1. 1. Print the Objective: The synthesis of dihydrogen monoxide
Welcome to class. My name is Charlie Arbuiso and I will be your chemistry teacher.
Copy the objective, and get ready to learn…
Put the other papers away now.
1. Print the Objective: The synthesis of dihydrogen monoxide

2. Since it’s a chemistry class, let’s examine what we are dealing with…
2. dihydrogen monoxide =
3. Its formula is written as ____________________
4. ____ is the symbol for ________________________
5. ____ is the symbol for _________________________
6. The Word equation for this reaction is:
______________ and ________________ yields _________________________
7. The Skeleton equation (proper chemistry symbols, but not balanced yet):
_______ _______ __________________

3. Since it’s a chemistry class, let’s examine what we are dealing with…
2. dihydrogen monoxide = 2 hydrogen atoms and 1 oxygen atom
3. Its formula is written as H2O (note the “2” is a subscript!)
4. H is the symbol for Hydrogen
5. Ois the symbol for oxygen
6. HYDROGEN and OXYGEN yields DIHYDROGEN MONOXIDE (WATER)
7. The Skeleton equation (proper chemistry symbols, but not balanced yet):
H + O H2O

4. Something that you didn’t know, and couldn’t know is that both hydrogen and oxygen are atoms that are not happy being single. They exist in nature in the pure form only as paired partners, like H2 and O2. Seven atoms are like this. You’ll learn them.
So let’s fix this symbol equation to a skeleton equation:
H O H2O
Math counts. Keeping track of atoms counts. This equation is not “balanced” Not balanced means BAD. We need to fix that.
(you should not be able to do this, so don’t sweat, just copy for now)
H O H2O
This is called a balanced chemical equation, the same amount of atoms on the start side of the reaction, and at the end copy this : (4 H atoms + 2 O atoms form into the same 4 H’s + 2 O’s but they are combined differently – that’s chemistry!)

5. Something that you didn’t know, and couldn’t know is that both hydrogen and oxygen are atoms that are not happy being single. They exist in nature in the pure form only as paired partners, like H2 and O2. Seven atoms are like this. You’ll learn them.
So let’s fix this symbol equation to a skeleton equation:
H O H2O
Math counts. Keeping track of atoms counts. This equation is not “balanced” Not balanced means BAD. We need to fix that.
(you should not be able to do this, so don’t sweat, just copy for now)
H O H2O
This is called a balanced chemical equation, the same amount of atoms on the start side of the reaction, and at the end copy this : (4 H atoms + 2 O atoms form into the same 4 H’s + 2 O’s but they are combined differently – that’s chemistry!)

6. Now we need to add phase symbols, there are three phases of matter in our course What are phase symbols? ________________
12. Rewrite this balanced equation with phase symbols now.
2H O H2O
H2 gas
+ O2 gas in the air

7. Now we need to add phase symbols, there are three phases of matter in our course What are phase symbols? They tell if the matter is solid, liquid or gas (there’s a few more, but not today, okay?)
12. Rewrite this balanced equation with phase symbols now.
2H2(G) O2(G) H2O(G)
H2 gas
+ O2 gas in the air

8. #13

9. You will not get hurt, but it is rather loud. BANG!
This will be a fun, memorable chemical reaction.
14. It’s called the synthesis of dihydrogen monoxide, or wata.
It will happen very fast, and will release lots of energy. Lots.
So much I have to teach you safety now, before we can continue.
You will not get hurt, but it is rather loud. BANG!
15. What do we call a chemical reaction that gives off or emits energy?

10. You will not get hurt, but it is rather loud. BANG!
This will be a fun, memorable chemical reaction.
It’s called the synthesis of dihydrogen monoxide, or wata.
It will happen very fast, and will release lots of energy. Lots.
So much I have to teach you safety now, before we can continue.
You will not get hurt, but it is rather loud. BANG!
15. What do we call a chemical reaction that gives off or emits energy? EXOTHERMIC

11. 2H2(G) + O2(G) 2H2O(G) + energy
16. Let’s write out the fully balanced thermochemical reaction…
2H2(G) + O2(G) H2O(G) + energy
17 (copy this) The synthesis of water is exothermic.
Hydrogen and oxygen are elements.
Water is a compound.
Chemistry is the study of matter and how matter acts and reacts.

12. Homework:
1. Read the handout for the course 2. Fill in the student data form, with parents
3. Bring back the student data form, filled in, and with your parent’s signature
4. Get a loose-leaf binder and some paper NO SPIRAL NOTEBOOKS for chemistry.
5. Tell your family about making wata and how much you will love this class.

13. Measurement Class 1
OBJECTIVE: To learn to distinguish between qualitative and quantitative measures, and between error and percent error; finally, to calculate percent error.

14. Paper is cheap. Knowledge is valuable.
Let’s have some fun, guess my weight.
Measure my mass, using your eyes and mind as your tools.
In science we measure (and estimate) all the time.
18. Write your answer down.

