Download Chemistry Final Test 1999-2000 - Nashoba Valley Technical High

Chemistry Final Exam Review Topics 2014-2015
Date: *Seniors Wednesday, May 20, 2015
Juniors Wednesday, June 10, 2015
* Please note this is one day different
from original publication.
Chapters: 1-4, 6, 18, 8, entropy (ch.10), 11, parts of 12 & 13, 15 Holt: Chemistry
Weighting: 20% of second semester grade (13% of grade for the whole year)
Format: 100 multiple choice questions (Honors 120 multiple choice questions)
Provided:
periodic table, polyatomic ions, electronegativity values, calculator
PREAPPROVED: 8.5” x 11” note sheet (Honors: 3” x 5” note card) which must be
handwritten.
Bring: # 2 pencils, eraser, something to read when you are done.
In the following packet are the topics studied during the entire school year. This final
exam is cumulative. Sample test questions are also included.
Study Resources:
 Your worksheets, your labs (Chromatography, Half-Life, Flame Test, Periodic
Trends, Lego, class action, pH, etc.), your tests (You may come in and look them
over). It is possible you will see some of these questions or similar questions on
your final exam.
 Content Review problems at the end of each chapter.
 The SparkNotes website has a chemistry section at
http://www.sparknotes.com/chemistry
 This website provides sample practice questions in the style of chemistry MCAS
questions
http://www.practicequiz.com/MCAS-Chemistry-Exam-Practice
Ways to Study:
 Start studying NOW.
 Review in short study sessions.
 Quiz a friend over the material and practice explaining topics to each other.
 DO NOT look at the answers until you have tried the problems! If you get stuck
DO NOT look at the answers until you have tried as hard to get yourself unstuck
as you would try in the real exam.
 Rewrite your notes and rework problems from your homework worksheets.
 Schedule study sessions with friends (and chemistry teacher). Try explaining how
to do the problems to each other—by the time you’ve finished explaining
something completely, you’ll understand it well.
 Review the “objectives” at the beginning of each chapter and the summaries at the
end. Quiz yourself. Anything you don’t remember or have trouble with is
something you need to re-read, study, or ask about.
Go to sleep no later than 10:00 P.M. the night before the exam! Eat a medium sized
healthy breakfast. Yes, really! You are much more likely to think clearly during the test
if you are well rested, relaxed and have some energy to focus on your work.
1
Chapter 1: The Science of Chemistry and 2: Matter & Energy
 What is chemistry?
 Density problems
 Lab Safety
 Temperature scales (Kelvin –
Celsius)
 Scientific Method
 Categorize matter
 Metric and SI units (prefixes)
(heterogeneous, compound, etc)
 Accuracy and Precision
 Techniques to separate mixtures,
 Measuring
Chromatography lab
 What are significant figures?
 Four states of matter
 Rules of significant figures
 Chemical and Physical properties
(honors)
& changes
 Significant Figures in
 Laws of conservation of energy,
calculations (honors)
matter
 Scientific Notation
 Percent error calculations
Book problems: p. 9 #3,4,5,12,13,14, p.14 #1-3, p.19 #3, 6-12, p.28 # 1-8, 13, 14, p. 31
#1-15, p. 32 # 2-23, 26-28, p.45 # 1,-3, 5-10, p.53 #1-7, p.59 # 1,2 p.63 #1,4-6,8,9,
p.66#17, 19, p.67#20-26, 30-34, 36-40
Chapters: 3 Atoms & Moles and 18 Nuclear Chemistry:
 Models of atom
 Nuclear reactions (alpha, beta,
gamma)
 Laws: Multiple Proportions,
Definite Composition
 Fusion, Fission
 Development of atom
 Half life, Carbon dating (half(history/scientists/experiments)
Life lab)
 Dalton’s Atomic Theory
 Write Electron Configurations
 Rutherford’s experiment
 Valence electrons and Octet Rule
 Structure of atom
 Predict charge of ions formed
from Periodic Table
 Subatomic particles
 Noble gases – stability
 Atomic number, mass number vs.
