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

4. How is that weight calculated? (.9325*20) + (.067302*22) + (.000117*21) = 39.0983 amu a weighted average 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…. 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 in nature have a mass of 35. The other 25% have a mass of 37. What should we report as the atomic weight for chlorine? [(.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 a mass of 22, and 72% atoms had a mass of 23. What would the average atomic weight of sodium be?

8. 2. Suppose that there were two natural isotopes of Copper. 80% of the atoms had a mass of 63, and 20% of the atoms had a mass of 65. What would that average 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.