Name That

1
Name That
Dead Guy!!
2
Atomic Models
1. Some people have said that his model of the
atom was a bit fruity.
J.J. Thompson
2. He told the early philosophers that their
theory was full of hot air and cold water.
Democritus
3. He was sure his theory was a ringer.
Bohr
4. His theory was out of this world.
Bohr
5. He coined the term atom.
Democritus
3
Atomic Models
6. His model was the first to be solid at the
core if a bit fuzzy elsewhere.
Rutherford
7. He was a scientist of indivisible intentions.
Dalton
8. His model earned him a gold star.
Rutherford
9. He was feeling very uncertain about the
probability of his model being accepted.
Schrödinger
10. He believed that atoms came in many shapes
and sizes.
Democritus
4
Atomic Models
11. He played well with electrons.
J.J. Thompson
12. His model is probably the newest.
Schrödinger
13. He was a school teacher and a scientist who
enjoyed saying the Pledge every morning.
Dalton
14. He wanted to try out the plum pudding to see
if it was as doughy as it sounded.
Rutherford
15. He was a great thinker because his equipment
was lacking.
Democritus
5
Named Gas Laws
1. He made a name for himself by producing a
volume of work when under pressure.
Boyle, P1V1 P2V2
2. This fellows ego expanded as the temperature
went up.
3. This hothead could always feel his temperature
rise when under pressure.
6
Named Gas Laws
4. When in doubt, order a combo.
5. Moles think this ones a gas!
Ideal Gas Law, PVnRT
6. He was certain his temperature scale was
absolute.
Kelvin
7. He always had a solution when under pressure.
7
Named Gas Laws
8. Many thought he was a cracker, but actually he
was just effusive.
9. Though some thought he was a bit green and
mush-minded, he believed in keeping everything in
proportion.
Avogadros Law of Proportionate Volumes
10. While liquids and solids cant use this
excuse, gases often use it to explain their
disorderly conduct.
The Entropy of gases is gtgt than liquids or solids
8
Round 2
What is that??
9
Element, compound, solution or heterogeneous
mixture??
1. One type of atom.
Element
2. Sugar dissolved in water.
Solution
3. Dirt.
Heterogeneous mixture
4. Air.
Solution
5. A 24 caret gold ring.
Element
10
Element, compound, solution or heterogeneous
mixture??
6. Water.
Compound
7. Carbon dioxide gas.
Compound
8. An 8 caret gold ring.
Solution
9. The contents of your junk drawer.
Heterogeneous mixture
10. Ice.
Compound
11
Name That
Compound!!
12
Warming up with a few ionic compounds
1. Ca2C
Calcium carbide
2. (NH4)3PO4
Ammonium phosphate
3. Mg(OH)2
Magnesium hydroxide
4. K2O
Potassium oxide
5. NH4Cl
Ammonium chloride
6. Sn(NO3)2
Tin(II) nitrate
7. FeHPO4
Iron(II) hydrogen phosphate
8. Cu2S
Copper(I) sulfide
9. Ni(C2H3O2)2
Nickel(II) acetate
10. HgClO4
Mercury(I) perchlorate
13
Working out the kinks with a few covalent
compounds
Carbon dioxide
1. CO2
2. N2O4
Dinitrogen tetroxide
3. SF6
Sulfur hexafluoride
4. PCl5
Phosphorus pentachloride
Sulfur trioxide
5. SO3
6. H2S
Dihydrogen sulfide
7. BCl3
Boron trichloride
8. NO
Nitrogen monoxide
9. CF4
Carbon tetrafluoride
10. XeF4
Xenon tetrafluoride
14
Feel the burn! Ionic and covalent together
1. K2SO4
Potassium sulfate
2. PCl3
Phosphorus trichloride
3. BF3
Boron trifluoride
4. (NH4)3PO4
Ammonium phosphate
5. ZnCl2
Zinc chloride
6. Au2O3
Gold(III) oxide
7. SeF6
Selenium hexafluoride
8. NCl5
Nitrogen pentachloride
9. OCl2
Oxygen dichloride
10. Ca(OH)2
Calcium hydroxide
15
Cooling down with some acid naming
1. HNO3
Nitric acid
2. HBr
Hydrobromic acid
3. H2SO4
Sulfuric acid
(battery acid)
4. HF
Hydrofluoric acid
(dissolves glass)
5. HClO4
Perchloric acid
(ignites organic cmpds)
6. H2SO3
Sulfurous acid
7. HBrO3
Bromic acid
8. HCl
Hydrochloric acid
(stomach acid)
9. H3PO4
Phosphoric acid
(acid in colas)
10. HClO
Hypochlorous acid
16
Final Round
17
How many protons, neutrons and electrons in
1. Helium-3
2p, 1n, 2e
6p, 8n, 6e
3. Pb-207
82p, 125n, 82 e
4. Oxygen-14
8p, 6n, 8e
15p, 16n, 15e
18
Math with Significance
1) 1.0 (1.001.000)
1.0 (2.00) 2.0
2) (1.000 1.000)/(0.09 0.01)
2.000/0.10 20.
3) 0.50 (2 2.0)
0.50 (4) 2
4) A rock weighing 7.05 g is dropped into a
graduated cylinder containing 5.1 mL of water.
What is the density of the rock if the final
volume of water is 10.5 mL?
D m/V 7.05 g/(10.5 mL -5.1 mL) 7.05 g/5.4 mL
D (1.3055556 g/mL) 1.3 g/mL
19
Of half-lives and nucleides and radioactive stuff
1) Element X has a half-life of 11 days. If you
start out with 80 g, how many grams of X are left
after 33 days?
80 g (0.5)3 10 g
2) What fraction of a radioactive isotope is left
after 4 half lives?
(0.5)4 0.0625
3) What does I-131 transmutate into following an
alpha decay?
