass of 23. Whatwould the average atomic weight of sodium be?

  8. 2. Suppose that there were two natural isotopes ofCopper. 80% of the atoms had a mass of 63, and 20%of the atoms had a mass of 65. What would thataverage atomic weight of copper be?

  9. 3. Suppose that a new element (E) were discovered that existed as three natural isotopes. 25% of the atoms had a mass of 278, 38% had a mass of 281, and the remainder had a mass of 285. What would be listed as the atomic weight of this element?

  10. Practice! • Let’s do the More Average Atomic Mass worksheet.