Download Semester 1 exam review

Semester 1 Physical Science Exam review
This is not an assignment, it is a review of the vocabulary, concepts, and sample
questions for the exam. I suggest that you split it into parts and use them to study
for the exam.
Vocabulary
Chapter 1 Scientific Method
Scientific method
Observation
Question
Hypothesis
Experiment
Results
Conclusion
Variable
Control
Control group
Controlled experiment
Independent variable
Dependent variable
Metric system
Prefix
Deka
Kilo
Mega
Giga
Deci
Centi
Milli
Micro
Nano
Scientific notation
Dimensional Analysis\
Conversion factor
Ch. 3 States of matter
Kinetic energy
Kinetic theory of matter
Cohesion
Liquids
Viscosity
Gas
Plasma
Pascal’s law
Hydraulics
Boyle’s law
Pressure
Celsius
Kelvin
Charle’s law
Phase
Condensation
Freezing
Melting
Freezing point
Melting point
Evaporation
Boiling
Vaporization
Sublimation
Deposition
Density
Exothermic
Endothermic
Ch. 4 Atoms
Continuous theory of matter
Discontinuous theory of matter
Tin oxide experiment
Law of conservation of mass
Law of definite proportions
Law of multiple proportions
Dalton’s atomic theory
Crook
Crook’s tube
Thompson
Rutherford
Gold foil experiment
Neils Bohr
Quantum energy levels
Electron cloud model
Protons
Neutrons
Electrons
Isotopes
Gravity
Electromagnetic force
Strong force
Weak force
Quark
Ch. 5 Periodic table
Mendeleev
Valence electrons
Henry Moseley
Families
Period
Luster
Ductile
Malleable
Metals
Nonmetals
Metalloids
Alkali metals
Alkaline earth metals
Transition metals
Boron family
Carbon family
Nitrogen family
Oxygen family
Halogens
Noble gasses
Rare earth elements
Atomic radius
Ionization energy
Electron affinity
Electronegativity
Chapter 6 Chemical Bonding
Ion
Ionic compounds
Bohr model
Crystal lattice
Cation
Anion
Formula
Chemical name
Covalent bonds
Lewis structure
Molecule
Network solid
Polyatomic ions
Metallic bond
Polar
Nonpolar
Electronegativity
Ch. 7 Chemical Reactions
Chemical reaction
Chemical equation
Coefficient
Mole
Conversion factor
Molar mass
Synthesis
Combustion
Decomposition
Single replacement
Double replacement
Exothermic
Endothermic
Reaction rate
Surface area
Catalyst
Equilibrium
Concepts
Chapter 1 Scientific Method
Know why you should know science
Know the scientific method, be able to create your own, be able to list parts from an
existing experiment
Be able to explain the control in an experiment
Be able to give the dependent and independent variables
Know prefixes
Know how scientific notation works
Know how to use excel
Be able to set up and use dimensional analysis
Chapter 3 States of Matter
Know what cohesion and kinetic energy have to do with the state of matter
Be able to draw solids, liquids, and gasses at the atomic level
Know how a gas moves
Know pascals law
Know how hydraulics work
Know and be able to use the formulas for hydraulics
Know and be able to use boyle’s law
Know and be able to use charle’s law
Know how to explain boyles and charles laws using the kinetic molecular theory
Know how to explain what is going on at the atomic level in phase changes
Know why the boiling point is lower at high altitudes
Chapter 4 atoms
Know what the Greeks thought of matter and how they differed
Understand how the tin oxide experiment works
Understand the law of conservation of mass
Understand how the law of definite proportions and the law of multiple proportions work
and be able to prove them with an example (I give the compound(s) and break them
down, you give the ratio)
Know the crook’s tube and what he put inside and what it proved
Know what Thompson did with a crook’s tube and what he proved
Know Thompson’s model of an atom
Know Rutherford’s gold foil experiment
Know Rutherford’s three conclusions and explain how he got them
Know Dalton’s atomic theory, including what two are false and how he got them
Know what happens to an atom according to the Bohr model when light is absorbed or
released
Be able to draw an atom using the electron cloud model
Be able to find the number of electrons, protons, and neutrons in an atom
Know the 4 forces that act in or on an atom
Chapter 5 Periodic Table
Know how Mendeleev organized the periodic table
Know Mendeleev’s problems in the periodic table and how he solved them
Know what Henry Moseley did with the periodic table
Know the metals, nonmetals, and metalloids including their general properties
Know the different parts of the periodic table including their general properties
Know 3 uses of each family (aka three elements in the family and 1 use for each)
Know how atomic radius is measured
