1. This is easy – I got this Mrs. White
MOLAR MASS
1/9 Find your new seat – match your #
Show how you would set up a math equation for the following in your composition book:
How many dollars do you have when you have…
28,220 nickels
28,220 pennies
28,220 quarters
This is easy – I got this Mrs. White

2. Explain to your neighbor what you think a mole is in your own words.
What is a MOLE?
Explain to your neighbor what you think a mole is in your own words.

3. Molar Mass vs. Formula Mass – what is the difference?
The mass of a mole of any substance is called the molar mass of the substance. For example, the molar mass of a monatomic element is numerically equal to the atomic mass of the element, but expressed in grams/mole.
The mass in grams of a mole of any substance is called the formula mass of the substance.
Examples:
Units are important to be attached after every number in chemistry!
Ex. Fe is g/mole as molar mass but it is g for formula mass
Element
Molar Mass
Formula Mass Fe Au

4. Determine the molar mass for the following:
Sodium HCl
Chromium Mg3N2
Oxygen Ca(OH)2
Potassium Al(NO3)3

5. 1/10 Convert to mole from grams
COPY:
Formula mass (g)= 1 mole = 6.02X1023 atoms or molecules = 22.4 L of a gas  1. 2. 3.
4. What changes if you have to solve for the number of atoms or molecules?
5. How would you use this informaiton to find molar mass instead of formula mass?
Amount given in your problem & compound
Formula mass of compound
Solve for how many moles are in it?
286 g Ag
98 g MgNO35H2O
125 g iron (III) oxide

6. Equivalence values for money are: 1 dollar = 4 quarters = 10 dimes = 20 nickels = 100 pennies
Equivalence values in chemistry are: 1 mole = formula mass (g) = 6.02X1023 atoms = 22.4 L for gases only Sometimes atoms is interchanged with the words molecule, or particles. So if you are asked to solve for molecules or particles it is the same process as if it were atoms

7. General STEPS TO SOLVE grams to mole problems: #g of compound X = ??
Set up what is called “factor label method or dimensional analysis”, basically this is just math ratios using equivalence values to be able to change units
You do this by starting with the given amount & it’s unit; add up the formula mass to use as part of the “equivalence ratio” for grams along with the 1 mole

9. 1/9 Molar Mass Competition (you need your composition notebook to write out your work, your periodic table, & a calculator)
login on quizizz.com
Join using the code _______
Use your first name & last name initial (ex. Penny W.) so I can get your grade.

10. 1/9 &1/10 After you finish quizizz work then Finish the worksheet from yesterday’s class now. Solve for the “Molar Mass” on the sheet as a group.
Put all your names in the group on the top margin
Show your math work!
Check your answers with the back.
Under the side with the answers, write out the steps you must go through in order to determine the molar mass of a compound.

11. 1/5 How do we prove that the samples used in this data table were 1 mole of that sample mathematically?
Element
Sulfur
Silicon
Zinc
Iron
Mass of bag with sample
33.6
30.4
66.8
56.6
Mass of empty bag
1.5
Mass of one mole of the sample
32.1
28.8
65.3
55.1

12. 1/11 Convert between grams and moles:
Show all
math work!
How many moles are in 47.8 g of fluorine gas?
2. How many grams are in 2.01 moles of K2O?
3. List the steps you need to think through in order to set up a mole conversion calculation:

13. Mole Conversions What are you given? What are you looking for?
When converting like units are to be diagonal from each other : TO BE CANCELLED OUT
Multiply across the top and divide by the bottom

14. HOW MANY MOLES ARE THERE IN 15.96g OF PHOSPHORUS TRIOXIDE?
GRAMS TO MOLE
HOW MANY MOLES ARE THERE IN g OF PHOSPHORUS TRIOXIDE?

15. HOW MANY GRAMS ARE THERE IN .9 MOLES OF HCl?
MOLE to GRAM
HOW MANY GRAMS ARE THERE IN MOLES OF HCl?

16. Gram ↔ Moles use molar mass or atomic mass Ex. 32.3 g Na = ? mol Na
Ex mol Fe = ? g Fe

17. 1/12
(turn in HW worksheet up front at beginning of class –late after the first few minutes of class)
Review Mole & Gram conversions: Show your work:
1. How many moles are in g of CaO?
2. How many grams are in 4.5 moles of Sodium?

