1. AP Chemistry
Day 3 – Chapter 1 Review

2. Warm Up
SIT AT: Table 1, 2, or 3 SIT: With two different people SHARE OUT: Your name tent TIME: 2 minutes WHEN DONE ENTIRE TABLE IS DONE: Share one thing you did this weekend and be prepared to introduce all people at your table

3. AP Chemistry Agenda
Class Norms
Set Up Spiral Notebooks
Chapter 1 questions
- If time: Check out lab equipment and Lab Notebooks
Next Class: Bring Book and Mini-Lab - Measuring Density of Liquids
Remember: Safety Contract DUE NEXT CLASS, THU 9/8 (if you have it now, turn it into class box by end of class)
Remember: Chapter 1 Quiz and Turn in Homework Packet (Mon 9/12)

4. Listen Do Your Work Be cool Classroom Norms Be Here
Why do we have Classroom Norms?
Think of your favorite class (not necessarily the easiest) – where you were comfortable, but able to grow.
What did it look like? What did it sound like?
Be Here
Listen
Do Your Work
Be cool

5. Classroom Norms and Expectations
DO: Record as many specific examples of the class norms on the table group handout. How you should “Be here”? How you should you “Listen”? How you should “Do your work”? Lastly, what is it like to “Be Cool”? TIME: 7 minutes WHEN DONE: Take out highlighter and highlight top 2 in each category and the person with the shortest hair writes the top 2 on the white board in under each category.

6. Everyone Pose at the Front of the Classroom
DO: Stand up at front of the room for picture (underneath periodic table) BE READY: For your picture to be taken as a group TIME: 45 seconds

7. Glue Sticks are in the pencil/pen bins at your table
IF YOU NEED MORE SUPPLIES: COME TO FRONT OF ROOM
(Scissors and Glue Sticks)
Notebook Set Up
FIND: Notebook Set Up Instructions in blue bins on table DO: Follow the instructions on the notebook set up page. Ask for help if you need it! The last thing you should work on is the “Who I Am” page! TIME: 16 minutes WHEN DONE: Show Ms. Myriah Day your back cover!
Glue Sticks are in the pencil/pen bins at your table

8. Chemistry
Chemistry is the study of the properties and behavior of matter.
It is central to our fundamental understanding of many science-related fields.

9. Chapter 1 Book Notes How do I classify states of matter? EQ:
How do I use measurement in chemistry?
EQ:
1.2 Classifications of Matter
States of Matter
Composition of Matter

10. Matter
Matter is anything that has mass and takes up space.

11. Matter Atoms are the building blocks of matter.
Each element is made of a unique kind of atom.
A compound is made of two or more different kinds of elements.
Note: Balls of different colors are used to represent atoms of different elements. Attached balls represent connections between atoms that are seen in nature. These groups of atoms are called molecules.

12. Methods of Classification
State of Matter
Composition of Matter

13. States of Matter The three states of matter are
solid
liquid
gas
In this figure, those states are ice, liquid water, and water vapor.

14. Classification of Matter Based on Composition
If you follow this scheme, you can determine how to classify any type of matter.
Homogeneous mixture
Heterogeneous mixture
Element
Compound
Matter
And
Measurement

15. Classification of Matter—Substances
A substance has distinct properties and a composition that does not vary from sample to sample.
The two types of substances are elements and compounds.
An element is a substance which can not be decomposed to simpler substances.
A compound is a substance which can be decomposed to simpler substances.

16. Compounds and Composition
Compounds have a definite composition. That means that the relative number of atoms of each element that makes up the compound is the same in any sample.
This is The Law of Constant Composition (or The Law of Definite Proportions).

17. Classification of Matter—Mixtures
Mixtures exhibit the properties of the substances that make them up.
Mixtures can vary in composition throughout a sample (heterogeneous) or can have the same composition throughout the sample (homogeneous).
Another name for a homogeneous mixture is solution.

18. Check for Understanding
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Check for Understanding
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19. Apple juice is an example of a(an)
DISCUSS WITH YOUR TABLE GROUP: Which answer is correct and be prepared to justify your answer
Apple juice is an example of a(an)
element
compound
homogeneous mixture
heterogeneous mixture
Answer: c

20. Which of the following is not a pure substance?
DISCUSS WITH YOUR TABLE GROUP: Which answer is correct and be prepared to justify your answer
Which of the following is not a pure substance?
water
carbon dioxide
carbon
air
Answer: d

21. Chapter 1 Book Notes How do I classify states of matter? EQ:
How do I use measurement in chemistry?
EQ:
1.3 Properties of Matter
Physical and Chemical Changes
Separation of Mixtures

22. Types of Properties
Physical Properties can be observed without changing a substance into another substance.
Some examples include boiling point, density, mass, or volume.
Chemical Properties can only be observed when a substance is changed into another substance.
Some examples include flammability, corrosiveness, or reactivity with acid.