Sb-127
4) What happens when O-16 is bombarded by one
alpha particle and a neutron?
20
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q What does this graph describe?
The heating curve of a substance
21
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q What is the freezing point of this substance?
-10C
22
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q The DHfus of this substance is 300 J/g. How
many grams of this substance were used?
0.05 g
23
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q Which phase has the lowest Cp?
The gas
24
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q If 10 grams of this substance was used, what
is the DHcond in J/g?
-1 J/g
25
Temperature (C)
30
20
10
0
-10
-20
10
20
30
40
50
0
60
Heat input (J)
Q What would a cooling curve for this substance
look like?
26
Use the activity series in your reference packet
to predict whether the reactions below will occur
or not.
F2 2 NaCl ? 2 NaF Cl2
Yes, F is more active than Cl
No, I is below Br on the activity scale
I2 CaBr2 ? CaI2 Br2
Li 2 H2O ?2 LiOH H2
Yes, Li can replace H in water
K LiCl ? KCl Li
No, K is lower on the activity scale
Zn MgO ? Mg ZnO
No, Zn is lower on the activity scale
No, Co is not active enough to replace H in water
Co 2 H2O ? Co(OH)2 H2
Ni H2SO4 ? NiSO4 H2
Yes, Ni will replace H in acids
27
Which transition in the hydrogen emission
spectrum is responsible for
The only red line in the visible spectrum?
3 ?2
The highest energy photon?
4 ? 1
The lowest frequency photon?
4 ?3
Blue-green
What color is emitted by the n4 to n2
transition?
Which set of transitions result in the excited
electron returning to the ground state?
The UV emission lines
28
How many grams of copper(II) oxide are formed
when 2.5 g of copper metal is heated strongly in
air?
2 Cu (s) O2 (g) ? 2 CuO (s)
Given the laboratory data below, what is the
formula of the tin oxide that is formed?
Wt. crucible 3.5 g Wt. crucible Sn metal 5.0
g Wt. crucible Sn oxide 5.4 g
1.5 g Sn
0.4 g oxygen
SnO2
29

• For an experiment in which you are determining
  the freezing point of an unknown chemical, you
  record the temperature every minute for 20
  minutes. In this example, time is the
• A. control C. independent variable
• B. dependent variable D. hypothesis

2) In the chemistry lab, chemicals that you are
finished working with should be A. poured
into the sink B. returned to their original
containers C. mixed together and dumped in a
designated container D. disposed of as directed
by your teacher
30
3) In chemistry lab, a student was instructed to
find the density of a rectangular piece of
aluminum. After careful measurement, he recorded
a mass of 31.44 g and a volume of 11.7 cm3. Using
the formula density mass/volume and a
calculator, his answer was 2.6871794 g/cm3. Which
of these is the correct answer to report for the
density of the aluminum? A. 2.7 g/cm3 B. 2.69
g/cm3 C. 2.687 g/cm3 D. 2.68 g/cm3
31
4) The table shows the data obtained by four
groups of students during a lab investigation
designed to determine the boiling point of
methanol. The accepted value for the boiling
point of methanol is 78.5C. Whose data was the
most precise? A. Group A B. Group B C. Group
C D. Group D
32
5) A student told the class that she takes 500 mg
of vitamin C every day. What is this mass
expressed in grams? A. 0.05 g B. 0.5 g C. 5.0
g D. 500,000 g
6) The density of carbon dioxide gas is 1.8 x
103 g/cm3. This value can be expressed in
ordinary notation as A. 0.0018 g/cm3 B. 0.018
g/cm3 C. 0.18 g/cm3 D. 1.800 g/cm3
33
Temperature (C) Time
(minutes) 10 33 20 16 30 8 40 4 50 2 A
group of students investigated how temperature
affects the rate of chemical reactions. They used
hydrogen peroxide, which breaks down into oxygen
and water, for their experiment. The students
measured how long it took to obtain 50 mL of
oxygen gas from a given volume of hydrogen
peroxide heated to different temperatures. Their
data is shown in the table above.
7) Select the best way for the students to reduce
the experimental error in their
investigation. A. Test more than one variable at
a time. B. Perform repeated trials. C. Change
their answers if they do not match their
hypothesis. D. Perform the experiment only one
time.
34
8) Characteristics of a substance can be
classified as physical properties or chemical
properties. Which of the following is a chemical
property? A. Boils at 56C B. Tastes
sour C. Has a density of 2.9 g/cm3 D. Reacts
with acid to produce hydrogen gas
11) Select the observation that does NOT support
the conclusion that a chemical reaction took
place. A. Liquid water changed to water
vapor. B. A precipitate was formed. C. An
odor developed. D. Temperature rose.
35
9) The diagram above shows a chemical equation
representing a chemical reaction. The name and
mass of each substance involved in the chemical
reaction are also shown. Which of these are the
reactants? A. HCl and NaOH B. NaCl and H2O C.
HCl and H2O D. NaOH and NaCl
10) According to the law of conservation of mass,
mass is neither created nor destroyed during a
chemical reaction. On the basis of this law, what
mass of water was produced in the reaction shown
in the above diagram? A. 16.0 g B. 18.0 g C.
20.0 g D. 22.0 g
36
12) Reeses teacher gave her three test tubes,
each containing a different unknown liquid sample
of a given density. Reese added orange food
coloring to each test tube and then calculated
the density of the sample. She place the data she
collected in the data table. She concluded that
the added food color increased the density of the
sample. What is another reasonable interpretation
of the data? Initial Food Color
Final Density Added Density (grams/cm3) (mL)
(grams/cm3) Final Color Sample
A 0.91 1 1.1 light orange Sample
B 0.94 5 1.2 orange Sample C 0.92 7 1.2 blue A
. Sample A is a different substance than Sample
B. B. Sample C is a different substance than
Samples A or B. C. All three samples contain
water. D. None of the samples contain water.
