NAME: _________________
Midterm Review
Unit 1 – Science Review Topics
QUALITATIVE VS. QUANTITATIVE WORK SHEET
Determine which of the following statements are quantitative and which are qualitative.
1. _____________ The cup had a mass of 454 grams.
2. _____________ The temperature outside is 250 C.
3. _____________ It is warm outside.
4. _____________ The tree is 30 feet tall.
5. _____________ The building has 25 stories.
6. _____________ The building is taller than the tree.
7. _____________ The sidewalk is long.
8. _____________ The sidewalk is 100 meters long.
9. _____________ The race was over quickly.
10. _____________ The race was over in 10 minutes.
Practice Identifying Parts of the Scientific Method
Directions: The following are experimental scenarios. Read the experiments and then identify
the components of the scientific method by completing the graphic organizer provided.
Experimental Scenario #1
A student investigated the effect of radiation on the germination of bean seeds. He
thought that exposure to radiation would limit the seeds ability to germinate (grow) much like ultraviolet light causing skin cancer. Three hundred seeds were soaked in distilled water for one hour.
They were then divided into three groups. One group was placed in a microwave oven on high for
three seconds. Another group was microwaved on high for six seconds. The last group was not
microwaved. The seeds were then planted in three separate flats and given the same amount of
water. The seeds were then planted in three separate flats and given the same amount of water.
The flats were placed in a location with a constant temperature of approximately 27 degrees
Celsius. Each day for two weeks the number of seeds that germinated each group was recorded.
Total Number of Bean Seeds Germinated after Microwave Radiation
Three Seconds of Radiation
54
Six Seconds of Radiation
26
No Radiation
88
Analysis of Experimental Scenarios
– Graphic Organizer –
Problem/Observation:
Question:
Hypothesis:
Experiment:
Procedures
Independent Variable
Dependent Variable
Controls
Control Group
Experimental Group(s)
Conclusions:
Conversions-Metric to Metric
Conversion between the different units within the metric system is accomplished by using
the ‘Quick Conversion Line’ to move the decimal point the appropriate number of places
in the appropriate direction.
kilo
1000
hecto
100
deka
10
Unit
meter
liter
gram
1
deci
0.1
centi
0.01
How can you remember this?
Kids Having Doughnuts Usually Drink Chocolate Milk
In-class examples:
58.9 kg =
g
9,852,614 mm =
km
852,614 mL =
L
.007621 kL =
L
3 meters = _______ centimeters
10 kilometers = ______ meters
15,050 milligrams into grams
3,264 milliliters = ______ liters
Scientific Notation
Part A: Express each of the following in standard form.
1. 5.2 x 103
2. 9.65 x 10–4
5. 3.6 x 101
6. 6.452 x 102
3. 8.5 x 10–2
7. 8.77 x 10–1
4. 2.71 x 104
8. 6.4 x 10–3
milli
0.001
Part B: Express each of the following in scientific notation.
1. 78,000
5. 16
2. 0.00053
6. 0.0043
3. 250
7. 0.875
4. 2,687
8. 0.012654
Unit 2 – Scientific Measurement
1. Give the number of significant figures in each of the following.
a) 10.0005 g ______
b) 0.003423 mm ______
2. Determine the answer for each of the following. Be sure to use the correct number of
significant figures.
a) 27.34
6.90
+ 13.124
c) 0.32 x 14.50 x 120 =
b) 2.8023
- 4.762
d) 24.1 / 0.005 =
3. Round each of the following to 3 significant figures.
707.5 ____________
2,301.2 ______________
0.0003350 _____________
10.26730 _______________
18.95 x 1021 ______________
NAME: ________________
Unit 3 – Matter and Change
1. Provide at least 2 characteristics of solids.
2. Provide at least 2 characteristics of liquids.
3. Provide at least 2 characteristics of gases.
In the diagram below, compare solids, liquids, and gases. Where one or more
circles overlap, list the ways that those states of matter are alike. Where
the circles do not overlap, list the ways that each of these states of matter
is unique.
Solids
Liquids
Gases
% by mass = (mass element/mass compound) x
100
% by mass (law of definite
proportions)
1.
A 25.3g sample of an unknown compound contains 0.8g of oxygen (O). What is the percent by
mass of oxygen in the compound?
2.
28.2g of carbon monoxide (CO) is formed when 8.57g of oxygen (O) reacts with carbon (C). What
is the percent by mass of the carbon in carbon monoxide?
MATCHING
_____1. A phase change in which energy is
absorbed from its surroundings.
A. Plasma
B. Gas
_____2. Matter in which state are vibrating
in a fixed location.
