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Isotopes & Average Atomic Mass. What are isotopes? Atoms of the same element that have different numbers of neutrons and different atomic masses.

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Presentation on theme: "Isotopes & Average Atomic Mass. What are isotopes? Atoms of the same element that have different numbers of neutrons and different atomic masses."— Presentation transcript:

1 Isotopes & Average Atomic Mass

2 What are isotopes? Atoms of the same element that have different numbers of neutrons and different atomic masses.

3 Are these isotopes? 1. Yes 2. No

4 The average atomic mass of Carbon is 12.011 amu. Which isotope of Carbon would you expect to find in nature the majority of the time? 1. Carbon - 12 2. Carbon - 13 3. Carbon - 14 4. They are all equally found in nature

5 Weighted Averages Ages: Find average age:

6 What is average atomic mass? ► The mass calculated when we take into account all of the isotopes that exist and the abundance (percentage) of each type. Chlorine 35 Abundance = 24.23% Abundance = 75.77% Chlorine 37

7 How to calculate IsotopeNumber of Protons Number of Neutrons Cl – 35 Cl - 37 (35 x 0.7577) + (37 x 0.2423) = 35.5 amu Example: Chlorine 75.77% - Cl 35 24.23% - Cl 37 Step #1 Step #2 Predict: Average atomic mass based on masses and percentages: amu Step #3 Calculate average mass: (mass x percent) + (mass x percent) +... = average atomic mass

8 What is different between isotopes of the same element? 1. Atomic # only 2. Mass # only 3. # of protons only 4. # of neutrons only 5. Both atomic # and # of protons 6. Both mass # and # of neutrons 7. Both # of neutrons and # of protons

9 M&M lab


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