37
13) The atomic mass of an element is the weighted
average mass of the isotopes of that element.
Based on this definition, which of these does NOT
show the correct atomic mass for an element? A.
Hydrogen 1.008 amu C. Oxygen 15.999 amu B.
Carbon 12.011 amu D. Copper 63.017 amu
38
14) The diagram above shows the results of
Rutherfords experiment in which he used a
radioactive source to shoot alpha particles at
a thin sheet of gold foil. Based on these
results, what were Rutherfords conclusions? A.
Atoms are solid matter with positive and negative
charges scattered throughout. B. Atoms are
solid, positively charged matter with
negatively charged electrons scattered
throughout. C. Atoms are mostly empty space
with small, dense, positively charged
centers. D. Atoms are mostly empty space with
small, dense, negatively charged centers.
39
15) In the fourth century BC, Greek scholars
rejected Democrituss ideas about the atom. This
rejection was most likely based on A.
experimentation B. government legislation C.
religious beliefs D. the popularity of
Aristotles ideas on nature
16) When a potassium compound is placed in a
flame, energy is released and a violet color is
produced. This energy release is due to A. the
release of gamma rays from the nucleus B. the
return of excited electrons to lower energy
levels C. the movement of electrons to higher
energy levels D. the absorption of photons by
the electrons
40
17) Which of these is the ground-state electron
configuration for an atom of fluorine (atomic
number 9)? A. 1s2 2s2 B. 1s2 2s2 2p3 C. 1s2
2s2 2p4 D. 1s2 2s2 2p5
18) The electron configuration for an atom of
iron is Ar 3d6 4s2. Which of the above
diagrams is the correct electron-dot structure
for iron? A. A. B. B. C. C. D. D.
19) What is the wavelength of the wave shown
above? A. 3.2 cm B. 3.5 cm C. 3.7 cm D. 4.0 cm
41
20) Why are there no electronegativity values for
the elements with atomic numbers 2,10, and
18? A. The noble gases form very few compounds
because they are gases. B. The noble gases
form very few compounds because they are
rare. C. The noble gases form very few
compounds because they are radioactive. D.
The noble gases form very few compounds because
their electron configurations are very stable.
42
21) Metal is to malleable as nonmetal is
to___. A. brittle B. solid C. dull D. gaseous
22) The periodic table has an unusual shape
because it is divided into blocks representing
the energy sublevel being filled with valence
electrons. In the periodic table shown above,
which sequence lists these blocks in s-p-d-f
order? A. Y, W, Z, X B. W, Y, X, Z C. Y, Z, W,
X D. X, Y, Z, W
43
23) Which of the following elements has the
lowest ionization energy? A. Li B. Na C. K D. Rb
24) Which element does the following electron
configuration describe? Ar 4s2 3d10 4p5 A.
selenium B. nickel C. manganese D. bromine
25) Select the largest atom from the following
list. A. Rb B. Sr C. I D. Xe
26) Select the number of electrons a beryllium
atom will gain or lose when it forms a beryllium
ion. A. gain 2 B. gain 4 C. lose 2 D. lose 4
44
27) Which of the following BEST describes the
difference in first ionization energy between
selenium (Se) and krypton (Kr)? A. Krypton has
a greater ionization energy than
selenium because it is a halogen. B. Krypton
has a greater ionization energy than
selenium because it has more protons in its
nucleus, so that electrons are bound more
tightly to it. C. Selenium has a greater
ionization energy than krypton because it is
the larger atom. D. Selenium has a greater
ionization energy than krypton because it has
fewer protons in its nucleus, so electrons are
bound less strongly.
45
28) Mendeleev left blank spaces in his periodic
table where he thought elements that had not yet
been discovered should go. He was able to predict
the properties of these elements by A.
studying the spectra of stars that contained
them B. testing their properties such as
melting point, density, and valence C. noting
periodic trends in the properties of known
elements that surrounded the blank spaces in
the periodic table D. studying the new elements
produced by radioactive decay
46
29) Use the electronegativity chart to determine
which of the following compounds contains ionic
bonds.
A. SOCl2 B. P(OH)4 C. Mg(OH)2 D. HCN
30) Some nuclear reactors use heavy water to slow
down neutrons produced during nuclear fission.
Heavy water contains deuterium, an isotope of
hydrogen. What is the mass number of
deuterium? A. 1 B. 2 C. 3 D. 4
47
31) A family of colorless, inactive gases was
unknown at the time Mendeleev conceived his
periodic table. Eventually, these gases were
discovered on Earth in the late 1890s. What group
does this family occupy in the modern periodic
table? A. 15 B. 16 C. 17 D. 18
32) Lithium (Li), an alkali metal, has properties
similar to and has a diagonal relationship with
A. hydrogen (H) B. beryllium (Be) C. sodium
(Na) D. magnesium (Mg)
33) Transition metals with unpaired valence
electrons are attracted to a magnetic field.
Which of these elements is NOT able to form a
permanent magnet? A. Cobalt B. Copper C.
Nickel D. Iron
48
34) In the periodic table, as you move from left
to right across a period A. atomic radius
increases and ionization energy
increases B. atomic radius increases and
ionization energy decreases C. atomic radius
decreases and ionization energy
increases D. atomic radius decreases and
ionization energy decreases
35) As you move from top to bottom down a group
in the periodic table, which of the following
happens? A. Valence electrons move farther from
the positively charged nucleus. B. Valence
electrons move farther from the
negatively charged nucleus. C. Valence
electrons move closer to the positively
charged nucleus. D. Valence electrons move
closer to the negatively charged nucleus.
