1. Chemistry !!
The study of the composition,
__________, and properties of matter
and the ____________________
Chemists make measurements to ________________ of matter. To keep things consistent, we all work in __________

2. Matter?
Matter is anything that occupies space and has mass. Chemistry is the study of matter and how it changes

3. Matter Volume - _____________ Mass - measure of __________.
(even air !)
measured in ____and ____
Mass - measure of __________.
____in ____________

4. Chemical
Any substance that has a definite composition
Examples:

5. Atom The smallest unit of an Element that _____________
Properties of that element

6. Classification of Matter

7. Elements/Compounds
Elements _____ be separated into simpler substances by chemical means. Example: __________ Smallest part is an ______
Compounds are composed of atoms of _________ elements. Examples:_________________

8. Phases of Matter There are three common phases of matter:
____ – closely spaced and _____
____ – closely spaced but _____
____ – large separation; mostly _____________

9. 3 States of Water

10. Phase
Atom Movement
Shape
Volume
Energy
Solid
Liquid
Gas

11. Properties
An ________ property _______ on __________ matter is being considered. Example:
An _________ property _______ depend on __________ matter there is. Example:

12. Properties?
In Chemistry we study of matter and how it changes; we need to be able accurately observe properties to do this!

13. Properties
A __________ property is a characteristic that can be observed or measured _______ changing the identity of the substance.
Examples include

14. Properties
A _________ property is a characteristic that describes the _______ of a substance to undergo changes that alter its identity.
Examples include the _____ of coal ______ and the _____ of iron _______.

15. Properties
A _______ change is when a substance changes physical condition but ________ involve a change in composition.
A _______ change is when a substance changes a substance ______________________ of substances.

16. Properties
Classify each of the following as either a physical change or a chemical change:
Tearing a sheet of paper
Melting a piece of wax
Burning a log
Milk turns sour -

17. Mixtures/Substances
Mixtures contain two or more substances and generally can be __________________.
Pure substances have a _______ _____________ and distinct properties.

18. Mixtures
Homogeneous means the ______ throughout. ________ separate by filtering. Ex.
Heterogeneous means that it is ___________. ____ separate by filtering. Ex.

19. Scientific Method

20. Definitions ___________ – a testable statement
______ – an explanation of how phenomena occur and how data and events are related
_________ – a broad generalization that explains a body of facts

21. Equipment Commonly used for liquid measures

22. Liquid Volumes Volume read to the bottom of the _________

23. SI Units?
Measurements can be made in many different units. To be consistent, all scientists use the metric system to report measurements. Metric system units are called ________
_________________

24. SI Units Examples Measurement Unit Abbrev. mass gram length meter
volume
liter
time
second
temperature
Kelvin
energy
Joule
Amount of sample
Moles

25. Label each instrument with the SI correct units

26. Temperature Conversions
Like most measurements, temperature has many forms. There are three common ways to report temperature: Fahrenheit (F ), Celsius (C ), and Kelvin (K ).
K = C or C = K
F = (1.8)(C ) + 32

27. Temperature Conversion?
So, if it is 35 C , would you go skiing or swimming?
What is the temperature inF ?
In K ?
____  F
____ K

28. Base Unit – meter (m), liter (l), or grams (g)
SI Subunits
Prefix
Abbrev.
Factor
Mega M-
1 x 106
Kilo K-
1 x 103
Hecto H-
1 x 102
Deka D-
1 x 101
Base Unit – meter (m), liter (l), or grams (g)
deci- d-
1 x 10-1
centi- c-
1 x 10-2
milli m-
1 x 10-3
micro- m
1 x 10-6
nano- n-
1 x 10-9
pico- p-
1 x 10-12

29. Metric Conversions
Meter (m)
Liter (l)
Gram (g)
Joule (J)

30. Unit Conversion?
In Chemistry, we can make measurements in many different units. So, we often need to convert to another set of units. We need three things: where you are __________ where you are _______, and 3. the __________________ to get you there.

