Name: _________________________________
Integrated Science Final Exam Study Guide Answer Key
Spring 2009
Your Integrated Final Exam addresses the basic study of Chemistry including Scientific Method,
Laboratory Techniques and Physics.
CHAPTER 1
1.
Use the chart below to convert the following measurements.
a.
3 inches = 7.60 cm
b.
2 km = 1.24 miles
c.
4 kg = 8.8 lb
d.
2m = 78.74 in
METRIC-ENGLISH EQUIVALENTS
2.54 centimeters = 1 inch
1 meter = 39.37 inches
1 kilometer = 0.62 miles
1 liter = 1.06 quarts
250 millimeters = 1 cup
1 kilogram = 2.2 pounds
28.3 grams = 1 ounce
0
C = 5/9 x (0F– 32)
2.
Define the following terms:
Control – standard used for comparison of test results in an experiment.
Data - information gathered through an experiment.
Experiment – organized procedure for testing a hypothesis that tests the effect of one
thing or another under controlled conditions.
Hypothesis – educated guess using what you know and what you observe.
Conclusion – explanation of results based on data.
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3.
List the steps of the scientific method in order.
a.
b.
c.
d.
e.
f.
g.
4.
state the problem
gather information
form a hypothesis
test the hypothesis (experiment)
analyze data
draw conclusions
repeat (if necessary)
Read the passage below then answer the questions that follow.
a.
b.
c.
d.
e.
f.
g.
h.
i.
In the late nineteenth century, the French scientists Louis Pasteur investigated a
disease called anthrax, which was killing sheep and cattle.
He suspected that the disease was caused by a particular kind of bacteria.
Pasteur heated a sample of the bacteria just enough to weaken, but not kill them.
Using a group of 50 sheep, he injected 25 sheep with the weakened bacteria, and
left the other 25 sheep alone.
The injected sheep became slightly ill, but soon recovered.
Several weeks later, Pasteur injected all 50 sheep with large doses of healthy
Bacteria, strong enough to kill a normal sheep.
After a few days, all 25 sheep that had been injected with weakened bacteria were still
alive, while the other 25 sheep were all dead of anthrax.
Questions:
A.
Which sentence/s describe(s) the problem? a, b
B.
Which sentence/s describe(s) the procedure? c, d, e, g, h
C.
Which sentence/s describe(s) the data being collected? f, i
D.
Which sentence/s describe(s) the results? i
E.
Which sentence/s describe(s) the control? e
5.
6.
List the type of SI measurement best used for the following:
a.
The volume of a pitcher of iced tea - liter
b.
The mass of a person - kilogram
c.
The length of a pencil- centimeters
d.
The height of a person - meters
Explain how to properly use the following instruments to measure substances:
a.
triple beam balance – zero out scale, put object on scale, move riders until scale is
balanced – start w/ heaviest rider relative to object being weighed.
b.
7.
graduated cylinder (glass) – fill g.c. midway , record measurement, add object, record
new measurement, subtract 1st measurement from 2nd, make sure to read the meniscus.
What is the formula for density? D = M/V
2
8.
If 96.5g of aluminum has a volume of 35 cm3, what is the density of aluminum?
m
96.5g
m = 96.5 g
d = ----d = --------d = 2.8 g/cm3
v
35 cm3
3
v = 35 cm
d=?
9.
If the density of a diamond is 3.5 g/cm3, what would be the mass of a diamond whose volume
is 0.5 cm3?
d = 3.5 g/cm3
m=dxv
m=?
m = 3.5 g/cm3 x 0.5 cm3
m = 1.75 g
v = 0.5cm3
On the provided graph, graph the data found in the chart below.
Why should temperature be placed on the X-axis?
Why should mass be placed on the Y-axis?
Solubility of Salt in Water
Temperature( 0C)
Mass of Solute (g)
20
40
60
80
40
42
44
46
Temperature vs Mass
Mass of Solute (g)
10.
47
46
45
44
43
42
41
40
39
0
20
40
60
Temperature Degrees C
80
100
3
Based on the graph above, what conclusions can you draw about the effect of temperature on the
solubility of salt in water?
As the temperature increases, the solubility of the salt in water increases.
11.
Imagine walking up to your radio and hearing the DJ give a weather report like this:
“It’s going to be a beautiful day today with sunny skies and a high temperature of 300 K!”
Should you wear a coat to school? Use the illustration below to help you determine your
answer. Explain how you determined your answer. No, you should not wear your coat to
school because when calculating K to degrees F its about 80.6 degrees F.