49
36) More than three times as much energy is used
to make a new aluminum can than to process a
recycled one. The main reason for this difference
is that A. aluminum is not an abundant
element B. aluminum has a high melting
point C. it is difficult to extract aluminum
from its ore D. aluminum is not a reactive
metal
37) Which statement below correctly explains the
polarity of water? A. Hydrogen atoms are much
smaller than oxygen atoms. B. Water molecules
have a bond angle greater than 100 degrees. C.
Water molecules form hydrogen bonds with other
water molecules. D. Oxygen nuclei attract
electrons more strongly than hydrogen nuclei
attract electrons.
50
38) Which of the following compounds has the
lowest melting point? A. NaCl B. C6H12O6 C.
Al2O3 D. SiO2
39) A molecule is formed when two or more atoms
form a covalent bond. According to this
definition, which of these is NOT a molecule? A.
NaCl B. H2 C. HCl D. NH3
41) Which of the following intermolecular forces
is the strongest? A. London forces B. hydrogen
bonding C. dipole-dipole D. van der Waals
42) How many moles of nitrogen atoms are
contained in one mole of Ba(NO3)2? A. 1 B. 2 C.
6 D. 9
51
40) The table below shows some of the prefixes
used to name binary covalent compounds. What name
would be given to the compound PBr5? Number
Number of atoms Prefix of atoms Prefix
1 mono- 6 hexa- 2 di- 7 hepta- 3 tri- 8 o
cta- 4 tetra- 9 nona- 5 penta- 10 deca- A.
phosphorus tetrabromide C.
phosphorus pentabromide B. monophosphorus
tetrabromide D. phosphorus hexabromide
43) Zinc is used as a coating on iron and steel
to prevent corrosion. What is the mass, in grams,
of 0.0650 mol Zn? A. 3.25 g B. 3.90 g C. 3.94
g D. 4.25 g
52
44) Mole is to atom as gram is to A. amu B.
mass C. molecule D. particle
45) What is the total number of atoms contained
in 2.00 moles of helium? A. 15.999 B. 32.0 C.
6.02 x 1023 D. 1.20 x 1024
46) Potassium nitrate, also known as saltpeter,
is used in matches. What is the percent by mass
of potassium (K) in potassium nitrate (KNO3)? A.
38.67 B. 45.94 C. 55.71 D. 56.58
47) Baking soda is the common name for sodium
hydrogen carbonate (NaHCO3). What is the mass in
grams of 2.75 moles of sodium hydrogen
carbonate? A. 63.2 g B. 84 g C. 210 g D. 231 g
48) A mole of atoms will have a total mass of
A. 12 kg B. 12 g C. 12 amu D. 6 amu
53
Zn(s) HCl(aq) ? ZnCl2(aq) H2(g)
49) The skeleton equation above represents a
chemical reaction. Which of these are the
reactants? A. Zn and HCl B. ZnCl2 and H2 C. HCl
and ZnCl2 D. Zn and H2
50) The skeleton equation (above) for this
chemical reaction violates the law of
conservation of mass. Which of these is the
correct balanced chemical equation? A. 2 Zn(s)
HCl(aq) ? 2 ZnCl2(aq) H2(g) B. Zn(s) 2
HCl(aq) ? ZnCl2(aq) 2 H2(g) C. Zn(s) 2
HCl(aq) ? ZnCl2(aq) H2(g) D. 2 Zn(s) 2
HCl(aq) ? 2 ZnCl2(aq) H2(g)
51) The chemical reaction represented by the
equation would be classified as a A. synthesis
reaction C. single-replacement reaction B.
decomposition reaction D. double-replacement
reaction
54
Zn(s) HCl(aq) ? ZnCl2(aq) H2(g)
52) Which of these is a spectator ion in this
chemical reaction? A. Cl(aq) B. H(aq) C.
H2(g) D. Zn2(aq)
53) Which of these is NOT evidence of a chemical
reaction? A. An iron nail changes to a
brownish-orange color. B. An ice cube melts
into liquid water. C. An antacid tablet
produces bubbles of gas when placed
in water. D. A piece of zinc raises the
temperature of an acid as it reacts with it
55
54) The diagram shows the activity series of some
metals (left) and nonmetals (right). A student
set up four beakers, each containing 100 mL of
dilute hydrochloric acid (HClaq). She added 5 g
of a metal to each beaker in this order aluminum
(Al), copper (Cu), sodium (Na), and zinc (Zn).
Which metal will NOT react with the acid? A.
Aluminum B. Copper C. Sodium D. Zinc
56
55) A chemist is about to synthesize
tetraphosphorus decoxide by combining X grams of
phosphorus with sufficient oxygen to react
completely with the phosphorus. If he wants to
determine the amount of tetraphosphorus decoxide
that will be produced, all of the following need
to be answered before initiating the experiment
EXCEPT... A. What is the balanced chemical
equation for this reaction? B. What are the
number of moles for each reactant? C. What is
the mole ratio of the two reactants D. Which is
the limiting factor and which is the
excess reactant?
57
56) The above graph shows the number of mole
ratios that can be determined given the number of
reactants and products of a chemical reaction. If
this trend continues, how many mole ratios can be
formed with a chemical reaction that has a sum of
eight reactants and products? A. 54 B. 56 C.
58 D. 60
58
57) Chemists normally use an excess of one
reactant in a chemical reaction because A. the
reaction will continue until all of the limiting
reactant is consumed B. the reaction will
continue until all of the excess reactant
is consumed C. reactions do not take place
unless there are unequal amounts of
reactants D. reactions occur too quickly if
equal amounts of reactants are used
58) Stoichiometry is the study of quantitative
relationships between amounts of A. the
reactants and products of a chemical reaction
relative to time B. the products of a chemical
reaction only C. the reactants and products of a
chemical reaction D. the reactants of a chemical
reaction only
59
59) Three moles of carbon dioxide are produced
when one mole of propane gas is burned. How many
moles of carbon dioxide will be produced if 30
moles of propane gas are burned? A. 10 moles B.
