1. Name__________________________Date______________Period_______________
Physical Science Midterm Review
This review was given in class on 12/2/2011
It is due completed on 12/9/2011.
1. This review is simply a guide. It consists of a few example questions. Anything we’ve covered
is considered “fair game” on the final. Review your notes, re-do problems, and read in your
textbook. Do the practice problems in the text.
2. The resources provided for you to use for the final exam will include a periodic table, your
polyatomic ion sheet. You need to bring a pencil and a calculator.
3. Good luck studying! If you’ve kept up all along, you’ll do fine with this review sheet. If you’ve
had trouble, I suggest you find a study buddy to re-teach you the things you’re still confused
with. Plan your study time NOW so that you’ll leave enough time for each class.
Topics Covered
Introduction Atomic History and Structure
o Safety o History of the Atom
o Measurement o Atomic Structure, Isotopes, and
o Calculations/Dimensional Ions
Analysis
o Graphing – can “read” data in Periodic Table
order to create interpretations o History of the Periodic Table
o Theory and Law o Parts of the Periodic Table
o Scientific Method o Element Location
o Phases of Matter/Particle
Pictures Chemical Bonds and Formulas
o Density o Bond Types
o Temperature changes o Writing Formulas
o Chemical vs. Physical Changes o Naming Bonds
o Kinetic Theory
o Elements, Compounds, Chemical Reactions and Balancing
Mixtures o Reaction Types
o Balancing Equations
Solutions, Nuclear, Acids/Bases
o Solution types and parts
o Nuclear chemistry
o Acids/Bases

2. Name__________________________Date______________Period_______________
1. In which of the following situations would you need to wear goggles? (circle) All of
them!!!)
Heating a liquid Lighting a Bunsen burner Mixing acids and bases
2. Define the following:
a. Kilo- 1000 b. Hecta- 100
c. Deka- 10 d. Deci- 1/10
e. Centi- 1/100 f. Milli- 1/1000
3. Give the SI units for the following measurements:
a. Length: _M___ b. Time: __s___
c. Mass: ___kg___ d. Temperature: _Celsius__
4. How many meters are in 6.893 cm? .06893 m
5. How many dekaliters are in 890mL? .0089 DkL
6. Write the following in scientific notation or standard notation
a. 3.45 x 10-3g _____0.00345 g________ b. 22450000m_2.245 x 107m
c. 1.847 x 102 mL ___184.7 mL________ d. 0.01400 cg __1.4 x 10-2cg
7. In graphing, what do you plot on the x-axis?
Independent variable
8. Define chemistry.
The study of matter and it’s properties.
9. Define the following:
Hypothesis: An answer to a question proposed. An educated guess as to what the
outcome will be.
Experiment: a test of a question and hypothesis carefully set up to ensure
accurate data collection.
Control: the part of an experiment that does not change. This would be what you
compare your data against.
10. List the steps of the scientific method
Observe
Formulate a question
Record and collect data
Form a hypothesis
Test the hypothesis
Observe
Draw Conclusion.
This is not a linear process. You can go back at any point of the experiment and we
formulate ideas and the experiment.

3. Name__________________________Date______________Period_______________
11. Sketch particles in the three states of matter. How close are the particles and how
much do they move?
Solid Liquid Gas
Really far apart.
Really close Able to slide past They do not touch
together each other. and will fill their
container.
12. What is the density of liquid hand soap if 450 mL of the soap has a mass of 130g?
D= m/v 130g/450mL= 0.28 g/mL
13. What is the density of a paperclip with a mass of 2.3g and a volume of 1.2 cm3?
D=m/v D= 2.3g/1.2 cm3 = 1.91 g/cm3
14. How does density affect whether something will sink or float?
The more closely packed the particles in an object are, the more likely it is that they will
sink in a solution, however, this also depends upon the density of the solution
15. Define the following:
a. Boiling point from liquid to gas
b. Melting point from solid to liquid
c. Freezing point from liquid or gas to solid
d. Absolute zero the point at which all particles stop moving. 0 on the Kelvin
scale
16. Classify the following as physical or chemical changes:
a. spoiling of milk ___c________________
b. bending wire _____p________________
c. cutting paper ______p_______________
d. rusting of a nail ___c________________
17. What is viscosity?
The resistance of flow from a liquid. Honey is more viscous than water.
18. Identify the following as elements, compounds, or mixtures
a. copper _________element_____________
b. sweetened tea ____mixture____________
c. sand and water ___mixture____________
d. calcium carbonate (CaCO3) _____compound___________________
19. Atomic Models:
 John Dalton
 List the four postulates of Dalton’s Atomic Theory:
 All atoms are indivisible.

