1. Introductory Chemistry:
Chapter 1
Chemistry and You

2. Tuesday, 9/9/14
Learning Target: Students must be able to explain why chemistry is central to many human endeavors.
Chapter 1

3. Learning Chemistry Different people learn chemistry differently.
What do you see in the picture?
Some people see a vase on a dark background, some people see two faces.
Chapter 1

4. Problem Solving Connect the 9 dots using only four straight lines.
Experiment until you find a solution.
However, we have used 5 straight lines.
No matter which dot we start with, we still need 5 lines.
Chapter 1

5. Problem Solving Are we confining the problem?
We need to go beyond the 9 dots to answer the problem.
Chapter 1

6. Lab Safety Symbols Identify the following symbols
A. B. C.
D. E. F.
G. H. I.

7. What is the definition of chemistry?
The science that studies the composition of matter and its properties.

8. Chemistry: The Central Science
Why????
Most other sciences demand an understanding of basic chemical principles, and Chemistry is often referred to as the Central Science
Chapter 1

9. Modern Chemistry
Chemistry is a science that studies the composition of matter and its properties.
Chemistry is divided into several branches:
Organic chemistry is the study of substances containing carbon
Inorganic chemistry is the study of all other substances
Biochemistry is the study of substances derived from plants and animals
Analytical is the study of matter and ways to study the properties of matter.
Physical is the physics of chemistry. Thermodynamics and quantum mechanics.
Chapter 1 9

10. Wednesday, 9/10/14
Learning Target: Students must know the metric system, SI units and derived units. Learning Outcome: Measurement Pre-Lab
Chapter 1

11. The Standard Units
Scientists have agreed on a set of international standard units for comparing all our measurements called the SI units
Quantity
Unit
Symbol
length
meter m
mass
kilogram kg
time
second s
temperature
kelvin K

12. Length SI unit = meter Commonly use centimeters (cm) About a yard
1 m = 100 cm
1 cm = 0.01 m = 10 mm
1 inch = 2.54 cm

13. Mass Measure of the amount of matter present in an object
weight measures the gravitational pull on an object, which depends on its mass
SI unit = kilogram (kg)
about 2 lbs. 3 oz.
Commonly measure mass in grams (g) or milligrams (mg)

14. Time
measure of the duration of an event
SI units = second (s)

15. Temperature Scales Fahrenheit Scale, °F Celsius Scale, °C
used in the U.S.
Celsius Scale, °C
used in all other countries
Kelvin Scale, K
The SI unit for temperature

16. Prefix Multipliers in the SI System
Symbol
Decimal
Equivalent
Power of 10
mega- M
1,000,000
Base x 106
kilo- k
1,000
Base x 103
deci- d
0.1
Base x 10-1
centi- c
0.01
Base x 10-2
milli- m
0.001
Base x 10-3
micro-
Base x 10-6
nano- n
Base x 10-9
pico p
Base x 10-12

17. What Is a Measurement? quantitative observation
every measurement has a number and a unit
every digit written is certain, the last one which is estimated

19. Estimation in Weighing
What is the uncertainty in this reading?

20. Thursday, 9/11/14
Learning Target: Students must be able to compare and contrast accuracy and precision in measurement. Learning Outcome: Complete “Measurement Lab”
Chapter 1

21. Uncertainty in Measured Numbers
uncertainty comes from:
limitations of the instruments used for comparison,
the experimental design,
the experimenter,
nature’s random behavior

22. Precision and Accuracy
accuracy is an indication of how close a measurement comes to the actual value of the quantity
Percent error =
precision is an indication of how reproducible a measurement is

23. Accuracy vs. Precision

24. Precision imprecision in measurements is caused by random errors
errors that result from random fluctuations
we determine the precision of a set of measurements by evaluating how far they are from the actual value and each other called standard deviation.
Do multiple trials to lesson error and improve precision.

25. Accuracy inaccuracy in measurement caused by systematic errors
errors caused by limitations in the instruments or techniques or experimental design
we determine the accuracy of a measurement by evaluating how far it is from the actual value
Use percent error to calculate how accurate you are

26. Mass & Volume mass and volume are extensive properties
the value depends on the quantity of matter
extensive properties cannot be used to identify what type of matter something is
if you are given a large glass containing 100 g of a clear, colorless liquid and a small glass containing 25 g of a clear, colorless liquid - are both liquids the same stuff?