23. Types of Properties
Intensive Properties are independent of the amount of the substance that is present.
Examples include density, boiling point, or color.
Extensive Properties depend upon the amount of the substance present.
Examples include mass, volume, or energy.
End Here 9/6/2016

24. Types of Changes
Physical Changes are changes in matter that do not change the composition of a substance.
Examples include changes of state, temperature, and volume.
Chemical Changes result in new substances.
Examples include combustion, oxidation, and decomposition.

25. Changes in State of Matter
Converting between the three states of matter is a physical change.
When ice melts or water evaporates, there are still 2 H atoms and 1 O atom in each molecule.

26. Chemical Reactions (Chemical Change)
In the course of a chemical reaction, the reacting substances are converted to new substances. Here, the elements hydrogen and oxygen become water.

27. Separating Mixtures
Mixtures can be separated based on physical properties of the components of the mixture. Some methods used are
filtration
distillation
chromatography

28. Filtration
In filtration, solid substances are separated from liquids and solutions.

29. Distillation
Distillation uses differences in the boiling points of substances to separate a homogeneous mixture into its components.

30. Chromatography
This technique separates substances on the basis of differences in the ability of substances to adhere to the solid surface, in this case, dyes to paper.

31. Check for Understanding
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Check for Understanding
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32. Descriptions of a sample that are based on the amount of substance are called
physical properties
chemical properties
intensive properties
extensive properties
Answer: d

33. Properties that describe the way a substance reacts to form other substances are called
physical properties
chemical properties
homogeneous properties
heterogeneous properties
Answer: b

34. Acetic acid that was liquid when stored was solid when a student looked for it on a cold morning. This illustrates
Answer: d
a change in solubility
a chemical change
an equilibrium state
a physical change

35. A copper wire placed in a silver nitrate solution turns dark and “fuzzy.” This illustrates
an accident
a chemical reaction
an extensive property
a physical change
Answer: b

36. A solution with a boiling point of 105 C contains either sugar or salt. How would you determine which is present?
distill the solution
filter the solution
use chromatography
taste the solution
Answer: a
Boiling Point: Sugar = 320

37. Chapter 1 Book Notes How do I classify states of matter? EQ:
How do I use measurement in chemistry?
EQ:
1.4 Units of Measurement
SI Units

38. Numbers and Chemistry
Numbers play a major role in chemistry. Many topics are quantitative (have a numerical value).
Concepts of numbers in science
Units of measurement
Quantities that are measured and calculated
Uncertainty in measurement
Significant figures
Dimensional analysis

39. Units of Measurements—SI Units
Système International d’Unités (“The International System of Units”)
A different base unit is used for each quantity.

40. Units of Measurement—Metric System
The base units used in the metric system
Mass: gram (g)
Length: meter (m)
Time: second (s or sec)
Temperature: degrees Celsius (oC) or Kelvins (K)
Amount of a substance: mole (mol)
Volume: cubic centimeter (cc or cm3) or liter (l)

41. Units of Measurement — Metric System Prefixes
Prefixes convert the base units into units that are appropriate for common usage or appropriate measure.

42. Mass and Length These are basic units we measure in science.
Mass is a measure of the amount of material in an object. SI uses the kilogram as the base unit. The metric system uses the gram as the base unit.
Length is a measure of distance. The meter is the base unit.

43. Volume
Note that volume is not a base unit for SI; it is derived from length (m × m × m = m3).
The most commonly used metric units for volume are the liter (L) and the milliliter (mL).
A liter is a cube 1 decimeter (dm) long on each side.
A milliliter is a cube 1 centimeter (cm) long on each side, also called 1 cubic centimeter (cm × cm × cm = cm3).

44. Temperature
In general usage, temperature is considered the “hotness and coldness” of an object that determines the direction of heat flow.
Heat flows spontaneously from an object with a higher temperature to an object with a lower temperature.