average atomic mass
 Write orbital diagram
 Isotopes
 Radioactivity/stability of nucleus
Book problems: p.78 #1-6, p.86 # 1-4, p.89 # 1, 2, & 1-6, p. 99 # 1, 2, 4-8, p.1071-11,
25, p.108# 30-35, p.109 # 52, 55, 65, 66, p. 653 #1-4, p.657 #2 ,5, p.660 # 3, p.662 # 13, p.669 #4, 5, 8, 18, 19, p.670 # 34
Chapter 4: The Periodic Table
 Historical development of modern periodic table
 Identify different parts/families on periodic table
 Predict properties of elements
 Describe the electromagnetic spectrum (flame test lab and light emission)
2

Describe the model of the atom according to modern quantum theory using
o energy levels, sublevels, orbitals & electron spin
 Write electron configuration of element based on location on periodic table using
o Aufbau principle,
o Pauli Exclusion principle,
o Hund’s Rule
 Know 4 trends across period and down family:
o Atomic radius
o Ionic radius
o Ionization energy
o Electronegativity
Book problems: p. 122 # 4-7, 12, 13, p.131 # 1, 5, 7, 13 p.141 #1, 3, 5, 10, 13, p.150# 13,7, 9, 12, 14, 21, 31, 32, , 41, p.15359-64, p.155 # 11,12
Chapter 5: Ions & Ionic Compounds and Chapter 6: Covalent Compounds
 Valence electrons and Octet Rule
 Predict charge of ions formed from Periodic Table
 Noble gases – stability
 Transition metals – how to determine charge from name or formula
 Lewis Dot diagrams
 Describe Ionic bonding, Covalent bonding, metallic bonding
 Identify, name and write cations, anions, polyatomic ions, & the 7 diatomic
elements
 Identify if compound is ionic or molecular
 Lewis dot diagrams/structures of covalent molecules
 Shapes (geometry) of covalent molecules, VSEPR Theory
 Polarity of covalent bonds and molecules
 Write names & formulae for ionic, covalent, and acid compounds
Book problems: p.165 # 1-4, 7,8,10,11,12 p.175 # 1, 2, p.180 #2-8 but not 8b, p. 183 #
1-4, 7, 17-19, p.202, # 1, p.205 # 1,2, p.207 # 3,6,7,9,10, p. 213 # 1,2,4,6-8, p.216 #
8,9,11,15,16,17,20,22,25-27,30,32, 33, 35,38,39, p.220 #3
Chapter 8 – Chemical Equations & Reactions
 Describe a chemical reaction and signs one has occurred
 Identify and use various symbols used in writing chemical equations
 Balance chemical equations
 Identifying 5 types of chemical reactions (combustion, decomposition, synthesis,
double replacement, single replacement)
Chapter 10 - Energy
 Temperature
 Entropy
- Law of Conservation of mass
- Law of Conservation of energy
Chapter 11 & 12 – States of Matter
 Describe the 3 main states of matter and their phase changes
3
Chapter 13 – Solutions
 Describe the properties of a solution including the 4 colligative properties
 Distinguish between solutions, suspensions & colloids
 Describe solvation – the dissolving process
 Compare solubility, concentration & saturation
 Describe factors that affect dissolving rate for solids & gases
 Describe & identify an electrolyte
 Interpret a solubility graph
Chapter 15 – Acids and Bases Describe each of the following:
 2 definitions of acids & bases (Arrhenius, Brønstëd-Lowry)
 Properties of acids & bases
 Neutralization reaction
 Strength of acids and bases
 Identify an acid, base or salt
 Naming acids and bases
 pH scale – use to identify acid or base; calculate it, pOH or [H+] or [OH-]
 What’s a buffer? How’s it used?
 Titration
 Indicators: litmus, phenolphthalein, universal (ph paper)
Below are some sample questions – they are not meant to be a comprehensive
review. You MUST study more but these are questions similar to the style you will
see on your final exam.
STRAND 1: PROPERTIES OF MATTER
*1) Which of the following statements explains why a pitcher of Kool-Aid is classified as a
mixture not as a pure substance?
A. Kool-Aid comes in a variety of colors.
B. Kool-Aid is made of sugar, water, red dye and other ingredients.
C. Kool-Aid can be made in different concentrations.
D. Both B & C
*2) Which of the following statements describes a difference between a chemical change and
a physical change in a substance?
A. A physical change occurs only in elements; a chemical change occurs only in
compounds.
B. A chemical change involves a change in heat; a physical change does not.
C. A chemical change creates a new substance; a physical change is the same
substance in a different form.
D. A chemical changes involves a color change; a physical change does not.
3) The decrease in the kinetic energy of a chemical process would best be measured in
the lab by using which of the following?
a. A beaker b. a balance c. a test tube d. a thermometer
4
4) A sample of sand from the beach contains bits of silicon dioxide, seashells made of
calcium carbonate, water, and small microorganisms. Which of the following best
describes this sand?
a. compound b. element c. heterogeneous mixture d. homogeneous mixture
5) Which of the following is an example of a physical change?
a. burning a scented candle
b. separating water into hydrogen gas and oxygen gas
c. freezing liquid water into an ice cube
d. using AAA batteries in your calculator
6) The table below shows the physical properties of selected metals.