15. What were your guesses? Fast and loud.
Your eye “measurements” in pounds
19. On the bathroom scale, what is the ACTUAL mass of your teacher in pounds? ______
20. Measurements that are close to the correct weight are called ______________
21. Measurements that are close together (close to correct or not) are called: ____________
22. In our class we will measure our best to be _______________________

16. What were your guesses? Fast and loud.
Your eye “measurements” in pounds
19. On the bathroom scale, what is the ACTUAL mass of your teacher in pounds?
20. Measurements that are close to the correct weight are called ACCURATE
21. Measurements that are close together (close to correct or not) are called: PRECISE
22. In our class we will measure our best to be both ACCURATE + PRECISE

17. Accurate measurements are close to the actual or correct measure.
Precise measurements are close together.
23. If your measures are precise, your tool is ______________
Precise and accurate together is great.
Precise alone means that your tool is good.
24. Measurements that are not precise means that your ________________________________________ working well.

18. Accurate measurements are close to the actual or correct measure.
Precise measurements are close together.
23. If your measures are precise, your tool is CONSISTENT
Precise and accurate together is great.
Precise alone means that your tool is good.
24. Measurements that are not precise means that your tool (or you) are not working well.

19. 25. Qualitative measures: use only words
26. Quantitative measures use numbers with units
In chem we will sometimes use qualitative measures, but sometimes quantitative ones.
Examples:
27. Quantitative measure:
Mr. Arbuiso is ___________________
28. Qualitative measure:
Mr. Arbuiso is ____________________

20. 29. Error
How far away your measure is from accurate.
What was your “error” in measuring the mass of the teacher?
_______________________________________________________________________
It’s always a positive number (no need for a sign)
30. Error is the difference between your measure and the actual measure
Error = |Measured value – Actual value| (those lines indicate absolute value)

21. MV – AV AV %E = X 100% or Measured value – actual value actual value
31. Percent Error is much more important in our class. Percent error is how far off you were from your measured value to the actual value expressed as a percentage, with the +/- sign to indicate if you were over or under in your measuring.
32. Formula:
% Error =
Measured value – actual value actual value
X 100% or
MV – AV AV
%E =
X 100%
Calculate the % Error now.

22. What is your % Error? Let’s talk about your answers now.
33. Quick, measure with your eyes, how many inches it is to the top of the door. Write your measurement down.
The actual height is _________”.
Do your Error and %E NOW.
Write the formulas!

23. MV – AV AV
%E =
X 100%
Error = |Measured value – Actual value|

24. 34. Standard Units in our class are:
Length: METER, also millimeter, centimeter
Volume: LITER and MILLILITER
Mass: GRAM, and kilogram and milligram
Density: GRAMS/CENTIMETER CUBED or GRAMS PER MILLILETER
Temperature: KELVIN and CENTIGRADE (AKA celcius)
Time: SECONDS
Hand in your student data form now. Put everything, EVERYTHING, into the inbox.
Do not hand me stuff - put it into the inbox (unless it is money or chocolate chip cookies)

25. Measurement Class 2
35. OB: To determine what density is and how it’s measured; what are the two temperature scales in chemistry and how to convert one to another.

26. 36. MASS: The amount of “stuff” in something
Some background info…
36. MASS: The amount of “stuff” in something
37. VOLUME: The amount of space stuff takes up
38. WEIGHT: The affect of GRAVITY on a mass
39. Mass is a ______________________________
40. Weight ___________ depending upon __________________
41. Density is the mathematical relationship between _____ + ______ The formula you to learn is:

27. Some background info…
MASS: The amount of “stuff” in something
VOLUME: The amount of space stuff takes up
WEIGHT: The affect of GRAVITY on a mass
Mass is a CONSTANT
Weight VARIES depending upon STRENGTH OF GRAVITY (what planet you’re on)
Density is the mathematical relationship between MASS + VOLUME
The formula to learn is:
m V
D =

28. Units for density are most often:
43. __________________________ _________ or
44. __________________________ _________
45. __________= _____________ There is NO SUCH THING as an ______
If you don’t GET That, RAISE YOUR HAND AND ASK!

29. Units for density are most often:
43. grams/centimeter cubed g/cm3 or
44. grams/milliliter g/mL
cm3 = 1 mL, There is NO SUCH THING as an mL3
If you don’t GET That, RAISE YOUR HAND AND ASK!

30. Calculate the density of this metal.
47. A cube or metal has a mass of 4506 grams and it is 10.0 cm per side. (V = s x s x s)
Calculate the density of this metal.
(you must, must write the formula for each problem!)

31. 47. A cube or metal has a mass of 4506 grams and it is 10
47. A cube or metal has a mass of 4506 grams and it is 10.0 cm per side. (V = s x s x s)
Calculate the density of this metal.
(you must, must write the formula for each problem!)
m V
D = =
4506 g cm3
D = g/cm3

32. 48. What metal is it? (how could you know this?)

33. 48. What metal is it? (how could you know this?)
You could have memorized the density tables from a chem book, or you could just look it up! It’s titanium, Ti.

34. 49. FIVE pennies together have a mass of 14. 5 grams
49. FIVE pennies together have a mass of grams. Their total volume is 1.75 cm Calculate the density of the pennies.