45. Temperature
In scientific measurements, the Celsius and Kelvin scales are most often used.
The Celsius scale is based on the properties of water.
0C is the freezing point of water
100C is the boiling point of water
The kelvin is the SI unit of temperature.
It is based on the properties of gases
There are no negative Kelvin temperatures
The lowest possible temperature is called absolute zero (0 K)
K = C

46. Temperature
The Fahrenheit scale is not used in scientific measurements, but you hear about it in weather reports!
The equations below allow for conversion between the Fahrenheit and Celsius scales:
F = 9/5(C) + 32
C = 5/9(F − 32)
Many theories of why Fahrenheit was used, but the main reason was the myth that the body would freeze to death at 0 and experience heat stroke at 100. Also,, German born scientist Daniel Gabriel Fahrenheit used mercury for his thermometer and it was more accurate or easy to use than the alcohol-based thermometer developed by Danish scientist Olaus Roemer. (Countries that use Fahrenheit: Bahamas, Belize, Cayman Islands, Palau, United States and associated territories).

47. Density Density is a physical property of a substance.
It has units that are derived from the units for mass and volume.
The most common units are g/mL or g/cm3.
Density = Mass/Volume (D=m/V)

48. Numbers Encountered in Science
Exact numbers are counted or given by definition. For example, there are 12 eggs in 1 dozen.
Inexact (or measured) numbers depend on how they were determined. Scientific instruments have limitations. Some balances measure to ±0.01 g; others measure to ±0.0001g.

49. Check for Understanding
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Check for Understanding
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50. Heat flows from an object
at high temperature to an object at low temperature
at low temperature to an object at high temperature
to another object at the same temperature
at high elevation to an object at low elevation
Answer: a

51. An average car holds .05 kL of gasoline. How many L is 0.05 kL?
Answer: a

52. Chapter 1 Book Notes How do I classify states of matter? EQ:
How do I use measurement in chemistry?
EQ:
1.5 Uncertainty in Measurement
Precision
Accuracy
Significant Figures

53. Uncertainty in Measurements
Different measuring devices have different uses and different degrees of accuracy
All measured numbers have some degree of inaccuracy

54. Accuracy versus Precision
Accuracy refers to the proximity of a measurement to the true value of a quantity.
Precision refers to the proximity of several measurements to each other.

55. Check for Understanding
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Check for Understanding
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56. In three trials, a student measures a sample’s mass to be to be 0
In three trials, a student measures a sample’s mass to be to be g, g, and g. The accepted value is g. The student’s data have
good accuracy and good precision.
good accuracy, but poor precision.
poor accuracy, but good precision.
poor accuracy and poor precision.
Answer: b

57. Significant Figures
The term significant figures refers to digits that were measured.
When rounding calculated numbers, we pay attention to significant figures so we do not overstate the accuracy of our answers.

58. Significant Figures All nonzero digits are significant.
Zeroes between two significant figures are themselves significant.
Zeroes at the beginning of a number are never significant.
Zeroes at the end of a number are significant if a decimal point is written in the number.

59. Significant Figures
When addition or subtraction is performed, answers are rounded to the least significant decimal place.
When multiplication or division is performed, answers are rounded to the number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation.

60. Check for Understanding
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Check for Understanding
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61. The measured quantity 0.0860 g contains _____ significant figures.
three
four
five
six
Answer: a

62. 4.1 g g = _____ g
11.180
11.18
11.2 11
Answer: c

63. 6.9 g – 5.07 g = _____ g
1.830
1.83
1.8 1
Answer: c

64. 5.2 cm × 7.01 cm = ____ cm2 36
36.4
36.45
36.452
Answer: a

65. 6.03 g ÷ 7.1 mL = _____ g/mL
0.8
0.85
0.849
Answer: b

66. Chapter 1 Book Notes How do I classify states of matter? EQ:
How do I use measurement in chemistry?
EQ:
1.5 Dimensional Analysis
Converting Units
Conversion Factors

67. Dimensional Analysis
We use dimensional analysis to convert one quantity to another.
Most commonly, dimensional analysis utilizes conversion factors (e.g., 1 in. = 2.54 cm).
We can set up a ratio of comparison for the equality either 1 in/2.54 cm or 2.54 cm/1 in.
We use the ratio which allows us to change units (puts the units we have in the denominator to cancel).

68. Check for Understanding
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Check for Understanding
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69. 120 mL = _____ fl oz 2 4 6 8
Answer: b
30 mL = 1 fl oz

75. Significant Figures All nonzero digits are significant.
Zeroes between two significant figures are themselves significant.
Zeroes at the beginning of a number are never significant.
Zeroes at the end of a number are significant if a decimal point is written in the number.