Final Review

1
Final Review

• Chemistry 09

2

• Lab Safety and Equipment

3

• 1. When diluting sulfuric acid
• a. add the sulfuric acid to plenty of water
• b. add plenty of water to the sulfuric acid
• 2. If you do not understand a direction or part
  of a lab procedure, you should
• a. figure it out as you do the lab
• b. try several methods until something works
• c. ask the instructor before proceeding
• d. skip it and go on to the next part
• 3. After completing an experiment, all chemical
  wastes should be
• a. left at your lab station for the next class
• b. disposed of according to your instructors
  directions
• c. dumped in the sink
• d. taken home

4

• 4. If an acid is splashed on your skin, wash at
  once with
• soap
• oil
• concentrated base
• plenty of water
• 5. Sarah accidently broke a glass beaker while
  conducting a lab. The first safety procedure for
  Sarah to do is to
• a. sweep up the broken glass immediately and put
  it in the trash
• b. inform her teacher immediately so that her
  teacher can sweep up the glass
• c. leave it for the next class to clean up
• d. none of the above

5

• 6.________
• 7. ________
• 8. ________
• 9.________

b

• . The object may cause a burn.
• . There is a potential of punctures or cuts.
• . Use the chemical under a fume hood.
• . The chemical is corrosive.

c
a
d
6

• 10. ________
• 11. ________
• 12. ________

c

• . graduated cylinder- used to measure accurate
  liquid volumes
• . flask- glassware used to contain reaction
  solutions
• . beaker- multi-purpose glassware that is used to
  hold and heat substances

b
a
7

• 13. Define a meniscus and how you use it when
  reading a graduated cylinder.
• 14. What is the reading on the graduated cylinder
  below? _________ mL

Meniscus- the curve (dip) of a liquid substance
in a graduated cylinder read the graduated
cylinder from the bottom of the meniscus
43
8

• 15. A triple beam balance is used to measure
  _______________. What is the reading on the
  triple beam balance below? _________ g

mass
545.2
9

• 16. The phrase used to remember metric conversion
  prefixes is King Henry __________________________
  ________________________________________.
• 17. A student has 0.45 L of a liquid. What is the
  volume in mL? 0.45 L ________ mL

King Henry Died by Drinking Chocolate Milk
450
10

• Scientific Method Graphs

11

• 1. The scientific method is a process that
  scientist use to _________________________________
  ______.
• 2. Organize the 6 steps of the scientific method
  in the correct order 1-6.
• ________ Conclusion
• ________ State the problem
• ________ Experiment
• ________ Gather information
• ________ Analyze the data
• ________ Formulate a testable hypothesis

Solve a problem
6
1
4
2
5
3
12

• 3. Tommy conducted an experiment and concluded
  that a species of mosquitoes (sp. S. ouch) will
  grow larger when exposed to microwaves for long
  periods of time. What could Tommy do to make his
  conclusion more valid?
• A. Try a different species of mosquitoes
• B. Repeat the same experiment multiple times with
  the same species of mosquitoes
• C. Use a large number of the mosquitoes (sp S.
  ouch)
• D. Both b and c
• 4. A hypothesis is _______________________________
  ______. The format for writing a TESTABLE
  hypothesis is If IV then DV? (Ex. If I eat 20
  pieces of chocolate then I will have a stomach
  ache)

an educated guess
13

• 5. In an activity, a ball is dropped from a
  height of 100 cm onto five different materials.
  The rebound height of each drop is shown in the
  graph. Which of the following describes the
  hypothesis most likely being tested?
• A. The mass of the ball affects the rebound
  height.
• B. The material the ball is made of affects the
  rebound height.
• C. The height the ball is dropped from affects
  the rebound height.
• D. The surface the ball is dropped onto affects
  the rebound height.