35. 49. FIVE pennies together have a mass of 14. 5 grams
49. FIVE pennies together have a mass of grams. Their total volume is 1.75 cm Calculate the density of the pennies.
m V
D = =
14.5 g 1.75 cm3
D = 8.29 g/cm3

36. 50. Assuming the pennies are made up of pure copper, what is your % Error?

37. %E = -7.48% 3SF MV – AV AV %E = 8.29 – 8.96 g/cm3 8.96 g/cm3
50. Assuming the pennies are made up of pure copper, what is your % Error?
MV – AV AV
%E =
MV – AV AV
8.29 – 8.96 g/cm g/cm3
%E = =
%E = -7.48% SF

38. 51. Is your measured value for density UNDER or OVER the actual measurement for the density of copper? How would you KNOW?

39. -7.48% means it was close, (~ 8%) but it was not perfect.
51. Is your measured value for density UNDER or OVER the actual measurement for the density of copper? How would you KNOW?
A Negative percent error means YOUR measure is under the actual measurement.
-7.48% means it was close, (~ 8%) but it was not perfect.
It’s like getting about a 92% correct on a quiz.

40. 52. A bar of metal is 27.73 g and has volume of 4.70 cm3. Is it gold?

41. D = = m V D = 5.90 g.cm3 (3SF!) Is that the density of gold?
52. A bar of metal is g and has volume of 4.70 cm3. Is it gold?
m V
D = =
27.73 g 4.70 cm3
D = 5.90 g.cm (3SF!)
Is that the density of gold?
Check NOW! No guessing.

42. Temperature
We will not use Fahrenheit (normal for you) temperature in chemistry class.
53. We will use _______________ AKA _____________________
54. As well as ________________________
55. Fill in the chart carefully.

43. 55.
Water boils
Water freezes ?

44. Temperature
We will not use Fahrenheit (normal for you) temperature in science class.
We will use Centigrade AKA Celsius
As well as KELVIN F C K
Water boils
212°F °C K
32°F °C K
Water freezes
Absolute Zero
-273 C
O K

45. ____________ 56. Converting Kelvin to Centigrade Formula:
57. Calculate room temperature in Kelvin It’s 26.0°C today. (write the formula to calculate this)

46. 56. Converting Kelvin to Centigrade Formula:
K = C + 273

47. 57. Calculate room temperature in Kelvin. It’s 26. 0°C today
57. Calculate room temperature in Kelvin It’s 26.0°C today. (write the formula to calculate this)
K = C + 273
K = = 299 K
NOT DEGREES, it’s just Kelvins!
3 SF!

48. Measurement Class 3
58. OB: defining and understanding significant figures in measuring and in math equations.
Handout: The Significance of Significant Figures.

49. Significant figures are the numbers in our math that are important enough to count. They have real, or significant, value to the measurement.
We will measure so many things in chemistry, and we’ll use so many formulas, we need to learn how to deal with the numbers. The rules to significant figures is how we’ll do so.
Officially, significant figures is defined this way:
59. In a measurement, all numbers you know that you measured properly, plus one more estimated place, are significant.

50. You want to be sure that your measurements are as correct as possible
You want to be sure that your measurements are as correct as possible. You never want to round away how exact you can be. You also are not permitted to be magically more exact than your tool will let you.
For instance, 6 grams is not really the same as 6.0 grams, or 6.00 grams, or grams.
The are all measured to different levels of exactness.

51. If we are going to measure the temperature in this room right now, with our centigrade thermometer, let’s look at the tool now What temperature is it?
This tool indicates temperature in degrees centigrade. Whole degrees.

52. With tools that we read with our eyes, like a thermometer, or a ruler, we measure to the closest measure, then estimate out ONE more place. Our eyes can estimate one place, but not two or three more decimal points.
You can’t be “more accurate” than your tool let’s you. You should never give up how exact you can be, (don’t just say it’s 20 degrees centigrade, estimate to the tenth of a degree.
61. ____________________________

53. Let’s look over these rules on the back of this handout and see if we can’t figure out what this is all about.
For any measures:
Rule 1. Any digit 1-9 is going to be significant (it’s important and we need to keep track of how many SF we have).
62. How many significant figures in these temperatures? Which is most/least exact?
23°C °C °C

54. For any measures:
1. Any digit 1-9 is going to be significant (it’s important and we need to keep track of how many SF we have).
62. How many significant figures in these temperatures? Which is most/least exact?
23°C °C °C
2 SF SF SF
Least exact Most exact

55. RULE 2. If there’s a ZERO digit between significant figures, that is significant too (it’s not just a placeholder)
63. How many SF are in these measures?
101 grams joules ,445,567 kilocalories
110 grams joules ,445, 567 kilocalories
20,456,056 seconds

56. RULE 2. If there’s a ZERO digit between significant figures, that is significant too (it’s not just a placeholder)
63. How many SF are in these measures?
101 grams joules ,445,567 kilocalories
110 grams joules ,445, 567 kilocalories
20,456,056 seconds
3 SF
4 SF
8 SF
2 SF
3 SF
8 SF
8 SF

57. Rule 3. Zeros before SF are not significant
(they are placeholders)
64. How many SF in these measures?
kilograms _________
kPa ________
0.565 grams ___________