30 moles C. 90 moles D. 120 moles
60) In the movie The Wacky World of Chemistry, a
chemist wrote down the following equation on a
chalkboard Ti C 2Cl2 ? TiCl2 C
This equation is NOT correct because A. the
titanium atoms are not equal on both sides of
the equation B. there are not enough chlorine
atoms on the right side of the equation C.
the carbon atoms are equal on both sides of the
equation D. the right side of the equation
should have a greater number of atoms than the
left side
60
61) In the periodic table, a series of elements
that is arranged in a horizontal row is called
a A. cluster B. family C. period D. group
62) Which of these phase changes does NOT involve
the absorption of heat energy? A. Boiling B.
Condensation C. Melting D. Vaporization
63) Distillation is a separation technique that
involves A. using a porous barrier to separate a
solid from a liquid B. separating dissolved
substances based on their tendency to be drawn
across a surface C. the formation of pure,
solid particles of a substance from a solution
containing the dissolved substance D.
separating two or more liquids based on
differences in their boiling points
61
64) Each diagram above shows the particles of a
substance in a closed container. Which of these
shows the substance that is most easily
compressed? A. Q B. R C. S D. T
62
65) The tables show the chemical analyses of two
compounds baking soda and sodium hydrogen
carbonate. Because they have the same percent by
mass, they must be the same compound according to
the A. law of definite proportions C. law of
conservation of energy B. law of multiple
proportions D. law of conservation of mass
63
Figure 1 shows a graduated cylinder that
contained 25 mL of water. The mass of the
cylinder and water was 68.0 g. Fig. 2 shows the
same cylinder after a metal sample was lowered
into the cylinder. The water level rose to the
30.0 mL mark the mass of the cylinder, water and
sample increased to 77.0 g.
66) What is the identity of the substance? A.
iron B. nickel C. titanium D. magnesium
64
67) There is some error associated with the
density calculation of the metal in the cylinder.
What is its MOST likely source? A. improperly
reading the volume of the sample B. selecting
an irregularly shaped metal sample C. selecting
the wrong glassware for this measurement D. use
of the wrong liquid medium
68) Thymol blue is a pH indicator with a
transition range between 1.2 and 2.8. Below 1.2,
the indicator is red. Above 2.8, the indicator is
yellow. Thymol blue is used to determine the
approximate pH of the following solutions. Which
solution is yellow? A. 1 M HCl B. 0.1 M HCl C.
0.01 M HCl D. 0.001 M HCl
69) Select the type of ion produced when a strong
acid is added to water. A. hydrated B.
hydride C. hydroxide D. hydronium
65
70) Which of the following is NOT a strong
acid? A. hydrochloric acid B. sulfuric acid C.
acetic acid D. nitric acid
72) Which statement is NOT true of sulfuric
acid? A. Sulfuric acid is a proton
acceptor. B. Aqueous sulfuric acid is almost
completely dissociated. C. Aqueous sulfuric acid
will conduct electricity. D. Sulfuric acid will
neutralize a strong base such as KOH.
73) Apple juice has a potential of hydroxide
(pOH) of 10.5. Which of the following BEST
describes its level of acidity? A. strong
acid B. weak acid C. nearly neutral D. weak base
66
71) Hydrofluoric acid is used industrially for
glass etching. It is a contact poison and should
be handled with extreme care, beyond that
accorded to other mineral acids. Part of its
danger lies with its low dissociation constant
in solution, HF remains bound to a fairly large
extent. For this reason, HF penetrates tissues
more deeply than other acids. By the time
dissociation occurs, the chemical is already
absorbed in the skin and burns are often in the
deep tissue. Symptoms of exposure to
hydrofluoric acid may not be immediately evident.
HF interferes with nerve function and burns may
not initially be painful. Accidental exposures
can go unnoticed, delaying treatment and
increasing the extent and seriousness of the
injury. Skin surface exposures of less than 3
have been fatal. Describe the acidity of HF
based on this passage. A. It is a very strong
acid. C. It is a weak acid. B. It is a
moderately strong acid. D. It is a weak base.
67
74) Which statement most accurately describes the
state of a reaction after it has reached chemical
equilibrium? A. At chemical equilibrium, equal
amounts of products and reactants are
present. B. The forward and reverse reactions
are producing equal concentrations. C. The
forward and reverse reactions are occurring at
equal rates. D. At equilibrium, the reaction
is continuing in either the forward or reverse
direction.
75) Which of these is the correct way to express
the equilibrium constant expression for the
following reaction? Cu(OH)2(s) ? Cu2(aq)
2 OH(aq) A. K Cu2OH2 C. K
Cu2OH2 B. K Cu2OH2 Cu(OH)2 D.
K Cu2OH2 Cu(OH2)
68
76) The reaction below is exothermic. To produce
less product, what experimental change would be
most effective? 2 SO2(g) O2(g) ? 2 SO3(g)
?Hrxn -198 kJ A. Decrease
volume C. Increase pressure B. Decrease the
temperature D. Increase the temperature
77) According to this table, which compound has
the greatest solubility in pure water? Solubility
Product Constants at 298K Compound Ksp
value PbBr2 6.6 x 10-6 Ag2S 8.0 x
10-51 PbCl2 1.7 x 10-5 MgCO3 6.8 x
10-6 A. PbBr2 B. Ag2S C. PbCl2
D. MgCO3
69
78) The common ion effect alters the amount of
solid that will dissociate in solution. The
addition of solid silver chromate to an aqueous
solution of potassium chromate will affect the
silver chromates solubility because A. solids
are always subject to the common ion effect
in solution B. the ion chromate is common to
both solutions and will decrease silver
chromates solubility C. the combination of two
common metals, silver and potassium, will
decrease solubility D. the ion chromate is
common to both solutions and will increase
solubility
70
79) Which experimental disturbance will produce
more NH3 (ammonia) in the following reaction?