Physical Properties of Selected Elements
Element
Molecular
Melting
Boiling
Density at
o
o
mass (amu)
point ( C)
point ( C)
STP
(g/cm3)
2.02
−259.16
−252.879
0.00008988
Hydrogen
32.00
-218.79
-182.962
0.001429
Oxygen
24.31
650
1091
1.738
Magnesium
28.09
1414
3265
2.3290
Silicon
A chemical sample has a volume of 23.13 cm3 and a mass of 40.25 g. Based on the data
in the table above, what is the identity of this element?
A. hydrogen
B. oxygen
C. magnesium
D. silicon
7) Which of the following correctly describes magnesium sulfide?
A. It is composed of one element.
B. It is composed of one compound.
C. It is composed of a heterogeneous mixture of two or more substances.
D. It is composed of a homogeneous mixture of two or more substances.
8) Which of the following is an example of a chemical change?
A. Iron exposed to air produces rust.
B. Carbon dioxide combined with water forms seltzer water.
C. Melting butter onto popcorn.
D. Dry ice (CO2) subliming into gaseous carbon dioxide.
9) How would you separate a mixture of salt and water?
A. Use electrolysis to separate the water into hydrogen, oxygen, sodium and
chlorine.
B. Use a filter to separate the salt from the water.
C. Let the water evaporate.
D. Let the salt evaporate.
10) Identify how you can separate the components of a mixture while avoiding doing a
chemical reaction?
A. decompose it
B. use a nuclear reaction
C. neutralize it
D. use chromatography
5
11) A student used a hydrometer to estimate the density of very salty sea water. The
hydrometer contains water and used to compare the density of water to the density of the
liquid that you put it in. The hydrometer floated in the seawater. What does this tell you
about the density of the sea water?
A. The sea water has a density greater than 1 g/mL
B. The sea water has a density equal to 1 g/mL
C. The sea water has a density less than 1 g/mL
D. The sea water contaminated the water in the hydrometer.
12) In the following diagrams, the spheres represent particles. Different shadings
represent different particles. Which diagram(s) show a mixture?
A. A only
B. B Only
C. Several are mixtures
D. All of them are mixtures
STRAND 2: ATOMIC STRUCTURE & NUCLEAR CHEMISTRY
13) Cesium (Cs) has 55protons in each atom. Based on this information, which of the
following also describes an atom of cesium?
A. It has 55 electrons.
B. It has 55 neutrons.
C. It has 28 neutrons and27 electrons.
D. It has a total of 133 neutrons and electrons.
14)) Which of the following statements describes an alpha particle?
A. It has no mass.
B. It has a positive charge.
C. It is the strongest form of radiation.
D. It is the same as a gamma ray.
15) Which of the following comparisons correctly describes subatomic particles?
A. An electron has a negative charge and a mass equal to a neutron.
B. A neutron has a negative charge and a mass equal to the mass of a proton.
C. An electron has a negative charge and is much smaller than a proton.
D. A proton has a positive charge and a mass smaller than the mass of an
electron.
6
16) C-12, C-13, and C-14 are all isotopes of carbon. Which of the following statements best
compares these isotopes?
A. The C-12 has the smallest net charge.
B. The C-14 has a larger atomic radius.
C. The all have the same number of protons and electrons.
D. The C-12 atom has more particles in its nucleus.
17) Which of the following represents a pair of isotopes?
A. 1H1+ and 11Na1+
B. 54Cr and 54Mn
C. 31P3- and 80Br1D. 32S and 35S
18) The three main types of nuclear radiation are alpha, beta, and gamma. Which of the
following lists these types of radiation from lest dangerous to most dangerous?
A. alpha, gamma, beta
B. beta, alpha, gamma
C. alpha, beta, gamma
D. gamma, beta, alpha
19) Which of the following statements correctly describes nuclear fission and nuclear fusion?
A. Powerplants use only fusion and nuclear bombs use fission.
B. Fission forms heavier elements, and fusion forms lighter elements.
C. They are opposites of each other; Fission creates a larger atom, fusion breaks an atom
apart.
D. They are opposites of each other; Fission breaks an atom apart, fusion creates a larger
atom.
20) Tritium (H-3) has a half-life of approximately 12 years. If a 1000 g sample of tritium decays for
48 years, approximately how much remains in the sample?
A. 63g
B. 125 g
C. 250 g
D. 500 g
21) Whose research resulted in the discovery of electrons?
A. Rutherford’s gold foil experiment
B. Moseley’s experiments.
C. Bohr’s experiments.
D. Thomson’s cathode ray experiments.
22) Where are the neutrons located?
A. Orbiting around the atom with the electrons
B. In the nucleus alone.
C. In the nucleus with the protons
D. In the nucleus with the protons and electrons
23) When uranium-238 undergoes radioactive decay, it emits an alpha particle and produces
thorium-234 as shown: 23892U  42 + 23490Th. When americium-241 undergoes alpha-decay,
which isotope is produced?
