Easy way to understand moles. 1 mole has the same number of particles present in 12 grams of Carbon-12. Carbon-12 is an isotope of carbon which is taken as standard. Mass of 1 mole of atoms = Atomic mass, Mass of 1 mole of molecules = molecular mass.
Easy way to understand moles. 1 mole has the same number of particles present in 12 grams of Carbon-12. Carbon-12 is an isotope of carbon which is taken as standard. Mass of 1 mole of atoms = Atomic mass, Mass of 1 mole of molecules = molecular mass.
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9Shivam Parmar
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Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
MORE ABOUT MOLE
WHAT IS THE MOLE CONCEPT?
MORE ABOUT MOLE CONCEPT
RELATIONSHIP BETWEEN MOLE, AVOGADRO NUMBER, AND MASS
AVOGADRO NUMBER
FEW MORE EXAMPLES
Every topic of this chapter is well written concisely and visuals will help you in understanding and imagining the practicality of all the topics.
By Shivam Parmar (PPT Designer)
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9Shivam Parmar
I have expertise in making educational and other PPTs. Email me for more PPTs at a very reasonable price that perfectly fits in your budget.
Email: parmarshivam105@gmail.com
Chapter - 3, Atoms And Molecules, (Mole Concept) Science, Class 9
INTRODUCTION
MORE ABOUT MOLE
WHAT IS THE MOLE CONCEPT?
MORE ABOUT MOLE CONCEPT
RELATIONSHIP BETWEEN MOLE, AVOGADRO NUMBER, AND MASS
AVOGADRO NUMBER
FEW MORE EXAMPLES
Every topic of this chapter is well written concisely and visuals will help you in understanding and imagining the practicality of all the topics.
By Shivam Parmar (PPT Designer)
We all have good and bad thoughts from time to time and situation to situation. We are bombarded daily with spiraling thoughts(both negative and positive) creating all-consuming feel , making us difficult to manage with associated suffering. Good thoughts are like our Mob Signal (Positive thought) amidst noise(negative thought) in the atmosphere. Negative thoughts like noise outweigh positive thoughts. These thoughts often create unwanted confusion, trouble, stress and frustration in our mind as well as chaos in our physical world. Negative thoughts are also known as “distorted thinking”.
2024.06.01 Introducing a competency framework for languag learning materials ...Sandy Millin
http://sandymillin.wordpress.com/iateflwebinar2024
Published classroom materials form the basis of syllabuses, drive teacher professional development, and have a potentially huge influence on learners, teachers and education systems. All teachers also create their own materials, whether a few sentences on a blackboard, a highly-structured fully-realised online course, or anything in between. Despite this, the knowledge and skills needed to create effective language learning materials are rarely part of teacher training, and are mostly learnt by trial and error.
Knowledge and skills frameworks, generally called competency frameworks, for ELT teachers, trainers and managers have existed for a few years now. However, until I created one for my MA dissertation, there wasn’t one drawing together what we need to know and do to be able to effectively produce language learning materials.
This webinar will introduce you to my framework, highlighting the key competencies I identified from my research. It will also show how anybody involved in language teaching (any language, not just English!), teacher training, managing schools or developing language learning materials can benefit from using the framework.
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The French Revolution, which began in 1789, was a period of radical social and political upheaval in France. It marked the decline of absolute monarchies, the rise of secular and democratic republics, and the eventual rise of Napoleon Bonaparte. This revolutionary period is crucial in understanding the transition from feudalism to modernity in Europe.
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2. The Mole
• A counting unit
• Similar to a dozen (12), except instead
of 12, it’s 602 billion trillion
602,000,000,000,000,000,000,000
• 6.02 X 1023 (in scientific notation)
• This number is named in honor of
Amedeo Avagadro (1776 – 1856), who
studied quantities of gases and
discovered that no matter what the
gas was, there were the same number
of molecules present
13. 4
Just How Big is a Mole?
• Enough soft drink cans to cover the
surface of the earth to a depth of over
200 miles.
14. 4
Just How Big is a Mole?
• Enough soft drink cans to cover the
surface of the earth to a depth of over
200 miles.
• If you had Avogadro's number of
unpopped popcorn kernels, and
spread them across the United States
of America, the country would be
covered in popcorn to a depth of over
9 miles.
15. 4
Just How Big is a Mole?
• Enough soft drink cans to cover the
surface of the earth to a depth of over
200 miles.
• If you had Avogadro's number of
unpopped popcorn kernels, and
spread them across the United States
of America, the country would be
covered in popcorn to a depth of over
9 miles.
• If we were able to count atoms at the
rate of 10 million per second, it would
take about 2 billion years to count the
atoms in one mole.
16. How Big is a Mole?
One mole of marbles would cover the entire Earth
(oceans included) for a depth of three miles.
