1. PWISTA Math of Chemistry
Scientific measurement
Accuracy and Precision
Sig Figs
Metric System

2. Types of measurement Quantitative- use numbers to describe
Qualitative- use description without numbers
4 feet
extra large
Hot
100ºF

3. Scientists prefer Quantitative- easy check
Easy to agree upon, no personal bias
The measuring instrument limits how good the measurement is

4. How good are the measurements?
Scientists use two word to describe how good the measurements are
Accuracy- how close the measurement is to the actual value
Precision- how well can the measurement be repeated

5. Differences
Accuracy can be true of an individual measurement or the average of several
Precision requires several measurements before anything can be said about it
examples

6. Let’s use a golf analogy

7. Accurate? No
Precise?
Yes

8. Accurate?
Yes
Precise?
Yes

9. Precise? No
Accurate?
Maybe?

10. Accurate?
Yes
Precise?
We cant say!

11. In terms of measurement
Three students measure the room to be m, 10.3 m and 10.4 m across.
Were they precise?
Were they accurate?

12. Significant figures (sig figs)
How many numbers mean anything
When we measure something, we can (and do) always estimate between the smallest marks. 2 1 3 4 5

13. Sig Figs
Significant digits, which are also called significant figures, are very important in Chemistry.
Each recorded measurement has a certain number of significant digits.
Calculations done on these measurements must follow the rules for significant digits.

14. Sig Figs
The significance of a digit has to do with whether it represents a true measurement or not.
Any digit that is actually measured or estimated will be considered significant.
Placeholders, or digits that have not been measured or estimated, are not considered significant.
The rules for determining the significance of a digit will follow.

15. Significant figures (sig figs)
The better marks the better we can estimate.
Scientist always understand that the last number measured is actually an estimate 1 2 3 4 5

16. Sig Figs
What is the smallest mark on the ruler that measures cm?
142 cm?
140 cm?
Here there’s a problem does the zero count or not?
They needed a set of rules to decide: which zeroes count?
All other numbers do count

17. The Standard Rules 1) Digits from 1-9 are always significant.
2) Zeros between two other significant digits are always significant. (sandwich rule)
3) One or more additional zeros to the right of both the decimal place and another significant digit are significant.
4) Zeros used solely for spacing the decimal point (placeholders) are not significant.

18. Too Confusing! Heads will spin!

20. EXAMPLES
# OF SIG. DIG.
COMMENT
453 kg 3
All non-zero digits are always significant.
5057 L 4
Zeros between 2 sig. dig. are significant.
5.00
Additional zeros to the right of decimal and a sig. dig. are significant.
0.007 1
Placeholders are not sig.

21. Alternate Rule for Significant Digits
Rules Courtesy of Fordham Prep website.
When you look at the number in question, you must determine if it has a decimal point or not.  If it has a decimal, you should think of "P" for "Present".  If the number does not have a decimal place, you should think of "A" for "Absent".

22. Alternate Rule for Significant Digits
Example, for  the number , think "P", because the decimal is present.
For the number 6500, you would think "A", because the decimal is absent.

23. Alternate Rule for Significant Digits
Now, the letters "A" and "P" also correspond to the "Atlantic" and "Pacific" Oceans, respectively. 
Assume the top of the page is North, and imagine an arrow being drawn toward the number from the appropriate coast. 
Once the arrow hits a nonzero digit, it and all of the digits after it are significant.

24. How many significant digits are shown in the number 20 400 ?
Example 1
  How many significant digits are shown in the number ? 
(remember that we use spaces, rather than commas, when writing numbers in Science.
Well, there is no decimal, so we think of "A" for "Absent".  This means that we imagine an arrow coming in from the Atlantic ocean, as shown below; 

25. Example 1
The first non-zero digit the arrow hits would be the 4, making it, and all digits to the left of it significant. There are 3 significant digits 

26. Example 2
  How many significant digits are shown in the number ? 

27. Example 2
Well, there is a decimal, so we think of "P" for "Present".  This means that we imagine an arrow coming in from the Pacific ocean, as shown below;
0.090

28. Example
The first nonzero digit that the arrow will pass in the 9, making it, and any digit to the right of it significant.

