Presentation is loading. Please wait.

Presentation is loading. Please wait.

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

Similar presentations


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 amu. Which isotope of Carbon would you expect to find in nature the majority of the time? 1. Carbon Carbon Carbon 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 ) + (37 x ) = 35.5 amu Example: Chlorine 75.77% - Cl % - 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


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

Similar presentations


Ads by Google