27. Mass vs. Volume of Brass

28. Monday 9/15/14
Learning Target: Know how to use significant figures in labs and in problems. Learning Outcome: Complete significant figures problems.
Chapter 1

29. Accuracy versus Precision
Chapter 1

30. Significant Figures
the non-place-holding digits in a reported measurement are called significant figures
significant figures tell us the range of values to expect for repeated measurements
We use significant figures in science because measurement is always involved.

31. Counting Significant Figures
All non-zero digits are significant
1.5 has 2 sig. figs.
Interior zeros are significant
1.05 has 3 sig. figs.
Leading zeros are NOT significant – has 4 sig. figs.

32. Counting Significant Figures
Trailing zeros may or may not be significant 1) If a decimal is present, trailing zeros are significant
1.050 has 4 sig. figs.
2) If a decimal is NOT present, trailing zeros are NOT significant.
if 150 has 2 sig. figs. then 1.5 x 102
but if 150. has 3 sig. figs. then 1.50 x 102
**These are considered ambiguous and should be avoided by using scientific notation

33. Determining the Number of Significant Figures in a Number
How many significant figures are in each of the following? m km
1.000 × 105 s mm
10,000 m
4 sig. figs.; the digits 4 and 5, and the trailing 0
5 sig. figs.; the digits 5 and 3, and the interior 0’s
4 sig. figs.; the digit 1, and the trailing 0’s
1 sig. figs.; the digit 2, not the leading 0’s
Ambiguous, generally assume 1 sig. fig.

34. Multiplication and Division with Significant Figures
when multiplying or dividing measurements with significant figures, the answer must reflect the fewest number of significant figures
1) × , × =
2) ÷ 6.10 =

35. Addition and Subtraction with Significant Figures
when adding or subtracting measurements with significant figures, the answer should reflect the largest uncertainty
1) =
2) =

36. Rounding
if the number after the place of the last significant figure is:
0 to 4, round down
drop all digits after the last sig. fig. and leave the last sig. fig. alone
5 to 9, round up
drop all digits after the last sig. fig. and increase the last sig. fig. by one
To avoid accumulating extra error from rounding, round only at the end, keeping track of the last sig. fig. for intermediate calculations

37. Rounding rounding to 2 significant figures 2.34 rounds to 2.3

38. Rounding rounding to 2 significant figures 0.0234 rounds to 0.023

39. Rounding rounding to 2 significant figures 234 rounds to 230

40. Both Multiplication/Division and Addition/Subtraction with Significant Figures
First, evaluate the significant figures in the parentheses
Second, do the remaining steps
× ( – ) =

41. Perform the following calculations to the correct number of significant figures

42. Example 1.6 Perform the following calculations to the correct number of significant figures

43. Tuesday 9/16/14
Learning Target: Know how to use and convert numbers into scientific notation. Learning Outcome: I will be able to use scientific notation in problems and convert standard notation into scientific notation.
Chapter 1

44. Why are significant figures not important in your math class?
Chapter 1

45. Density Ratio of mass:volume
Solids = g/cm3
1 cm3 = 1 mL
Liquids = g/mL
Gases = g/L
Volume of a solid can be determined by water displacement – Archimedes Principle

46. Density Density : solids > liquids >>> gases
except ice is less dense than liquid water!
Heating an object generally causes it to expand, therefore the density changes with temperature

47. Density
Iron has a density of 7.86 g/cm3. Could a block of metal with a mass of 18.2 g and a volume of 2.56 cm3be iron?

48. Density
What volume would a g sample of air occupy if the density of air is 1.29 g/L?

49. Wednesday, 9/17/14
Learning Target: Be able to apply dimensional analysis to convert from one unit of measure to another. Learning Outcome: I will be able to complete single-step unit conversion problems.
Chapter 1

50. Units Always include units in your calculations
you can do the same kind of operations on units as you can with numbers
cm × cm = cm2
cm + cm = cm
cm ÷ cm = 1

51. Dimensional Analysis
Using units as a guide to problem solving is called dimensional analysis
This is the technique that we have learned to convert between two different units.