14

• 6. A control is the standard to which test
  results can be compared
• 7. The independent variable is the variable that
  is manipulated or changed (MIX)
• 8. The dependent variable is the variable that
  responds to the changes in the independent
  variable (DRY)

15

• 9. An experiment was designed to investigate the
  effect of caffeine on the heartbeat of water
  fleas. Two populations of water fleas was
  cultured. Both populations had water with the
  same mineral content, were supplied with
  identical amounts of bacteria food, received the
  same amount of light, and had their temperature
  maintained at 20oC. Every two hours, water fleas
  from both populations were selected and their
  heartbeats were monitored. The fleas of
  population one had caffeine administered five
  minutes before their heartbeat was checked. The
  fleas of population two were given nothing.
• I. What part of the experiment above is
  population two?
• a. Independent variable
• b. Dependent variable
• c. Control
• II. What part of the experiment above was the
  caffeine?
• a. Independent variable
• b. Dependent variable
• c. Control

16
Independent

• 10. The ________________________ variable is
  graphed on the x- axis. The ___________________
  variable is graphed on the y- axis.
• 11. You are measuring the how the temperature in
  your room changes over a period of time. What
  type of graph would you use to graph this data?
• A. Line graph B. Bar graph C. Pie Chart
• 12. A researcher determined the percentage of
  electrical energy transformed into different
  forms of energy by a toaster. The best way to
  communicate these results is to display the data
  using a
• A. Line graph B. Bar graph C. Pie (Circle) graph

Dependent
17

• 13. The line graph below shows the month and the
  number of bathing suites sold each month. What
  variable does the number of bathing suits sold
  represent in the research?
• A. independent variable
• B. dependent variable
• C. control
• D. constant

18

• Precision and Accuracy

19

• Which of the following sets of measurements is
  most precise?
• A. 18.56, 20.56, 22.56
• B. 18, 20, 22
• C. 17.5, 20.5, 21.5
• D. 18, 19, 20
• Which of the following will allow measurement of
  a liquids volume with the greatest precision.
• A. 50 mL cylinder graduated in 1 mL increments
• B. 100 mL cylinder graduated in 0.5 mL increments
• C. 100 mL cylinder graduated in 1 mL increments
• D. 100 mL cylinder graduted in 5 mL increments

20

• Density

21

• 1. Write the formula for density
• 2. Complete the triangle below for the density
  formula.
• 3. Write the unit(s) of measure for density,
  volume, and mass.
• Density units of measure ____________
  ______________
• Mass unit of measure _______________
• Volume units of measure _____________
  ______________

Density mass/volume
g/mL
g/cm3
g
mL
cm3
22

• 4. Calculate the density of a metal cube that has
  a mass of 30 g and a volume of 16 cm3.
• 5. If you have a graduated cylinder that was
  filled to 25 ml and you dropped a rock into it
  and water in the cylinder raises to 29 ml. What
  is the volume of the rock? If this same rock has
  a mass of 44g what would the density of this rock
  be?
• 6. What is the density of water? ___________ g/mL
• 7. If an object has a density of 1.3 g/cm3, it
  will _________ in water.
• A. sink B. float
• 8. If an object has a density of 0.7 g/mL it will
  ________ in water.
• A. sink B. float

D m/v ? D 30g/16cm3 ? D1.88 g/cm3
V (29ml 25mL 4mL ? D m/v ? D 44g/4mL ? D
11 g/mL
1
23

• Use the figure below to answer questions 9 and
  10.
• 9. Which liquid in the beaker above is the most
  dense? _______________
• 10. Which liquid in the beaker above is the least
  dense? _______________

Volume 4
Volume 1
24

• 11. The volume of object X in the figure on the
  right is
• a. 20 mL b. 25 mL c. 30 mL d. 35 mL

25

• Viscosity

26

• 1. Viscosity is a fluids ________________ to
  flow.
• 2. A fluid is any substance that flows. A fluid
  can be a liquid or a _______________.
• 3. Which substance below is the most viscous?
• A. water B. honey
• 4. Which substance below is the least viscous?
• A. water B. honey

resistance
gas
27

• 5. Students in a chemistry lab measure the time
  it takes four different 100 mL solutions to pass
  through a hole in the bottom of the cup. Which of
  the following properties of the solutions is most
  likely being measured?
• A. buoyancy B. mass C. viscosity D.
  volume
• 6. When compared to a high viscosity liquid, a
  liquid with a low viscosity
• A. must have a lower volume
• B. is easier to pour
• C. takes longer to pour from one container to
  another
• D. must have a higher density

