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Honors Chemistry
Final Exam Review
PROPERTIES OF MATTER
1.
A unit defined by a physical standard is
(a) Fundamental
(b) derived
(c) Metric
(d) British
(d) mass
2.
The metric prefix representing the factor 10 is
(a) deci
(b) k
(c) milli (d) da.
3.
The expression 100 milliliters represent
(a) Number
(b) quantity
(c) length
In the expression 100 grams, grams is the
(a) Number
(b) quantity
(c) unit
4.
5.
Chemistry is the study of
a. electrons and protons
b. the production of new substances
(d) abbreviation
c. explosives
d. the properties, structure, and changes of matter
6.
Chemistry is the study of
a. plants and animals, their origins, history, and physical characteristics
b. matter, its properties and composition, and the changes that matter undergoes
c. energy and its transformation from one form to another
d. the structure of the earth’s crust and the formation and development of its various layers.
7.
The general way or ways in which scientists go about solving a problem is often refereed to as
a. trial and error learning
c. the scientific method
b. hypothesizing procedures
d. scientific technology
8.
A scientific guess, based on observed facts, is called
a. an experiment
b. a law
c. a theory
9.
10.
11.
12.
The three phases of matter are
a. solid, solution, and gas
b. solid, solution, and liquid
Ice, water and steam are
a. made up of different elements
b. are chemically different
d. an hypothesis
c. solid, liquid, and gas
d. gas, solution, and liquid
c. have different percentage composition
d. are different phases of the same compound
Condensation refers to a phase change from
a. solid to liquid
b. liquid to solid
Chemical properties
a. include changes of state of a substance
b. include mass and color
c. liquid to gas
d. gas to liquid
c. have to do with change that alters the identity of a substance
d. can be observed without altering the identity of the substance
13.
All of the following are physical properties of gold except
a. shininess or luster
c. dissolves in strong acids
b. conducts electricity
d. has the ability to be hammered into thin sheets
14.
All of the following could be considered physical properties of copper except
a. reacts with air to produce copper(I) oxide c. has a density of 8.8 g/mL
b. has a yellow-bronze color
d. conducts electricity.
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Honors Chemistry
Final Exam Review
15.
Physical changes differ from chemical changes in that physical changes result in
a. formation of precipitate
c. formation of gas
b. identity of materials does not changes
d. change in color and texture of the substances
16.
Among the following, the process which describes a chemical change is
a. heat water to boiling
c. dissolve iodine in alcohol
b. burn wood in air
d. detect an odor
17.
The burning of hydrogen is a chemical change, because
a. a gas changes to liquid
c. heat is produced with production of flame
b. a change in volume occurs
d. a new substance with different properties is produced
18.
Which formula represents a mixture?
a. NH3(aq)
b. NH3(l)
c. NH3(g)
Note: (g) means gas; (l) = liquid; (s) = solid (aq)= aqueous or in water
19.
Which is the formula of a compound?
a. C
b. Cl2
c. HF
d. NH3(s)
d. N2
20.
The energy required to change a unit mass of a solid to a liquid at constant temperature is called its heat of
a. sublimation
b. condensation
c. vaporization
d. fusion
21.
Which substance has a definite shape and a definite volume at STP (standard temperature (273K, and pressure (1 atm)?
a. NaCl (aq)
b. Cl2(g)
c. CCl4(l)
d. AlCl3(s)
22.
The temperature at which a substance in the liquid state freezes is the same as the temperature at which the substance
a. melts
b. sublimes
c. boils
d. condenses
23.
Which may be heterogeneous?
a. a substance
b. an element
24.
25.
26.
27.
c. a compound
d. a mixture
In what type of reaction is heat being released during the reaction?
a. endothermic
b. exothermic
c. spontaneous
Which is not a form of energy
a. light
b. electricity
c. temperature
d. combustion
d. heat
Which change of phase is exothermic?
a. gas to liquid
b. solid to liquid
c. solid to gas
d. liquid to gas
Which change of phase represent sublimation?
a. solid to liquid
b. solid to gas
c. liquid to gas
d. liquid to solid
28.
A cube has a volume of 8.0 cm3 and a mass of 21.6 grams. The density of the cube, in grams per cubic centimeters, is best
expressed as
a. 2.7
b. 2.70
c. 0.37
d. 0.370
29.
Which is characteristic of a compound?
a. It consists of single element.
b. It is homogenous
30.
c. Its chemical composition can be varied.
d. It can be decomposed by a physical change.
