Name ________________________________________ Date ______________ Period _______
Fall Semester Final Review Guide
Inquiry and the Scientific Method
1. Vocabulary
 observation
 dependent variable
 hypothesis
 control group
 inference
 precision
 independent variable
 conclusion
2. A student performed an experiment with a metal sphere. The student shot the sphere
from a slingshot and measured its maximum height. Six different trials were performed
with the sphere being shot at a different angle from the horizontal for each trial.
 What is the relationship being studied? angle vs. height
 What are the independent and dependent variables in this experiment?
independent variable – angle; dependent variable – height
 What variables must be held constant throughout this experiment?
metal sphere, pull, slingshot
3. A science class puts wide wheels onto a small cart and lets it roll down an inclined ramp
and then across the floor. They measure the distance the cart travels. The investigation is
repeated using the same cart but this time fitted with narrow wheels. The angle of the
incline of the ramp remains constant. The mass of the cart is kept constant.
 What is the relationship being studied? width of wheels vs. distance
 What are the independent and dependent variables in this experiment?
independent variable – width of wheels; dependent variable – distance
 What variables must be held constant throughout the experiment?
angle of incline, surface, mass of cart
4. Explain the difference between an observation and an inference.
An observation is something detected through the senses while an inference is an assumption that
is based on an observation.
5. Explain how you can use the scientific method to solve scientific problems. What are the steps in
the scientific method and what are their purposes?
6. Use the graph below to draw a conclusion about the relationship between the number of yeast
cells and the temperature of incubation. Identify the dependent and the independent variable.
independent variable – temperature; dependent variable – number of yeast cells
As the temperature increases by 1C, the number of yeast cells increases by 1.
40
35
30
25
20
15
10
5
0
20
9
Period
15
W
P
7. Graph the data in the tables below and explain the relationship between the variables in each data
set.
They have an inverse relationship. They have a direct relationship. They have no relationship.
10
5
1
2
3
4
5
6
7
8
9 10
3
0
0
0
6
0
1
V
2
3
4
5
A
V (m3)
P (Pa)
A (months)
W (lbs)
0.1
0.5
1
2
4
5
8
10
40
8
4
2
1
0.8
0.5
0.4
1
2
3
4
5
6
7
8
7.3
9.4
10.5
12
13
14.3
15.2
16.7
6
7
8
0
5 10 15 20 25 30 35 40
Mass
Mass
(g)
Period
(s)
5
10
15
20
25
30
35
40
4
4
4
4
4
4
4
4
Matter and Change
1. Vocabulary
 law of conservation
 heat/temperature
 mass
 vaporization
 volume
 density
2. Use the law of conservation of mass to explain what happens in the following situations
 Burning steel wool
 Alka-seltzer in water
 Melting ice
 Dry ice before and after
 Dissolving sugar
3. Explain how the law of conservation of mass applies to both physical and chemical changes in a
system. Be sure to talk about both open and closed systems.
The law of conservation of mass says that for a closed system, the mass before and after a change
is the same. This is true for both physical and chemical changes. In an open system, the mass will
change if mass is transferred from the system to the surroundings or from the surroundings to the
system.
4. Find the density of substance A and B using the graph below. A is 12 g/mL and B is 8 g/mL
5. Ethanol has a density of 0.789 g/cm3. What is the mass of 225 cm3 of ethanol? What is
the volume of 75.0 g of ethanol? 178 g; 95.1 cm3
6. The cup is a volume widely used by cooks in the U.S. One cup is equivalent to 237 cm3.
If 1 cup of olive oil has a mass of 216 g, what is the density of olive oil in g/cm3?
0.911 g/cm3
Energy and States (Kinetic Molecular Theory)
1. Vocabulary
 Kinetic molecular theory
 Units of pressure
 Solid
 Combined gas law
 Liquid
 Kelvin
 Gas
2. Explain how molecular motion is related to temperature.
As temperature increases, the speed of particles increases.
3. Draw the graph for the relationship between the absolute temperature and pressure, the absolute
temperature and volume, pressure and volume, and Celsius temperature and pressure.
4. List the assumptions of the kinetic molecular theory.
Particles are in constant, random motion.
All collisions between particles are elastic, meaning they occur without a loss of energy.
Particles move in straight lines until they collide with each other or the walls of their container at
which point they change speed and direction.
5. Explain how and when you should convert Celsius to Kelvin.
You should convert Celsius temperature to Kelvin temperatures for all gas law problems by
adding 273 to the Celsius temperature.
6. A sample of gas occupies 150 mL at 25 ˚C. What is its volume when the temperature is increased
to 50˚C? 160 mL
7. The pressure in a bicycle tire is 105 psi at 25˚C in Fresno. You take the bicycle up to Huntington,
where the temperature is – 5˚C. What is the pressure in the tire? 94.4 psi
8. What would be the new volume if 250 cm3 of gas at 25˚C and 730 mm pressure were changed to
standard conditions of temperature and pressure? 220 mL
9. A 350 mL sample of gas has a temperature of 30˚C and a pressure of 1.20 atm. What temperature
would be needed for the same amount of gas to fit into a 250 mL flask at standard pressure?
180 K
10. A 475 cm3 sample of gas at standard temperature and pressure is allowed to expand until it
occupies a volume of 600. cm3. What temperature would be needed to return the gas to standard
pressure? 345 K
Energy and States (Thermal Chemistry)
1. Vocabulary
 Kinetic
 Melting
 Specific heat
energy
capacity
 Condensing
 Boiling
 Q = mcΔT
 Molecular
 Freezing
motion
 Joules
2. Explain phase changes in terms of energy and particle motion.
When a solid changes to a liquid, the particles in the solid vibrate faster and faster until they
overcome the attraction holding them in place and become a liquid. When a liquid changes to a
gas, the particles move faster and faster until they have enough energy to escape the attraction of
the liquid. Energy must enter the system from the surroundings to change from a solid to a liquid
or from a liquid to a gas. Energy must leave the system and enter the surroundings to change for a
liquid to a solid or a gas to a liquid.
3. Some of the water you spilled on your shirt evaporates.
4. Water vapor in the room condenses on a cold surface.
5. A cube of ice melts as it sits on the table.
6. A cup of hot coffee cools as it sits on the table.
7. Draw a heating and cooling curve, explaining each phase of the diagram in terms of temperature
and phase change. Label the phases and energy storage mechanisms for each portion.
Check your representing phase change assignment for the answer to this one.
8. How much energy is released into the surroundings when 684 g of water at 80°C is
cooled to room temperature (20°C)? 172,000 J or 172 kJ
9. How much energy is absorbed from the surroundings when 846 g of water at room
temperature (20°C) is warmed to 75°C? 194,000 J or 194 kJ
Describing Substances
1. Vocabulary
 Mass
 Density
 Melting point
 Physical property
 Hardness
 Flammability
 Chemical property