4. Name__________________________Date______________Period_______________
 You cannot create or destroy and atom
 All atoms of an element are alike
 All molecules of a compound are alike.
 J.J. Thompson
Plum Pudding model. Discovered electrons and believed that the positive and negative
charges were distributed in the same areas. (like a blueberry muffin)
 Earnest Rutherford
Gold foil experiment, discovered the nucleus of the atom. Determined that there was a
small, positively charged nucleus at the center of the atom.
 Niels Bohr
Solar system model. Electrons belonged to specific levels of energy that they orbited the
nucleus in. Each level could only hold so many electrons.
 Quantum mechanical model (Electron Cloud):
The electrons do not orbit in orderly elliptical orbits. They exist in a cloud of negative
charge and their position cannot be determined.
20. Characteristics of subatomic particles
Particle Mass Charge Location in atom
Proton 1.67 x 10-27 Positive Nucleus
Neutron 1.67 x 10-27 Neutral Nucleus
Electron 9.11 x 10-31 Negative Orbiting nucleus
21. Draw Bohr models of the following atoms:
a. Silicon b. Boron c. Chlorine
22. The atomic number of an element represents the number of _protons or electrons in
the atom
23. What is an isotope?
A version of an atom that has more or less neutrons than a normal atom. Can be
radioactive.

5. Name__________________________Date______________Period_______________
24. A common isotope of neptunium is neptunium-235. How many protons and
neutrons does it have?
Atomic mass – atomic number = number of neutrons
P +N - p = neutrons
235 – 93 = 142
25. What is an ion?
A version of an atom that has either gained or lost electrons and now has a charge.
26. Who developed the first periodic table and how did they arrange it.
Mendeleev and he arranged it by increasing atomic mass.
How is the current periodic table arranged?
By atomic number. Henry Mosely rearranged it.
27. Locate or define parts of the periodic table:
 Groups a vertical column of elements in the periodic table. Elements in a group
share chemical properties.
 Periods a horizontal row of elements in the periodic table. Decreases in metallic
properties as you go from left to right.
 Transition metals One of the metals in the center of the periodic table that have
fluctuating ionized states.
 Alkali metals, Alkaline Earth metals, Halogens, Noble Gases
Group 1, highly reactive, group 2 still really reactive, group 17 highly reactive bond with
group 1. Noble gases have full outer shells and do not bond.
28. From their positions on the periodic table, what charges would the ions of have?
Gains or loses electrons? Symbol for ion Gains or loses electrons? Symbol for ion
Be Loses Be+2 N Gains N-3
Li Loses Li+1 Mg Loses Mg+2
I Gains I-1 S Gains S-2
29. How many electrons are needed in the outer levels of most atoms for the atom to be
chemically stable? 8
30. How many valence electrons do the following groups have?
a. Group 1: ___1_____ e. Group 15 (5A): ___5____
b. Group 2: ____2__ f. Group 16 (6A): ____6___
c. Group 13 (3A): __3_____ g. Group 17 (7A): _____7__
d. Group 14 (4A): ___4____ h. Group 18 (8A): ______8_
31. What is the total number of atoms in Sr3(PO4)2? 13

6. Name__________________________Date______________Period_______________
32. Properties of Metals vs. Nonmetals vs. Metalloids
Metals Nonmetals Metalloids
Luster? Yes No Have properties of
both. Refer back to
Malleable vs. Brittle Malleable Brittle
your text or your
Conducts electricity Yes No notes.
& heat?
Typical state(s) at Solid Gas
room temperature
33. Define the following:
Malleable-able to be pounded into a sheet Ductile-roll into a wire
34. Using the periodic table, what is the atomic number and symbol of gold? Au
Strontium? Sr
35. Ionic bonds are formed when a _metal_____ and a __nonmetal______ combine.
36. Metals lose electrons and form __Cations___________ while nonmetals gain and
electrons form ___anions_______.
37. Covalent compounds form when a ___nonmetal_____ and a
_____nonmetal__________ combine as they share electrons.
38. Identify the following pairs of atoms as potentially forming an ionic or covalent
compound:
Mg and Cl __ionic_______ I and F ___covalent_______ P and Cl ___covalent____
Ag and S __Ionic______ K and Br ___ionic_________ Sn and O ___ionic________
39. Write formulas for the following compounds
Ba2+ with OH– __Ba(OH)2___ NH4+ with PO43– __(NH4)3PO4_________
Be+2 with O-2 _BeO_________ C4+ with F1- ____CF4___________
40. Naming molecular compounds
 Name: N2O: ____Dintrogen Monoxide____________________
 Name: NO2: _____Nitrogen Dioxide_______________________
 Name: P3N2: ____Triphosphourous Dinitride________________________
41. Naming Ionic Compounds
 Name: Li2O ____Lithium Oxide_______________________
 Name:(NH4)2SO4 :___Ammonia Sulfate_______________________

