3. He just couldn't put it down.
Date: – Bring Calculator to class every day Day Plan: Seating Chart, Pre-Lab, Lab Groups Homework - Worksheet Opener: Have you heard the one about a chemist who was reading a book about helium?
He just couldn't put it down.

4. Where we came from and where we are going!
Semester 1
Semester 2
Intro to Chemistry
Atoms and Isotopes
Periodic Table
Covalent and Ionic Bonds
Moles & Chemical Reactions
Chemical Quantities & Energy
Gas Laws/ Reactions in aqueous solutions
Equilibrium & Acid/Base

5. “Counting by Weighing”
When you go to the store to by apples
When you by Jelly Beans
When you by Chicken Breast

6. Notes A – The Mole
Write what is in red

7. “ When we attempt to conceive the number of particles in an atmosphere (Gas), It is somewhat like attempting to conceive the number of stars in the universe; we are confounded with the thought. But if we limit the subject, by taking a given volume of any gas, we seem convinced that…. The number of particles must be fixed” – John Dalton 1808
John describes his approach to the theory of the atom. Atoms may be invisible, immeasurable small, . Furthermore, as finite particles, atoms must have real properties.

8. All atoms of a given element have the same atomic mass.
We Know all Matter is made up of Atoms, Molecules, and Ions
Dalton stated
All atoms of a given element have the same atomic mass.
Atoms of different elements have different atomic masses.
These statements – the cornerstone of Dalton’s Atomic Theory – provide a starting point for calculating relative atomic masses of atoms based on the mass percentage of elements in compounds. There was still a long way to go, before Dalton's suggestion of actually counting atoms would be possible.

9. In 1811 Amedeo Avogadro, an Italian chemistry professor, published a hypothesis – that equal volumes of gases at equal pressures and temperatures contained equal number or atoms or molecules.
These hypothesis was so stunning that it was completely ignored for more then 50 years. It was not until many years after Avogadro’s death that his hypothesis became enshrined as a law and acquired a numerical value to go along with it.
Avogadro’s Number (THE MOLE) is defined as the number of represented particles (Atoms or Molecules) contained in a specific mass, called the Molar Mass of any pure substance.

10. Average atomic mass of atoms and Avogadro’s number are routinely used today by chemists all over the world to count both atoms and molecules- chemists count atoms by weighing them.
“Counting by Weighing” Makes it possible to analyze compounds found in nature and synthesis new compounds in lab.

11. Example Problems 1) 5.5 dozen apples = _____ kg apples
(1 dozen = 2.0 kg apples)
2) 3 dozen apples = _____ bushel apples
(1 dozen apples = .20 bushel apples)
3) 4 Moles of HCl = ___________ Molecules of HCl

12. Homework – Must show all work and label units!

13. WHY Assigned LAB GROUPS - For 3 quarter
All Chemistry Classes that I have been in and heard of have assigned lab groups
So I know who is at each table without having to make a sign up sheet each week
Safety – People are not wondering looking for materials or goofing around.
So people work with the same people every week – get to know who is a better recorder, team leader, experimenter.
To make sure materials are organized and ready for other lab groups.

14. Tomorrow Pre- Lab
Do the pre-lab questions with your group
Get to know your group
Try using the scales
Go to your lab and try to turn on the scales
Tare the scale (Make sure it reads Zero's)
Measure one bean

15. Labs If you are late to lab – DO
take a packet on top of the microwave and sit down and work on it.
Do not come back into Lab
Do not disturbed any of the students doing the lab
If you are Late to Lab – DO NOT – join a lab
Reason
Its not fair to the people who were here on time doing the work
I would have to talk to you about which group/ what packet/ or to put on googles taking my attention off of the class
For safety reasons you missed any direction I gave you at the beginning of class.

16. 12 2 3000 6.022 X 10 23 Quiz Time – NO its not graded!
How many dogs are in a dozen dogs?
How many apples are in a pair of apples?
If there are 1000 soldiers in a division, how many soldiers are in 3 divisions?
If there are X carbon atoms in 1 mole of carbon … how many hamburgers are there in 1 mole of hamburgers? 12 2
3000
6.022 X 10 23