31. Converting Units Example
To convert units you need to know where you are starting, finishing, and the conversion factor.
Find the number of cm in 2.1 meters.
We know: 1 m = 100 cm
2.1 m cm = ____ cm 1 m

32. Converting Units Find the number of Kg in 8,200 g.
We know: g = 1 Kg
8,200 g 1 Kg = ____ Kg g

33. SI Subunits Conversions
10.5 g = _________ kg
1.57 km = _______ m
3.54 mg = __________ g
3.5 J = _________ DJ
1.2 L = _____ ml
358 cm3 = _________ m3

34. 2.8 in = ____ cm How many inches in 12.4 cm? 12.4 cm = ____ in
Converting Units
How many cm are in 2.8 inches.
Conversion Factor: in = 2.54 cm
2.8 in = ____ cm
How many inches in 12.4 cm?
12.4 cm = ____ in

35. Unit Conversion Examples
First we need conversion factor !
12 oz. = 355 ml
How many ounces in 600 mls?
mls = ______ oz

36. Converting Time How many days are there in 52,480 minutes?
How many minutes are there in 2.4 months?
= ___________
minutes

37. Conversions with two units
If you are traveling 20 miles/hour, how many meters/seconds is this?
Change one unit at a time. Note, many ways to do this.

38. Conversions with two units
Convert 25 miles/gallon to km/liter
= ______ km/l
Convert 10 kg/liter to g/ml
= ______ g/ml

39. Precision vs. Accuracy

40. _________
_______
Accuracy and
Precision
_________
_______________

41. Precision Refers to the closeness of a set of measurements __________
Requires that ____________ measuring the same thing be done
Example:
2.22,2.23,2.21 shows good precision

42. Accuracy
Refers to how close an answer ________ is to __________ or correct value
Requires that the accepted value is ______
Use ___________ to express accuracy

43. Percent Error _________ = experimental value – accepted value
(value can be _______ or ________)
___________
experimental value – accepted value x 100
accepted value
(absolute value)

44. Significant figures?
In most cases it is __________ to obtain the exact value for a measurement. We need to _____________ the significant figures - the meaningful digits in a measured or calculated quantity. The trick is _______ _____________________!

45. Significant Figures Rules for determining sig. figs.:
1.All non-zero #’s are sig.
2. Zeros between non-zeros are sig. (a zero sandwich!)
3. Zeros to the left of the first non-zero # are not sig.
-> ______
-> _______
-> ______

46. Significant Figures Rules
4. Zeros at the end of a number and to the right of a decimal are sig. They are holding a place!
For #’s w/out decimals, the trailing zero may or may not be sig. We use Sci. notation on these.
-> ______

47. 1,000,000 years –
now 1,000, years ??
Which zeros are important?
Use scientific notation: Could be _________
or ________ or ____________, etc.

48. Significant Figures Determine the sig figs & Rule #: 6.002 cm 0.0020 m
7000 kg
-> _____________
-> _____________
-> ______________
-> _______________ _________________

49. Scientific Notation Examples
Distance to Sun:
93,000,000 miles -> _______ miles
2. Vacuum pressure:
torr -> _______ torr

50. Sci. Not. w/ Calculators Example: 4 x 1023 x 5 x 10-12 = ? Action
Display
Enter “4” 4
Press “EE”
4 00
Enter “23”
4 23
Press “x“
Enter “5” 5
5 00
Enter “-12”
5 -12
Press “=“
(2 x 1012)

51. Significant Figures Rules for adding and subtracting:
Answer cannot have more digits to the right of decimal point than the original!!
89.332
+ 1.1
90.432
____
round off

52. Significant Figures Rules for multiplying and dividing:
Answer cannot have more significant figures than the original!
s.f.
x s.f.
___
round off

53. Significant Figures Report with the correct # of sig. fig.:
11,254.1 g g
66.59 L – 3.13 L
8.16 m x m
kg / 88.3 ml
-> ______ g
-> _______ L
-> ____m;__ sf.
-> _________ kg/ml; ___ s.f.

54. Measurements?
Chemists make measurements to study the properties of matter. To keep things consistent, we all work in SI Units and use significant figures. We also make many conversions between different types of _________ ________. We also make many ________________

55. Derived Units
Mathematical combinations of units
Examples are:

56. Density?
Density is a common physical property that relates the mass and volume of a substance:
Density =
Units: grams/mls or
grams/cm3

57. Density Example Density = mass/volume
What is the density of a substance that has a mass of 84.7 g and a volume 55.4 cm3.
Density = mass/volume
g = _____ g/cm3
cm3

58. Density Example g cm3 = ___ cm3 g
What is the volume of a substance that has a density of 1.73 g/cm3 and a mass of 7.75 g.
g cm3 = ___ cm g
Density is a conversion factor g = 1.00 cm3
or 1.00 cm3 = 1.73 g