The document provides an overview of key concepts in chemistry including the structure of atoms, states of matter, properties of matter, and the periodic table. It defines atoms as the smallest particle of an element and notes they are composed of protons, neutrons, and electrons. The periodic table is introduced and elements are organized based on atomic number and recurring properties within periods and groups. Key terms like atomic number and mass number are defined. States of matter such as solids, liquids, and gases are contrasted based on properties like volume and shape. Physical and chemical properties and changes in matter are also distinguished.

1. Unit 1
Structure and Properties of Matter
States of Matter
Structure of Atoms
Periodic Table
1st 6wks

2. Important SI Base Units
Quantity Symbol Unit Abbreviation
Length l meter m
Mass m kilogram kg
Time t second s
Temperature T Kelvin K
Amount n mole mol

3. Prefixes
• Prefixes are added to the base unit names to
represent quantities smaller or larger
M mega 106 1,000,000 larger
k kilo 103 1,000 larger
c centi 10-2 1/100 smaller
m milli 10-3 1/1000 smaller
μ micro 10-6 1/1,000,000 smaller

4. Controls and Variables
1. Experiments are comprised of controls and
variables.
1. Controls provide a standard for comparison.
1. You compare the results of your
experiment to the control to determine if
change has occurred.
2. If controls are missing, no comparison of
test data to a known standard is possible,
rendering the data meaningless.

5. 1.Independent variable – the part of the
experiment that you are manipulating
2.Dependent variable – the part of the
experiment that responds to changes in the
independent variable (i.e. what you are
measuring)

6. What is the Independent and Dependent variable?
What axis are each found on ?

7. Bart believes that mice exposed to microwaves will become
extra strong (maybe he's been reading too much Radioactive
Man). He decides to perform this experiment by placing 10
mice in a microwave for 10 seconds. He compared these 10
mice to another 10 mice that had not been exposed. His test
consisted of a heavy block of wood that blocked the mouse
food. He found that 8 out of 10 of the microwaved mice were
able to push the block away. 7 out of 10 of the non-
microwaved mice were able to do the same.
14. What is Bart trying to
test?
15. Control group?
16. Constants?
17. Independent Variable?
18. Dependent Variable?
19. What should Bart’s
conclusion be?
20. How could this
experiment be improved?

8. Success in chemistry will depend highly on your ability to measure
correctly. Measurements need to be both correct and
reproducible
Accuracy- how close a measurement comes to the actual
value of what is being measured.
•determined by how well the measuring tool is used
Precision- how close a series of measurements of the
same object are to one another
•determined by type of instrument used

9. Accurate or Precise?

10. The acceleration time of a car is 11.4 m/s2
Which Group(s) are more precise or more accurate ?

11. Matter and Its Properties

12. Solid
»definite volume
»definite shape
»atoms in fixed positions
»strong attractive forces
»only vibrate in place
»Water freezes at 0°C or
32°F

13. Liquid
» definite volume
» indefinite shape
» close together
» Overcome
attractive forces to
flow
•Water melts at 0°C
or 32°F

14. Gases
»Indefinite volume
»indefinite shape
»move very quickly
»Far apart
»Weak attractive forces
»Water becomes a gas
at 100°C or 212°F

15. Changes of State

16. Plasma
• high temperature state in which atoms lose
their electrons
– Ionized or deionized
• Ex. the sun

17. B. Heating Curves
• Kinetic Energy
– motion of particles
– related to temperature
• Potential Energy
– space between particles
– related to phase changes

18. B. Heating Curves
Solid - KE 
Melting - PE 
Liquid - KE 
Boiling - PE 
Gas - KE 

19. Pure

20. Terms
• Matter- anything that has mass and volume
• Atom- smallest unit of an element that keeps the
properties of element
• Element- pure substance made of only one type
of atom
• Compound- substance made of 2 or more types
of atoms that are chemically bonded

21.  looks like one thing , but its
not
Examples
air, tap water, soda, jewelry
(metal alloys)
 Can be separated by physical means (filtering,
distillation, etc.)
Homogeneous mixture (solutions) Heterogeneous mixture
 looks different throughout
 all the different stuff can
be seen
Examples
soup, sand, concrete, salad,
salad dressing

22. Types of Properties
• Physical- characteristics that can be observed
or measured without changing the identity of
a substance
• Ex. melting point, boiling pt
• Chemical- relates to a substances ability to
undergo changes that transform it into a
different substance
• Easiest to see when a chemical is reacting

23. Physical Changes in Matter
• change in a substance that doesn’t change the
identity of the substance
• Ex. grinding, cutting, melting, boiling
• Includes all changes of state (physical changes
of a substance from one state to another)

24. Chemical Changes in Matter
• a change in which a substance is converted
into a different substance- chemical reaction
• doesn’t change the amount of matter present
• reactants- substances that react
• products- substances that form

