- Students were taught how to convert between moles and atoms/molecules using Avogadro's number as a conversion factor.
- Examples were worked through as a class to show the 3 step process: 1) write starting unit, 2) write conversion factor with starting units on bottom, 3) cancel units and multiply.
- Students then worked in pairs on whiteboard practice questions applying the method.
- An exit slip quiz assessed students' understanding of key concepts like Avogadro's number and performing mole-to-particle conversions.
- Homework assigned was to finish the practice question worksheet.
This lesson will help you know how atoms of each element are arranged in an orbital and where atoms are exactly located that give distinct characteristics to the element.
This lesson will help you know how atoms of each element are arranged in an orbital and where atoms are exactly located that give distinct characteristics to the element.
Acids, bases and salts according to the syllabus of CAIE and IGCSEjaveriakhan123
It gives a detailed overview on the concept of acid, bases and salts which includes the preparation of salts and the test for the identification of cations.
Worksheet for working out the Percentage by Mass of various compounds. Pupils will need a data sheet or a list of relative atomic masses to be able to complete the questions.
Acids, bases and salts according to the syllabus of CAIE and IGCSEjaveriakhan123
It gives a detailed overview on the concept of acid, bases and salts which includes the preparation of salts and the test for the identification of cations.
Worksheet for working out the Percentage by Mass of various compounds. Pupils will need a data sheet or a list of relative atomic masses to be able to complete the questions.
This PowerPoint covers Stoichiometry and the concept of the Mole for my CHEM 2800 class that teaches elementary education majors the basics of chemistry
This activity is designed to introduce a convenient unit used by.docxhowardh5
This activity is designed to introduce a convenient unit used by chemists and to illustrate uses of the unit.
Part I: What Is a Mole And Why Are Chemists Interested in It?
Counting things is a normal part of everyday life. How many days left until vacation? How many eggs do I need for the recipe? If large numbers of things are involved, we use grouping
strategies to make the numbers easier to manage. For example, 4 more
weeks
until vacation, tells
us that there are twenty-eight days. One
dozen
eggs is the common way of expressing the quantity
12.
Half of a dozen of anything would be 6 units. One
gross
is 144 items (12 dozen) and a
ream
of paper contain 500 sheets.
Chemist are faced with a unique problem when dealing with numbers of atoms or molecules. The particles are so small that any amount of them that we are able to physically handle contains a number of particles so large that there is nothing else in our experience that contains so many units. This
incredibly
large number calls for a special counting group -
the MOLE.
A
MOLE
is
6.022
x
1023
particles
. This is often referred to as
Avogadro=s
number
. Let=s make sure we understand how big this is. One mole of the element carbon has a mass of 12.01 grams. The smallest particle of an element is an atom. So one mole of carbon contains 602,200,000,000,000,000,000,000 atoms of carbon.
Look for the element carbon on the periodic table. Do you notice anything special about the value 12.01? Explain
The mass of one mole of the element magnesium is 24.30 grams. How many atoms does a sample of magnesium with a mass of 24.30 grams contain?
Stated in general terms, the mass of one mole of any element is equal to the
of that element expressed in grams. The mass of a mole of any element can be found by looking on .
The mass of 0.5000 moles of carbon is and contains
atoms of carbon.
Remember when dividing numbers written in scientific notation the number portion is divided
normally and the exponents are subtracted.
6.022x1023
divided by 2 is the same as 6.022 x1023/2
x
100.
So the answer is found by dividing 6.022 by 2 = 3.011 and the subtracting exponent 0
from exponent 23.
The answer in scientific notation is 3.011x1023
atoms
of carbon.
Calculator tip
: for exponential notation use the EE or EXP key (not 10^)
If you have a bottle containing 8.10 grams of magnesium, how many Mg atoms are present in the bottle? Show your work. What is different about this problem compared to the last one involving carbon?
Remember that some elements, when alone, exist in the form of diatomic molecules: H2, O2, N2, I2, F2, Cl2, Br2, Their smallest piece is a molecule containing two atoms. If one mole of oxygen were required for an experiment you would be using O2 the gas. One mole of O2 would have a mass of
and contain particles (molecules).
The characteristic unit of the compound CO2 is a molecule. Each CO2 molecule has atoms. In order to find the mass .
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June 3, 2024 Anti-Semitism Letter Sent to MIT President Kornbluth and MIT Cor...Levi Shapiro
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• The Committee on Education and the Workforce has been investigating your institution since December 7, 2023. The Committee has broad jurisdiction over postsecondary education, including its compliance with Title VI of the Civil Rights Act, campus safety concerns over disruptions to the learning environment, and the awarding of federal student aid under the Higher Education Act.
