1. Matter and Change

5. II. Matter and Its Properties A. Properties of Matter
I. Chemistry: the study of matter, its structure, & the changes it undergoes (or the science of materials around us).
1. Branches of Chemistry
Inorganic Organic Analytical Physical Biochemistry Theoretical
II. Matter and Its Properties
A. Properties of Matter
1. Physical Property: a characteristic that can be observed or measured without changing the identity of the matter

6. a. Extensive: properties that depend on the. amount of
a. Extensive: properties that depend on the amount of matter that is present
Ex: volume, mass, energy in substance
b. Intensive: properties that do not depend on the amount present
Ex: melting point, boiling point, density
2. Chemical property: relates to a substance’s ability to undergo changes that transform into different substances
B. Changes in Matter
1. Physical change: a change in a substance that does not involve a change in the identity of the substance (examples)

7. 2. Chemical change: a change in which one or more substances are converted into different substances Examples: digestion, rusting, milk souring a. reactants: the substances that react b. products: the substances that are formed

8. Matter C. Classify Matter (+ Justify) * 4 Classes  Heterogeneous
Element, Compound, Homogeneous Mixture (solution), Heterogeneous Mixture
Matter
Heterogeneous
Homogeneous
Mixture
Solution
Pure Substance
Compound
Element

9. III. Building Blocks of Matter A
III. Building Blocks of Matter A. An atom is the smallest unit of an element that maintains the chemical identity of that element B. An element is a pure substance that cannot be broken down into simpler, stable substances and is made of one type of atom C. Classification of elements 1. Metals: - have luster - reflectors - conductors (of heat or electricity) - ductile - malleable

10. Metallic Elements

11. 2. Nonmetals: *properties are opposite of metals - brittle
- non-ductile
- dull (no luster)
- does not conduct heat or electricity
3. A metalloid is an element that has some characteristics of metals and some characteristics of nonmetals
4. Noble gases: are generally unreactive (or inert)

12. Nonmetallic
Elements

13. Metalloids
Silicon
Arsenic

15. B. Scientific Graphs – used to show relationships between variables
1. Criteria for the graphs:
a. Plot the independent variable on the x-axis & the dependent on the y-axis.
b. Label each axis with the name of each variable and put the units for each variable in parenthesis
c. Choose the appropriate increments for each axis.
d. Convert each “ordered pair’ of measurements to plotted points on the graph.
e. Analyze the trend & draw the “best fit” line or curve.
f. Title the graph.
g. Interpret the graph (look for trends- direct or indirect)

17. States of Matter
The three common states of matter are solid, liquid, and gas.
Solids:
1.) definite volume, definite shape.
2.) Particles are tightly packed together.
3.) Least amount of kinetic energy.
4.) Adding energy to a solid changes it into a liquid.
Liquids:
1.) definite volume, indefinite shape.
2.) Particles are loosely packed together.
3.) Moderate amount of kinetic energy.
4.) Adding energy to a liquid changes it into a gas.
5.) Removing energy from a liquid changes it into a solid.

18. States of Matter
Gases:
1.) indefinite volume, indefinite shape.
2.) Particles are the farthest apart.
3.) Greatest amount of kinetic energy.

19. Measurements and Calculations

20. I. Measurements & the Metric System
A. Why Measure? In order to get complete observations, quantifying is essential. `
B. Measurements consist of:
1. Quantity
a. Anything that can be measured
b. Involves a number followed by a unit
c. Examples: Volume, Mass, Length, Time
2. Unit (can be English or metric)
Is what the quantity is measured in
Examples:
English: Gallon, Foot, Pound, Second
Metric: Liter, Meter, Gram, Second
C. Why Use the Metric System?
1. It’s easier because it is based on units of 10
2. Everyone uses it so it gives consistency
3. There are standards that everyone can compare to

21. D. International System of Units – called SI
1. Composed of fundamental or base units.
Chart 1-1
Quantity
Standard Unit
Symbol
Length
Meter m
Mass
Kilogram kg
Time
Second s
Temperature
Kelvin K
Amount/Count
Mole
mol

22. millimeters of mercury
2. Derived units: measurements that use a combination of the base units
Chart 1-2
Quantity
Name
Symbol
Area
square meter m2
Volume
cubic meter m3
Voltage
volt V
Frequency
hertz Hz
Pressure
pascal Pa
millimeters of mercury
mmHg
atmospheres
atm
Energy/Work
joule J
Speed/Velocity
meters per second
m/s

23. Multiplication Factor
3. Metric System Prefixes: attached to a unit, making it more convenient or easy to use
Chart 1-3
Symbol
Prefix
Multiplication Factor G
giga –
109
1,000,000,000 M
mega –
106
1,000,000 k
kilo –
103
1,000 h
hecto –
102
100 da
deka –
101 10
BASE UNIT
NO PREFIX d
deci –
10-1 .1 c
centi –
10-2
.01 m
milli –
10-3
.001 μ
micro –
10-6
.000,001 n
nano –
10-9
.000,000,001