_____3. The most common type of matter in
the universe.
C. Solid
D. Sublimation
E. Liquid
_____4. The phase change in which a solid goes
directly to a gas without becoming a liquid.
_____5. In this phase change the arrangement of
particles becomes very orderly.
F. Endothermic
G. Vaporization
H. Freezing
_____6. The phase change in which a substance
goes from a liquid to a gas.
_____7. It has a definite volume but no definite
shape.
_____8. It will take the shape of its container, and
expand to fill the available space.
Classify each of the following as elements (E), compounds (C) or Mixtures (M).
Write the letter X if it is none of these.
___Diamond (C)
___Sugar (C6H12O6)
___Milk
___Air
___Sulfuric Acid (H2SO4) ___Gasoline
___Krypton (K)
___Bismuth (Bi)
___Uranium (U)
___Water (H2O)
___Alcohol (CH3OH)
___Pail of Garbage
___Ammonia (NH3) ___Salt (NaCl)
___Energy
(Au)
___Wood
___Bronze
___Ink
___Dry Ice (CO2)
___Baking Soda (NaHCO3) ___Titanium (Ti)
___Iron (Fe)
___Electricity
___Popcorn
___A dog
___Gold
___Pizza
___Concrete
Match each diagram with its correct description. Diagrams will be used once.
A
B
C
D
___1. Pure Element – only one type of atom present.
___2. Mixture of two elements – two types of uncombined atoms present.
___3. Pure compound – only one type of compound present.
___4. Mixture of two compounds – two types of compounds present.
___5. Mixture of a compound and an element.
E
Column A lists a substance. In Column B, list whether the substance is an
element (E), a compound (C), a Heterogeneous Mixture (HM), or a Solution (S).
(Remember a solution is a homogeneous mixture.) In Column C, list TWO
physical properties of the substance.
Column B
Column C
Column A
1. Summer Sausage
2. Steam
3. Salt Water
4. Pencil lead (Pb)
5. Dirt
6. Pepsi
7. Silver (Ag)
8. Toothpaste
(Na2HPO4)
9. A burrito
10. Italian Dressing
11. Chicken Soup
12. Lemonade
DENSITY: D = M/V Find the unknown quantity:
a) d = 3 g/mL
V = 100 mL
M=?
b) d = ?
V = 950 mL
M = 95 g
c) d = 0.5 g/mL
V=?
M = 20 g
PHYSICAL PROPERTY
1. observed with senses
2. determined without destroying matter
CHEMICAL PROPERTY
1. indicates how a substance
reacts with something else
2. matter will be changed into a new
substance after the reaction
Identify the following as a chemical (C) or physical property (P):
______1.
______2.
______3.
______4.
______5.
______6.
______7.
blue color
density
flammability (burns)
solubility (dissolves)
reacts with acid
supports combustion
sour taste
PHYSICAL CHANGE
1. a change in size, shape, or state
2. no new substance is formed
______8. melting point
______9. reacts with water
______10. hardness
______11. boiling point
______12. luster
______13. odor
______14. reacts with air
CHEMICAL CHANGE
1. a change in the physical and
chemical properties
2. a new substance is formed
Identify the following as physical (P) or chemical (C) changes.
_____1.
_____2.
_____3.
_____4.
_____5.
_____6.
_____7.
_____8.
water.
NaCl (Table Salt) dissolves in water.
Ag (Silver) tarnishes.
An apple is cut.
Heat changes H2O to steam.
Baking soda reacts to vinegar.
Fe (Iron) rusts.
Alcohol evaporates .
Ice melts.
______9. Milk sours.
______10. Sugar dissolves in water
______11. Wood rots.
______12. Pancakes cook.
______13. Grass grows.
______14. A tire is inflated.
______15. Food is digested.
______16. Paper towel absorbs
Unit 4 – Atomic Theory
12. Complete the chart:
Element
Number of
Protons
Number of
Neutrons
6
8
Number of
Electrons
Mass
Number
Atomic
Number
Lithium
(Li)
41
Argon (Ar)
47
109
Lead (Pb)
19
Tantalum
(Ta)
73
88
Chromium
(Cr)
Uranium
(U)
24
149
74
Tungsten
(W)
53
COMPLETE THE CHART
CHARGE
LOCATION
ELECTRON
NEUTRON
PROTON
Given the relative abundance of the following naturally occurring isotopes of oxygen,
calculate the average atomic mass of oxygen:
oxygen-16: 99.760%
oxygen-17:
0.037%
oxygen-18:
0.204%
A research team has just discovered a new element called Likhitium. Now, they need to
determine the average atomic mass in order to complete an entry for the periodic table.