58. Rule 3. Zeros before SF are not significant
(they are placeholders)
64. How many SF in these measures?
kilograms 2SF
kPa 1 SF
0.565 grams SF

59. Rule 4. Zeros with a decimal point or without a decimal point
(the dot counts!)
150 grams has a zero at the end, and this means we are SURE of 1 one hundred, and 5 tens of grams, but not too sure of the rest. This means it has 2 SF
If the measure is 150. grams, that’s different.
We are now sure of all three digits. 3 SF

60. 65. What about these measures, how many sig figs?
250 atm _____ grams ______
55,678,900 seconds ________
14,050. cm _______

61. 48. What about these measures, how many sig figs?
250 atm 2 SF grams 3 SF
55,678,900 seconds 6 SF
14,050. cm 5 SF

62. RULE 5. Zeros at the end of a decimal number are significant, these ARE NOT PLACEHOLDERS, but indicate you measured to that decimal place and found it to contain NO digits How many SF in these 4 measures?
1.50 grams _______ seconds _______
98,754, g _______ days _______

63. RULE 5. Zeros at the end of a decimal number are significant, these ARE NOT PLACEHOLDERS, but indicate you measured to that decimal place and found it to contain NO digits How many SF in these 4 measures?
1.50 grams 3 SF seconds 2 SF
98,754, g 10 SF days 2 SF

64. RULE 6 - Unlimited Significant Figures Unlimited SF will be important whenever we use EQUALITIES, especially when converting from one unit to another.
67. For example, if we measured 1.5 pounds of butter and needed to convert it to grams, we’d use this EQUALITY or conversion factor: 1 pound = 454 grams
The calculator answer would be 681 g. This is NOT correct. Our equality has UNLIMITED SF, but our original measure does not, it has 2 SF. Our answer is limited to the LEAST amount of SF in the math.

65. 68. 1.00000… pounds = 454.000000… grams (to the nth degree)
That’s because
1 pound = 454 grams
Means
1.0 pounds = grams Or
… pounds = … grams (to the nth degree)
That last zero on the end would be significant, and all the zeros in between would be too, so equalities never “limit” SF.

66. 69. (copy all) In a math equations, the answers must not gain or lose SF. You can’t get MORE EXACT because you multiply or divide, nor should you round away how well you have measured.
70. If you measure your room to be 7.7 meters X 5.4 m, you’ll need a rug of m2
Not really.
If you only measure to 2 SF because that’s the limit of your tool, your answer can only have 2 SF.
Round the m2 to 42 m2 to be correct.

67. Last rule…
When using scientific notation, only the front part (the coefficient) has SF.
71. How many SF in this measure? x 1023 atoms has ___________ SF

68. Last rule…
When using scientific notation, only the front part (the coefficient) has SF.
71. How many SF n this measure? x 1023 atoms has SF, just the 6.02 part counts

69. Practice (talk together)
72. How many SF in these measures?
123 m _____ cm _____
0.345 g _____ seconds _____
22 Liters _____ liters _____
kg ______ x 107 years ______
9.70 x 107 years _____

70. Practice (talk together)
72. How many SF in these measures?
123 m 3 SF cm 5 SF
0.345 g 3 SF seconds 3 SF
22 Liters 2 SF liters 3 SF
kg 4 SF x 107 years 2 SF
9.70 x 107 years 3 SF

71. Density is the relationship between mass and volume of a substance
Density is the relationship between mass and volume of a substance. (how much stuff divided by how much space it takes).
The formula is d=m/v
73. If your unknown metal has mass of grams and volume of 1.15 cm3, what is the density?

72. Density is the relationship between mass and volume of a substance
Density is the relationship between mass and volume of a substance. (how much stuff divided by how much space it takes).
The formula is d=m/v
73. If your unknown metal has mass of grams and volume of 1.15 cm3, what is the density?
mass volume
D =

73. Density is the relationship between mass and volume of a substance
Density is the relationship between mass and volume of a substance. (how much stuff divided by how much space it takes).
The formula is d=m/v
73. If your unknown metal has mass of grams and volume of 1.15 cm3, what is the density?
11.46 g cm3
D =
= g/cm3 ???
Round to only 3 SF!!! g/cm3

74. Density is the relationship between mass and volume of a substance
Density is the relationship between mass and volume of a substance. (how much stuff divided by how much space it takes).
The formula is d = m/v
74. If your unknown metal has mass of g volume of 7.75 cm3, what is the density?

75. Density is the relationship between mass and volume of a substance
Density is the relationship between mass and volume of a substance. (how much stuff divided by how much space it takes).
The formula is d = m/v
74. If your unknown metal has mass of g volume of 7.75 cm3, what is the density?
mass volume
D =
35.46 g 7.75 cm3
= g/cm3

76. Measurement Class 4
75. OB: Learning the rules and operations of unit conversion math, AKA DIMENSIONAL ANALYSIS

77. 76. 2 Sneakers = 1 pair of sneakers Same thing, right?
In our lives, and in our studies, we will have to convert our math units from one form to another all the time.
Each time you put on your two sneakers in the morning, or your pair of sneakers, you put on the same number of sneakers, but you think it, or say it differently.
Sneakers = pair of sneakers
Same thing, right?