Who, in general, uses the 3 types of temperature scales shown in the illustration?
Why is it important to use units when describing quantitative measurements such as
temperature? It is important to use units to indicate what the numbers mean or what they are
describing.
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CHAPTER 2 AND 3
1. What is matter? Anything that has mass and takes up space.
2. Define Kinetic Theory of Matter and list three assumptions associated with it.
An explanation of how particles in matter behave:
1. all matter is composed of small particles (atoms, molecules, ions)
2. these particles are in constant random motion
3. these particles are colliding with each other and the walls of their container.
3. How are kinetic energy and temperature related?
The temperature of an object is the average kinetic energy in a substance
4. Define and give an example of Archimedes’s Principle.
The buoyant force on an object is equal to the weight of the fluid displaced by the object – ship
floating.
5. Define thermal expansion and give an example.
Increase in the size of a substance that results from the separation of its molecules when the
temperature is increased.
6. Define and give an example of Bernoulli’s Principle.
As the velocity of a fluid increases, the pressure exerted by the fluid decreases – airplane.
7. Label the following pictures as a solid, liquid, or gas.
SOLID
LIQUID
GAS
8. List and describe the 3 states of matter.
1. solids – definite shape and volume: only vibrate; low energy
2. liquids – indefinite shape and definite volume: some freedom to move; high energy
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3. gas – Indefinite shape and indefinite volume; high energy.
9. State whether the following phase changes absorbs or releases heat:
a. Solid to liquid
absorb
b. Liquid to gas
absorb
c. Gas to liquid
release
10. Explain and give an example of the following:
a. Charles’ Law
Temperature ↑ Volume ↑
Temperature ↓ Volume ↓
Example – hot air balloon
b. Boyle’s Law
Pressure ↑
Pressure ↓
Volume ↓
Volume ↑
Example – squeezing a balloon
11. What is a pure substance? A substance that can not be broken down into simpler components and
still maintain the properties of the original substance.
12. What are the two types of pure substances? An element and a compound.
13. Define element and give an example. A substance with atoms that are all alike.
14. Define compound and give an example. Substance in which the atoms of two or more elements
are combined in a fixed proportion.
15. What is the difference between heterogeneous and homogenous mixtures??
In an heterogeneous mixture the materials are unevenly distributed and are easily identified; in a
homogenous mixture you have a solid, liquid, or gas that contains two or more substances
blended together evenly throughout.
Heterogeneous example: concrete
Homogeneous example: kool aid
16. Identify the following as chemical or physical changes:
a. Burning coal - chemical
b. Baking brownies - chemical
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c. Digesting food - chemical
d. Dissolving sugar in hot water - physical
e. Melting butter - physical
f. Exploding fireworks - chemical
g. Rusting iron - chemical
17. Explain how to separate a mixture of salt, sand, rocks, and metal.
1. you can pick or sift out the rocks;
2. use a magnet to remove the metal assuming that it is magnetic;
3. add water, the salt will dissolve and the sand will sink;
4. filter out the sand;
5. evaporate the water away and you’re left with the salt.
CHAPTER 4
1. Define and list the location of:
a. Proton – positively charged particle, composed of quarks; inside the nucleus of an atom
b. Neutron – neutral particle, composed of quarks; inside the nucleus of the atom.
c. Electron- negatively charged particle surrounding the nucleus of an atom.
2. The atomic number of an atom is always equal to its number of electrons and protons.
3. In the Bohr model, how many electrons are in the following shells?
2 1st shell
8 2nd shell
8 3rd shell
4. What element has 25 electrons and 25 protons? Explain how you determine your answer.
Manganese (Mn)
5. An element has an atomic number of 15 with 16 neutrons. What is the number of protons? 15 ,
atomic mass number? 31, number of electrons? 15
6. The square below represents information about elements typically found on the Periodic Table.
Use the information given in the square to answer the questions.
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Cr
Chromium
51.99
a.
b.
c.
d.
e.
f.
g.
What is the atomic mass of the given element? 51.99
What is the atomic number of the given element? 24
What is the symbol of the given element? Cr
What is the name of the given element? Chromium
How many protons does the element have? 24
How many electrons does the given element have? 24
How many neutrons does the given element have? 28
7
3
7. List the number of subatomic particles in the following isotope:
Protons – 1, electrons – 1, neutrons - 2
1
H
Explain how you determined your answer.