A. 23490Th
B. 23793Np
C. 24597Bk
D. 23892U
abc
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STRAND 3: PERIODICITY (& ELECTRON CONFIGURATIONS FROM STRAND 2)
24) The diagram below shows the relative locations of five unidentified elements in the periodic
table: A, B, C, D, and E.
A
C
E
D
B
If element E is a noble gas, which element will form an ion with a -2 oxidation number?
A. element A
B. element B C. element C D. element D
25) Which of the following correctly describes a trend from top to bottom in the group 1 (1A)
elements on the periodic table?
A. electronegativity decreases.
B. Ionic charge decreases.
C. Atomic radius decreases.
D. Atomic number decreases.
26) Which of the following is the same for both beryllium and magnesium?
A. atomic mass
C. number of protons
B. total mass of neutrons
D. charge of their ion
27) Based on its position on the periodic table, which of the following elements is a metal?
A. calcium (Ca)
B. hydrogen (H)
C. arsenic (As)
D. iodine (I)
28) Which element on the periodic table has the ground state electron configuration:
1s22s22p63s23p1?
A. Na
B. K
C. Sc
D. Al
29) Which of the following elements has the largest atomic radius?
A. O (oxygen)
B. B (boron)
C. C (carbon)
D. N (nitrogen)
3o) Which of the following elements is a semimetal?
A. hydrogen (H)
B. calcium (Ca)
C. zinc (Zn)
D. germanium (Ge)
31) Which of the following elements is a member of the boron family and is located in period 3?
A. boron (B)
B. aluminum (Al)
C. gallium (Ga)
D. nitrogen (N)
32) Which of the following observed properties is most reliable in classifying a substance as a metal?
A. poor conductor of heat
B. low boiling temperature
C. brittleness
D. ductility
33) The fact that elements in the same group of the periodic table have the same number of valence
electrons determines which of the following?
A. The elements have similar chemical properties
B. The elements have similar atomic sizes.
C. The elements have similar atomic masses.
D. The elements have similar numbers of protons.
34) In which of the following lists are the elements shown in order of decreasing electronegativity?
A. O, S, Se, Te
B. O, Te, S, Se
C. Te, Se, S, O
D. Te, S, O, Se
abc
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35)What does the graph below show about the first ionization about elements in a period?
A. ionization energy decreases as atomic number increases in a period
B. ionization energy increases as atomic number increases in a period
C. ionization energy shows no pattern for elements in a period
D. The graph only shows a pattern for elements in a group.
STRAND 4: CHEMICAL BONDING
36) The diagram below represents particles of different elements in a crystal.
What type of particles are these?
A. atoms
B. compounds
C. ions
D. molecules
37) What is the correct name for the compound with the chemical formula SrCO3?
A. strontium carboxide
B. strontium carbonate
C. strontium carbon trioxide
D. strontium carbon oxygen
38) When elements from group 2 (2A) react with elements from group 15 (5A),
they produce compounds. Which of the following is the correct combining ratio between group
2 (2A) elements and group 15 (5A) elements?
A. 2:2
B. 2:3
C. 3:2
D. 2:1
39) The illustration below shows two hydrogen molecules reacting with an oxygen molecule to
form two water molecules. What type of bonding is formed in the water molecules?
A. ionic
abc
B. hydrogen
Page 9
C. polar covalent
D. nonpolar covalent
5/8/2015
40) In magnesium oxide, the magnesium atom donates two electrons and the oxygen atom
accepts the two electrons. When the compound magnesium oxide is formed, which of the
following are formed?
A. ionic bonds
B. covalent bonds
C. nuclear forces
D. magnetic forces
41) Why is the bond in an oxygen molecule (O2) nonpolar covalent?
A. The oxygen atoms will share electrons equally because there is no difference in their
electronegativities.
B. One oxygen atom will take electrons from the other oxygen atom.
C. The oxygen atoms will keep their own valence electrons.
D. The The valence electrons have to equal 8 according to the octet rule.
42) Which of the following statements best explains why the noble gases are relatively unreactive?
A. They are chemically stable.
B. They have a full set of valence electrons.
C. They have electrons in the highest energy level. D. They have no room for any more electrons.
43) Which of the following is a correct Lewis dot structure for CH3Cl?
44) Which of the following models best represents the shape of a compound with bent geometry?
45) Which of the following is the electron configuration for silicon?
A. 1s22s22p4
B. 1s22s22p63s23p2
C. 1s22s22p63s23p6
D. 1s22s22p63s23p64s1
46) Lithium and phosphorous react to form an ionic compound. What is the chemical formula for
this compound?
A. LiP
B. LiP3
C. Li3P
D. Li3P3
47) What is the importance of valence electrons?