The amount of mass per unit volume refers to the
a. density
b. specific weight
c. volume
d. weight
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Honors Chemistry
Final Exam Review
31.
Which of the following is a physical property of sugar?
a. Its composition is carbon, hydrogen, and oxygen.
b. It turns black with concentrated sulfuric acid.
c. It can be decomposed with heat.
d. It is a white crystalline solid.
32.
A substance that can be farther simplified may be either
a. an element or a compound
c. a mixture or a compound
b. an element or a mixture
d. a mixture or an atom.
33.
A substance composed of two or more elements chemically combined is called
a. an isotope
b. a compound
c. an element
34.
An example of a chemical change is the
a. breaking of a glass bottle
b. rusting of iron
d. a mixture
c. sawing a piece of wood
d. melting of an ice cube
35.
A substance which cannot be farther decomposed by ordinary chemical means is
a. water
b. air
c. sugar
d. silver
36.
An example of a physical change is the
a. fermenting of sugar to alcohol
b. burning of paper
c. rusting of iron
d. dissolving sugar in water
37.
Chemical action may involve one of the following except:
a. combining of atoms of elements to form a molecule
b. separation of the molecules in a mixture
c. breaking down compounds into elements
d. reacting a compound and an element to form a new compound and a new element.
38.
The energy of a system can be
a. easily changed to mass
b. transformed into a different form
39.
40.
41.
42.
43.
c. measured only as potential energy
d. measured only as kinetic energy
Which of the following is classified as a diatomic element?
a. water
b. milk
c. chlorine
d. ozone
In this reaction XClO3 + A -------> XCl + O2
a. X
b. XClO3
c. A
d. XCl
+ A
which substance is the catalyst?
e . O2
How many calcium, Ca, atoms are represented in the formula Ca3(PO4)2?
a. 5
b. 8
c. 9
d. 12
The correct formula for calcium hydrogen carbonate is
a. CaHCO3
b. Ca2HCO3
c. Ca(HCO3)2
d. Ca2(HCO3)3
e. 3
e. Ca2 (HCO3)2
Which of the following involves a physical change?
a. The formation of HCl and H2 from H2 and Cl2
b. The color change when NO is exposed to air
c. The formation of steam from burning H2 and O2
d. The solidification of corn oil at low temperatures
e. the odor of NH3 when NH4Cl is rubbed together with Ca(OH)2 powder?
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Honors Chemistry
Final Exam Review
44
The Law of Definite Composition is based on definite composition by
a. mass
b. volume
c. density
d. specific mass
e. freezing point and boiling point
45.
Which of the following atoms normally forms monatomic molecules?
a. Cl
b. H
c. N
d. He
46.
How many total atoms are present in the formula KAl(SO4)2?
a. 7
b. 9
c. 11
d. 12
47.
48.
49.
50.
Which of the following is not a compound?
a. copper sulfate
b. carbon dioxide
e. 13
c. sugar
The simplest unit of water that retains its property is called
a. an atom
b. an element
c. a proton
d. air
d. a hydroxide
The number of atoms of nitrogen represented in the formula NH4NO3 is
a. 1
b. 2
c. 3
4. 4
5.
e. lime
e. a molecule
5
A Ca (+2) ion differs from a Ca atom in that the Ca ion has
a. more protons
c. more electron
b. fewer protons
d. fewer electrons
ATOMIC STRUCTURE
51.
What is the total number of nucleons (protons and neutrons) in an atom of selenium ( at. # = 34; at. Mass = 79)
a. 34
b. 45
c. 79
d. 113
52.
Isotopes of an element have a different
a. number of electrons
c. number of protons
b. atomic number
d. mass number
53.
A neutral oxygen atom, O, differs from an oxide ion in that the atom has
a. more electrons
c. more protons
b. fewer electrons
d. fewer protons
54.
What is the total number of neutrons in an atom of K, whose mass is 39, and atomic number is 19?
a. 19
b. 39
c. 20
d. 58
55.
The amount of hydrogen chloride that the formula HCl represents is one
a. atom
b. gram
c. liter
d. molecule
56.
The mass number of an atom is equal to the total number of its
a. electrons only
c. protons only
b. electrons and protons
d. protons and neutrons
57.
The number of protons in an atom of Cl - 36 is
a. 17
b. 35
c. 18
58.
d. 36
When a chlorine atom reacts with a sodium atom to form an ion, the chlorine atom will
a. lose one electron
c. lose two electrons
b. gain one electron
d. gain two electrons
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Honors Chemistry
59.