Given the following relative abundances, calculate the average atomic mass of Likhitium.
Likhitium-138: 44.7%
Likhitium-139: 52.3%
Likhitium-140: 00.5%
Likhitium-141: 02.5%
Elements, Compounds, and Mixtures
Elements, Compounds, and Mixtures
Classify each of the pictures below by placing the correct label in the blanks below:
A= Element
D= Mixture of compounds
B= Compound
E= Mixture of elements and compounds
C= Mixture of elements
Each circle represents an atom and each different color represents a different kind of
atom. If two atoms are touching then they are bonded together.
1. Write orbital filling diagrams, electron configurations, and electron dot diagrams
for the following elements.
Table:
Element
a. Aluminum
b. Carbon
c. Oxygen
d. Magnesium
e. Fluorine
f. Tellurium
Orbital Filling Diagram
Electron Configuration
Electron Dot
Diagram
History of the Atom
John Dalton (1766 – 1844):
John Dalton was an English chemist. His ideas form the atomic theory
of matter. Here are his ideas.




All elements are composed (made up) of atoms. It is impossible
to divide or destroy an atom.
All atoms of the same elements are alike. (One atom of oxygen
is like another atom of oxygen.)
Atoms of different elements are different. (An atom of oxygen
is different from an atom of hydrogen.)
Atoms of different elements combine to form a compound.
These atoms have to be in definite whole number ratios. For
example, water is a compound made up of 2 atoms of hydrogen
and 1 atom of oxygen (a ratio of 2:1). Three atoms of hydrogen
and 2 atoms of oxygen cannot combine to make water.
1. What is the name of John Dalton’s theory?
_____________________________________
2. What are elements made of?
________________________________________________
3. An atom of hydrogen and an atom of carbon are
_________________________________.
4. What are compounds made of?
_______________________________________________
5. The ratio of atoms in HCl is:
a) 1:3
b) 2:1
c) 1:1
J. J. Thompson (Late 1800s):
J. J. Thompson was an English scientist. He discovered the electron
when he was experimenting with gas discharge tubes. He noticed a
movement in a tube. He called the movement cathode rays. The
rays moved from the negative end of the tube to the positive end.
He realized that the rays were made of negatively charged particles
– electrons.
1. What did J.J. Thompson discover?
_____________________________________________
2. What is the charge of an electron?
____________________________________________
3. What are cathode rays made of?
______________________________________________
4. Why do electrons move from the negative end of the tube to the
positive end?
______________________________________________________
____________________
5. What was Thompson working with when he discovered the
cathode rays?
______________________________________________________
____________________
Lord Ernest Rutherford (1871 – 1937):
Ernest Rutherford conducted a famous experiment called the gold
foil experiment. He used a thin sheet of gold foil. He also used
special equipment to shoot alpha particles (positively charged
particles) at the gold foil. Most particles passed straight through
the foil like the foil was not there. Some particles went straight
back or were deflected (went in another direction) as if they had hit
something. The experiment shows:
 Atoms are made of a small positive nucleus; positive nucleus
repels (pushes away) positive alpha particles
 Atoms are mostly empty space
1. What is the charge of an alpha particle?
_______________________________________
2. Why is Rutherford’s experiment called the gold foil experiment?
_____________________
______________________________________________________
____________________
3. How did he know that an atom was mostly empty space?
__________________________
______________________________________________________
____________________
4. What happened to the alpha particles as they hit the gold foil?
_____________________
______________________________________________________
____________________
5. How did he know that the nucleus was positively charged?
_________________________
______________________________________________________
____________________
Niels Bohr (Early 1900s):
Niels Bohr was a Danish physicist. He proposed a model of the atom
that is similar to the model of the solar system. The electrons go
around the nucleus like planets orbit around the sun. All electrons
have their energy levels – a certain distance from the nucleus.
Each energy level can hold a certain number of electrons. Level 1
can hold 2 electrons, Level 2 - 8 electrons, Level 3 - 18 electrons,
and level 4 – 32 electrons. The energy of electrons goes up from
level 1 to other levels. When electrons release (lose) energy they
go down a level. When electrons absorb (gain) energy, they go to a
higher level.
1. Why could Bohr’s model be called a planetary model of the atom?
__________________
______________________________________________________
____________________
2. How do electrons in the same atom differ?
_____________________________________
______________________________________________________
____________________
3. How many electrons can the fourth energy level hold?
____________________________
4. Would an electron have to absorb or release energy to jump from
the second energy level to the third energy level?
_____________________________________________________
5. For an electron to fall from the third energy level to the second
energy level, it must ___________________________________
energy.