18. 1/12 Other Mole conversions
Make the following conversions: SHOW ALL MATH WORK
3. How many atoms are in 2.5 moles of Aluminum nitride?
4. What is the volume of 2.5 moles of N2?
5. How many grams are in 3.25 x 1024 atoms of lead?

19. 1/12 Quizizz.com assignment:
Login using the code
For your name use: 8penny,w
your period #, first name & last initial

20. 4 Steps you must think through to set up unit conversions:
1) pick out # unit & compound to set up bracket
2) move the unit & compound you start with down to bottom right of bracket
3) put on the top bracket the unit you are asked to solve for
4) Plug in #’s to make the “equivalence ratio”, to make the top & bottom to equal each other
Unit asked to solve for & same cpd started with
# Given unit cpd # = #
unit cpd you started with 1

21. 1/16 1. What all does 1 mole equal?
2. How many moles are in 8.25 x 1023 atoms of aluminum?
3. How many atoms are in g of sodium nitride?

22. Write specific goals on the index card for the following:
1) classes
2) attendance
3) college

23. 1/16 Mixed up Mole Conversions
Make the following conversions: SHOW ALL MATH WORK
How many grams in 5.5 moles of potassium oxide?
2. How many moles are there in 115 g of dinitrogen dioxide?
3. How many atoms are in 3.25 moles of sodium nitride?
4. What is the volume of 2.5 moles of O2?

24. 1/17 More Mole Conversions.
Make the following conversions: SHOW ALL MATH WORK
1. How many molecules are there in 555 g of CO2?
2. What is the volume of 2.5 moles of Ne gas?
3. How many atoms are in 585,225 g of lead?

25. Add as #7 on your quiz today:
7. How many grams does a C3H8 (propane) gas tank weigh when it is filled with 7500 L of C3H8?

26. 1/17 Do the following calculations – show your work:
How many grams are in 8.22 x 1025 molecules of CO2?
How many liters are in 8.22 x 1025 molecules of CO2?
How many moles are in 8.22 x 1025 molecules of CO2?

27. 1/18 % Composition
Use the pack of color paper to discuss in your group how you would determine the % composition of the different colors in the pack.
Write your steps down on the paper provided & then solve for the % composition of each color in your package

28. 1/19 Turn in % composition ws on front table
Do “Mixed Mole Conversions (1/19)” Quiz on Moodle
You need to write out your problems in your composition book to set them up correctly.

29. % Composition
Equation: Individual elements mass (g) X 100 = % Total formula mass of cpd (g) Example: find the % of each element in MgCl g Mg x 100 = % Mg g MgCl g Cl2 x 100 = % Cl

30. We need your help reiterating and enforcing district and Eagle expectations.
All students should enter your classroom with their ID on every period every day – if they don’t have one send them to get one
Students can’t wear hats, hoods, toboggans in the building unless it is a spirit day – please ask them to take them off
Students should not be using cell phones during class unless for school work (teacher may request phones to be put away to help students focus on learning in our classrooms)
Students are not to stand at your door before bell rings
No PDA and students shouldn’t be kissing (we agreed that a simple hug was okay but nothing more)

31. 1/22 Empirical Formula What if you are given the % composition of the elements in a compound and now need to figure out what the compound looks like, what do you do?
STEPS:
1) take out of % by assuming this is out of a 100 g by just removing the % sign & put on a gram unit to replace the % sign
2) Now that it is in gram solve for how many moles are in each element using the formula mass of the element from the periodic table
3) Compare the mole answers & divide all by the smallest answer to get a whole number & these will be the subscripts used in the chemicals empirical formula of the compound (if you get a .5 then you will need to multiply all by 2 since you must use whole numbers in compounds)
Example: What is the chemical formula when there is 88.8% copper; 11.2% oxygen?
Copy the steps down in your composition book

32. What are the empirical formulas for the following % compositions
What are the empirical formulas for the following % compositions? Show your work in your composition book:
40% carbon; 6.7% hydrogen; 53.3% oxygen
92.3% carbon; 7.7% hydrogen
70.0% iron; 30.0% oxygen

33. Show your work. Find the molecular formulas using the % composition:
4) 5.88% hydrogen; 94.12% oxygen
5) 38.7% chlorine; 61.3% fluorine
6) 7.19% phosphorus; 92.81% bromine
7) 30.4% nitrogen; 69.6% oxygen