Know what happens to the atomic radius as you go down or across the periodic table
Know why the atomic radius changes
Know what happens to the ionization energy as you go down or across the periodic table
Know why the ionization energy changes
Know what happens to the electron affinity as you go down or across the periodic table
Know why electron affinity changes
Know what happens to the electronegativity as you go down or across the periodic table
Know why electronegativity changes
Ch. 6 Chemical Bonding
Be able to draw ionic bonds using the bohr model
Be able to draw a crystal lattice
Given a chemical name be able to write a formula
Given a formula be able to write a chemical name
Be able to draw covalent bonds using the bohr model
Be able to draw Lewis structures of single and double bonded molecules
Know what metallic bonds are
Be able to draw Lewis structures of polyatomic ions
Chapter 7 Chemical Reactions
Know how to balance equations
Be able to convert from masses to moles
Be able to convert from moles of one substance to moles of another substance
Be able to convert from moles to masses
Be able to tell if a reaction is synthesis, decomposition, combustion, single replacement,
or double replacement
Know the difference between exothermic and endothermic reactions
Know what can change a reaction rate
Know what chemical equilibrium is and what can change it
Review Questions for the test on Scientific Method
1. Why should you know science, list at least three reasons.
2. Using the scientific method, write your own experiment (different than one we
used in class or you did before) include all steps of the scientific method.
3. In your experiment above what is your control group?
4. In your experiment above, what is your dependent and independent variable?
5. What is the function of a control group?
6. Why is the metric system is better than the standard system.
7. I have 2 hairs stacked on top of each other to be used in a CSI forensic scan that
blonde hair is 8.9x10-4 m high and the brunet hair is 2.2x10-4 m high. How high is
my stack of hairs. Put your answer in scientific notation.
8. We have developed lasers that are so precise they can write your name on a single
piece of hair. If your name is 6.2 micrometers express this size as a decimal.
9. A blood cell is .00004 m. Write this number in words and in scientific notation.
10. I have a small stack of papers that are 8.7x10-5 m tall. If I take one off that is
2.1x10-5 meters tall, how tall is the stack?
11. I have 3.83 x 107 grams of water in my pool, express this number in number
format and in words.
12. If density = Mass/ Volume, what is the density of belly button lint that is 6.7x10-8
grams and has a volume of 4.9x10-2 cubic meters?
13. Watching strong men in the park tearing phone books in half in the park one day
(June 23, 1998), I came up with a theory that the bigger the man the bigger the
phone book he can tear in half. Matt weighs 97 pounds and can only tear a
Where’s Waldo book (15 pages) in half. Waldo (weighing in at 210 lbs) can tear
To Kill a mockingbird in half (the book, not the bird) (527 pages). Franz (at
weighing 252 lbs) can tear a Harry Potter book in half (645 pages). Haans (302
lbs.) can tear Mein Komph (1043 pages). Make a table that shows this data.14.
14. What is one mistake in the experiment above that makes me a bad scientist?
15. 16. Knowing that distance = speed x time, if a lightning bolt travels at 3.7x106
meters per second for 1.7x10-1 seconds, how far from earth did the lightning bolt
begin?
17. The largest hot cross bun was made by staff at Pegrums Bakery in the UK. The
bun weighed 94.35 lbs and had a diameter of 4 ft 3 in. What was its weight in
grams?
18. The human bladder can hold up to 2 cups of urine. (for those of you that need to
go to the bathroom all the time) How many liters is this?
Review questions for test on Ch. 3
1. What is the kinetic theory of matter?
2. What are the two definitions of a gas?
3. What makes air pressure on the atomic level?
4. What is pascal’s law?
5. The hydraulics on a high-low have a small piston with 3 cm2 and a large piston
with 21 cm2. If the motor pushes with 524 lbs of force, how many tons can it lift?
If the small piston moves 172 cm how far will the load rise?
6. A garbage compactor has a hydraulic unit set up with a large piston that is 12
inches across (and square) and a small piston is 1 inch in diameter (and round). If
the motor can push on the small piston with 20 pounds of pressure how much
pressure is compacting the garbage?