N2(g) 3 H2(g) ? 2 NH3(g) A. Decrease in
pressure C. Decrease in volume B. Addition of
more ammonia D. Addition of a catalyst
80) Which of these increases when the sign of ?S
is negative? A. Disorder B. Temperature C.
Order D. Kinetic energy
81) When you eat a slice of pizza, the crust is
often less hot than the toppings or sauce. This
most likely occurs because the toppings and sauce
have a greater A. molar enthalpy of
formation C. heat of fusion B. specific heat D.
mass
71
82) The equation shows the change in enthalpy
when one mole of liquid water vaporizes into
water vapor. This is called the molar heat of
vaporization. Given this information, which of
these is the proper value for the molar heat of
condensation? A. ?Hcond 40.7 kJ C. ?Hcond
571.6 kJ B. ?Hcond 0 kJ D. ?Hcond 571.6 kJ
83) Which of these is required for a reaction to
be called exothermic? A. The enthalpy of the
reactants must be less than that of
the products. B. The sign of the change in
enthalpy for the reaction must be positive. C.
The enthalpy of the products must be less than
that of the reactants. D. Heat must flow from
the surroundings into the system.
72
84) Leila is given a sealed flask of sugar water
at room temperature. She places it over a Bunsen
burner for a few minutes and notes condensation
on the sides. Then she places the flask in an ice
bath for ten minutes, and notices that ice
crystals begin to form. Leila knows that the one
statement that cannot be true is that A. the
kinetic energy of the sugar water at the end of
the experiment is less than at the beginning of
the experiment B. the total energy in the sugar
water at the end of the experiment is less than
at the beginning of the experiment C. the
entropy of the sugar water at the beginning of
the experiment is greater than at the end of the
experiment D. the total energy in the sugar
water at the beginning of the experiment is
greater than at the end of the experiment
73
85) Fusion, or melting, is an endothermic process
because it A. requires heat to be transferred
from system to surroundings and has a ?H that is
negative B. requires heat to be transferred
from surroundings to system and has a ? H that is
positive C. involves a decrease in entropy D.
involves a decrease in kinetic energy
86) Which of the following is NOT a variable in
the Gibbs free energy equation, which determines
reaction spontaneity? A. Entropy B. Endothermy C.
Temperature D. Enthalpy
87) Professor Bothwell determined from the
wrapper the number of calories in a candy bar. He
then burned the entire candy bar and measured the
amount of heat released. His experiment was most
likely designed to demonstrate the A. law of
conservation of matter B. law of disorder C. law
of conservation of energy D. law of constant
composition
74
88) Which of these would always be called a
spontaneous reaction? A. A reaction with a ?S
and a ?H B. A reaction with a ?H and a
?S C. A reaction with a ?H and a ?S D. A
reaction with a ?S and a ?H
89) Which of the following reactions is a
spontaneous process at 25C? A. 2 Fe2O3(s) ? 4
Fe(s) 3 O2(g) ?H 1625 kJ B. H2O(l) ?
H2O(s) ?H 6.01 kJ C. 4 Fe(s) 3 O2(g) ? 2
Fe2O3(s) ?H 1625 kJ D. CO2(g) 2 H2O(l) ?
CH4(g) 2 O2(g) ?H 891 kJ
75
The following slides are from the NY State
Regents Exam, which is much more rigorous than
NCs EOC Chemistry Exam.
76
1. Which gas should not be collected over water
because of its high solubility in water? (A) H2
(B) CO (C) CH4 (D) HCl
2. The solubility of a solid in H2O at different
temperatures is indicated in the accompanying
diagram. What mass of the solid will crystallize
when 40. mL of a solution that is saturated at
80C is cooled to 20 C? (A) 12 g (B) 24 g (C)
30 g (D) 36 g
77
3. Which is the net ionic equation for the
reaction when 0.10 M solutions of silver nitrate
and sodium sulfide are mixed? (A) Ag1 (aq) S1
(aq) ? AgS (s) (B) Ag2 (aq) S-2 (aq) ? AgS
(s) (C) Ag2 (aq) S1 (aq) ? AgS2 (s) (D) Ag1
(aq) S-2 (aq) ? Ag2S (s)
4. What is the total mass, in grams, of products
when 2.20 g of propane is burned in excess
oxygen? C3H8 5 O2 ? 3 CO2 4 H2O (A) 2.20 (B)
3.60 (C) 6.60 (D) 10.2
5. What volume, in mL, of concentrated sulfuric
acid (18.0 M H2SO4) is needed to prepare 2.50 L
of a 1.00 M solution? (A) 7.20 (B) 14.4 (C)
69.4 (D) 139
78
6. Under which conditions is the solubility of
oxygen gas in water the greatest? Pressure
Temperature (A) high high (B)
High low (C) low high (D) low low

• 7. Which pure compounds form intermolecular
  hydrogen bonds?
• HF
• H2S
• III. CH4
• (A) I only (B) II only
• (C) I and II only (D) II and III only

79
8. What is the molar mass of a gas if 10.0 grams
of it occupy 4.48 liters at 273 K and 101.3 kPa
(1.00 atm)? (A) 2.00 g/mol (B) 25.0 g/mol (C)
50.0 g/mol (D) 100. g/mol
9. Which process requires the greatest amount of
energy for 1 mole of H2O? (A) breaking the O-H
bonds (B) melting (C) evaporating (D)
subliming
10. Which substance boils at the highest
temperature? (A) CH3Cl (B) CH2Cl2 (C) CHCl3
(D) CCl4
80
11. What can be concluded about the substance
represented by this phase diagram? (A) The normal
boiling point of the liquid is 80 C. (B) The
solid is more dense than the liquid. (C) The
solid sublimes at temperatures above 20 C. (D)
The vapor can be converted to liquid by
compressing it at temperatures below 20 C.
