1. Isotopes Ms Fedor Arts and College Preparatory Academy

2. ChemCatalyst An atom has a mass of 22 and 11 protons. 1. What element is this atom? 2. How many neutrons and electrons does it have?

3. ChemCatalyst Draw a Bohr Diagram for magnesium

4. A chemist investigating a sample of lithium found that some lithium atoms have a lower mass than other lithium atoms. The chemist drew models of the three different types of lithium atoms. 1. What is different about the two atoms? 2. What is the atomic number of each atom? 3. What is the atomic mass of each atom?

5. What is an isotope?

6. Atomic mass

7. ChemCatalyst Why did Ernest Rutherford conclude that the nucleus was so small?

8. Atoms with the same number of protons, but a different number of neutrons are called Isotopes The nuclei of these 3 hydrogen atoms are different, because they have different numbers of neutrons Most hydrogen atoms are this

9. Isotopes of the same element still have the same properties and behave the same way in a chemical reaction. = This carbon is actually a mixture of C-12, C-13, and C-14

10. Symbols associated with isotopes Isotopes can be represented using their atomic symbol

11. What is the atomic mass and atomic number of chlorine? Mass = 35 Atomic number = 17

12. We also write the atomic mass after the name to distinguish them Carbon-12 6 P +, 6 N 0 Carbon-136 P +, 7 N 0 Carbon-146 P +, 8 N 0

13. Percent Abundance

14. Atomic mass is an average value It is calculated based on how much of that element is made up of the isotope. The average mass is closest to the mass of the most common isotope For example: Most Carbon is Carbon-12, so the mass will be closer to 12 than 13 or 14.

15. Calculating Average Atomic Mass 1. Multiply the atomic mass of each isotope by its percent abundance. 2. Add them all up. For example: If the abundance of O-16 is 75%, and the abundance of O-17 is 25% than the atomic mass would be: (16 x 0.75) + (17 x 0.25) = 12 + 4.25 = 16.25

16. Practice: Calculating Atomic Mass What is the atomic mass for neon (Ne) if 20 Ne has a relative abundance of 19.91%, and 21 Ne has a relative abundance of 80.09%? (20 x 0.1991) + (21 x 0.8009) = 1.991 + 8.8099 = 10.8009 Known 1: 10 Ne mass = 20 10 Ne abundance = 19.91% Known 2: 11 Ne mass = 21 11 Ne abundance = 80.09% unknown: Atomic mass of Ne

17. Q: Which copper isotope is more abundant: Cu-63 or Cu-65 (atomic mass of copper is 63.546? A: A: The atomic mass of 63.546 is closer to 63 than to 65. Because the atomic mass is a weighted average of these two isotopes, Cu-63 must be more abundant than Cu-65

18. ChemCatalyst Draw Bohr diagrams for the three isotopes of hydrogen: hydrogen-1 (atomic mass of 1), hydrogen-2 (atomic mass of 2), and hydrogen-3 (atomic mass of 3)

19. ChemCatalyst Magnesium has three isotopes, Magnesium- 24, Magnesium-25, and Magnesium 26. Which do you think is the most common isotope of magnesium and why?

20. ChemCatalyst How many protons, neutrons, and electrons are in phosphorus-32?

21. ChemCatalyst Which of the following are isotopes of copper, Cu? Explain your reasoning. 631976387 Cu Cu Cu Cu 29792829 3465 Cu Cu29

22. Quiz test corrections 1. For each multiple choice question missed: ◦ Explain which answer is correct and why 2. For each short answer missed: ◦ retry the question, and explain why your answer was incorrect/insufficient

23. ChemCatalyst What would be the average atomic mass of chlorine given the following information: Chlorine with 18 neutrons: 75.77% Chlorine with 20 neutrons: 24.23%

24. How are “atoms”, “isotopes”, and “elements” related? Remember: All matter is made of atoms Atoms with the same number of protons belong to the same element. ◦ This means that all atoms with the same number of protons, have the same properties. Different forms of an element are called isotopes. ◦ This means that atoms of the same element can differ slightly in the number of neutrons, and consequently, the mass.

25. Naturally Occurring Isotopes The neutrons stabilize the nucleus. Lower numbered elements (40 and below), have an even number of P + and N 0 Higher numbered elements have more neutrons than protons.

26. Radioactive Isotopes Atoms that are unstable are called “radioactive” Unstable nuclei will emit particles and break down over time Those atoms are lost over time because they decay into smaller atoms.

27. Some elements have naturally occurring radioactive isotopes Elements above bismuth (84 and up) are all radioactive Elements above uranium (93 and up) are all man-made elements

28. ChemCatalyst Write the isotope for neon with 11 neutrons in two ways.