24. II. Uncertainty in Measurement
A. There is ambiguity in every measurement. Why?
1. Instruments are never completely free of flaws.
2. Measuring involves estimation – because humans are reading displays (either digital or scale)
* The last number in any measurement is estimated and therefore uncertain
B. Accuracy: how close a measurement is to the true or accepted value
𝑷𝒆𝒓𝒄𝒆𝒏𝒕 𝑬𝒓𝒓𝒐𝒓= 𝐄𝐱𝐩𝐞𝐫𝐢𝐦𝐞𝐧𝐭𝐚𝐥 𝐕𝐚𝐥𝐮𝐞−𝐀𝐜𝐜𝐞𝐩𝐭𝐞𝐝 𝐕𝐚𝐥𝐮𝐞 𝐀𝐜𝐜𝐞𝐩𝐭𝐞𝐝 𝐕𝐚𝐥𝐮𝐞 𝒙 𝟏𝟎𝟎
*Note – the experimental value will be the average if more than one trial is performed for the experiment.

25. III. Working with Numbers
C. Precision: how reproducible the measurements are (how closely related the measurements are)
III. Working with Numbers
A. Scientific Notation:
M x 10n
M  move the decimal so you get a number less than 10 but greater than 1
n  how many spaces decimal was moved
(+)  if moved decimal left
(-)  if moved decimal right
1. Ex: Write numbers in scientific notation
a. 4, 000 ________
4 x 103
b. 72, 000, 000 ________
7.2 x 107

26. 2. Ex: Write numbers in positional notation.
c ________
2.5 x 10-4
d ________
9.05 x 10-2
2. Ex: Write numbers in positional notation.
a. 6.1 x 108 ________
610,000,000
b. 4.3 x 10-3 ________
.0043
c x 10-7 ________
d x 102 ________
428
B. Significant Figures: the digits in a measurement that are certain, plus the one that is uncertain.
*Tells the accuracy of the measuring instrument!!

27. 1. Rules for Individual measurements (page 47)
All non-zero digits are significant.
a. Zeros appearing between non-zero digits are significant.
examples: L = ________ sig figs; 870,009 km = ________ sig figs;
mm = ________ sig figs; =________ sig figs 3 6 5 4
b. Zeros appearing in front of all nonzero digits are not significant
examples: m = ________ sig figs; kg = ________ sig figs;
0.140 g = ________ sig figs; =________ sig figs 5 1 3 4

28. 0.006700 km = ________ sig figs; 0.01200700 L=________ sig figs
c. Zeros at the end of a number and to the right of a decimal point are significant.
examples: g = ________ sig figs; mm= ________ sig figs;
km = ________ sig figs; L=________ sig figs 4 10 4 7
d. Zeros at the end of a number but to the left of a decimal point are not significant unless there is a decimal point after the zeros.
examples: m = ________ sig figs; m= ________ sig figs;
1780 cm = ________ sig figs; mL=________ sig figs 1 4 3 5
2. Ex: How many significant figures for the measurements?
a cm _____ e L _____
b. 205 kg _____ f. 700 mL _____
c. 4,000 mm _____ g Mg _____
d. 6.7 x 103 km _____ h. 10,680 mg _____ 4 2 3 1 1 5 4 2

29. 4. Rules for Operations – Multiplication & Division
a. Perform operation, then round answer to the least significant number for the measurements given.
b. Ex: Perform the operation and round answer to the correct # of significant figures.
.028
1.) 4.50 x ________
2.) (5.622)(72.3) 320 ________
1.3
3.) (6.5 x 10-2) (3.27 x 10-3) ________
2.1 x 10-4
3.6 x 10-5
4.) (2.35)(.45723)(546) ________
(379)(4.3 x 104)

30. 3. Rules for Operations – Addition & Subtraction
a. Perform operation, then round answer to the leftmost doubtful digit for the measurements you are adding or subtracting.
b. Ex: Perform the operation & then round the answer to the correct # of significant figures.
1.) – ________
13.78
2.) – .20 ________
.07

31. VII. Problem Solving
A. Dimensional Analysis: technique for converting between units
1. Within the Metric System – move the decimal for how many jumps the multiple makes on the prefix chart 1-3
a. Ex: Convert 43 m to . . .
1.) km ________
2.) cm ________
3.) mm ________
.043
430
4,300

32. b. Convert 276 g to . . . 1.) mg ________ 276,000 27,600 0.276
2.) cg ________
2.) kg ________
276,000
27,600
0.276