A.They determine chemical bonding
C.They give identity to the atom
B. They determine the charge of the atom
D. Both A & B
48) Two elements in a molecule have an electronegativity difference greater than 1.7. Which of the
following most likely holds the elements together and why?
A. an intermolecular force, because the elements will not form a chemical bond
B. an ionic bond, because electrons will completely transfer from one element to the other
C. a nonpolar covalent bond, because the elements share electrons equally
D. a polar covalent bond, because the elements will not share electrons equally
abc
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STRAND 5: CHEMICAL REACTIONS
49) Which of the following chemical reactions is a double replacement reaction?
A.
NaOH + HCl  H2O + NaCl
B.
Cu + AgNO3  Ag + CuNO3
C.
CaCO3  CaO + CO2
D.
2H2 + O2  2H2O
50) An unbalanced chemical equation is shown here:
What are the coefficients of the balanced equation?
A. 2:1:3
B. 2:2:3
C. 2:3:1
___NH3
___H2 + ___N2
D. 3:2:2
51) Before the invention of antacids, baking soda (NaHCO3) was a common remedy for upset
stomachs because it neutralizes stomach acid (HCl). The partially balanced equation for the
reaction of 2 moles of baking soda with 2 moles of stomach acid to produce sodium chloride,
water and carbon dioxide is given here:
2NaHCO3 + 2HCl  ___NaCl + 2H2O + 2CO2
When this equation is balanced, what is the coefficient for sodium chloride?
A. 2
B. 3
C. 6
D. 9
52) Magnesium reacts vigorously and exothermically with cobalt(V) bromide. Which
of the following is the balanced equation for this reaction?
A. Mg + CoBr5  MgBr2 + Co
B. Mg + 2CoBr5  5MgBr2 + Co
C. 5Mg + 2CoBr5  5MgBr2 + 2Co
D. 10Mg + 2CoBr5  5MgBr2 + 10Co
53) The reaction that produces rust (Fe2O3) is shown here: 4Fe(s) + 3O2(g) 2Fe2O3 (s). What
type of reaction is it?
A. decomposition B. synthesis C. single displacement
D. double displacement
54 ) A student heated a 5g sample of a compound in an open container. A chemical reaction
occurred. The mass of the sample was measured again and found to be the same as in the
beginning. Which of the following explains why the mass didn’t change?
A. The heat just melted the compound but didn’t change anything else.
B. In a chemical reaction the identity of the substance changes but mass is conserved.
C. No reaction occurred.
D. One of the reaction products was a gas.
55) An unbalanced equation is shown here: AuNO3 (aq) + Ca (s)  Ca(NO3)2 (aq) + Au (s)
Which of the following statements correctly compares the mass of the reactant with the mass
of the products in this reaction?
A. The mass of the reactants is less than the mass of the products.
B. The mass of the reactants is more than the mass of the products.
C. The mass of the reactants is equal to the mass of the products.
D. The mass of the reactants is ½ the mass of the products.
abc
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56) The figure below represents a reaction. What type of reaction is shown?
A. synthesis
B. decomposition
C. single displacement
D. double displacement
57) A student places a 1.24g piece of aluminum foil into a beaker containing 3.00 g of
concentrated hydrochloric acid. The experiment begins to bubble as the reaction below takes
place.
2Al + 6HCl  2AlCl3 + 3H2
When the reaction finishes, the student takes the mass again and determines that there is
3.98g left in the beaker. How much hydrogen escaped into the air?
A. 0.26 g H2
B. 1.24 g H2
C. 3.98 g H2
D. 4.24 g H2
58) When pure CaCO3 is heated under certain conditions, CaO and CO2 are produced. What type
of reaction is this?
A. combustion B. single displacement
C. double displacement
D. analysis
59) Which of the following equations represents the law of conservation of mass?
A.
TiCl4 +
O2

TiO2 +
2Cl2
B.
2TiCl4 +
O2

TiO2 +
4Cl
C.
TiCl4 +
2O2

2TiO2 +
Cl2
D.
2TiCl4 +
2O2

2TiO2 +
Cl4
60) When you eat Total cereal it is possible to digest 100% of your required daily value of iron when
the iron in the cereal reacts with your stomach acid (HCl). If this reaction were done in a
beaker the products would be FeCl3 and hydrogen gas. What is the balanced equation for
this reaction?
A.
Fe
+
HCl 
FeCl3 +
H2
B
Fe
+
3HCl 
FeCl3 +
3H
C.
Fe
+
6HCl 
FeCl3 +
3H2
D.
2Fe
+
6HCl 
2FeCl3 +
3H2
61) The table below shows the procedures for and results of two experiments using copper(II)
chloride, CuCl2.
