1. Unit 3: Atomic Theory & Periodicity

2. Monday, October 26 Warm-up: Pick up the Learning Target Tracker
LEARNING OBJECTIVE A: Atomic Information
State the location & charge of each subatomic particle within the atom
Use the periodic table to determine the number of protons, neutrons, and electrons in an atom of an element
Define atomic number as it relates to subatomic particles
Warm-up: Pick up the Learning Target Tracker
Highlight the quiz and test dates and copy them into your planner
Independent Practice #1 is due on Friday 10/30

3. Video
Take careful notes on the video, think about the learning targets as you are watching

5. Video Wrap up What are the 3 common particles in an atom?
What 2 particles are in the nucleus?
If an atom were expanded to the size of a stadium what size would the nucleus be?
What’s between the atom’s nucleus and the electrons?
Where is the majority of the mass in an atom?

6. In your notes Particle Location in atom Charge Mass in AMU
Make a table in your notes to complete with the information you have learned.
Particle
Location in atom
Charge
Mass in AMU

7. BOHR MODEL
A Bohr Model is a simplified version of what an atom looks like. The protons and neutrons are located in the nucleus and the electrons are in “shells” or rings around the nucleus
You draw a Bohr Model by placing two electrons maximum in the shell closest to the nucleus and a maximum of eight electrons in each of the other shells.

8. Check in How many protons does Iodine (I) have?
How many protons does Tungsten (W) have?
Which subatomic particle has a negative charge?
What is the mass of one neutron?
Where in an atom are electrons located?
Draw a Bohr Model of a neutral atom of Sodium (Na)

9. LEARNING OBJECTIVE A: Atomic Information
Tuesday, October 27
LEARNING OBJECTIVE A: Atomic Information
Warm-up: How many protons does Bromine (Br) have? How do you know?
Independent Practice #1 is due on Friday 10/30

10. Isotopes
Each table will need a sheet of Model 1 and each member of your group will need their own Isotopes packet and a periodic table.
Choose your roles. Facilitator will appoint a reader for the activity. Spokesperson will appoint a clean up person for the activity.
Work through carefully, making sure you reach consensus on each question. Switch your cup to yellow at stop signs (pretend they are yield signs ) but keep moving.

11. I will be able to calculate average atomic mass.
Wednesday, October 28
LEARNING OBJECTIVE
I will be able to calculate average atomic mass.
WARM UP
How many neutrons are in…
U-235 (atomic number 92)
Pb-207 (atomic number 82)
Hydrogen-3 (atomic number 1)
What are isotopes?

12. today
Relative Abundance Lab

13. I will be able to calculate average atomic mass.
Wednesday 10/28 Exit Slip
Learning Objective
I will be able to calculate average atomic mass.
Why is average atomic mass so important it was included in the periodic table?

14. Thursday - October 29
Learning Objective B: Isotopes and Relative Atomic Mass
Today we discover why the mass number on the periodic table has a decimal!
Warm-up: Calculate the average number of students at each table in the classroom. Be ready to show your work and explain your reasoning.
REMINDER: Independent Practice #1 is DUE TOMORROW!!! Quiz 1 is TOMORROW

15. Average Atomic Mass

16. Check point 1
12. Propose a possible way to calculate the average atomic mass of 100 magnesium atoms
Spokesperson Question: How would you propose to calculate this average? Why?

17. Check point 2
15. Calculate the average atomic mass of Oxygen with one of the proposed methods
Spokesperson Question: Which method worked best? Why?

18. Extension Questions

19. Wrap Up
1. The average atomic mass of nitrogen is amu. Predict which isotope listed below is most abundant in nature
a. Nitrogen-13
b. Nitrogen-14
c. Nitrogen-15
2. Explain why a weighted average is used to calculate the average atomic mass of an element. Why is it not sufficient to calculate a simple average of the isotope data?
3. A certain element was originally named “muriaticum” by its discoverer. This element exists on Earth as a mixture of two isotopes. The most abundant isotope (75.76%) has a mass of amu; the other isotope (24.24%) has a mass of amu. Calculate the average atomic mass and identify the element by its modern name. B
When you calculate a simple average you assume equal representation by all the isotopes. Natureal matter does not consist of isotopes with equal distribution so a weighted average is needed.
(0.7576)( amu) + (0.2424)( ) = amu Chlorine

20. Friday – October 30 Learning Target C: Half-Life
Warm-up: Have your independent practice out and ready to turn in.
We will go over questions for 5 minutes and then you will have 15 minutes to take the quiz

21. Quiz
Pile your independent practice on the corner of the table. Clear your table of everything except something to write with, a calculator, and a periodic table.
When you are done gather the lab from the front of the class and begin reading through the procedure