17. How Big is a Mole?
One mole of marbles would cover the entire Earth
(oceans included) for a depth of three miles.
18. How Big is a Mole?
One mole of marbles would cover the entire Earth
(oceans included) for a depth of three miles.
One mole of $100 bills stacked one on top of another
would reach from the Sun to Pluto and back 7.5 million
times.
19. How Big is a Mole?
One mole of marbles would cover the entire Earth
(oceans included) for a depth of three miles.
One mole of $100 bills stacked one on top of another
would reach from the Sun to Pluto and back 7.5 million
times.
It would take light 9500 years to travel from the
bottom to the top of a stack of 1 mole of $1 bills.
38. How small are atoms?
• There are more atoms in one gram of salt than
grains of sand on all the beaches of all the
oceans in all the world.
39.
40. • Just one granule of sugar contains 1 x 10 17
molecules
41. • Just one granule of sugar contains 1 x 10 17
molecules
42. • Just one granule of sugar contains 1 x 10 17
molecules
43. • Just one granule of sugar contains 1 x 10 17
molecules
• Each time you take a breath of air, you inhale
about 2 x 1022 molecules of nitrogen and 5 x
10 21 molecules of oxygen.
44.
45. • In chemistry we don’t work with single atoms
or molecules because they are too small to be
weighed or measured
46. • In chemistry we don’t work with single atoms
or molecules because they are too small to be
weighed or measured
47. • In chemistry we don’t work with single atoms
or molecules because they are too small to be
weighed or measured
• We have to work with LOTS of atoms in
order to measure them
48. • In chemistry we don’t work with single atoms
or molecules because they are too small to be
weighed or measured
• We have to work with LOTS of atoms in
order to measure them
THAT’s WHERE THE
49. • In chemistry we don’t work with single atoms
or molecules because they are too small to be
weighed or measured
• We have to work with LOTS of atoms in
order to measure them
THAT’s WHERE THE
MOLE COMES IN!
55. Examining Molar Relationships in
Balanced Equations
6 CO2 + 12 H2O → 6 O2 + C6H12O6 +6 H20
Balanced equations
–Law of conservation of mass / matter
56. Examining Molar Relationships in
Balanced Equations
6 CO2 + 12 H2O → 6 O2 + C6H12O6 +6 H20
Balanced equations
–Law of conservation of mass / matter
• ATOMS are not created or destroyed during a chemical reaction,
they are only rearranged to form new substances.
57. Examining Molar Relationships in
Balanced Equations
6 CO2 + 12 H2O → 6 O2 + C6H12O6 +6 H20
Balanced equations
–Law of conservation of mass / matter
• ATOMS are not created or destroyed during a chemical reaction,
they are only rearranged to form new substances.
• # atoms on reactant side = # atoms on product side
58. Examining Molar Relationships in
Balanced Equations
6 CO2 + 12 H2O → 6 O2 + C6H12O6 +6 H20
Balanced equations
–Law of conservation of mass / matter
• ATOMS are not created or destroyed during a chemical reaction,
they are only rearranged to form new substances.
• # atoms on reactant side = # atoms on product side
– The Coefficient for each molecule tells you how many
“moles” of the molecule are in the reaction.
59. Examining Molar Relationships in
Balanced Equations
6 CO2 + 12 H2O → 6 O2 + C6H12O6 +6 H20
Balanced equations
–Law of conservation of mass / matter
• ATOMS are not created or destroyed during a chemical reaction,
they are only rearranged to form new substances.
• # atoms on reactant side = # atoms on product side
– The Coefficient for each molecule tells you how many
“moles” of the molecule are in the reaction.
• For example: 6 CO2 = 6 moles of CO2
60. Learning Check #1
Suppose we invented a new unit called a rapp.
One rapp contains 8 objects.
1. How many paper clips in 1 rapp?
a) 1 b) 4 c) 8
2. How many oranges in 2.0 rapp?
a) 4 b) 8 c) 16
3. How many rapps contain 40 gummy bears?
a) 5 b) 10 c) 20
61. Learning Check #1 - Answers
Suppose we invented a new unit called a rapp.
One rapp contains 8 objects.
1. How many paper clips in 1 rapp?
a) 1 b) 4 c) 8
2. How many oranges in 2.0 rapp?
a) 4 b) 8 c) 16
3. How many rapps contain 40 gummy bears?
a) 5 b) 10 c) 20
64. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
65. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
66. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
67. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
• 1 dozen Al atoms = 12 Al atoms
68. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
• 1 dozen Al atoms = 12 Al atoms
• 1 mole of Al atoms = 6.02 X 1023 atoms
69. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
• 1 dozen Al atoms = 12 Al atoms
• 1 mole of Al atoms = 6.02 X 1023 atoms
Note that the NUMBER is always the same, but
the MASS is very different!