81
12. Which of these conversions has a positive
?So? I. combustion of charcoal II.
condensation of Br2 (g) III. precipitation of
AgCl (s) (A) I only (B) II only (C) III only
(D) II and III only
13. Given these reactions A ? 2B ?H 40 kJ B ?
C ?H -50 kJ 2C ? D ?H -20 kJ Calculate ?H
for the reaction D A ? 4 C. (A) 100 kJ (B)
60 kJ (C) 40 kJ (D) 100 kJ
82
14. An ice cube of unknown mass at 0 C is added
to 265 g of H2O at 25.00C in a calorimeter. If
the final temperature of the resulting H2O is
21.70C, what is the mass of the ice
cube? Properties of Water Cp4.18 J/(g K)
?Hfus 333 J/g (A) 2.47 g (B) 8.63 g (C) 10.3
g (D) 11.0 g
15. Which reaction is spontaneous at all
temperatures at standard pressure and
concentration? (A) exothermic reaction with a
decrease in entropy (B) exothermic reaction with
an increase in entropy (C) endothermic reaction
with a decrease in entropy (D) endothermic
reaction with a increase in entropy
83
16. When 100. mL of 1.0 M HCl is added to a 2.0 g
piece of CaCO3, CO2 is produced at a certain
rate. Which of the changes below will NOT
increase the rate of this reaction? (A) adding
100. mL of 2.0 M HCl in place of 100. mL of 1.0 M
HCl (B) heating the 100. mL of 1.0 M HCl before
adding it to the CaCO3 (C) adding 100. mL of 1.0
M HCl to 2.0 g of powdered CaCO3 (D) adding 150.
mL of 1.0 M HCl in place of 100. mL of 1.0 M HCl
17. If N2H4 (g) disappears at a rate of 0.12
mol/Lmin, at what rate does N2 (g) appear? 2
N2H4 (g) N2O4 (g) ? 3 N2 (g) 4 H2O( g) (A)
0.080 mol/Lmin (B) 0.12 mol/Lmin (C) 0.18
mol/Lmin (D) 0.36 mol/Lmin
84
18. Use the data to determine the orders of A and
B in the reaction A B ? products Experiment
A B Rate 1 0.10 0.10 0.0090 2
0.20 0.10 0.036 3 0.10 0.20
0.018 (A) Rate kAB (B) Rate
kA2B (C) Rate kAB2 (D) Rate
kA2B2
19. An iron catalyst is used in the Haber process
in which gaseous N2 and H2 react to produce NH3.
What is the role of this catalyst? (A) It
provides a pathway with a lower activation
energy. (B) It increases the equilibrium constant
of the reaction. (C) It raises the kinetic
energies of the reactants. (D) It interacts with
the NH3.
85
20. What is the correct equilibrium expression
for this reaction? 2 NO2 (g) 7 H2 (g) ? 2 NH3
(g) 4 H2O (l)
21. The equilibrium reaction shown is endothermic
as written. Which change will increase the amount
of NO2 at equilibrium? N2O4 (g) ? 2 NO2 (g) (A)
adding a catalyst (B) decreasing the
temperature (C) increasing the volume of the
container (D) adding an inert gas to increase the
pressure
86
22. Which weak acid has the strongest conjugate
base? (A) acetic acid (Ka 1.8105) (B) formic
acid (Ka 1.8104) (C) hydrofluoric acid (Ka
6.8104) (D) propanoic acid (Ka 5.5105)
23. What is the pH of a 0.20 M HA solution (Ka
1.0106) that contains 0.40 M NaA? (A) 3.15 (B)
3.35 (C) 5.70 (D) 6.30
24. What is the Mg2 in 0.10 M NaF that is
saturated with MgF2 at 25C? (Ksp of MgF2
6.410-9) (A) 0.050 M (B) 1.910-3 M (C)
1.210-3 M (D) 6.410-7 M
87
25. Which change represents an oxidation? (A)
NO21 ? N2 (B) VO2 ? VO31 (C) ClO1 ? Cl1
(D) CrO42 ? Cr2O72
26. What is the oxidation number of Mo in
MoO2Cl2? (A) 0 (B) 3 (C) 5 (D) 6
27. What is the coefficient for H when the half
equation is balanced with the smallest whole
number coefficients? __ S2 __ H2O ? __SO2
__H1 __e (A) 2 (B) 4 (C) 6 (D) 8
28. Which metal is the most reactive? (A) silver
(B) lead (C) iron (D) cesium
88
29. Which element has the largest first
ionization energy? (A) Li (B) B (C) N (D) Na
30. All of the energy levels listed are allowed
EXCEPT (A) 3f. (B) 4d. (C) 5p. (D) 7s.
31. A sulfur atom has the electron
configuration 1s2 2s2 2p6 3s2 3p4. How many
orbitals in this ground state atom are occupied
by at least one electron? (A) 12 (B) 9 (C) 8
(D) 5
32. The shapes of s and p orbitals are determined
by which quantum number(s)? I. n II. m III.
ml (A) I only (B) II only (C) III only (D) II
and III only
89
33. What are the elements called for which the 4f
subshell is being filled? (A) transition metals
(B) metalloids (C) lanthanides (D) actinides
34. Which ionic compound has the smallest lattice
energy? (A) NaF (B) MgO (C) AlN (D) MgCl2
35. Which species have one or more atoms that
violate the octet rule? I. NO II. SF2 III.