29. Answer Example 2 There are 2 significant digits in the number 0.090
Here are the significant digits, shown in boldface.  0.090

30. Which zeros count?
Those at the end of a number before the decimal point don’t count
12400
If the number is smaller than one, zeroes before the first number don’t count
0.045

31. Which zeros count? Zeros between other sig figs do. 1002
zeroes at the end of a number after the decimal point do count
If they are holding places, they don’t.
If they are measured (or estimated) they do

32. Sig Figs Only measurements have sig figs. Counted numbers are exact
A dozen is exactly 12
A a piece of paper is measured 11 inches tall.
Being able to locate, and count significant figures is an important skill.

33. Sig figs. How many sig figs in the following measurements? 458 g

34. Sig Figs.
405.0 g
4050 g
0.450 g g g
Next we learn the rules for calculations

35. Problems Same # - Different # sig figs …
50 is only 1 significant figure
if it really has two, how can I write it?
A zero at the end only counts after the decimal place
Scientific notation
5.0 x 101
now the zero counts.

36. Adding and subtracting with sig figs
The last sig fig in a measurement is an estimate.
Your answer when you add or subtract can not be better than your worst estimate.
have to round it to the least place of the measurement in the problem

37. For example
27.93
6.4 +
First line up the decimal places
27.93
6.4 +
27.93
6.4
Then do the adding
Find the estimated numbers in the problem
34.33
This answer must be rounded to the tenths place

38. Rounding rules look at the number behind the one you’re rounding.
If it is 0 to 4 don’t change it
If it is 5 to 9 make it one bigger
round to four sig figs
to three sig figs
to two sig figs
to one sig fig

39. Adding and Subtracting
RULE: When adding or subtracting your answer can only show as many decimal places as the measurement having the fewest number of decimal places.

40. add 3.76 g g g = g
We look to the original problem to see the number of decimal places shown in each of the original measurements.
2.1 shows the least number of decimal places.
We must round our answer, 20.69, to one decimal place (the tenth place).
Our final answer is 20.7 g

41. Practice
6.0 x x 103
6.0 x x 10-3

42. Multiplication and Division
Rule is simpler
Same number of sig figs in the answer as the least in the question
3.6 x 653
Calculated answer =
3.6 has 2 sig figs, 653 has 3 sig figs
answer can only have 2 sig figs
2400

43. Multiplying and Dividing
RULE: When multiplying or dividing, your answer may only show as many significant digits as the multiplied or divided measurement showing the least number of significant digits.

44. EX: cm x 3.10 cm x cm = cm3
We look to the original problem and check the number of significant digits in each of the original measurements:
22.37 shows 4 significant digits.
3.10 shows 3 significant digits.
85.75 shows 4 significant digits.

45. EX: cm x 3.10 cm x cm = cm3
Our answer can only show 3 significant digits because that is the least number of significant digits in the original problem.
shows 9 significant digits, we must round to the tens place in order to show only 3 significant digits.
Our final answer becomes 5950 cm3.

46. Multiplication and Division
Same rules for division
practice
4.5 / 6.245
4.5 x 6.245
x .043
3.876 / 1983
16547 / 714

47. The Metric System An easy way to measure

49. Measuring The numbers are only half of a measurement
It is 10 long what?
Numbers without units are meaningless.
I’ll pay you 100 to mow the lawn … then give the person 100 cents. Won’t make friends that way.

50. The Metric System Easier to use because it is a decimal system
Every conversion is by some power of 10.
A metric unit has two parts
A prefix and a base unit.
prefix tells you how many times to divide or multiply by 10.

51. Base Units Length - meter more than a yard - m
Mass - grams - a bout a raisin - g
Time - second - s
Temperature - Kelvin or ºCelsius K or C
Energy - Joules- J
Volume - Liter - half f a two liter bottle- L
Amount of substance - mole - mol

53. Prefixes kilo k 1000 times deci d 1/10 centi c 1/100 milli m 1/1000
kilometer - about 0.6 miles
centimeter - less than half an inch
millimeter - the width of a paper clip wire

54. Volume calculated by multiplying L x W x H
Liter the volume of a cube 1 dm (10 cm) on a side
so 1 L = 10 cm x 10 cm x 10 cm
1 L = 1000 cm3
1/1000 L = 1 cm3
1 mL = 1 cm3