60.
61.
The nucleus of a fluorine atom has a charge of
a. 1+
b. 19+
c. 9+
Final Exam Review
d. 0
The correct formula for aluminum sulfate is
a. Al2S3
b. Al2(SO4)3
c. Al3S2
d. Al3(SO4)2
The correct formula for nickel (III) sulfate is
a. Ni2S3
b. Ni2(SO4)3
c. Ni3S2
d. Ni3(SO4)2
62.
What is the total number of neutrons in an atom of fluorine, whose atomic number is 9 and whose mass is 19?
a. 9
b. 19
c. 10
d. 28
63.
Which particle has exactly a mass of approximately 1 mass unit and a unit positive charge?
a. neutron
b. electron
c. proton
d. alpha particle
64.
What is the total number of electrons in a magnesium (+2) ion?
a. 10
b. 12
c. 2
d. 24
65.
Which species has a negative charge?
a. a lithium ion
b. an aluminum ion
66.
Which particle is electrically neutral?
a. proton
b. positron
c. an electron
c. neutron
d. a sodium atom
d. electron
67.
An atom that contains 35 protons, 45 neutrons, and 35 electrons has an atomic number of
a. 35
b. 45
c. 80
d. 115
68.
Two isotopes of the same element will have the same number of
a. neutrons and electrons
c. neutrons and nucleons
b. protons and nucleons
d. protons and electrons
69,
Which sample contains the same number of atoms as 24 grams of carbon?
a. 80. g Ar
b . 1 0 . g He
c. 2 4 g M g
d . 4 . 0 g He
70.
How many neutrons are in the nucleus of an atom that has an atomic number of 17 and mass number of 35?
a. 17
b. 18
c. 35
d. 52
71.
Isotopes are atoms which have different
a. atomic masses
b. atomic numbers
c. atomic radii
72.
What is the total charge on anion that contains 10 electrons, 13 protons, and 15 neutrons?
a. -1
b. +1
c. -3
d. +3
73.
The element whose properties are most similar to those of tellurium is
a. Be
b. O
c. S
d. Po
74.
How many electrons are in a neutral atom of Li-7?
a. 4
b. 7
c. 10
d. number of electrons
d. 3
75.
The number of protons in the nucleus of carbon-13 is
a. 19
b. 13
c. 7
d. 6
76
The mass number of an atom is equal to the total number of its
a. electrons, only
c. protons, only
b. electrons and protons
d. protons and neutrons
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Honors Chemistry
77.
78.
79.
80.
81.
Which pair of atoms are isotopes?
a. C-14 and N-14
b. K - 40 and Ar - 40
c. Ra-222 and Rn - 222
d. K-40 and K-42
Which pair of nuclei contain the same number of neutrons?
a. Li-7 and Be-9
b. K - 40 and Ar - 40
c. Na -23 and Na - 22
d. Na - 23 and Mg -24
An atomic mass unit is equal to
a. the mass of a hydrogen atom
b. the mass of a C-12 atom
1
1
H
85.
b.
2
1
H
c.
The number of protons in an atom of
b. 18
4
2
35
17
He
d.
3
2
He
Cl is
c. 35
d. 36
Which nucleus contains a total of 2 protons and 1 neutron?
a.
84.
d. protons and neutrons
Which atom has a mass of approximately two atomic mass units?
a. 17
83.
c. 1/1836 the mass of hydrogen atom
d. 1/12 the mass of a C-12 atom
The mass number of an atom is equal to the total number of its
a. electrons, only
b. protons, only
c. electrons and protons
a.
82.
Final Exam Review
1
1
H
b.
2
1
H
What is the mass number of a
a. 1
b. 2
c.
2
1
4
2
He
H atom?
c. 3
d.
3
2
He
d. 4
The neutral atoms in as given sample of an element could have different
a. mass number
b. number of protons
c. atomic numbers
d. number of electrons
86.
The accepted value for the boiling point of a substance is 120 oC. A student performs an experiment and reports the
boiling point to be 110 oC. The percent error of the student’s observation is
a. 83%
b. 120%
c. 20 %
d. 80%
e. 8.0%
87
Which of the following does not have a net charge?
a. a proton
b. a neutron
c. an electron
d. an ion
e. the nucleus
88.
What is the total number of subatomic particles in an atom having an atomic number of 17 and atomic mass of 35?
a. 17
b. 18
c. 34
d. 35
e. 52
89.