78. No matter if you are playing 52-Pickup or watching a magician, you know that there are 52 cards in the deck of cards. A deck of cards has 52 cards.
77. A deck of cards EQUALS 52 cards.
If your brother ripped the ace of diamonds in half during a minor fit of insanity, you no longer have a deck of cards (although if he’s under eight years old he might not notice). =

79. 78. If I said how many cards are in 2 decks of cards, or how many shoes are in three pairs of shoes, could you tell me? (104 and 6)
To figure these problems out, you would probably just “do it in your head”, but in fact you are doing dimensional analysis computations.
3 pairs of shoes 1 X
2 shoes 1 pair of shoes
= 6 shoes
This is how your “mind” converted from pairs to shoes in units.
You didn’t even realize (probably) that 2 shoes = 1 pair of shoes is called an Equality, which can be changed into 2 different CONVERSION FACTORS.

80. Two Conversion Factors
79. List these
Conversion factors are used to convert one unit to another.
All conversion factor numerators must = their denominators.
They MUST have units top and bottom. MUST.
They will always equal “1” - right side up or upside down.
Every equality can make 2 different conversion factors, and conversion factors equal 1.
12 inches = 1 foot
80.
An Equality
Two Conversion Factors
From one equality =
12 inches 1 foot
1 foot 12 inches

81. 81. Let’s convert your teacher’s mass (________ pounds) into ounces.
Do you know of an equality with pounds & ounces? pound = 16 ounces

82. = X ___ pounds 1 16 ounces 1 pound
81. Let’s convert your teacher’s mass (________ pounds) into ounces.
Do you know of an equality with pounds & ounces.
___ pounds 1
16 ounces 1 pound = X
ounces
_____ ounces. WHOA! What about SF? How many SF in the math?
How many SF are supposed to be in the answer? What’s the real answer?
_____________ ounces has 2 SF, which is as close as we can measure.

83. 82. Convert 1.2 kilograms into grams (1 kg = 1000 g).
Let’s try a few one step unit conversion problems in a row.
Set it up correctly, with our “starting point” over 1, use units, cancel units, talk to each other and check to see if your neighbor has the same answer as you do.
82. Convert 1.2 kilograms into grams (1 kg = 1000 g).
83. Convert 56,750 mL into liters (l L = 1000 mL).

84. Starting point ◊ watch units ◊ watch SF ◊ BANG!
82. Convert 1.2 kilograms into grams (1 kg = 1000 g).
1.2 kg 1 X
1000 g 1 kg =
1200 g
83. Convert 56,750 mL into liters (l L = 1000 mL). X
1 L 1000 mL
56,750 mL 1
= L
Starting point ◊ watch units ◊ watch SF ◊ BANG!

85. 84. Convert your age (you are 15.4 years old right now) into minutes.
Multiple step unit conversions…
You can sometimes get a problem that you can’t simply convert from one unit to another because you don’t know a conversion factor. But you know other ones, so you can go in steps.
84. Convert your age (you are 15.4 years old right now) into minutes.
How many minutes are in one year? There is an answer to that, and if you know it, you can make this a one step conversion problem.
Since you don’t let’s think.
All conversion factors must equal 1.
If you multiply 15.4 x a conversion factor = 15.4
If you multiply 15.4 x a conversion factor x another one = 15.4
You can multiply any number by 1 as many times as you like, it’s ok.

86. Convert 15.4 years into minutes.

87. 84. Convert 15.4 years into minutes.
15.4 yr 1
365 days 1 yr
24 hours 1 day
60 minutes 1 hour X X X =
15.4 yr 1
365 days 1 yr
24 hours 1 day
60 minutes 1 hour X X X =
Be sure to see how you started OVER 1, and ALL of the units cancel, and the last unit left (minutes) is the one that the answer needs to have!
Do the math, and consider your ANSWER’S SF BEFORE you multiply. How many SF does your answer NEED to have?
8,094,240 min. with just 3 SF: 8,090,000 min.

88. 85. Convert the 400. meter race into yards so the football players can easily compare that length to their field inch = 2.54 centimeters

89. 85. Convert the 400. meter race into yards so the football players can easily compare that length to their field inch = 2.54 centimeters
400. m 1
100 cm 1 m
1 inch 2.54 cm
1 yard 36 inches X X X =
400. m 1
100 cm 1 m
1 inch 2.54 cm
1 yard 36 inches X X X =
How many SF in the answer?! Do the math across the top and write your answer, then CLEAR your calculators. Do the math across the bottom, write your answer, then clear again. Then do the division.
40,
= changes to 437 yards with 3 SF