7. I have a piston at 11 atm and 9 ml. I let the piston up until there is 101.325 kPa of
pressure (normal air pressure). What is my new volume in cm3?
8. Explain how Boyles law works with the kinetic molecular theory.
9. You are now a multimillionaire trying to circumnavigate the earth by hot air
balloon. On earth the pressure is 101.325 kpa and your balloon is holding 300
cubic meters of air. At 30,000 feet the air will be only .25atm. You built your
balloon to hold 1250 cubic meters of air. Will your balloon hold, making you the
first person to complete such a feat or will your balloon rip sending you
plummeting to the earth.
10. My rubber duckey in bath water (30 degrees C.) holds 15 cm3 of air. When the
bath water turns cold (21 degrees C.) how much air will my rubber duckey hold?
Assume that I put a cork in my duckey when it was in the warm water.
11. You are filling paintball cartridges to make your paintball gun shoot as far and as
fast as possible. The side of the cartridge says to not fill it over 150 ml or it will
blow up in your face. If you fill it with 100 ml of CO2 at 10 degrees Celsius, how
much can you let it warm up (in C) until it blows?
12. Explain how Charles law works with the kinetic theory of matter.
13. What is a phase change?
14. list the three states of matter, and tell what the name of the phase change for each
is, for example the phase change between a solid changing to a liquid is melting.
15. Why does the temperature of a compound stop changing when it is going through
a phase change? (critical thinking)
16. What is an endothermic change, give an example in real life.
17. What is an exothermic change, give an example in real life.
18. How is boiling and vaporization different?
19. What is sublimation, how about deposition?
20. What is going on at the atomic level when a liquid turns into a gas?
21. How is boiling different than evaporation?
22. Can you make water hotter than 100 C? If so, how?
23. Liquid is forming on the outside of my glass containing ice water right now, what
is this process called and what is going on at the atomic level. Is this process an
exothermic or endothermic process?
24. .I have .84g of carbon dioxide in a 50 ml container at 105 kPa. If I release
pressure (by making my volume bigger) until the gas is 25 kPa what is the density
of my gas?
25. Why does sweating cool you down?
Chapter 4 Review Questions
1. What were the two theories that the Greeks came up with and how are they
different?
2. What three experiments led to the discovery of electrons, describe each.
3. Dalton said that atoms can not be divided, created, or destroyed, explain why he
was wrong.
4. Dalton said that all atoms are identical in size, mass, and other properties.
Explain why he was wrong.
5. What are isotopes and give one use of them.
6. What was JJ Thompson’s model of matter and how did he come up with it?
7. Why did Rutherford conclude that atoms are made of mostly empty space?
8. What are quantum energy levels?
9. What happens to the electrons when energy is added to an atom according to
Neils Bohr?
10. If your shirt is red, describe how the atoms in your shirt make it that way?
11. How many protons, neutrons, and electrons are in a fluorine atom?
12. How many protons, neutrons and electrons are in Oxygen- 18 (Oxygen-18 is an
isotope of oxygen with an atomic mass of 18)?
13. How many protons, neutrons and electrons are in K?
14. Draw a boron atom, include orbitals and electron placement according to the
electron cloud model.
15. Draw a Cl atom, include orbitals and electron placement according to the electron
cloud model.
16. Deuterium is a H-2 isotope (hydrogen with an atomic mass of 2), how many
protons, electrons and neutrons are in deuterium?
17. List and describe the four forces that act in or on atoms.
18. Draw calcium using the electron cloud model. \
Review Question on Chapter 5 Periodic Table
1. Who created the first periodic table and what two criteria did he use to do it?
2. Who came along and fixed the periodic table, how did he do it?
3. How many electrons does the oxygen family want to gain or lose to become
stable?
4. What are the general properties of the nonmetals?
5. Aluminum wants to lose how many electrons?
6. How did Mendeleev know where to leave spaces in his periodic table?
7. Explain how the atomic mass of an element is affected by the distribution of its
isotopes in nature.
8. Does all the elements in a family have identical, or just similar properties, why?
9. Give me your best hypothesis on why it was difficult to find the Noble Gasses.
10. Give three elements and uses that are in the transition metals family.
11. Why are the transition metals called the transition metals
12. Give three elements in the alkaline earth metals family and a specific use of each.
13. What are the general properties of the halogen family?
14. What are three elements and their uses that are found in the nitrogen family?
15. What is electronegativity? What happens to electronegativity as you go across the
periodic table? Why?