Which of the following is not part of Dalton’s Atomic Theory?
a. Atoms of a given element have the same mass.
b. All elements are made of indivisible, indestructible atoms.
c. Atoms of one element can be converted into a different element.
d. Compounds are the result of the combination of atoms of different elements.
e. All atoms of a given element are identical.
90.
The term nucleon refers to
a. protons, only
b. neutrons, only
d. both protons and neutrons
91.
c. electrons, only
e. both protons and electrons
What is the net charge on an atom with 20 protons, 20 neutrons, and 18 electrons?
a. 0
b. 2+
c. 2d. 18e. 20+
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Honors Chemistry
Final Exam Review
92
A Ca+2 ion differs from a Ca atom in that the Ca+2 ion has
a. more protons
b. fewer protons
c. more electrons d. fewer electrons
93.
At the end of 12 days, ¼ of an original sample of a radioactive element remains. What is the half-life of the element.
a. 24 days
b. 48 days
c. 3 days
d. 6 days
94.
What is the total number of nucleons (protons and neutrons) in an atom of selenium ( atomic number = 34, atomic mass =
79)
a. 34
b. 45
c. 79
d. 113
95.
When a chlorine atom reacts with a sodium atom to form an ion, the chlorine atom will
a. lose one electron
b. lose two electrons
c. gains one electron
d. gain two electrons
96.
As a substance changes from a liquid to a gas, the average distance between the molecules
a. decreases
b. increases
c. remains the same
97.
The correct formula for sodium nitrate is
a. NaNO3
b. NaNO2
c. Nal2(NO3)3
d. Na3(NO3)2
98.
Which particle has a mass of approximately 1 mass unit and a unit positive charge?
a. neutron
b. proton
c. electron
d. alpha particle
99.
When a radioactive nucleus emits a beta particle (a negatively charged particle) , the atom’s
a. mass number is increased by 1
c. atomic number is increased by 1
b. mass number is decreased by 1
d. atomic number is decreases by 1
100.
The structure of an alpha particle is the same as a
a. lithium atom
b. neon atom
c. hydrogen nucleus
d. helium nucleus
101.
What is the total number of electrons in a magnesium (+2) ion?
a. 10
b. 2
c. 12
d. 24
102.
Which species has a negative charge?
a. a lithium ion
b. an alpha particle
c. an aluminum ion
c. a beta particle
An electron has a charge identical to that of
a. a neutron
b. a proton
c. an alpha particle
d. a beta particle
103.
104.
Two isotopes of the same element will have the same number of
a. neutrons and electrons
c. protons and nucleons
b. neutrons and nucleons
d. protons and electrons
105.
How many neutrons are in the nucleus of an atom that has an atomic number of 27 and a mass number
a. 17
b. 35
c. 8
d. 52
106.
Isotopes are atoms which have different
a. atomic masses
b. atomic numbers
107.
c. atomic radii
of 35?
d. electron configuration
What is the total charge on anion that contains 10 electrons, 11 protons, and 15 neutrons?
a. -1
b. +1
c. -3
d. +3
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Honors Chemistry
Final Exam Review
108.
In the Bohr model of the hydrogen atom, what is the value of n in the ground state?
109.
Give the total capacity for electrons of the principal energy level for which
a. n= 1
b. n=2
c. n=3
d. n=4
110.
Which has higher energy, an electron in the
a. 1st or 2nd energy level?
b. 1s or 2s sublevel?
c. 2s or 2p sublevel?
d. 3d or 4d sublevel?
111.
What is the highest energy sublevel in the principal energy level for which n is
a. 1
b. 2
c. 3
d. 4
112.
What is the capacity for electrons in each of the following sublevels?
a. s
b. p
c. d
d. f
113.
What is the total capacity for electrons in
a. an orbital
b. an s sublevel
d. the 1st principal energy level
c. a p orbital
e. the 3rd principal energy level?
Which of the following sublevels do not exist?
a. 2 p
b. 1p
c. 2 d
d. 3d
114.
e. n=5
e. 3 f
115.
Arrange the following sublevels in order of increasing energy:
1s, 3p, 2s, 2p, 3s
116.
In the third principal energy level, what is the total electron capacity?
How many different sublevels are in this level?
List them in order of increasing energy.
117.
How many orbitals are there in the following sublevels?
a. s
b. p
c. d
d. f
118.