70. The Mole
• 1 dozen cookies = 12 cookies
• 1 mole of cookies = 6.02 X 1023 cookies
• 1 dozen cars = 12 cars
• 1 mole of cars = 6.02 X 1023 cars
• 1 dozen Al atoms = 12 Al atoms
• 1 mole of Al atoms = 6.02 X 1023 atoms
Note that the NUMBER is always the same, but
the MASS is very different!
Mole is abbreviated mol (gee, that’s a lot
quicker to write, huh?)
71. A Mole of Particles
Contains 6.02 x 10 23 particles
72. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C
1 mole H2O
1 mole NaCl
73. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C
1 mole H2O
1 mole NaCl
74. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O
1 mole NaCl
75. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 10 23 H2O molecules
1 mole NaCl = 6.02 x 1023 NaCl “molecules”
76. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 10 23 H2O molecules
1 mole NaCl = 6.02 x 1023 NaCl “molecules”
(technically, ions not molecules)
6.02 x 1023 Na + ions and
77. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 10 23 H2O molecules
1 mole NaCl = 6.02 x 1023 NaCl “molecules”
(technically, ions not molecules)
6.02 x 1023 Na + ions and
6.02 x 1023 Cl– ions
78. A Mole of Particles
Contains 6.02 x 10 23 particles
1 mole C = 6.02 x 1023 C atoms
1 mole H2O = 6.02 x 10 23 H2O molecules
1 mole NaCl = 6.02 x 1023 NaCl “molecules”
(technically, ions not molecules)
6.02 x 1023 Na + ions and
6.02 x 1023 Cl– ions
Note that a particle could be an atom
OR a molecule!
79. Avogadro’s Number as
Conversion Factor
6.02 x 1023 particles
1 mole
or
1 mole
6.02 x 1023 particles
Note that a particle could be an atom OR a molecule!
80. Learning Check #2
1. Number of atoms in 1.0 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2. Number of moles of S in 6.02 X 1023 S atoms
a) 1.0 mole S atoms
b) 6.02 mole S atoms
c) 1 x 1023 mole S atoms
81. Learning Check #2
1. Number of atoms in 1.0 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2. Number of moles of S in 6.02 X 1023 S atoms
a) 1.0 mole S atoms
b) 6.02 mole S atoms
c) 1 x 1023 mole S atoms
82. Learning Check #2 - Answers
1. Number of atoms in 1.0 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2. Number of moles of S in 6.02 X 1023 S atoms
a) 1.0 mole S atoms
b) 6.02 mole S atoms
c) 1 x 1023 mole S atoms
83. Learning Check #2 - Answers
1. Number of atoms in 1.0 mole of Al
a) 500 Al atoms
b) 6.02 x 1023 Al atoms
c) 3.01 x 1023 Al atoms
2. Number of moles of S in 6.02 X 1023 S atoms
a) 1.0 mole S atoms
b) 6.02 mole S atoms
c) 1 x 1023 mole S atoms
87. Molar Mass
• The Mass of 1 mole in grams
• Equal to the numerical value of the average
atomic mass. This number is found on the
periodic table, below the symbol for each
element.
88. Molar Mass
• The Mass of 1 mole in grams
• Equal to the numerical value of the average
atomic mass. This number is found on the
periodic table, below the symbol for each
element.
89. Molar Mass
• The Mass of 1 mole in grams
• Equal to the numerical value of the average
atomic mass. This number is found on the
periodic table, below the symbol for each
element.
90. Molar Mass
• The Mass of 1 mole in grams
• Equal to the numerical value of the average
atomic mass. This number is found on the
periodic table, below the symbol for each
element.
91. Molar Mass
• The Mass of 1 mole in grams
• Equal to the numerical value of the average
atomic mass. This number is found on the
periodic table, below the symbol for each
element.
92. Molar Mass
The Atomic Mass # does not have units in the
periodic table. Often, chemists use “amu” for the
atomic mass unit. To determine the molar mass,
we change “amu” into “grams/mole”
1 amu = 1 gram check on your
periodic table!!!