28
Buoyancy
29

• 1. Buoyancy is the __________ force exerted on an
  object by a fluid that it is immersed in.
• A. downward B. upward
• 2. List two examples that illustrate buoyancy
  (example ship on the sea) _______________________
  _________
• ______________________________________________
• _________________________________

30
Kinetic Theory and States of Matter
31

• 1. When a substance is heated, the molecules
  or atoms that make up the substance move _____.
• A. faster B. slower
• 2. List the 4 states of matter and 2
  characteristics of each.
• ____________________- definite shape, definite
  volume
• ____________________- no definite shape, definite
  volume
• ____________________- no definite shape, no
  definite volume
• ____________________- no definite shape, no
  definite volume, charged particles, matter
  consisting of high-temperature gas

solid
liquid
gas
plasma
32

• 3. List the phase of water in order, from the
  phase with the slowest molecular movement to the
  phase with the fastest molecular movement.
• A. gas ? liquid ? solid
• B. liquid ? solid ? gas
• C. solid ? liquid ? gas
• D. gas ? solid ? liquid
• 4. Matter that has a definite volume and a
  definite shape is a _______.
• A. gas B. liquid C. plasma D. solid

33

• 5. Fill in the heating curve for water using the
  following terms freezing point, melting point,
  condense, and boiling point

GAS
Condense
Decreasing Temperature
Boiling point
LIQUID
Freezing point
Increasing Temperature
Melting point
SOLID
34
GAS
LIQUID
SOLID

• 6. Use the graph above to determine the freezing
  point of water ______ OC and the boiling point of
  water ______ OC.

100
0
35
Classification of Matter
36

• 1. Pure substance have a definite composition
  (Ex. Elements or compounds)
• 2. Element simplest pure substance which CAN
  NOT be broken down through physical or chemical
  means
• 3. Compound- is a pure substance composed of 2 or
  more elements that are chemically combined in
  definite proportions (Ex. H2O, CO2)
• 4. Mixture composed of 2 or more different
  substances that can be separated through physical
  means
• 5. Homogeneous mixture a mixture that is the
  SAME throughout
• 6. Heterogeneous mixture a mixture that is NOT
  THE SAME throughout
• 7. Chemical reaction when 2 or more substances
  react to form a new substance
• 8. Chemical change A change of one substance to
  a new substance that differ in appearance and
  chemical make-up (Ex. Rusting, digestion,
  burning)
• 9. Physical change a change in the appearance
  or state of a substance but NOT its chemical
  make-up

37

• 10. Classify each of the following as a physical
  or chemical property
• ___ hardness
• ___ color
• ___ reactivity
• ___ melting point
• ___ chalk breaks easily
• ___ salt water conducts electricity
• ___ flammability
• ___ plastic does not rust
• ___ density

PP
PP
CP
PP
PP
CP
CP
CP
PP
38

• 11. Classify each of the following as a physical
  or chemical change
• ___ digestion
• ___ two clear liquids are mixed and the mixture
  turns blue
• ___ a tree is cut down
• ___ water evaporates into steam
• ___ burning a log

CC
CC
PC
PC
CC
39

• 12. Classify each as either a homogeneous mixture
  (HM), or heterogeneous mixture (HT)
• ____ marble
• ____ air
• ____ mixed vegetables
• ____ hot chocolate with marshmallows

HT
HM
HT
HT
40

• 13. The figure below shows an experimental setup
  used to separate the components of a colored ink
  sample. Which of the following describes this
  laboratory technique?
• A. filtration
• B. distillation
• C. chromatography

41

• Periodic Table

42

• 1. Who attempted to classify the elements by
  organizing them into a seven column table by
  atomic mass?
• Dalton B. Mendeleev C. Bohr
• 2. The metals are located on the __________ side
  of the zig-zag line.
• 3. The nonmetals are located on the __________
  side of the zig-zag line.
• 4. Boron, silicon, germanium, arsenic, antimony,
  tellurium, polonium, and astatine are located
  along the zig-zag line and are called
  _________________.