52. Problem Solving and Conversion Factors
Conversion factors are relationships between two units
May be exact or measured
Conversion factors are generated from unit equalities
e.g., 1 inch = 2.54 cm can give or

53. Problem Solving and Dimensional Analysis
Arrange conversion factors so given unit cancels
Arrange conversion factor so given unit is on the bottom of the conversion factor
May string conversion factors
So we do not need to know every relationship, as long as we can find something else the given and desired units are related to

54. Using a ruler from the front counter, measure the length, width and height of a Chemistry textbook to the nearest 1 cm.
How many meters wide is it?
How many inches is the width of the textbook (2.54 cm = 1 in)? 
How many feet is your textbook?

55. Thursday, 9/18/14
Learning Target: Be able to apply dimensional analysis to convert from one unit of measure to another. Learning Outcome: I will be able to complete multi-step unit conversion problems.
Chapter 1

56. Warm-Up
Convert – kPa to Pa
Chapter 1

57. Practice – Convert 154.4 lbs to kg57

58. Practice – Convert 30.0 mL to quarts (1 L = 1.057 qt)

59. Volume Derived unit (width x length x height)
any length unit cubed
Measure of the amount of space occupied
SI unit = cubic meter (m3)
Commonly measure solid volume in cubic centimeters (cm3)
1 m3 = 106 cm3
Commonly measure liquid or gas volume in milliliters (mL)
1 L is slightly larger than 1 quart
1 mL = 1 cm3

60. How many cubic centimeters are there in 2.11 yd3?

61. Impossible Conversions
Is it possible to find how many seconds in a kilogram?
In order to do unit conversions they must be able to correspond to the same quantity.
For example, kilograms and pounds are both units of mass.

62. Graphing in Science
All graphing that is done in science must include the following:
A descriptive title
X and Y axis labeled with units.
The X – axis is the manipulated variable and the Y- axis is the responding variable.
A trend line (or line of best fit) to show the trend in the data that has been plotted.

63. Volume vs. Mass of Brass Mass, g Volume, cm3 20 40 60 80 100 120 14020 40 60 80
100
120
140
160
0.0
2.0
4.0
6.0
8.0
10.0
12.0
14.0
16.0
18.0
Volume, cm3
Mass, g

64. Units & magnitude are correct
Convert 30.0 mL to quarts
Sort information
Given:
Find:
154.4 lbs
Lbs to kg
Strategize
Concept Plan:
Relationships:
1 L = qt
1 L = 1000 mL
Follow the concept plan to solve the problem
Solution:
Sig. figs. and round
Round:
qt = qt
Check
Check:
Units & magnitude are correct 64

65. Scientific Investigations
Science is the methodical exploration of nature followed by a logical explanation of the observations.
Scientific investigation entails:
planning an investigation
carefully recording observations
gathering data
analyzing the results

66. The Scientific Method
The scientific method is a systematic investigation of nature and requires proposing an explanation for the results of an experiment in the form of a general principle.
The initial, tentative proposal of a scientific principle is called a hypothesis.
After further investigation, the original hypothesis may be rejected, revised, or elevated to the status of a scientific principle.
Chapter 1

67. Scientific Method a test of a hypothesis or theory
a tentative explanation of a single or small number of natural phenomena
a general explanation of natural phenomena
the careful noting and recording of natural phenomena
a generally observed natural phenomenon 67

68. Conclusions Continued
After sufficient evidence, a hypothesis becomes a scientific theory.
A natural law is a measurable relationship.
Chapter 1

69. Conclusions
Scientists use the scientific method to investigate the world around them.
Experiments lead to a hypothesis, which may lead to a scientific theory or a natural law.
Chemistry is a central science with many branches.
The impact of chemistry is felt in many aspects of our daily lives.
Chapter 1

70. QUIZE - CHAPTER -1
What is the difference between a hypothesis and theory
According to the ancient Greeks, which of the following are not basic elements found in nature:
Air
Coal
Fire
Earth
Gold
Water
Chapter 1