90. Homework Tonight: Measurement HW _____
86. I live in a make believe world (sometimes) and in my world there are special magical ways that will allow me to convert from unusual units to even more unusual units. Sometimes I bring silly problems back to Earth, just to help my students think abstractly. As long as you have equalities, you can make conversion factors. Ergo, you can convert units easily.
A YOWZA is what a student yells when she earns an all correct on her quiz. 1 Yowza feels the same as 3.4 hoo-hoo’s
1 hoo-hoo is the same as hollaring 8.2 ka-ching’s
1 ka-ching is equal to 2.3 hmmmm’s
It takes 5.9 hmmmm’s to match up with 1.6 unh’s.
So, tell me quick! How many unh’s are the same as 7.00 Yowza’s?
(units are units, and they are there just to be crossed out)
Watch your starting point, and how many SF in your answer?
Homework Tonight: Measurement HW _____

91. = 718.1888 5.9 7.00 Y 1 3.4 Hoo 1 Y 8.2 ka-ch 1 Hoo 2.3 hmm 1 ka-ch
1.6 unh 5.9 hmm X = X X X
Set it up, watch the unit placement, cancel the units out, is your LAST UNIT the one that you need in the answer?
Do the math across the top, hit equal and write that down.
Do the same on the bottom.
Divide and check SF.
5.9
= … with 3 SF rounds to unh’s!
Do your homework tonight, I will collect it tomorrow.

92. 87. OB: Scientific Notation for fun and personal enjoyment
Measurement Class #5: Scientific Notation
87. OB: Scientific Notation for fun and personal enjoyment
You must start with a calculator in hand.
Do the math in the proper order and you’ll always be right!

93. 91. 0.000 000 000 154 meters (the radius of a carbon atom
Express the following as Scientific Notation:
,000,000,000 ants
89. 6,374,000 meters
gram
meters (the radius of a carbon atom
m (the diameter of a human hair)

94. Express the following as Scientific Notation:
,000,000,000 ants x 1010 ants
89. 6,374,000 meters x 106 m
gram 3.4 x 10-2 g
meters (the radius of a carbon atom x m
m (the diameter of a human hair) 8 x 10-6 m

95. 93. Scientific notation rule: the coefficient shall always be more than one, less than ten
For example, THESE ARE ALL EQUIVLENT, BUT…
60,500 = 605 x 102
60,500 = 60.5 x 103
60,500 = 6.05 x 104
60,500 = x 105

96. 94.
Convert 36.8 kilograms into ounces, answer to be given in scientific notation.
(hints: 454 g = 1 pound = 16 ounces) (1kg = 1000 grams) Round to correct SF.

97. MAKE SURE YOU SEE how the UNITS CANCEL OUT
94.
Convert 36.8 kilograms into ounces, answer to be given in scientific notation.
(hints: 454 g = 1 pound = 16 ounces)
36.8 kg 1
1000 g 1 kg
1 p 454 g
16 oz 1 p x x x = = oz
1.30 x 103 oz
MAKE SURE YOU SEE how the UNITS CANCEL OUT

98. Convert 300. seconds into years, answer as scientific notation
95.
Convert 300. seconds into years, answer as scientific notation
(hint: your answer will be a small fraction of years, your exponent must be negative)

99. MAKE SURE YOU SEE how the UNITS CANCEL OUT
95.
Convert 300. seconds into years, answer as scientific notation
(hint: your answer will be a small fraction of years, your exponent must be negative)
300. sec 1
1 min 60 sec
1 HR 60 min
1 day 24 HR
1 year 365 day x x x x =
= years = x 10-6 years
MAKE SURE YOU SEE how the UNITS CANCEL OUT

100. 96. Multiplication rules for scientific notation
Multiply coefficients, add powers of ten, adjust coefficient if necessary. (teapot)
97. (3 x 105)(2 x 102) =
x 104
X 3.0 x 102

101. Multiplication rules for scientific notation
Multiply coefficients, add powers of ten, adjust coefficient if necessary. (teapot)
97. (3 x 105)(2 x 102) = 6 x 107
x 104
X 3.0 x 102
15.0 x 106
1.50 x 107
1.5 x 107 with 2 SF

102. 99. Division Rules for Scientific Notation
Divide coefficients, subtract powers of ten, adjust coefficients (teapot) if necessary.
100.
101.
3.0 x 104
2.0 x 102 =
9.0 x 105
3.0 x 103 =

103. Division Rules for Scientific Notation
Divide coefficients, subtract powers of ten, adjust coefficients (teapot) if necessary.
3.0 x 104
2.0 x 102
3.0
2.0 = =
1.5 x 102
X 10(4-2)
9.0 x 105
3.0 x 103
9.0
3.0 =
X 10(5-3) =
3.0 x 102

104. 6.2 x 108 + 1.5 x 106 6.5 x 107 + 2.2 x 107 102. Addition rules:
Adjust scientific notation so both terms have the SAME POWERS OF TEN, add or subtract coefficients, then adjust answer if necessary (teapot)
6.2 x 108
+ 1.5 x 106
6.5 x 107
+ 2.2 x 107

105. Adjust scientific notation so both terms have the SAME POWERS OF TEN, add or subtract coefficients, then adjust answer if necessary (teapot)
6.2 x 108
+ 1.5 x 106
6.5 x 107
+ 2.2 x x 107
6.2 x 108
x x 108
6.2 x 108

106. 7.1 x 105 - 1.6 x 104 8.5 x 103 - 2.4 x 103 105. Subtraction rules:
Adjust scientific notation so both terms have the SAME POWERS OF TEN, add or subtract coefficients, then adjust answer if necessary (teapot)
7.1 x 105
x 104
8.5 x 103
- 2.4 x 103