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• The Committee on Ways and Means has been investigating several universities since November 15, 2023, when the Committee held a hearing entitled From Ivory Towers to Dark Corners: Investigating the Nexus Between Antisemitism, Tax-Exempt Universities, and Terror Financing. The Committee followed the hearing with letters to those institutions on January 10, 202
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Chapter 3 - Islamic Banking Products and Services.pptx
12 1 How Many Atoms
1. Launch: 12/1
Grab your binder and immediately take a seat!
Place homework (practice questions), binder paper, and
a pen/pencil on your desk.
Today’s Objective: I can convert between moles and
atoms using Avogadro’s number as a conversion
factor
Tonight’s HW: Finish the back of the practice
question worksheet
2. Launch 12/1
4. How many grams of NH3 are there in 2 moles of NH3?
a. 1.00 moles
b. 14.01 grams
c. 17.04 grams
d. 34.08 grams
3. Launch 12/1
5. How many moles of N2 are there in 14.01g of N2?
a. .5 moles
b. 2 mole
c. 14.01 moles
d. 28.02 moles
6. Review: How many moles?
Molar mass
used to convert between grams and moles
units = grams/mole
can be shown as a fraction
Molar mass of H2 = 2.02 g/mol
2.02 grams 1 mole
or
1 mole 2.02 grams
7. How many atoms?
Avogadro’s number… ..or particles, or molecules
is equal to 6.02 X 1023 atoms/mol
can be used to convert between moles and atoms
6.02 X 1023 atoms 1 mole
or
1 mole 6.02 X 1023 atoms
..or particles, or molecules
8. How many atoms?
There is a 3-step process for conversions:
1. Write down the starting unit.
2. Write the conversion factor with the starting units on
the bottom.
3. Cancel like terms and multiply across the top and
bottom.
9. Example #1
How many atoms are there in 2 moles of carbon (C)?
Step #1: Write down the starting unit.
2 moles
10. Example #1
How many atoms are there in 2 moles of carbon (C)?
Step #2: Write conversion factor with the starting units on the
bottom.
6.02 X 1023 atoms
2 moles X =
1 mole
11. Example #1
How many atoms are there in 2 moles of carbon (C)?
Step #3: Cancel like terms and multiply across the top and
bottom.
Ignore
6.02 X 1023 atoms 2 X 6.02 X 1023 atoms
2 moles X =
1 mole 1 +1
= 12.04 X 1023 atoms
= 1.204 X 1024 atoms
12. Example #2
How many atoms are there in 1.5 moles of CO2?
Step #1: Write down the starting unit.
1.5 moles
13. Example #2
How many atoms are there in 1.5 moles of CO2?
Step #2: Write conversion factor with the starting units on the
bottom.
6.02 X 1023 atoms
1.5 moles X =
1 mole
14. Example #2
How many atoms are there in 1.5 moles of CO2?
Step #3: Cancel like terms and multiply across the top and
bottom.
Ignore
6.02 X 1023 atoms 1.5 X 6.02 X 1023 atoms
1.5 moles X =
1 mole 1
= 9.03 X 1023 atoms
15. Example #3
How many moles are there in 3.01 X 1023 molecules of CO2?
Step #1: Write down the starting unit.
3.01X1023 molecules
16. Example #3
How many molecules are there in 1.5 moles of CO2?
Step #2: Write conversion factor with the starting units on the
bottom.
1 mol
3.01X1023 molecules X =
6.02X1023 molecules
17. Example #3
How many molecules are there in 1.5 moles of CO2?
Step #3: Cancel like terms and multiply across the top and
bottom.
1 mol 3.01 X 1 mol
3.01X1023 molecules X =
6.02X10 23 molecules 6.02
= .5 mol
18. Whiteboards
Work in pairs
Trade-off marker every question
You have 60 seconds to solve the question
Show all of your work!
Don’t forget units!
Lift board only when prompted
24. Exit Slip
1. What is Avogadro’s number?
a. 6.02 X 1024 atoms
b. 6.02 X 1023 atoms
c. 3.01 X 1023 atoms
d. 1.2 X 1024 atoms
25. Exit Slip
2. Which of the following shows the correct way to
calculate the number of atoms in 2 moles of O2?
32.00 grams
a. 16 moles X
1 mole
1 mole
b. 2 moles X 16.00 grams
1 atoms
c. 2 moles X 6.02 X 1023 moles
6.02 X 1023 atoms
d. 2 moles X
1 mole
26. Exit Slip
3. How many atoms of sodium (Na) are in 1 mole?
a. 3.01 X 1023 atoms
b. 6.02 X 1023 atoms
c. 12.04 X 1023 atoms
d. 1.204 X 1024 atoms
27. Exit Slip
4. How many molecules of C3OH are in .5 moles?
a. 3.01 X 1023 molecules
b. 6.02 X 1023 molecules
c. 9.03 X 1023 molecules
d. 1.204 X 1024 atoms
28. Exit Slip
5. If there are 1.204 X 1024 particles of gold (Au), how
many moles are there?
a. .5 moles
b. 1 mole
c. 2 moles
d. 4 moles