25. Energy Changes in Matter
• When any change occurs, energy is
always involved

26. Energy Changes in Matter
• Exothermic Reaction- gives off energy (feels warm)
• Endothermic Reaction- uses up energy (feels cold)

27. Chemical or
Physical Change
Draw a T-chart on you paper to categorize the following
pictures as either a physical or chemical change

28. Sublimation of Iodine

29. Filtration of a sand and salt-water mixture

30. Dissolving sugar in water

31. Crystallization of a supersaturated solution

32. Rusting Iron

33. Distillation of water and alcohol

34. Burning Candle

35. Boiling Water

36. Chewing Food

37. Digestion Of Food

38. Burning Wood

39. Evaporation of Water

40. Decomposition of water by electrolysis

41. Acid Rain acting on limestone

42. Metal salts burning in alcohol or
combustion of alcohol

43. Tarnishing Silver

44. Melting Wax

45. Carbonic acid reacting with limestone

46. Sodium Reacting with Water

47. Melting Ice

48. Matter and Its Properties cont.

49. • Mass divided by volume
– Objects that have a
greater density than
water sink.
m
d v
http://www.youtube.com/watch?v=VAevsIHDn
hQ&feature=related

50. Density
• ratio of mass to volume
• SI:
volume
mass
Density 
3
m
kg
 Density of an object doesn’t change with the amount
because as volume increases, mass also increases
 Density usually decreases as Temp increases
exception: ice is less dense than liquid water so it floats

51. Density of Water
• The density of pure water is 1g/cm3
• If an objects density is less than 1g/cm3 it will float on
water.
• Diamond 3.5
• Cork 0.2 - 0.3
• Magnesium 1.738
• Oil 0.8
• Glass 2.6
• Ice 0.92
• Glycerine 1.26
• Coal 1.5
• Concrete 2.4
• Liquid Ammonia 0.682
• Quartz 2.65
• Alcohol (Ethanol) 0.789
• Aluminum 2.7
SINK OR FLOAT

52. Example
A sample of aluminum metal has a mass of 8.4
g. The volume is 3.1 cm3. Find the density.
Known Unknown
m = 8.4 g D = ?
V = 3.1 cm3
33
7.2
1.3
4.8
cm
g
cm
g
V
m
D 
m
d v

53. Example
Known Unknown
D = 3.5 g/cm3 M = ?
V = ?
ggvdm 3.6cm8.1cm/5.3 33

m
d v

54. Example
A diamond has a density of 3.5g/cm3. The
volume is 1.8 cm3. Find the mass.
Known Unknown
D = 3.5 g/cm3 M = ?
V = 1.8 cm3
ggvdm 3.6cm8.1cm/5.3 33

m
d v

55. Example
A diamond has a density of 3.5g/cm3. The mass
is 9.7g. Find the volume.
Known Unknown
D = 3.5 g/cm3 V= ?
M= 9.7g
3
3
77.2
cm/5.3
7.9
cm
g
g
d
m
v 
m
d v

56. Viscosity-a fluid’s resistance to flow
– Thick syrup has a
higher viscosity than
water
Low viscosity
High viscosity

57. Buoyancy
• Buoyancy - the upward force that a fluid
exerts on an object.
• Archimedes Principle – the force exerted on
the object in a liquid is equal to the weight of
the fluid displaced by the object.
• Buoyancy is why objects float – a steel boat
will float because of it’s shape.

60. Ship is
pushing down
on water
Water is
pushing up on
the ship

61. Ship goes down
Water goes up
(displaced)
Ship is
pushing down
on water
Ship is
pushing down
on water

62. Ship goes down
Water goes up
(displaced)
Ship is
pushing down
on water
Ship is
pushing down
on water

63. Ship goes down
Water goes up
(displaced)

64. Ship goes down
Water goes up
(displaced)

65. The Periodic Table

66. Elements
• Elements are pure substances
• Organized by properties on periodic table
• Each square shows the name and letter
symbol for each element
• Some names originate from Latin.

67. Periodic Table
• Groups/Families
– vertical columns
– numbered 118
– similar chemical properties
• Periods
– horizontal rows
– properties changes consistently across a period

68. Periodic Table

69. Periodic Table
• two rows below the periodic table are the
lanthanide and actinide series
• these rows fit after #57 and #89
• they are only at the bottom to keep the width
of the chart smaller

70. Types of Elements
• Metals
– good conductor of electricity
– at room temp, most are solids
– malleable- can be rolled or hammered
into sheets
– ductile- can be made into wire
– high tensile strength- can resist
breakage
– most have silvery or grayish white
luster

71. Types of Elements
• Nonmetals
– poor conductor of heat and electricity
– many are gases at room temp
– some are solids: usually brittle, not malleable

72. Types of Elements
• Metalloids
– some characteristics of metals and nonmetals
– along staircase line
– B, Si, Ge, As, Sb, Te
– solids at room temp
– less malleable than metals- less brittle than
nonmetals
– semiconductors