107. Adjust scientific notation so both terms have the SAME POWERS OF TEN, add or subtract coefficients, then adjust answer if necessary (teapot)
7.1 x 105
x 104
8.5 x 103
- 2.4 x x 103
7.1 x 105
x x 105
6.9 x 105

108. 108.
8.72 x 1011
x 1010
109.
4.65 x 1014
x 1015

109. 108.
8.72 x 1011
x 1010
8.72 x 1011
x 1011
8.892 x 1011
8.89 x 1011
109.
4.65 x 1014
x 1015
0.465 x 1015
2.25 x 1015
1.785 x 1015
1.79 x 1015

110. 110.
6.02 x 1023
x 1.50 x 102
111.
(9.05 x 1019) ÷ (3.2 x 1016 ) =

111. 110.
6.02 x 1023
x 1.50 x 102
9.03 x 1025
111.
(9.05 x 1019) ÷ (3.2 x 1016 ) = 2.8 x 103
2 SF!

112. 112. Convert 2450 mL into gallons. Show all units (3 SF)
Take out your reference tables, calculators at the ready. (1.06 Qt = 1 L)
112. Convert 2450 mL into gallons. Show all units (3 SF)

113. = 2597/4000 = 0.64925 gallons = 0.649 gallons with 3 SF = X X X
112. Convert 2450 mL into gallons. Show all units (3 SF)
2450 mL 1
1 Liter 1000 mL
1.06 Qt 1 Liter
1 gallon 4 Qt = X X X
= 2597/4000 = gallons
= gallons with 3 SF

114. 113. How many millimeters are are in 1000. yards
113. How many millimeters are are in yards? Answer into scientific notation.

115. 113. How many millimeters are in 1000. yards
113. How many millimeters are in yards? Put answer into scientific notation.
1000. yd 1
36 inch 1 yd
2.54 cm 1 inch
10 mm 1 cm = X X X
= 914,400 mm = x 105 mm
With 4 SF

116. 114. If you have exactly 25.0 Liters of water, how much does that weigh in tons?
Hint: write the density of pure water first, then see if it helps you convert things around

117. If you have exactly 25.0 Liters of water, how much does that weigh in tons?
The density of pure water is 1.0g per mL
which should tell you how much 25.0 liters mass is.
1000 mL 1 L
1 g 1 mL
25.0 L 1
1 pound 454 g
1 ton 2000 p X X X X =
= 25000/ = tons
with 3 SF
2.75 x 10-2 tons

118. In dimensional analysis, the units are there just to be converted
In dimensional analysis, the units are there just to be converted. They don’t “really” even matter. In fact, they can be made up, make believe. As long as you have equalities, you can convert from one unit to another, even if they are fake units.
Using fake units is called abstract thinking. You need to be abstract now, not obtuse. OK?
Imagine you are working at a zoo. Different animals have different “values”, which are not real, but come into play when trading other zoos to get new cool animals. Think and get psyched for this one…

119. You wish you could get a new proboscis monkey for the empty cage at your zoo. You have an abundance of lemurs on hand and hope to trade them away. In a multi- zoo trade, you set it all up.
1 proboscis monkey = 14 zebras
8 zebras = 1 giraffe
2 giraffes = 1 elephant
1 elephant = 27 penguins
5 penguins = 1 lemur
115. If this is all true (it is, I promise), how many lemurs will it take to get one proboscis monkey? (don’t sweat SF)
Round to the nearest whole lemur!

120. 115.
1 proboscis monkey = 14 zebras
8 zebras = 1 giraffe
2 giraffes = 1 elephant
1 elephant = 27 penguins
5 penguins = 1 lemur

121. 115. 1 proboscis monkey = 14 zebras
8 zebras = 1 giraffe
2 giraffes = 1 elephant
1 elephant = 27 penguins
5 penguins = 1 lemur
1 lemur 5 penguins
14 zebra 1 P.M.
1 giraffe 8 zebra
1 elephant 2 giraffes
27 penguins 1 elephant
1 P.M. 1 = X X X X X
= 378/80 = or
5 lemurs are equal to 1 proboscis monkey!

122. 116. You have a special moment and discover a hunk of metal in your yard in the dirt. It’s stamped “pure osmium” and “100.0 grams” as well. It looks pretty new and you even believe this is real. What is the volume of this hunk of metal in cm3? Show a formula and all your work. SF are your initials.

123. D = = M v 22.587 g/cm3 1 100.0 g v 22.587 g/cm3 (v) = 100.0 g
116. You have a special moment and discover a hunk of metal in your yard in the dirt. It’s stamped “pure osmium” and “100.0 grams” as well. It looks pretty new and you even believe this is real. What is the volume of this hunk of metal in cm3? Show a formula and all your work SF are your initials.
M v
D =
g/cm3 1
100.0 g v =
g/cm3 (v) = g
v = … = cm3 with 4 SF

124. pigs equal 1.6 dogs
2.2 dogs is equal to 0.95 cats
1.9 cats is equal to 3.1 birds
1.0 bird is the same as 11.0 spiders
and finally, 3.7 spiders is the same as 8.5 bugs
If this is true, how many bugs make up 1.0 pig? (wow)
Please round (UP) to the nearest whole bug (or yuck!)