left
right
metalloids
43

• 5. Label the periodic table box below with the
  following terms atomic number, atomic mass,
  symbol, name, number of protons, number of
  electrons

Atomic number, Number of protons, number of
electrons
symbol
Atomic mass
Name
44

• 6. Periods on the periodic table are arranged in
  ________.
• A. horizontal rows
• B. vertical columns
• 7. Groups on the periodic table are arranged in
  _________.
• A. horizontal rows
• B. vertical columns
• 8. Periods are equal to ___________.
• A. valence electrons- electrons on outer energy
  level
• B. energy levels- electron rings
• 9. Group numbers are equal to __________.
• A. valence electrons- electrons on outer energy
  level
• B. energy levels- electron rings

45

• 10. Complete the table below. (halogens, noble
  gases, alkali metals, nitrogen group, carbon
  group, alkaline earth metals, oxygen group, boron
  group)

Group Group Family Name Valence Electrons Oxidation Number
1A Alkali Metals 1 1
2A Alkaline Earth Metals 2 2
3A Boron Group 3 3
4A Carbon Group 4 4 or -4
5A Nitrogen Group 5 -3
6A Oxygen Group 6 -2
7A Halogens 7 -1
8A Noble Gases 8 0
46

• 11. The group B elements are called the
  ________.
• A. noble gases
• B. halogens
• C. transition metals
• 12. Phosophorus (P) has ______ protons inside of
  the nucleus.
• 13. Aluminum (Al) has ______ electrons outside of
  the nucleus.
• 14. The symbol for lead is ________.
• 15. The most reactive metals are the _________.
• A. halogens
• B. noble gases
• C. alkali metals
• 16. The most reactive nonmetals are the ______.
• A. alkaline earth metals
• B. halogens

15
13
Pb
47

• 17. The __________ are the most stable elements
  and undergo the fewest chemical reactions.
• A. alkali metals B. halogens C. noble gases
• 18. Ca and Mg are located in the same _________
  and they have the same number of ___________
  electrons. Ca and Mg have similar
  ________________ and physical properties for this
  reason.
• 19. ________________ and ____________ are
  elements that have similar chemical properties to
  bromine (Br) and iodine (I)
• 20. What do lithium (Li), beryllium (Be) and
  carbon (C) all have in common?
• valance electrons B. atomic mass
• C. atomic number D. energy levels
• 21. Name the element that has 2 valence electrons
  and 2 energy levels ______________________
• 22. Name the element that has 7 valence electrons
  and 4 energy levels _______________________

group
valence
Chemical
Fluorine (F)
Chlorine (Cl)
Beryllium- Be
Bromine- Br
48

• Atomic Structure

49

• 1. Identify the parts of the atom by using the
  figure on the right. (proton, electron, neutron,
  nucleus, neutral, negative, positive)
• A. ___________ - has a ___________ charge.
• B. ___________ - the center of an atom gives an
  atom its mass
• C. ___________ - has a ____________ charge.
• D. ___________ - has a ____________ charge

Neutron
neutral
Nucleus
Proton
positive
Electron
negative
50

• 2. How do you determine the number of neutrons?
  _________________________________
• 3. A certain atom has 26 protons, 26 electrons,
  and 30 neutrons. Its mass number is _____.
• A. 26 B. 30 C. 56 D. 82
• 4. The diagram on the right represents _______
  which is currently the accepted model of an atom.
  
• A. a Bohr model B. an electron cloud
  model C. electron dot diagram

Neutrons atomic mass atomic number
51

• 5. What is the rule for the Bohr model of an
  atom? _____ _____ _____
• Bohr Model
• 6. The atoms in Group A are different from the
  atoms in Group B because only the atoms in Group
  A have
• A their outer energy levels filled with electrons
• B three energy levels of electrons
• C electron arrangements typical of metals
• D electron arrangements typical of nonmetals

8
2
8
52

• 7. The dots around an electron dot diagram
  represent the __________ electrons which is the
  same as the group number.
• 8. Complete the table below.