PF41 (A) I only (B) III only (C) I and II
only (D) II and III only
90
36. In which species is the carbon-nitrogen bond
the shortest? (A) CH3NH2 (B) CH2NH (C)
(CH3)4N1 (D) CH3CN
37. In which species is resonance most useful in
explaining the observed bond lengths? (A) NF3
(B) NH41 (C) NO21 (D) NO21
38. Which description best represents the
hybridization of the C1 and C2 atoms? (A) C1 -
sp2, C2 - sp2 (B) C1 - sp3, C2 - sp3 (C) C1 -
sp3, C2 - sp2 (D) C1 - sp2, C2 - sp
91
39. Which subatomic particles are located in the
nucleus of a neon atom? (1) electrons and
positrons (3) protons and neutrons (2) electrons
and neutrons (4) protons and electrons
40. The total mass of the protons in an atom of
gold-198 is approximately (1) 79 amus (3) 198
amus (2) 119 amus (4) 277 amus
41. In a calcium atom in the ground state, the
electrons that possess the least amount of energy
are located in the (1) first electron shell (3)
third electron shell (2) second electron shell
(4) fourth electron shell
42. Which isotopic notation represents an atom of
carbon-14? (1) (2) (3) (4)
92
43. An atom of argon rarely bonds to an atom of
another element because an argon atom has (1) 8
valence electrons (2) 2 electrons in the first
shell (3) 3 electron shells (4) 22 neutrons
44. Solid samples of the element phosphorus can
be white, black, or red in color. The variations
in color are due to different (1) atomic masses
(2) molecular structures (3) ionization
energies (4) nuclear charges
45. Which substance can be decomposed by chemical
means? (1) tungsten (3) krypton (2) antimony
(4) methane
93
46. Given the balanced equation representing the
reaction between propane and oxygen C3H8 5 O2
? 3 CO2 4 H2O According to this equation,
which ratio of oxygen to propane is correct?
47. Lithium and potassium have similar chemical
properties because the atoms of both elements
have the same (1) mass number (2) atomic
number (3) number of electron shells (4) number
of valence electrons
94
48. Which two substances are covalent
compounds? (1) C6H12O6 (s) and KI (s) (2)
C6H12O6 (s) and HCl (g) (3) KI (s) and NaCl (s)
(4) NaCl (s) and HCl (g)
49. Compared to a phosphorus atom, a P3 ion
has (1) more electrons and a larger radius (2)
more electrons and a smaller radius (3) fewer
electrons and a larger radius (4) fewer electrons
and a smaller radius
50. The balanced equation below represents a
molecule of bromine separating into two bromine
atoms. What occurs during this change? Br2 ?
Br Br (1) Energy is absorbed and a bond is
formed. (2) Energy is absorbed and a bond is
broken. (3) Energy is released and a bond is
formed. (4) Energy is released and a bond is
broken.
95
51. Which substance cannot be decomposed by
chemical means? (1) Water (2) gold (3)
salt (4) methane
52. Bronze contains 90 to 95 percent copper and 5
to 10 percent tin. Because these percentages can
vary, bronze is classified as (1) a compound
(2) an element (3) a mixture (4) a
substance
53. Compared to a 2.0 M aqueous solution of NaCl
at 1 atmosphere, a 3.0 M aqueous solution of NaCl
at 1 atmosphere has a (1) lower boiling point and
a higher freezing point (2) lower boiling point
and a lower freezing point (3) higher boiling
point and a higher freezing point (4) higher
boiling point and a lower freezing point
96
54. In which reaction are electrons transferred
from one reactant to another reactant? (1) 2Ca
(s) O2 (g) ? 2CaO (s) (2) AgNO3 (aq) KCl (aq)
? AgCl (s) KNO3 (aq) (3) HCl (aq) NaOH (aq) ?
NaCl (aq) H2O (l) (4) H3O1 (aq) OH1 (aq) ?
2H2O (l)
55. Which statement must be true for any chemical
reaction at equilibrium? (1) The concentration of
the products is greater than the concentration of
the reactants. (2) The concentration of the
products is less than the concentration of the
reactants. (3) The concentration of the products
and the concentration of the reactants are
equal. (4) The concentration of the products and
the concentration of the reactants are constant.
97
56. In terms of energy and entropy, systems in
nature tend to undergo changes toward (1) higher
energy and higher entropy (2) higher energy and
lower entropy (3) lower energy and higher
entropy (4) lower energy and lower entropy
57. Given the structural formula
H-CC-H What is the total number of electrons
shared in the bond between the two carbon
atoms? (1) 6 (2) 2 (3) 3 (4) 4
58. Which compound has hydrogen bonding between
its molecules? (1) CH4 (2) CaH2 (3) KH (4) NH3
98
59. Which ion is the only negative ion produced
by an Arrhenius base in water? (1) NO3-1 (2)
Cl1 (3) OH1 (4) H1
60. When the elements in Group 1 are considered
in order from top to bottom, each successive
element at standard pressure has (1) a higher
melting point and a higher boiling point (2) a
higher melting point and a lower boiling point
(3) a lower melting point and a higher boiling
point (4) a lower melting point and a lower
boiling point
61. The molar mass of Ba(OH)2 is (1) 154.3 g
(2) 155.3 g (3) 171.3 g (4) 308.6 g
99
62. At which temperature would atoms of a He (g)
sample have the greatest average kinetic
energy? (1) 25C (2) 37C (3) 273 K (4) 298 K
63. Given the balanced equation representing a
reaction 4 NH3 5 O2 ? 4 NO 6 H O What is
the minimum number of moles of O2 that are needed
to completely react with 16 moles of NH3? (1) 16
mol (2) 20. mol (3) 64 mol (4) 80. mol
64. A 10.0-gram sample of which element has the
smallest volume at STP? (1) Aluminum (2)
magnesium (3) titanium (4) zinc

• 65. At room temperature, a mixture of sand and
  water can be separated by
• Ionization (2) combustion
• (3) filtration (4) sublimation