The number protons and electrons is the same as the atomic number, 1. The number of neutrons
is the atomic mass minus the atomic number which equals 2.
8. Explain the process used to draw an electron dot diagram. Draw an example.
Use the symbol of the element and draw dots at the four quadrants around the symbol. You begin
at the 12 o’clock position with one dot for each valence electron the element has. You continue
adding dots at each point until you fill the symbol with the correct amount of valence electrons.
9. How do you determine the number of neutrons of an element?
Subtract the atomic number from the rounded atomic mass
10. Who is given credit for the arrangement of the modern periodic table? How is it arranged?
Mosley, by increasing atomic number
11. What do elements in the same period have in common?
Same number of outer energy levels
12. What do elements in the same group have in common?
Similar properties; same number of valence electrons
13. List properties of metals and nonmetals.
Metals
-good conductors of heat and electricity;
-all but one are solid at room temperature
-reflect light (luster)
-malleable and ductile
-generally have 1-3 valance electrons
-In chemical reactions, give up electrons (lose e-)
-form ionic and metallic bonds
Nonmetals
-usually gases or brittle solids at room
temperature
-not malleable or ductile
-do not conduct heat or electricity well
-dull
-can form ionic or covalent bonds
-in chemical reactions, gain electrons
14. Which family is considered to be the most active metals? Explain why.
Alkali metals; only have 1 valence electron so it’s easily lost
15. Which family is considered to be the most active nonmetals? Explain why.
Halogens; have 7 valence electrons so it’s easy to gain one electron
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16. What is a metalloid? List the metalloids by symbol. Where are metalloids located on the
periodic table? Elements that shares some properties with metals and nonmetals; B, Si, Ge, As,
Sb, Te, Po, At; they are located on the zigzag line except for aluminum.
17. Define malleable. What elements would be malleable? Ability of metals to be hammered or
rolled into thin sheets; metals.
18. On the periodic table, the greater proportions of the elements are classified as metals.
19. A horizontal row on a Periodic Table is most often referred to as a row or period.
A vertical column on the Periodic Table may be referred to as group or family.
20. On the Periodic Table below, label all the families and valence/oxidation numbers.
PERIOD
F
A
M
I
L
Y
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CHAPTER 5
1. What makes an atom stable? A full outer energy level (8 electrons)
2. Define ionic bonding and covalent bonding.
Ionic – attraction formed between oppositely charges ions in an ionic compound; bond
between a metal and nonmetal that transfer electrons.
Covalent – attraction formed between atoms when they share electrons; bond between two
nonmetals sharing electrons.
3. For the compounds below identify the type of chemical bond which will form between the
elements. Explain how you determined your answers.
a. Li and O - ionic
b. Cl and Br - covalent
c. Mg and N - ionic
d. Br and Ne – no bond forms. Ne is a noble gas.
e. Ca and O - ionic
4. Define: chemical formula – chemical shorthand that uses symbols to tell what elements are in
a compound and their ratios.
5. Draw a Bohr model for the atom with the atomic number of 17. Then answer the questions in
the box about the atom.
a.
b.
c.
d.
e.
What is the name of the element? chlorine
Is it a metal or nonmetal? nonmetal
What is its oxidation number? -1
What is its family name? halogen
What type of bond will form with this
element if it reacts with oxygen? covalent
6. Name the following ionic compounds:
a. MgCl2 – magnesium chloride
b. K2O - potassium oxide
c. Sr3N2 - strontium nitride
7. Write formulas for the following ionic compounds:
a. Potassium nitride – K3N
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b. Calcium iodide – CaI2
8. What is an oxidation number? Positive or negative number that indicates how many electrons
an atom has gained, lost, or shared to become stable.
9. What are organic compounds? Large number of compounds containing the element carbon.
10. What element is known as the basis of life? Carbon
11. What isotope of carbon do scientists use to date things? Carbon 14
CHAPTER 6
1. What is the difference between reactants and products? Reactants are substances that react in
a chemical equation, whereas products are the new substances formed in the reaction.
2. What is a chemical reaction? Process in which one or more substances are changed into new
substances.
3. State the law of conservation of mass. States that the mass of all substances that are present
before a chemical reaction equals the mass of all substances that are remaining after the
reaction.
4. What is a coefficient? The number in a chemical reaction that represents the number of units
of each substance taking part in a chemical reaction.