Experiment 1
Experiment 2
Procedure
Procedure
Put 0.5 g of table sugar in a crucible. Heat under
Put 0.5 g of table sugar into a beaker
a fume hood over a Bunsen burner flame.
containing50 mL of water.
Results
Results
The crystals change from white to yellowThe crystals seem to disappear. A clear
brown to black. A strong odor is given off.
colorless liquid remains. No odor is given off.
Which of the following conclusions can be made based on the results of the experiments?
A. Physical changes occurred in both experiments.
B. Chemical changes occurred in both experiments.
C. A chemical change occurred in experiment 1, and a physical change occurred in
experiment 2.
D. A physical change occurred in experiment 1, and a chemical change occurred in
experiment 2.
abc
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STRAND 8: ACIDS& BASES AND OXIDATION-REDUCTION REACTIONS
62) Sulfuric acid (H2SO4) is a strong acid. The dissociation of H2SO4 in an aqueous solution is
given below.
H2SO4 (aq)  2H+(aq) + SO42According to the Arrhenius theory, why is sulfuric acid an acid?
A. H2SO4 is a neutralizer.
B. H2SO4 is a proton donor.
C. H2SO4 forms hydrogen ions in water.
D. H2SO4 is an electron pair acceptor.
63) A student was assigned to test various solutions during a lab. She measured the
pH of one of the liquids as 12.0. Which of the following best describes this sample of water?
A. Highly acidic
B. Slightly acidic
C. Highly basic
D. Slightly basic
64) The table below shows pH values of some foods.
A patient has chronic indigestion due to an overproduction of stomach acid. Which food would
be the worst for the patient to eat?
A. Limes
B. oranges
C. milk
D. crackers
65) The alkaline diet is a common fad diet that some people follow because they believe that
some foods cause your body to produce too much acid, which could be bad for you.
There is no proof this diet works but they believe that eating specific foods makes your
body more alkaline and therefore more healthy. What might these alkaline foods contain
or produce in your body?
A. Both H+ or OH- ions.
B. High concentrations of OH- ions.
C. High concentrations of H+ ions.
D. Neutral salts.
66) The pH of four different solutions of common materials is measured. Which of the following
lists the solutions in order from most basic to most acidic?
A. ammonia, milk, vinegar, stomach acid
B. stomach acid, vinegar, milk, ammonia
C. milk, ammonia, stomach acid, vinegar
D. vinegar, stomach acid, milk, ammonia
67) Due to soil conditions, some people can grow grass in their lawn, while others can only grow
moss. Lime, (Ca(OH)2), is used to kill the moss and change the pH of the soil so more
grass can grow. What is the most likely pH for a mossy lawn?
A. 3
B.7
C. 9
D. 14
abc
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68) A chemical equation representing the reaction of water (HOH) and ammonia (NH3) is
shown below.
Which of the following statements best explains the chemical action of the products in this
equation?
A. Both NH4+ and OH- are conjugate acids.
B. Both NH4+ and OH- are conjugate bases.
C. NH4+ is a conjugate acid, and OH- is a conjugate base.
D. NH4+ is a conjugate base, and OH- is a conjugate acid.
69) The pH of freshly made lye soap can range from 10-14. Why do manufacturers of lye soap
have to cure it before selling it?
A. It is very basic & would give you a chemical burn C. It is slightly basic & smelly
B. It is very acidic & could give you a chemical burn. D. It is slightly acidic & smelly.
70) When you eat acidic or basic foods, the pH of your blood does not change. How is the pH of
your blood able to remain constant?
A. Buffers catalyze chemical reactions in the body cells.
B. Buffers maintain a constant pH in the blood.
C. The pH of you blood does change, it’s just not measurable.
D. The foods you eat neutralize one another.
71) Under certain conditions, hydrogen gas (H2) and oxygen gas (O2) will violently combine to
form water (H2O). The oxidation-reduction reaction is shown below.
2H2(g) + O2 (g)  2H2O gs)
Which of the following is the oxidation number for O in H2O in this reaction?
A. +1
B. -1
C. +2
D. -2
72) How does a buffer work?
A. It speeds up a reaction
B. It acts as an inhibitor
C. It contains a weak acid & base to neutralize either kind
D. It contains water which is neutral.
73) What does a buffer do?
A. It decreases the rate of a reaction.
B. It neutralizes chemicals until the buffer capacity is reached.
C. It can neutralize chemicals limitlessly.
D. It acts as a spectator ion.
74) A sample of blood a pH of 7.45, and a sample of baking soda has a pH of 8.3. Which of the
following statements best describes these two substances?
A. Both samples are bases, and baking soda is more basic.
B. Both samples are acids, and baking soda is more acidic.
C. Both samples are bases, and blood is more basic.
D. Both samples are acids, and blood is more acidic.
abc
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75) Refer to the table below to answer the following question: Which indicator would be the best choice
for a titration with an end point at a pH of 5.2?