1 mole
1 mole of He atoms = 4.0 g
1 mole of C atoms = 12.0 g
1 mole of Mg atoms = 24.3 g
1 mole of Cu atoms = 63.5 g
93. Learning Check #3
Find the molar mass for the following elements:
(round to the tenths place for decimals)
A. 1 mole of Br atoms
B. 1 mole of Sn atoms
C. 2 moles of C atoms
94. Learning Check #3 - Answers
Find the molar mass for the following elements:
(round to the tenths place for decimals)
A. 1 mole of Br atoms
B. 1 mole of Sn atoms
C. 2 moles of C atoms
95. Learning Check #3 - Answers
Find the molar mass for the following elements:
(round to the tenths place for decimals)
A. 1 mole of Br atoms = 79.9 g/mol
B. 1 mole of Sn atoms
C. 2 moles of C atoms
96. Learning Check #3 - Answers
Find the molar mass for the following elements:
(round to the tenths place for decimals)
A. 1 mole of Br atoms = 79.9 g/mol
B. 1 mole of Sn atoms = 118.7 g/mol
C. 2 moles of C atoms
97. Learning Check #3 - Answers
Find the molar mass for the following elements:
(round to the tenths place for decimals)
A. 1 mole of Br atoms = 79.9 g/mol
B. 1 mole of Sn atoms = 118.7 g/mol
C. 2 moles of C atoms = 12 g/mole * 2 moles
= 24 g/mol
98. Molar Mass of Molecules & Compounds
ADD UP THE MASS FROM ALL ATOMS IN THE
MOLECULE !!!!!
***The subscript tells you how many atoms for
each element are present in the molecule
1 mole of the molecule CaCl2 = 111.1 g/mol
HOW????
1 mole Ca x 40.1 g/mol
+ 2 moles Cl x 35.5 g/mol = 111.1 g/mol CaCl
100. Learning Check #4 - Answers
What is the Molar Mass of the molecule
K2O?
****Units = g/mol
2 moles of K = 39 g/mol * 2 = 78 g/mol
+ 1 mole of O = 16 g/mol
TOTAL = 94 g/mol !!!!
102. What is Dimensional Analysis?
Dimensional analysis is just a fancy name
for a method of calculating that:
103. What is Dimensional Analysis?
Dimensional analysis is just a fancy name
for a method of calculating that:
104. What is Dimensional Analysis?
Dimensional analysis is just a fancy name
for a method of calculating that:
1. uses numbers in the form of fractions.
105. What is Dimensional Analysis?
Dimensional analysis is just a fancy name
for a method of calculating that:
1. uses numbers in the form of fractions.
2. lets us convert from one type of unit
measurement to another.
106. What is Dimensional Analysis?
Dimensional analysis is just a fancy name
for a method of calculating that:
1. uses numbers in the form of fractions.
2. lets us convert from one type of unit
measurement to another.
3. In chemistry, this lets us convert from
moles to grams or visa-versa
107. What is a Unit?
A unit is something that gives definition
to a numerical value, quantity, or
measurement.
• Length : meters, centimeters, feet, inches,
miles, kilometers
• Mass : Kilograms, grams, pounds
• Time : hours, minutes, seconds, days,
months
• Volume : cups, teaspoons, liters,
milliliters, gallons, quarts
• Currency: dollars, cents, dimes
110. Conversion Factors
Conversion factors can be written in 2
ways:
The unit you want goes on top or the
numerator and the unit you want to
cancel goes on the bottom or
denominator.
111. Converting Moles and Grams
Aluminum is often used for the structure
of light-weight bicycle frames. How many
grams of Al are in 3.00 moles of Al?
3.00 moles Al ? g Al
114. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
115. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
116. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
117. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
118. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
119. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
120. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
3. Setup 3.00 moles Al x 27.0 g Al
121. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
3. Setup 3.00 moles Al x 27.0 g Al
1 mole Al
122. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
3. Setup 3.00 moles Al x 27.0 g Al
1 mole Al
4. Math 3 * 27/1 = 81
123. 1. Molar mass of Al 1 mole Al = 27.0 g Al
2. Conversion factors for Al
27.0 g Al or 1 mol Al
1 mol Al 27.0 g Al
Why? Because I want to “cancel” mol and be left with g. g must be on top.
3. Setup 3.00 moles Al x 27.0 g Al
1 mole Al
4. Math 3 * 27/1 = 81
5. Answer = 81.0 g Al
Editor's Notes
To play the movies and simulations included, view the presentation in Slide Show Mode.\n
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6.02 x 1023 softballs = volume of Earth\n6.02 x 1023 Olympic shot puts = mass of Earth\n6.02 x 1023 atoms H laid side by side would encircle Earth ~1,000,000 times\n
6.02 x 1023 softballs = volume of Earth\n6.02 x 1023 Olympic shot puts = mass of Earth\n6.02 x 1023 atoms H laid side by side would encircle Earth ~1,000,000 times\n
6.02 x 1023 softballs = volume of Earth\n6.02 x 1023 Olympic shot puts = mass of Earth\n6.02 x 1023 atoms H laid side by side would encircle Earth ~1,000,000 times\n
6.02 x 1023 softballs = volume of Earth\n6.02 x 1023 Olympic shot puts = mass of Earth\n6.02 x 1023 atoms H laid side by side would encircle Earth ~1,000,000 times\n
6.02 x 1023 softballs = volume of Earth\n6.02 x 1023 Olympic shot puts = mass of Earth\n6.02 x 1023 atoms H laid side by side would encircle Earth ~1,000,000 times\n