55. Volume 1 L about 1/4 of a gallon - a quart
1 mL is about 20 drops of water or 1 sugar cube

56. Mass weight is a force, is the amount of matter.
1gram is defined as the mass of 1 cm3 of water at 4 ºC.
1000 g = 1000 cm3 of water
1 kg = 1 L of water

57. Mass 1 kg = 2.5 lbs 1 g = 1 paper clip
1 mg = 10 grains of salt or 2 drops of water.

58. Converting k h D d c m
how far you have to move on this chart, tells you how far, and which direction to move the decimal place.
The box is the base unit, meters, Liters, grams, etc.

59. k h D d c m Conversions 5 6 Change 5.6 m to millimeters
starts at the base unit and move three to the right.
move the decimal point three to the right 5 6

60. k h D d c m Conversions convert 25 mg to grams convert 0.45 km to mm
convert 35 mL to liters
It works because the math works, we are dividing or multiplying by 10 the correct number of times

61. Conversions k h D d c m
Change 5.6 km to millimeters

62. Which is heavier?
it depends

63. Density how heavy something is for its size
the ratio of mass to volume for a substance
D = M / V
Independent of how much of it you have
gold - high density
air low density.

64. Calculating The formula tells you how (d=mass / volume)
BETTER YET … the UNITS tell you how!
units will be g/mL or g/cm3

65. We know the units for density are g/ml
A piece of wood has a mass of 11.2 g and a volume of 23 mL what is the density?
We know the units for density are g/ml
The unit tells us that grams goes on top and ml goes on the bottom; so let’s do that.
11.2g / 23ml = 0.49 g/ml

66. The Unit you want to find ALWAYS goes on top.
A piece of wood has a density of 0.93 g/mL and a volume of 23 mL what is the mass?
The Unit you want to find ALWAYS goes on top.
We have 0.93 g/ml. We want to get rid of the ml on the bottom. So multiply by ml on top. (ml on top and bottom cancel out)
0.93g/ml x 23 ml / 1 = g

67. Calculating
A piece of wood has a density of 0.93 g/mL and a mass of 23 g what is the volume?
The units must always work out.
Algebra 1
Get the thing you want by itself, on the top.
What ever you do to onside, do to the other

68. Floating Lower density floats on higher density.
Ice is less dense than water.
Most wood is less dense than water
Helium is less dense than air.
A ship is less dense than water

69. Density of water 1 g of water is 1 mL of water.
density of water is 1 g/mL
at 4ºC
otherwise it is less

70. Measuring Temperature
0ºC
Celsius scale.
water freezes at 0ºC
water boils at 100ºC
body temperature 37ºC
room temperature ºC

71. Measuring Temperature
273 K
Kelvin starts at absolute zero (-273 º C)
degrees are the same size
C = K -273
K = C + 273
Kelvin is always bigger.
Kelvin can never be negative.

72. Heat
a form of energy

73. Temperature is different
than heat.
Temperature is which way heat will flow (from hot to cold)
Heat is energy, ability to do work.
A drop of boiling water hurts,
kilogram of boiling water kills

74. Units of heat are calories or Joules
1 calorie is the amount of heat needed to raise the temperature of 1 gram of water by 1ºC
a food Calorie is really a kilocalorie
How much energy is absorbed to heat 15 grams of water by 25ºC
1 calorie = 4.18 J

75. Some things heat up easily
some take a great deal of energy to change their temperature.
The Specific Heat Capacity amount of heat to change the temperature of 1 g of a substance by 1ºC
specific heat SH
S.H. = heat (cal) mass(g) x change in temp(ºC)

76. Specific Heat Water has a high specific heat 1 cal/gºC
units will always be cal/gºC
or J/gºC
the amount of heat it takes to heat something is the same as the amount of heat it gives off when it cools because...

77. Problems
It takes 24.3 calories to heat 15.4 g of a metal from 22 ºC to 33ºC. What is the specific heat of the metal?
Iron has a specific heat of 0.11 cal/gºC. How much heat will it take to change the temperature of 48.3 g of iron by 32.4ºC?