7. Name__________________________Date______________Period_______________
 Name: FeO :_____Iron (II) Oxide (Focus on roman numeral naming please!!!!)
 Name:Sn3(PO4)4 :___Tin Phosphate______________
42. Chemical reactions can often be classified as one of five types. Write the general
form for each type of reaction.
 Direct Combination (or synthesis): A +B AB
 Decomposition AB A+B
 Single-Replacement AB + X A + XB
 Double-Replacement AB + CD AD + CB
 Combustion (C +H) +O2 H2O + CO2
43. What is a coefficient and what is it used for?
The big Number, you use it to increase the number of molecules
What is a subscript and what is it used for?
The little number, it tells you how many of each atom are in a compound.
44. Using the five types of reactions listed above, classify AND balance the following
equations:
_2__Na(s) + ___Br2(l)  _2_NaBr(s) ____Synthesis______________
heat
___CH4(g) + _2_O2(g)  ___CO2(g) + 2_H2O(g) __Combustion____________
___K2CrO4(aq) + ___Ba(NO3)2(aq)  ___BaCrO4(s) + _2_KNO3(aq) ___DR_______
_2_Al(s) + ___Fe2O3(s)  ___Al2O3(s) + _2_Fe(s) ___SR_________________
__2_H2(g) + O2(g)  _2__H2O(l) _____Synthesis_____________
heat
__2_C8H18(l) + _25__O2(g)  _18__CO2(g) + _16__H2O(g) ___Combustion________
45. What is the Law of Conservation of Mass?
Matter can be neither created nor destroyed.
46. Define the following:
Exothermic Reaction Releases energy in the form of heat.

8. Name__________________________Date______________Period_______________
Endothermic Reaction Absorbs energy
47. Classify the following as endothermic or exothermic
a. Paper burning with a bright flame exo
b. Plastics becoming brittle after being left in the sun endo
c. Firecracker exploding exo
. 48. Define the following:
Solution a homogeneous mixture, Colloid mixture in which the
particles are uniformly distributed particles can’t settle out and they can’t
dissolve in.
Solute thing that dissolves Saturated solution holds as
much solute as it possibly can.
Solvent thing that the solute
dissolves into.
Unsaturated
Suspension mixture in which the The solution could hold more solute.
particles of a material are large enough
to settle out
49. What are some ways to help a solute dissolve faster?
Increase temperature, increase surface area, increase contact with solvent, etc.
50. What is an acid? Any compound that increases the number of hydronium ions when
dissolved in water.
51. What is an indicator? Give examples a compound that can reversibly change color
when introduced to an acid or base. Cabbage juice is a good one.
52. What is a base? Any compound that increases the number of hydroxide ions when
dissolved in water.
53. What is pH? Where do acids and bases fit on the scale?
A value that is used to express the acidity or baseness of a system. Measures the amount
of H+ in a solution.
Acids 0-6.9 Bases 7.1-14
54. Write out and label the parts of a neutralization reaction.
H3O+ OH- 2 H2O

9. Name__________________________Date______________Period_______________
54. Classify the following as acidic, basic, or neutral
a. soapy solution, pH=9 base
b. sour liquid, pH=5 acid
c. solution with four times as many hydronium ions as hydroxide ions acid
d. pure water neutral
55. Define radioactivity
Refers to the particles that are emitted from the nuclei of unstable atoms.
56. Define nuclear fission and nuclear fusion
Fission-splits the atoms Fusion-nuclei fusing and forming new atoms.
57. Describe the ways in which radiation can cause damage to living tissues
Can kill the tissue, cause cancer,
58. List several uses for low-level radioactive tracers.
Used in several medical procedures to trace abnormalities, pinpoint problem areas and
insure that medicine gets where it needs to go.
Please make sure that you re-read over your notes, make graphic organizers or outlines of
this information. You have to know these topics with some depth. It is more important
that you know how to apply this information and how to do these things. Good luck.
Don’t forget if you would like some help you can schedule this with me. I am available
before school and during 3rd or 5th to help. Plus, on the half days, you could stick around
and get help then. If you would like to do any of this, please let me know because I need
to know that you are coming.
Ms. Meador.