Valence
Element Bohr Model Electron Dot Diagram
Lithium Li
Sodium Na
53

• 9. The ___________ is the subatomic particle that
  is responsible for the chemical behavior of an
  element.
• A. proton B. neutron C. electron
• 10. Observe the table above to determine the
  metal used during a fireworks display if a bright
  green spectrum was observed?
• Copper B. Strontium chloride C. Lithium
  D. Copper chloride

Substance Element Color
Copper chloride Bright green
Lithium chloride Carmine red
Sodium chloride Yellow orange
Strontium chloride Scarlet red
54

• 11. An atom that has lost or gained electrons is
  called a(n) _______ and can have a positive or
  negative charge.
• A. particle B. isotope C. ion D. neutron
• 12. A _________ atom equals ZERO and has an equal
  number of protons and electrons.
• A. negatively charged B. positively
  charged C. neutral
• 13. If an atom donates electrons it will have a
  _________ charge.
• A. positive B. neutral C. negative
• 14. If an atom accepts electrons it will have a
  _________ charge.
• A. positive B. neutral C. negative

55

• 15. All of these atoms donate electrons and form
  positive ions EXCEPT

56

• Writing Chemical Formula

57

• 1. What type of bond is pictured on the right
  between two chlorine atoms?
• A. covalent B. metallic C. ionic
• 2. A __________ bond is formed between two
  _____________. The electrons are ____________.
• 3. What type of bond is pictured on the right
  between sodium and chlorine?
• A. covalent B. metallic C. ionic

covalent
nonmetals
shared
58
nonmetal

• 4. A(n) _________ bond is formed between a
  ________ and a ___________ and the electrons are
  ______________.
• 5. What type of bond will be formed between the
  elements below? For a covalent bond write CB
  and for an ionic bond write IB
• ________ H and F ________ N and Cl
• ________ Ca and Br ________ K and I
• ________ H and S ________ Rb and Cl

ionic
metal
transferred
CB
CB
IB
IB
CB
IB
59

• 6. Write the chemical formula and name for the
  following binary ionic compounds.

Element Chemical Formula Compound Name
Li and S Li2S Lithium Sulfide
Mg and P Mg3P2 Magnesium Phosphide
Na and Cl NaCl Sodium Chloride
60

• Conservation of Mass and Reactions

61

• Law of Conservation of Mass-
• __________________________________________________
  _________
• 2. Exothermic Reaction
• __________________________________________________
  __________
• 3. Endothermic Reaction
• __________________________________________________
  _________
• 4. Exergonic Reaction -___
• __________________________________________________
  __________
• 5. Endergonic Reaction- __________________________
  _____________________________

62

• 6. The reaction of CaO and water is exothermic.
  A student mixes the two chemicals in a test tube
  and touches the side of the test tube. Which
  statement describes the students observation?
• A. The test tube becomes hot as heat is
  released.
• B. The test tube becomes hot as heat is
  absorbed
• 7. The reaction that takes place inside of a glow
  stick is best described as being a ________
  reaction
• A. endergonic B. endothermic C. exergonic
• 8. The law of conservation of mass requires a
  chemical equation to have the ________ number of
  atoms on each __________. To balance a chemical
  equation, you must add _____________ in front of
  the chemical formulas in the equation. You can
  not ________ or ____________________ subscripts.

same
side
coefficients
add
change/take away
63

• Count up the number of atoms that are found for
  each element on each side of the equation. State
  whether the equation is balanced or not for
  questions 9 and 10.
• 9. Ca(OH)2 2HNO3 ? Ca(NO3)2 2H2O
• Ca Ca
• O O Balanced or Not Balanced
• H H
• N N
• 10. Zn 2HCl ? ZnCl2 H2
• Zn Zn
• H H Balanced or Not Balanced
• Cl Cl

1
1
8
8
4
4
2
2
1
1
2
2
2
2
64

• Determine the mass of the unknown substances
  below for questions 11 and 12.
• 11. What is the mass of reactant X in the
  equation below? _______ g
• X ? X
• 50g __?__ g ? 80 g
• 12. What is the mass of product in the
  equation below? _______ g
• _at_ ? _at_
• 40g 30g ? 60g __?_
  g

30
10
65

• 13. Use the figure below to determine the type of
  reaction taking place in each letter. (synthesis,
  decomposition, single replacement, double
  replacement)
• F Single-displacement
• G Decomposition
• H Synthesis
• I Double-displacement