73. Types of Elements
• Noble Gases
– unreactive gases
– Group 18

74. Atomic Structure
IPC Unit 2

75. Atoms
• Smallest piece of matter
• All matter is made of atoms

76. Atomic Structure
3 subatomic particles
–Protons
–Neutrons
–Electrons
At the center is the
nucleus
• Highly Dense &
positively charged

77. Protons
• Positively charged in the nucleus

78. Neutrons
• Neutrally charged in the nucleus

79. Electrons
• Negatively charged outside the
nucleus

80. Atomic Symbol
• The abbreviation for the element
name

81. Atomic Number
• The # of protons

82. Average Atomic Mass
• The average mass of an atom of that
element

83. Mass #
• mass # = protons + neutrons
• Round Atomic Mass to nearest whole #
• Carbon-12
–The 12 represents the
mass #

84. The Bohr Model
• The arrangement of e- around the nucleus
• Each circle = energy level (periods)
• Each dot = electrons
• # of dots on each circle = # of elements in
that energy level (period)

85. Nucleus
P+:_______
No:_______
E-: _______
Mass #: _______

86. Neutral Atoms
• # of protons = # of electrons
• So for Carbon:
• 6 protons  +6
• 6 electrons  -6
• Net Charge 0

87. Examples:
Substance Symbol Mass #
P+N
Atomic #
=P
# of protons
=Atomic #
# of neutrons
=Mass-P
# of electrons
=P
4 2
Magnesium Mg 12 12
Bromine Br 80 35
Aluminum Al 14
Uranium U 146 92

88. Examples:
Substance Symbol Mass #
P+N
Atomic #
=P
# of protons
=Atomic #
# of neutrons
=Mass-P
# of electrons
=P
Helium He 4 2 2 2 2
Magnesium Mg 24 12 12 12 12
Bromine Br 80 35 35 45 35
Aluminum Al 27 13 13 14 13
Uranium U 238 92 92 146 92

89. Ions
• atom has lost or gained one or more electrons
and has a charge
• PROTONS CANNOT BE LOST OR GAINED

90. Cation
• an ion with a positive charge- less electrons
Anion
• an ion with a negative charge- more electrons

91. Valence Electrons and The Octet
Rule

92. Valence Electrons and Chemical Bonding
• Valence Electrons-outermost electrons
• Valence e- are involved in chemical bonding.

93. Octet Rule – Atoms are more stable when
they have a full shell of 8 electrons
• Except H and He-only 2 e-
• Only Group 18-Noble Gases have 8
• All other groups will gain or lose electrons to
become full
• The # of e- atoms gain or lose is their
oxidation number.

94. Group # 1 2 13 14 15 16 17 18
Valence e- 1 2 3 4 5 6 7 8
Oxidation # +1 +2 +3 +/-4 -3 -2 -1 0
E- gained or
lost
Lose
1
Lose
2
Lose 3
Lose or
gain 4
Gain 3 Gain 2 Gain 1 None

96. 1. Which of these elements is most likely
to donate or lose one electron?
a. Be c. Rn
b.Cs d. He

97. 2. According to the periodic table,
which of these elements will form an
ion with a –2 charge?
a.S c. F
b. Mg d. Rb

99. Bonds
 Bonds are what hold elements together in a
compound 
• Types of Bonds:
– Ionic-
– Covalent

100. Ionic Bonds = Ionic compound
• Formed between Ions  charged atoms.
– Ions are formed when one element gives up e- ,
and the other element receives the e-
• The compound is electrically neutral or
charges equal zero.
• Between metals and nonmetals.

101. Covalent Bonds
• They bond by sharing e-
• Non-Metal + Non-Metal

102. 3. The ionic compounds that result from combining
Group 2 and Group 16 elements have a 1:1 ratio
because —
a. Group 2 elements are electrically neutral
b. Group 2 elements have two valence electrons
c. Group 2 elements contain neutrons in the nucleus
d. Group 2 contains more elements than other groups

103. Review
• Ionic Bond
– Giving up and accepting e- that causes elements
to become ions.
– An Ionic Bond is the attraction of oppositely
charged ions.
• Covalent Bond
– The sharing of e-

104. Predicting the Type of Bond
• A compound formed between a metal and a
non-metal will be ionic
– Metals are mostly found on the left side of the
periodic table and they tend to lose their valence
e- easily.
– Non-Metals are found on the right side of the
periodic table and they tend to gain valence e-
easily.
• This loss/gain of e- forms an ionic bond.

105. Predicting the Type of Bond
• Bonds between non-metals tend to be
covalent.
– Non-metals are located on the right side of the
periodic table and therefore all want to gain e-.
Furthermore, since none of these elements want
to lose e- they share e- instead.
• This sharing of e- is a covalent bond.