5. Label the coefficients and subscripts in the following equation.
↓ coefficient
coefficient
→2 H2O
→ 2 H2 + O2
↑ subscript
↑ subscript ↑
6. Why can’t you change the subscripts in a chemical equation?
7. Define and give an example of the following:
a. Combustion – occurs when a substance reacts with oxygen to produce energy in the form
of heat and light.
C + O2 → CO2 + energy
b. Synthesis reaction – two or more substances combine to to form another substance.
2H2 + O2 → 2H2O
c. Decomposition reaction- one substance breaks down or decomposes into 2 or more
substances,
2H2O + 2H2 + O2
d. Single displacement reaction- one element replaces another element in a compound.
Cu + 2AgNO3 → Cu(NO3)2 + Ag
e. Double displacement reaction- the positive element of one compound replaces the positive
ion of the other to form two new compounds.
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Ba(NO3)2 + K2SO4 + 2KNO3
8. For the equation: MgCO3
+
2HCl
→ MgCl2 +
H2CO3, if the amount of HCl
increases, what happens to the amount of H2CO3? It increases.
9. Identify the following equations as balanced or unbalanced
a. PbO2 →
PbO + O2 unbalanced
b. BaCl2 + Na2SO4 → BaSO4 + 2NaCl
balanced
10. Balance the following equation: 2Al + __Fe2O3
→
__Al2O3 + 2Fe
CHAPTER 7
1. What is the difference between solute and solvent? A solute is the substance in a solution
being dissolved and the solvent is the substance in which the solute is dissolved.
2. How does size affect the rate of dissolving in a solution? Smaller particles dissolve faster
3. How does temperature affect the rate of dissolving in a solution? The higher the
temperature, the quicker the rate something will dissolve,
CHAPTER 8
PH
1-3
4-6
7
8-10
11-14
Substance
.37% Hydrochloric acid
Vitamin C
Distilled water
Milk of magnesia
4% lye solution
Color
Dark pink
Pink
Yellow
Green
Purple
1. Refer to the table above to answer the following questions:
a. Which substance has a pH between 4-6? Vitamin C
b. What substance turns the indicator yellow? Distilled water
c. Which substance(s) should we use the most caution with when handling? Why? 0.37%
HCl (strong acid); 4% lye (strong base)
d. Which substance is more basic than milk of magnesia? 4% lye solution
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2. What type of scale do we use to describe the acidity of a substance? What are indicators?
Give 2 examples of common indicators. Organic compound that changes color in an acid or
base.
3. What type of ions do bases release in water? Hydroxide ions, OH4. What type of ions do acids release in water? Hydronium ions, H3O+
5. Explain a neutralization reaction. Using a chemical equation, give an example of a
neutralization reaction. Chemical reaction that occurs when the H3O+ ions from an acid react
with the OH- ion to produce water molecules.
6. Define acid. Give several examples of acids along with their chemical formulas. Any
substance that form hydrogen ions in a water solution.
H2S
HCl
HNO3
H2SO4
hydrogen sulfide
hydrochloric acid
nitric acid
sulfuric acid
7. Define base. Give several examples of bases with their chemical formulas. Any substance
that releases hydroxide ions in a water solution.
Al(OH)3
Ca(OH)2
MG(OH)2
NaOH
aluminum hydroxide
calcium hydroxide
magnesium hydroxide
sodium hydroxide
Chapter 10 and 11
1. Define the motion. Motion is a change in an objects position.
2. What is the difference between distance and displacement? Distance is how far an object has
moved. Displacement is how far an object has moved from its original starting place.
3. How is instantaneous speed different from average speed? Instantaneous speed is speed at any
given point. Average speed is speed of motion when speed is changing.
4. Define balanced forces. What do balanced forces do? Balanced forces are equal in size and
opposite in direction. They do not move an object, and the net force is equal to zero.
5. Define unbalanced forces. What do unbalanced forces do? Unbalanced forces are unequal in
size and the direction is the same. They cause the object to move.
6. a. State the Law of Conservation of Momentum. Momentum can be transferred between two
objects, but momentum is not lost or gained in the transfer.
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c. Relate this law to the game of billiards (pool). Momentum is transferred from one billiard
ball to another when they hit each other, but no momentum is gained or lost during that
transfer.
7. State Newton’s Three Laws of Motion. 1st – an object in motion stays in motion and an object
at rest stays at rest until a net force acts upon the object. 2nd – f = m x a. 3rd – for every action
there is a reaction equal in magnitude but opposite in direction.
