Ions and Isotopes

1. Ions and Isotopes

2. Warm Up Objetivos • SWBAT distinguish between atoms, isotopes, and ions. • SWBAT calculate number of protons, neutrons, and electrons. • What’s the difference between a unicycle, a bicycle and a tricycle? (aren’t they the same thing?) • How many protons, neutrons, and electrons does Oxygen have?

3. Agenda • Warm Up • Agenda • Revisit Atom • FruitLoopyAtoms? • Ions & Isotopes • WS.4.2 • Exit Ticket Quiz tomorrow

4. Activity: Fruit Loopy Atoms Date

5. Background Info • VOCABS ARE HERE! • We will have a quiz on these 11 vocabulary terms tomorrow. • I expect that you will have the definitions of all 11 words in bold MEMORIZED.

6. Subatomic Particles • Proton – heavy and +1 charge • Neutron – heavy and 0 charge • Electron – tiny and -1 charge

7. Electron Shells Electron shell – orbit followed by electrons around an atom’s nucleus. How electron shells fill:

8. Picture of a Beryllium Atom Beryllium Atomic number: Protons: Neutrons: Atomic mass: 9

9. Atom = most common form of element, atoms are ALWAYS neutral (# protons = # electrons)

10. An atom has 5 protons … How many electrons does it have?

11. How can we tell atoms of different substances apart? • Each type of atom has a different number of PROTONS • ATOMIC NUMBER = # of PROTONS… what defines an element!

12. An atom has 82 protons … what element is it? • Look for number 82 on your periodic table!!

13. How many electrons does it have? • Atomic # = # Protons = # Electrons • 82 = 82 protons = 82 electrons

14. You Try!

15. So … in atoms protons = electronsWhat about neutrons???

16. Atoms have DIFFERENT amounts of Neutrons!!They are called ISOTOPESIsotope = atoms with same # protons, different # of neutrons

17. How can we figure out how many neutrons an atom has?

18. The mass of an atom can be calculated by adding protons + neutrons!Mass Number (sometimes all called “atomic number”) = # protons + # neutrons

19. Practice

20. Practice

21. Atomic Weight • Mass Number/Atomic Mass is not to be confused with atomic weight! • Atomic weight = weighted average of the atomic masses of the different isotopes of an element

22. Where is atomic weight on your PToE? 16 S 32.065

23. Ion • Ion = an atom that has either lost or gained electrons and now has a + or - charge

24. Materials/Methods: You will build an atom from the periodic table using a paper plate, fruit loops, and glue. It is important that you both use the same color for the same sub atomic particles.

25. Pick your Partner • Choose someone who know you will work well with • Move to a desk beside them

26. Fruit Loop Atoms • Complete first part of the Fruit Loop Activity • When you reach a , you should probably stop. • Make an ATOM of Lithium, Beryllium, or Boron

27. Notes Isotope An isotope is an atom with the same # of protons and electrons but a different # of neutrons. Example: The most common type of sulfur usually has 16 neutrons, but sometimes an isotope of sulfur will have 17 neutrons. ** Number of protons and electrons the same!

28. Notes Isotope Scientists like to have a quick way to write down isotopes! There are two ways: C – 14 Mass Number H 2 1 Mass Number 

29. Example • Write the isotope symbol in two ways for an isotope of fluorine that has a mass number of 22.

30. Notes You Try! • Write the isotope symbol in two ways for a carbon atom that has a mass number of 12. C C -

31. Notes Isotope Fill out the chart with your partner, then make a fruit loop isotope for Li – 9, Be – 11, B - 14.

32. Notes Ion An ion is an atom with the same number of protons and neutrons but a different number of electrons. This means the charge is no longer neutral! Two types: Cation = positive ion, lost electrons Anion = negative ion, gained electrons

33. Notes Ion Meet the atom’s family! Symbols: C4- F1+ New Electric Charge

34. Notes Ion Fill out the chart with your partner, then make a fruit loop Ion. Li1+, Be2+, B2-. **Use the same # of neutrons as when you made the original atom.

35. Conclusion • 1. How are each of your three atoms different? • 2. Why are the masses of the atom of the element and the isotope different? • 2. Calculate the average weight of your element. (Take the average of the atomic mass of the original atom and the atomic mass of the isotope.) Average weight= __________________________________ • 3. Are the atomic weights on the periodic table whole numbers or decimals? • 4. Why do you think the atomic weights are this way?

36. Complete WS 4.2

38. ??? Warm Up • EQ: How do we calculate average atomic weight? • HOT Q1: What does percent abundance mean? • HOT Q2: Why are the atomic weights on the PToE decimal numbers? • HOT Q3: What terms do we need to define for our quiz? • You have 3 skittles. The mass of all the skittles is 9 g. What is the mass of each skittle? • A bag of M&M’s has 40 M&M’s. There are 10 blue M&M’s. What percentage of all the M&M’s are blue?

39. Agenda • Warm Up • Agenda • Beanium • Quiz! • Exit Ticket

40. Beanium • On a periodic table, the values for atomic number and atomic weight are given for each element. The atomic number is the whole number and represents the number of protons in the atom. The atomic weight is a decimal number because it represents a weighted average of themasses of the isotopes of each element.

41. In the following lab, you will determine the average atomic weight for the element “beanium”. There are three naturally occurring isotopes of beanium: white-beanium (must have a black dot!), brown-beanium, and speckled-beanium. You will calculate the average atomic weight of a given sample of beanium.

42. When You Get to Your Lab Station… • READ the directions • If you are confused • 1) THINK • 2) Ask a person at your lab station BEFORE you ask Ms. Hoffman • 3) Ms. Hoffman is your last resort

43. At the lab station… • You are 30 minutes to complete this activity • By the end of 30 minutes, you have answered ALL questions on lab handout

44. Classroom Leaders! • People I will be pulling out to meet with: • Tucker • Ken’Dajha • Nigel • Kiana • Justin • Jalisa • Jenn • Aysha • Krishanni • Nevada • Josh

45. Beanium • 1. Separate the “atoms” of beanium in your sample into three groups based on type of isotope (white, brown, or speckled). THROW OUT ALL WHITE BEANS THAT DO NOT HAVE A BLACK DOT. Count the number of atoms of each isotope and record below:

46. 2. Using your balance, find the mass of each isotope in the sample and record below:

47. 3. Calculate the grams in one atom of each isotope and record below. To find the mass of one atom of beanium – divide the total mass by the number of atoms you have for that element. Example: Total Mass of White Beanium / # of White Beanium Atoms

48. 4. Determine the percent abundance of each isotope in your sample. This can be done by dividing the number of atoms of each isotope by the total number of atoms in your sample and multiplying by 100. Example: ( # of white beanium atoms / Total # of atoms ) * 100

49. Vocab Quiz! • Define the following terms: • Proton • Neutron • Electron • Atom • Atomic Number • Isotope • Mass Number (also called “atomic mass”) • Ion

50. Quiz! • Define the following terms: • Proton • Neutron • Electron • Atom • Atomic Number • Isotope • Mass Number (also called “atomic mass”) • Ion • Cation • Anion