Indicator
pH titration range
Congo red
3.0-5.0
Bromocresol green
2.0-5.6
Bromothymol blue
6.0-7.6
Phenolphthalein
8.0-9.8
A. congo red
B. bromocresol green C. bromothymol blue D. phenolphthalein
76) What is neutral in a neutralization reaction?
A. the acid reactant
B. the base reactant
C. the water product
D. the salt product
STRAND 6: STATES OF MATTER, KINETIC MOLECULAR THEORY AND THERMOCHEMISTRY
77) In order to make a supersaturated solution, it is necessary to heat up the solvent. Which of the
following statements best describes this process?
A. Energy is absorbed by the solution in an endothermic process.
B. Energy is released by the solution in an endothermic process.
C. Energy is absorbed by the solution in an exothermic process.
D. Energy is released by the solution in an exothermic process.
78) A common video on YouTube shows gallium metal melting in a person’s hand. What happens
to the entropy of the gallium sample as it is melting?
A. It remains unchanged because the identity of the metal is the same
B. It decreases because some energy is transferred to the person’s hand
C. It increases because liquids have more disorder than solids in their structure
D. It decreases because liquids are more orderly than solids in their structure
79) A sample of mercury liquid is frozen. During this time, what happens to the motion of the
molecules?
A. The motion of the atoms stops once the sample is completely solid.
B. The motion of the atoms increases once the sample is completely solid.
C. The motion of the atoms decreases to a vibration as the sample solidifies.
D. The motion of the molecules remains the same throughout the process.
80) Which of the following correctly pairs a state of matter with its description?
A. Solid: Particles vibrate in place but generally do not change their location.
B. Liquid: Particles expand to fill any container in which they are placed.
C. Gas: Particles have a lower amount of energy than when in the liquid
phase.
D. Liquid: Particles are more strongly attached to one another than when in
the solid phase.
81) The diagram at the right represents a phase change
for some argon atoms. Which of the following phase
changes are the argon atoms undergoing?
A. gas to liquid
B. liquid to gas
C. solid to liquid
D. liquid to solid
abc
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82) The average distance between molecules always increases during which of the following
phase changes?
A. freezing
B. condensing
C. melting
D. desublimation
83) Which of the following can be used to speed up the rate of a chemical reaction?
A. Radiation
B. an inhibitor
C. less reactants
D. a catalyst
84) Which of the following would have the least kinetic energy?
A. dry ice boiling at -57oC
C. a solid piece of iron at 130oC.
B. ice melting at 0oC.
D. cannot be compared
STRAND 7: SOLUTIONS
85) Which of the following helps explain why a sugar cube dissolves more slowly in cold water
than in hot water?
A. The reduced motion of cold water molecules disperses the sugar less quickly.
B. The sugar cube and cold water form more covalent bonds.
C. The sugar cube is more chemically reactive with the hot water.
D. The sugar cube breaks down into free atoms more quickly in the hot water.
86) A student pours a single-serve Kool-Aid packet into a bottle of cold water. What can the
student do to increase the dissolving rate of the Kool-Aid?
A. Shake the bottle to help raise the temperature of the water.
B. Shake the bottle to help start the chemical reaction.
C. Shake the bottle so more of the water can mix with the undissolved Kool-aid.
D. Pour some of the water out of the bottle.
87) On a cold January night, a person decided to try to prevent ice from forming on the driveway
and back steps of the house. On the driveway, he put out road salt (MgCl2) but ran out before
making back to the steps. He decided to try table salt (NaCl) from the kitchen on the steps. In
the morning one location still had ice on it. Which location the driveway or the steps were icy
and why?
A. The driveway froze because there was an overhang protecting the steps.
B. The steps froze because table salt has fewer particles than the road salt to lower the
freezing point.
C. The driveway froze because road salt has fewer particles than table salt to lower the
freezing point.
D. The steps froze because they are made of wood which doesn’t hold heat as well as the
tar driveway does.
88) A gallon of whole milk from the store contains healthy vitamins, fat and water. A student
describes the milk as white, homogenous, and unable to see through. She concluded milk
was_______________.
A. a solution because the ingredients don’t settle out.
B. a type of homogenous mixture called a colloid because the particles don’t settle
out but do scatter light.
C. a type of homogeneous mixture called a suspension because the particles scatter
light.
D. a pure substance because it look the same throughout.
abc
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89) Why does table salt (NaCl) dissolve in water?
A. The table salt reacts with water to form a new liquid substance.
B. Water and table salt are made of oppositely charges ions that form new attractions
with each other.
C. Water is a polar molecule with partial charges that are able to completely surround
each oppositely charged ion of the table salt, separating and dissolving it.