16. What is electron affinity? What happens to electron affinity as you go down the
periodic table? Why?
17. What is ionization energy? What happens to ionization energy as you go across
the periodic table? Why?
18. What is atomic radius? What happens to atomic radius as you go across the
periodic table? Why?
19. What happens to atomic radius as you go down the periodic table? Why?
20. What are the properties of a metalloid?
21. Benjamin Franklin found that you can take electrons from a rod when you rub it
with a wool cloth. What type of rod would you get more electrons from, a rod
made of silicon or a rod made of carbon? Why?
22. What halogen would be a better electron acceptor (better at getting electrons)
Chlorine or Bromine. (a better electron acceptor is more reactive, FYI)
23. In table salt (NaCl) what atom is going to get the electrons while in a bond?
24. Determine the average atomic mass for carbon given the following information:
The abundance of Carbon – 12 is 98.90% with a mass of 12.000 amu. The
abundance of carbon- 13 is 1.1% with a mass of 13.03335 amu.
Review Questions for Ch. 6 Bonding
1. What is an ionic bond? High school definition, not kindergarten.
2. Draw the bohr model for sodium phosphide.
3. Draw lithium bromide in a crystal lattice.
4. Draw Magnesium Oxide in a crystal lattice
5. Name the following formulas
a. MgCl2
b. Au2S3
6. Write the formula for the following compounds
a. Iron (III) Bromide
b. Aluminum Sulfide
7. Correct and rewrite the following formulas
a. Be2F4
b. Na2Br
8. What does it mean to be polar? (hint: use page 168)
9. Draw the bohr model for CH3OH covalently bonded (this one is a toughy, not for
the faint of heart!!)
10. Draw the bohr model of methane CH4 covalently bonded.
11. How is a covalent bond different than an ionic bond?
12. Draw a lewis structure for dichloromethane, CH2Cl2.
13. Draw the lewis structure for O2.
14. Draw the lewis structure for C2H5COOH
15. How are crystal lattices and network solids different, how are they the same?
16. What is a polyatomic ion.
17. Draw C2O42- in a Lewis structure
18. Draw Acetate C2H3O2- in a Lewis structure
19. Describe a metallic bond.
20. How is a cation different than an anion?
Review Questions on Ch. 7 Chemical reactions
1. 1. What steps should I do when balancing a chemical reaction?
2. Balance the following reaction: sodium and water react to make sodium
hydroxide (NaOH) and hydrogen. (this is used to make drain-o)
3. Balance the following reaction: C4H12 + O2  CO2 + H2O
4. Balance the following reaction: H2PO4 + Cl2  HCl + PO4
5. Why is it important to balance chemical reactions?
6. Write a balanced equation for the reactants and products in a match. Phosphorus
(P)reacts with potassium chlorate (KClO3)to make potassium chloride (KCl)and
phosphorus (V) oxide. (P2O5)
7. Balance the following reaction: Fluorine and aluminum bromide react to produce
bromine gas and aluminum fluoride.
8. What does one mole of aluminum oxide weigh?
9. The reaction that causes cake batter to rise involves the production of CO2 from
NaHCO3 (baking powder). How many liters of CO2 gas will be created when 15.0g
NaHCO3 are heated? The density of CO2 is 1.997 g/L
2NaHCO3  H2O + Na2CO3 + CO2
9. When potassium hits water it creates potassium oxide and hydrogen gas an makes
a large explosion (bigger than the one we did in class with sodium and water) If I
toss 3 grams of potassium into water, how many grams of hydrogen gas will it
make? H2O + K  KOH + H2
10. How are double replacement reactions different than single replacement
reactions?
11. Is the following reaction a synthesis, decomposition, single replacement, double
replacement, or combustion reaction? Ca + H2O  Ca(OH)2 + H2
12. Is the following reaction a synthesis, decomposition, single replacement, double
replacement, or combustion reaction?
13. Is the following reaction a synthesis, decomposition, single replacement, double
replacement, or combustion reaction? H2 + Cl2  HCl
14. Is the following reaction a synthesis, decomposition, single replacement, double
replacement, or combustion reaction? KClO3  KCl + O2
14. Why does raising the temperature of a reaction increase the reaction rate?
15. What is chemical equilibrium?