1. March 6, 2015 Pick up turned back docs Pick Up Calculator Warm up
Using the Sticky Note on your desk answer the following:
For the Unit Mole Conversions
I am strongest at ___________________
The question I still have is ________________________

2. Homework 3-6
Finish Empirical and Molecular Handout

3. Important Dates
Monday 3-2 – Smore Chemistry Tuesday 3-3 – ACT (homeroom) Wednesday 3-4 – Demo / Reaction Stoich Thursday 3-5 – Quiz / #TBT Friday 3-6 – Composition Stoich / Mole conversion assessment

4. Today is March 6, 2014 Topic: Reaction Stoichiometry
Lesson Objectives:
SWBAT achieve 85% or higher on their mole conversion assessment
Essential Question: 2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.

5. Agenda 3-6 Do Now 2 Practice Problems Assessment
Composition Stoich Guided Notes
HW Headstart

6. Mole Conversion Review
How many grams are in 6 moles of Iron? How many atoms are in 45 grams of water ?

7. Test

8. Today is March 6, 2014 Topic: Composition Stoichiometry
Lesson Objectives:
SWBAT to determine the composition of a substance using multiple composition stoich methods
Essential Question: 2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.

9. Calculating Percentage Composition
Calculate the percentage composition of magnesium carbonate, MgCO3.
Formula mass of magnesium carbonate:
24.31 g g + 3(16.00 g) = g
100.00

10. Practice
H2O (calculate O)
CaCOOH (Calculate Ca)
NaOH (Calculate H)

11. Empirical Formula
The formula that gives the simplest whole-number RATIO of the atoms of each element in a compound “Simplified”

12. Empirical Formula Chemical Formula (Molecular Formula)
H2O2 HO
C6H12O6
CH3O
C2H4O2

13. Determining Empirical Formulas
Steps:
Find mole amounts
Divide each mole by the smallest mole
Multiply until all whole numbers
Percent to mass
Mass to Mole
Divide by small
Multiply ‘till whole

14. Determine the empirical formula for a compound containing 2
Determine the empirical formula for a compound containing 2.128g Cl and 1.203g Ca

15. Molecular Formula
The formula that gives the ACTUAL NUMBER of atoms of each element in a compound “Real Life”

16. Determining Molecular Formula
Steps:
Find the empirical formula
Calculate the empirical formula mass or “EFM” (think molar mass)
Divide the molar mass by the “EFM” (this gives you the “factor”)
Multiply empirical formula by the factor

17. Find the molecular formula for a compound who molar mass is ~124
Find the molecular formula for a compound who molar mass is ~ and empirical formula is CH2O3