125. Rounded to the nearest whole bug, that’s 29 bugs!
117.
1.0 pig 1
1.6 dog 1.0 pig
0.95 cat 2.2 dogs
3.1 birds 1.9 cats
11.0 spiders 1.0 birds
8.5 bugs 3.7 spiders x x x x x
1.0 x 1.6 x 0.95 x 3.1 x 11.0 x = = bugs
1 x 1.0 x 2.2 x 1.9 x 1.0 x 3.7 =
Rounded to the nearest whole bug, that’s 29 bugs!

126. Measurement Class 6: REVIEW FOR CELEBRATION OF KNOWLEDGE Objective: more chemistry math, because you gotta love it!
Get a calculator in your hot little hand, sit with a few smart friends, let’s go…

127. 5,600 grams___ 5.600 kilograms___
First, determine how many significant figures are in each of these measurements:
5,600 grams___ kilograms___
4.305 mL___ °C___
moles Hg___ seconds___
The product of grams x 2.0 g/cm3___

128. Do the drills for SF if you need to. (you do)
First, determine how many significant figures are in each of these measurements:
5,600 grams 2 SF
5.600 kilograms 4 SF
4.305 mL 4 SF
0.678°C 3 SF
moles Hg 2 SF
1.400 seconds 4 SF
Product of grams x 2.0 g/cm3 2 SF
Do the drills for SF if you need to. (you do)

129. 10 Kelvin 10 centigrade 10 Fahrenheit 280 K 32°F 6°C Convert
In each set of temperatures, decide which is the coldest, which is the hottest.
10 Kelvin
10 centigrade
10 Fahrenheit
280 K
32°F
6°C
Convert
-15.0°C into K
350 K to C

130. 10 Kelvin COLDEST 10 centigrade HOTTEST 10 Fahrenheit 280 K HOTTEST
In each set of temperatures, decide which is the coldest, which is the hottest.
10 Kelvin COLDEST
10 centigrade HOTTEST
10 Fahrenheit
280 K HOTTEST
32°F COLDEST
6°C
Convert °C into K
K = C + 273
K = (-15) + 273
K = 258 K
Convert K to C
350 K = C + 273 =
77° C = C

131. Two quick (and easy) one step dimensional analysis problems to solve…
Convert 125 grams into kilograms
Convert liters into mL

132. Two quick (and easy) one step dimensional analysis problems to solve…
Convert 125 grams into kilograms
Convert liters into mL
125 g 1
1 kg 1000 g x =
0.125 kg with 3 SF
34.75 L 1
1000 mL 1 L x =
34,750 mL with 4 SF

133. How many light switches will equal one house? Equalities
In the funky world that your teacher resides, there are some weird equalities. Given a short list of them, you should be able to solve a funky problem like this…
How many light switches will equal one house?
Equalities
1.0 house = 8.0 rooms rooms = 3.0 windows
1.0 windows = 2.0 lights lights = 4.0 light switches

134. In the funky world that your teacher resides, there are some weird equalities. Given a short list of them, you should be able to solve a funky problem like this…
How many light switches will equal one house?
Equalities
1.0 house = 8.0 rooms rooms = 3.0 windows
1.0 windows = 2.0 lights lights = 4.0 light switches
1.0 House 1
8.0 Rooms 1.0 House
3.0 Windows 2.0 Rooms
2.0 Lights 1.0 Windows
4.0 Switches 3.0 Lights x x x x =
192 6
32 switches
(2 SF)

135. You measure some pure niobium metal to have a density of 8. 00 g/cm3
You measure some pure niobium metal to have a density of 8.00 g/cm3. What is your percent error? (hint, write the formula first)

136. You measure some pure niobium metal to have a density of 8. 00 g/cm3
You measure some pure niobium metal to have a density of 8.00 g/cm3. What is your percent error? (hint, write the formula first)
MV – AV AV
% E =
X 100% =
8.00 g/cm3 – g/cm g/cm3
X 100% =
% E =
% E = %

137. (3.5 x 106)(2.0 x 102) = ____________________________
Do what the math says to do:
(3.5 x 106)(2.0 x 102) = ____________________________
(8.0 x 108) ÷ (4.0 x 1012) = ___________________________

138. ANSWERS
(3.5 x 106)(2.0 x 102) = 7.0 x 108
(8.0 x 108) ÷ (4.0 x 1012) = 2.0 x 10-4

139. (3.3 x 108) + (1.2 x 107) = ___________________________
Do what the math says to do:
(3.3 x 108) + (1.2 x 107) = ___________________________
(5.64 x 105) – (2.33 x 104) = _________________________

140. ANSWERS
(3.3 x 108) + (1.2 x 107) = (3.3 x 108) + (0.12 x 108) = 3.42 x 108 = x 108
(5.64 x 105) – (2.33 x 104) = (5.64 x 105) – (0.233 x 105) = x 105 = x 105