8. Define friction. How does friction affect the motion of objects? Friction is the force that
opposes motion between two surfaces that are touching each other. It slows down the motion
of an object.
9. What are the 3 types of friction?


Static friction – friction between two surfaces that are not moving past each other;
Sliding friction – friction that opposes motion between two surfaces sliding past one
another;
 Rolling friction – friction between two a rolling object and surface it rolls on.
10. State which law applies best to each of the following examples:
a. An athlete can throw a baseball farther than he can throw a shot-put 2nd Law
b. A cat slides off the end of a counter top 1st Law
c. As air moves out of a balloon, the balloon moves the opposite direction 3rd Law
d. A small car accelerates quicker than a large truck 2nd Law
e. An object travels in a straight path until it hits the wall and is stopped 1st Law
11. State the Law of Gravitation: any two masses exert an attractive force on each other.
12. Define gravity: one of the four basic forces that give the universe its structure. The force of
gravity depends on the mass and the distance between the objects.
13. Why do objects fall at different rates? Air resistance and objects have different surface areas.
14. Define air resistance: air resistance is a type of friction that opposes the force of gravity.
15. What stays the same no matter where you are-weight or mass? Explain. Mass because it is the
amount of matter in an object.
16. What law explains why the planets orbit around the sun? The Law of Gravitation
17. Explain how to calculate the weight of a person on Earth. Multiply the person’s mass times
the gravitational pull on earth. W = m x 9.8 m/s2.
Chapter 12
18. Define energy: the ability to cause change.
19. List the three forms of energy. Kinetic, potential, and mechanical.
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20. Define kinetic energy and give its formula. Kinetic energy is energy in the form of motion.
KE = ½ mv2.
21. Define potential energy. Potential energy is energy stored in a motionless object that gives it
the potential energy to cause change.
22. What are the three types of potential energy? Elastic, chemical, and mechanical.
23. Explain mechanical energy. Mechanical energy is the total amount of potential and kinetic
energy in a system.
24. Draw a swinging pendulum and label the points of maximum kinetic energy, maximum
potential energy, and the point at which kinetic energy is equal to potential energy.
25. Explain the Law of Conservation or Energy. Energy may change from one form to another,
but the total amount of energy never changes.
26. Relate the figure below to the Law of Conservation of Energy.
The energy changes from kinetic energy to potential, but the amount of energy never changes.
Mechanical energy is converted to heat energy due to friction.
27. When a car begins to move, what type of energy conversion occurs? Chemical to mechanical.
28. Describe the energy conversions which take place when you rub your hands together.
Mechanical to thermal.
29. What types of energy are in fuel? Chemical potential energy.
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30. Explain the energy conversions that occur when you blow-dry your hair. Electrical to
mechanical to thermal.
31. In the roller coaster below, at which point is there:
a. Maximum kinetic energy? C
A
b. Maximum potential energy? A
B
C
c. Potential energy = kinetic energy? B
32. Define power: the amount of work done in a certain amount of time; the rate at which work is
done. Equals work divided by time and is measured in watts.
33. Define work and give examples. The transfer of energy that occurs when a force makes an
object move. Examples: moving a desk, lifting weights.
34. Give examples of situations in which work is NOT being done. Holding a barbell above your
head; standing still; pushing on an object that doesn’t move.
35. Define mechanical advantage. Is MA determined the same way for all simple machines?
Mechanical advantage is the number of times a machine multiplies the effort force. MA is not
determined the same for all simple machines. They all multiply the effort force but they
depend on different things. For example, an inclined plane depends on distance.
36. Give the units for energy, work, and power. Work – joules, Power – Watts, Energy – joules.
37. Could work input ever equal word output? Explain. No, because of friction.
38. How can the efficiency of a machine be increased? By using lubricants to reduce friction.
39. How can friction be reduced? Using lubricants.
40. One joule =1 N/m
41. One watt =1 J/s
42. A 900 Newton mountain climber scales a 100-meter cliff. How much work does the mountain
climber do? 90,000 joules.
43. Define the temperature. The average kinetic energy of an object’s atoms or molecules.
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44. How is kinetic energy related to the temperature of an object? Temperature is how much
kinetic energy an object has – as kinetic energy increases temperature increases.
45. Define heat. Thermal energy that flows from something at a higher temperature to something
at a lower temperature.
46. List the three methods of transferring thermal energy. Conduction (direct contact), convection
(currents), and radiation (air).
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