Heterogeneous
mixture
Homogeneous
mixture
Filtration
Distillation
Evaporation





Element
Compound
Pure substance
Chemical change
Physical change
2. Explain the difference between chemical and physical properties.
3. Explain the difference between chemical and physical changes.
4. Explain how you could use the physical properties of substances to separate mixtures of solids,
liquids, and a combination of solids and liquids.
History of the Atom
1. Vocabulary
 Democritus
 Dalton
 Atomic theory
 Thompson’s
model

Gold foil
 Theory
experiment
 Law
 Rutherford’s
 Principle
model
 Bohr’s model
 Hypothesis
2. Describe the historical development of the atom.
3. Contrast hypothesis, theory, and law.
A hypothesis is what you think will happen in a particular experiment, while a theory is a
proposed explanation for an observed phenomenon. A law does not attempt to explain a
phenomenon, but merely states what that phenomenon is.
4. List the contribution of the scientists who helped develop the atomic model.
Refer to your timeline.
Atomic Structure
1. Vocabulary
 Isotope
 Neutron
 Proton
 Energy levels
 Electron
 Electron configuration notation
2. Determine the identity of the following elements
 Atomic number 32
Ge
 Element with 18 protons
Ar
 1s22s22p63s23p64s23d104p4 Se
3. Determine the atomic number and mass number of the following elements
 Silicon
AN: 14
MN: 28
 Titanium
AN: 48
MN: 48
 Lead
AN: 82
MN: 207
 Uranium
AN: 92
MN: 238
 Radon
AN: 86
MN: 222




Calcium
Arsenic
Radium
Rubidium
AN: 20
AN: 33
AN: 88
AN: 37
MN: 40
MN: 75
MN: 226
MN: 85
4. Write the number of protons, neutrons, and electrons for the following elements
 Oxygen
P: 8
N: 8
E: 8
 Tin
P: 50 N: 69 E: 50
 Aluminum
P: 13 N: 14 E: 13
 Zinc
P: 30 N: 35 E: 30
 Magnesium
P: 12 N: 12 E: 12
 Potassium
P: 19 N: 20 E: 19
 Hydrogen
P: 1
N: 0
E: 1
 Nitrogen
P: 7
N: 7
E: 7
 Bismuth
P: 83 N: 126 E: 83
5. Explain what an isotope is. Provide two examples.
Isotopes are atoms of an element that contain different numbers of neutrons. Check your notes for
an example.
6. Write the long electron configuration for the following elements
 Sodium
1s22s22p63s1
 Argon
1s22s22p63s23p6
 Gallium
1s22s22p63s23p64s23d104p1
 Carbon
1s21s22p2
7. Write the short electron configuration for the following elements
 Krypton
[Ar]4s23d104p6
 Strontium
[Kr]5s2
 Tin
[Kr]5s24d105p2
 Magnesium
[Ne]3s2