66

• 14. Balance the chemical equations below.
• _____P _____O2 ? _____P2O5
• _____Na2O _____CO2 ? ______Na2CO3
• 15. Indications of a double displacement reaction
  are water, gas, and a(n) ____________.
• A. acid B. base C. precipitate
• 16. Count the atoms
• Ca(O2H4)2 Ca O H
• 2NaCl2 Na Cl

4
2
5
1
1
1
1
4
8
4
2
67

• 17. 2Fe2O3 ? 4Fe 3O2
• 1. Coefficient
• 2.Yield
• 3. Subscript
• 4. Reactants
• 5. Products
• 18. What is the function of the coefficient in a
  chemical equation?
• 19. What is the purpose of the subscript in the
  chemical equation?

Coefficient- tells the number of units of a
substance in a chemical equation
Subscript- tells the number of atoms in a
chemical formula
68
Solubility
69

• 1. Solute _______________________________________
  _____________________
• 2. Solvent ______________________________________
  ______________________
• 3. Solubility ___________________________________
  ________________________
• 4. Electrolyte __________________________________
  __________________________
• 5. Nonelectrolyte _______________________________
  ____________________________
• 6. Unsaturated __________________________________
  _________________________
• 7. Saturated ____________________________________
  ________________________
• 8. Supersaturated _______________________________
  _____________________________
• 9. Polar Molecule _______________________________
  _____________________________
• 10. Nonpolar Molecule ___________________________
  ______________________________________

70

• 11. To dissolve a polar solute, the solvent must
  be _________.
• A. polar B. nonpolar C. neutral
• 12. To dissolve a nonpolar solute, the solvent
  must be __________.
• A. polar B. nonpolar C. neutral
• 13. List 3 ways in which the rate of dissolving
  can be increased.
• 14. How do you increase the solubility of a gas
  into a liquid? (Ex. soda)

Stirring, increased temperature, increased
surface area
Cold temperature, high pressure
71

• 15. According to the graph below, if you had 80g
  of KBr dissolved in 100g water at 70 degrees C,
  what kind of saturation would it be?
• A. saturated B. unsaturated C. supersaturated
• 16. According to the graph on the right, the
  solubility of ________ is least affected by an
  increase in temperature.
• A. KNO3 B. KBr C. NaCl

72
polar

• 17. Water is ____________ because it has a
  partially positive region and a partially
  negative region.
• 18. _________________ is the universal solvent
  because of the polar nature of its molecules.
• 19. A solution that has ions in it can produce
  electricity and be classified as a(n) __
• A. nonelectrolyte B. electrolyte C. compound

water
73
Acids and Bases
74

• 1. Acid _________________________________________
  ___________________
• 2. Base _________________________________________
  ___________________
• 3. Hydroxide ion ________________________________
  ____________________________
• 4. Hydronium ion ________________________________
  ____________________________
• 5. Neutralization _______________________________
  __________________
• 6. Ionization ___________________________________
  _______________

75
0
14

• 7. The pH scale ranges from ________ to ________.
• 8. Classify the substances as acid (A), base (B)
  or neutral (N) based on the pH.

Substance pH Acid, Base, Neutral
A 2
B 7
C 9
Acid (0-6)
Neutral
Base (8-14)
76

• 9. What type of ions do acids form when dissolved
  in water?
• _______________
• 10. What type of ions do bases form when
  dissolved in water?
• _______________
• 11. List 3 properties of acids
• __________________________________________________
  ____

Hydrogen Ions (H)
Hydroxide Ions (OH-)
Corrosive, sour, electrolyte
77

• 12. List 3 properties of bases
• __________________________________________________
  ____________
• 13. What are the products of a neutralization
  reaction (acid base)? _
• _______________________________
• 14. Which solution below is a base that is also
  an electrolyte?
• A. solution 1 B. solution 2 C. solution 3 D.
  solution 4

Corrosive, bitter, electrolyte
Water and a Salt
78

• 15. A solution that has more H ions than OH-
  ions is ________.
• A. acidic B. neutral C. basic

The End !