1. How atoms differ

2. Mass Number The sum of the protons and neutrons BUT…Why is it not an even number??

3. Isotopes: Dalton was wrong in saying that every atom of an element is the same. Neutral atoms of an element always have the same number of protons and electrons. But, the number of neutrons of an element differs in different atoms

4. Isotopes: Atoms with the same number of protons in the nucleus but different number of neutrons

5. Isotopes Isotopes have a different mass Isotopes containing more neutrons have a larger mass But, isotopes react the same – WHY?

6. Examples: EX: Potassium has 3 isotopes – one with 20 neutrons, one with 21 neutrons, and another with 22 neutrons Potassium has 19 protons Potassium 39 – 19 protons 20 neutrons Potassium 40 – 19 protons 21 neutrons Potassium 41 – 19 protons 22 neutrons

7. Isotopes In nature, elements are found as a mixture of isotopes There is a set percent present of each isotope Example – Potassium in a banana 93.25% is 20 neutrons; 6.7302% is 22 neutrons; and 0.017% is 21 neutrons

8. Mass of an element: For elements - Instead of listing each isotope of every atom – scientists combine the isotopes to make the atomic mass of the element

9. Atomic Mass: Atomic mass of an element is the weighted average of the mass of the isotopes of that element

10. To find the Atomic Mass (Isotope 1 mass X % abundance) + (Isotope 2 mass X % abundance), etc…

11. Atomic Mass: EXAMPLE Chlorine has two isotopes –Chlorine – 35 with 75.770% abundance –Chlorine – 37 with 24.230% abundance

12. IsotopeNumber of protons Number of neutrons MassRelative abundance N 14 771499.64% N 15 78150.36%

13. Carbon has two isotopes, C-12 and C-13. C-12 has a percent abundance of 98.89%. C-13 has a percent abundance of 1.11%. Calculate the average atomic mass of Carbon.