1. AP Chemistry Unit 2 – Atoms, Molecules, and, Ions
Day 3 – Finish Analysis of Food Dyes and Mass Spectroscopy

2. Warm Up
SIT WITH LAB PARTNERS
TAKE OUT: lab NOTEBOOK Make: “Analysis” Section below data section find: Your graphs in blue bin FOLD, CUT, and tape graphS: Into ANALYSIS SECTION ON YOUR GRAPHs: FIND EQUATIONs for absorbance and %transmittance WRITE: equations in analysis section TIME: 6 MINUTES WHEN DONE: CHECK ANSWERS WITH MS. MYRIAH DAY

3. AP Chemistry Agenda Finish Analysis of Food Dyes Lab
Unit 2 notes (Mass spectroscopy)
GUIDED INQUIRY ASSIGNMENT
Next Classes:
Lab notebook due Tuesday with analysis, conclusion, sources of error, and Post-lab questions
MORE activities on chapter 2 and Chapter 6

5. Finish analysis of food dyes
FIND: lab HANDOUT “GUIDED INQUIRY” SECTION READ: 1,2, 4 Talk: with lab partners to determine an appropriate procedure TO DETERMINE CONCENTRATION OF BLUE DYE TIME: 6 MINUTES WHEN DONE: BE READY TO SHARE OUT

6. Finish analysis of food dyes
you will: observe how ms. Myriah obtains the absorbance of the Glacier freeze gatorade THEN: RECORD THE ABSORBANCE IN YOUR DATA TABLE IN ANALYSIS SECTION: CALCULATE THE number of milligrams OF THE GLACIER FREEZE GATORADE TIME: 6 MINUTES WHEN DONE: BE READY TO SHARE OUT

7. REMEMBER! Complete: the following sections by tuesday analysis section
Conclusion
Sources of error
Post lab questions
If you need help: refer to lab component for lab notebook, class website, the internet, or message me (include pictures if needed)
NOW: TAKE OUT NOTEBOOK OR BINDER

8. Various Models of the Atom- + + - +
Dalton
Thomson
Rutherford
Bohr
In one of your preliminary questions, you were asked to identify the experimental evidence that led to the development of the atomic models.
Dalton built on the work of other scientists to derive that atoms must combine in whole-number ratios. And that there is nothing smaller than an atom.
Thompson then experimented with the cathode ray tubes and magnetic fields, and determined that charged particles must exist within the atoms themselves, giving evidence that we had electrons, a smaller piece to the atom itself.
 Later on Rutherford, who is actually Thompson's former student, conducted the gold foil experiment in attempts to verify Thompson's plum pudding model. But instead, he derived that there must be a dense positive nucleus surrounded by negative charge within the atom.
And then Bohr used atom emission spectrum of hydrogen specifically to determine that there were quantized energy levels within the electron cloud.
Image sources:

9. Size of the Atom
1 A = 1 x m

10. Atomic Numbers, Mass Numbers, Isotopes

12. Atomic Weights 1 amu = 1.66054 x10-24 g 1 g = 6.02214 x1023 amu
Based on the measured and calculated mass of 1 Hydrogen atom
Derived from the mass of 1 Hydrogen atom – how many it would take to add up to 1 gram

13. Mass Spectroscopy Video
ON NOTEBOOK PAGE: Draw and write notes about Mass Spectroscopy from video
MAKE SURE TO: Write Flow Chart

14. Mass Spectrum of ________
51.5%
17.1%
17.4%
11.2%
Zirconium
2.8%

16. Guided Inquiry: Atomic Number and Mass
WITH THIS GROUP: Work on Atomic Number and Atomic Mass Guided Inquiry
CTQ = Critical Thinking Questions
TIME: Until End of Class
WHEN DONE: Have a GREAT WEEKEND and send a message if you have a question!

17. WHAT WILL YOU NEED TO KNOW FOR UNIT 2
WHAT DO YOU NEED TO KNOW?
Calculate isotopes (Guided Inquiry)
Mass Spectroscopy
Dalton’s laws
Empirical formulas
Electron configurations
How to use Planck’s equation
How to use beer’s law