D. Water is a polar molecule with partial charges that are able to completely surround
each similarly charged ion of the table salt, separating and dissolving it.
90) Which of the following statements best explains why sugar dissolve in water?
A. Water is a highly polar molecule with hydrogen bonding that helps it act as a
universal solvent.
B. Water and sugar are both covalently bonded.
C. Water has space between its molecules that the sugar fits into.
D. Any liquid will dissolve a solid because it’s warmer.
91) A solution that contains the maximum amount of solute than it can hold at a given
temperature and pressure is:
A. disassociated.
B. saturated. C. supersaturated.
D. unsaturated.
92) A sugar crystal dissolves in water. Which of the following statements explains why the dissolved
sugar does not recrystallize as long as the temperature and the amount of water stay
constant?
A. Sugar is reacts completely forming a new substance and is no longer present in the water.
B. Sugar gradually leaves leave the water through evaporation.
C. Water molecules for a large molecule with the sugar crystal.
D. Water molecules completely surround the sugar molecules preventing them from
rejoining each other.
93) The diagram below represents a cation and an anion surrounded by several water molecules.
This diagram can be used to represent which of the following?
A. How ionic compounds react
B. How ionic compounds form
C. How ionic compounds dissolve in water
D. How atoms form charges
94) An nonpolar solid is placed in a beaker of water. Which of the following occurs when there is a
no attraction between the solute and the solvent?
A. The solute melts.
B. The solute dissolves.
C. The solute remains intact.
D. The solute reacts to form a precipitate.
abc
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95) Three 10 g samples of sugar are represented below.
Which sample dissolves the most slowly?
A. Sample C because it is the largest quantity of sugar.
B. Sample C because it mixes the easiest.
C. Sample A because it has the least amount of surface area.
D. Sample A because it has the largest amount of surface area.
96) Which of the following statements explains why a busy restaurant puts salt in the boiling water in
which the pasta will cook?
A. The salt causes the water to boil at a higher temperature, cooking the pasta more quickly.
B. The salt lowers the boiling point of the water, making it safer to cook.
C. The salt serves no other purpose than making the pasta taste better.
D. The salt makes the pasta healthier.
97) An experiment is pictured below.
Solid KNO3 was added to a beaker with water and stirred until it
completely dissolved. A student determined that it took 10
minutes for the KNO3 to fully dissolve. What could the student
do next time to decrease the amount of time he needed to work in
the lab?
A. Crush the KNO3 into a powder before putting it in the
water.
B. Use warmer water.
C. Use warmer water and crush the KNO3.
D. Use colder water
98) What type of substances can be found as either solids, liquids or gases at room temperature?
A. metals
B. nonmetals
C. metalloids
D. plastics
99) A student used red litmus paper to test a sample of tap water and observed no change. What
information can the student conclude about the tap water from this test?
A. The water is neutral
C. The water is either acidic or neutral
B. The water is acidic
D. The water is basic.
100) A student tests an unknown chemical with blue litmus paper. The paper turns red. What
information can the student conclude about the chemical?
A. The chemical is neutral
C. The chemical is basic
B. The chemical is acidic
D. The chemical is acidic or neutral.
abc
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101) In a chemical equation, what can be used to determine a change in entropy?
a. The coefficients
b. The states of matter
c. Both A & B
d. Nothing in the equation alone can be used.
102) What is entropy?
a. It is the tendency of the universe to increase to a greater state of disorder or
disorganization
b. It is the tendency of the universe to become more orderly and organized
c. It is the degeneration of muscles
d. It is the awarding of a trophy
103) Steel can be described as which of the following?
a. an alloy
b. an pure element
c. a solution
d. both a & c
104) A can of orange juice concentrate can be mixed with water to make a tasty pitcher of orange
juice. Which of the following is a true statement?
a. Orange juice concentrate contains more oranges than water and is the solvent in the
pitcher.
b. Orange juice concentrate contains more oranges than water and is the solute in the
pitcher.
c. Orange juice concentrate contains more water than oranges and is the solvent in the
pitcher.
d. Orange juice concentrate contains more water than oranges and is the solute in the
pitcher.
105) A solution that contains fewer hydrogen ions than hydroxide ions is _____.
a. an acid
b. a base
c. neutral
d. ionized.
106) Use the solubility graph on the right to determine which of the following is true about a
solution of NaNO3 if 150g of NaNO3 are dissolved in 100g of water at 80oC?
a. it’s unsaturated
b. it’s saturated
c. it’s supersaturated
d. unknown
107) Use the solubility graph
on the right to determine
how much Copper(II) sulfate
could dissolve in 300mL of
water at 20oC.
_________________
108)What is the molar mass
of ozone (O3)?
A. 16 amu
C. 48 amu
B. 16g
D. 48 g
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