What is the total number of orbitals in the principal energy level for which n is:
a. 1
b. 2
c. 3
d. 4
119.
Give the outer electron configuration of the elements in the following groups of the Periodic Table:
a. 3
b. 5
c. 1 7
d. 18
e. 1 3
f. 8
Example: Group 2 ns2
120.
Which group in the Periodic Table has the outer configuration:
a. ns2
b. ns2np2
c ns2np5
121.
Give the total number of outermost level electrons (valence electrons) of an element in Group
a. 1
b. 13
c. 14
d. 16
e. 17
122.
In what group of the Periodic Table do all the elements have:
a. 2 valence electrons
b. 5 valence electrons
c. 6 valence electrons?
Write the electron configuration of
a. B
b . Ne
c. Al
e. Ca
123
124.
d. Cl
Identify the elements which have the following outer electron configuration:
a. 3s23p3
b. 4s1
c. 6s26p5
d. 5s25p4
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Honors Chemistry
125.
Final Exam Review
Determine the atomic number of the element in which there is (are):
a. a singe 2s electron
b. two 2p electrons
d. an equal number of 4s and 3d electrons
c. five 3d and two 4s electrons
126.
In a certain atom, the first and second principal energy levels are completely filled, as is the 3s sublevel. There are three
electrons in the 3p sublevel.
a. How many electrons are there in the atom?
b. Give the electron configuration of the atom.
c. What is the element’s symbol?
127.
Give the number of electrons in each of the 3p orbitals in each of the following elements:
a. Al
b. Br
c. Ca
d. O
e. Ar
f. Ti
g. Fe
h. Sb
I . Ge
j. C
PERIODIC TABLE:
128.
How many groups are in the periodic table? ______________ How many periods? ____________
129.
Define atomic number _____________________ What information does it convey? _____________
130.
What is mass number ? _____________________________________________________________
131.
What number, other than atomic number is represented for every element in the periodic table?____
132.
How many elements are in period 1_____________? 2? __________ 3? ____________ 4? _____
133.
In which group are the noble gases found? __________________________________
134.
Why are the noble gases special? _____________________________________________________
135.
In how many groups are the s-sublevels filled? ________ p-sublevels filled? __________________
d-sublevels filled? ________________ f-sublevels filled? ____________________________
136.
What block in the periodic table contains the transition elements? _______
The rare earth elements (lanthanoids and actinoids)? _____________
137.
What do the elements in a group have in common? _______________________________________
138.
What is an ion? ___________________________________________________________________
139.
How does an atom form an ion?________________________________________________________
140.
How does an atom form a cation?______________________________________________________
141.
How does and atom form an anion?____________________________________________________
142.
Which groups form cations? _________________________________
143.
Which groups form anions? _________________________________
144.
Draw the outermost energy electron diagrams (Lewis Structures) for elements in groups 1, 2, 13, 17, and 18.
145.
What is the charge on the ions formed by elements in groups 1, 2, 17, and 18. ( Indicate + or - as well as magnitude of the
charge)
146
For each of the following pairs, use the periodic table to select the atom that is larger in radius.
a. Rb, Sr
b. Cl, I
c. Na, Rb
d. Mg, Be
f. Ac, U
g. B, Al
h. Au, Ba
e. S, P
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Honors Chemistry
Final Exam Review
147.
How many electrons are lost or gained to complete the outer octet and produce the following ions?
a. K+1
b. O-2
c. Ga+3
d. P3e. Sn4+
12+
3+
f. Br
g. Ca
h. Sc
148.
Which atom in each of the following pairs would have the lower first ionization energy?
a . N, O
b. Te, Sn
c . Ne , F
d. C, Ge
e. B r , I
f. Mg, Ca
g. I, Sb
h. Al, N
I. F, S
149.
Within a group, do the radii of atoms increase or decrease as the atomic number increases?
150.
Does the radii of atoms within a period increase or decrease as the atomic number increases?
151.
In each of the following pairs of atoms, pick the one that is larger.
a. Mg, Na
b. K, Ca
c. Al, B
e. F, N
f. Ne, Ar
d. Br, Cl
152.
In a group, will the ionization energy tend to increase or decrease with increasing atomic number?
153.
In a period, will the ionization energy tend to increase or decrease with increasing atomic number?
PROPERTIES OF METALS AND NONMETALS
154.
Compare the following in terms of:
METALS
NONMETALS
Ionization Energy
Electronegativity
Luster
Deformability(Malleability, Ductittility)
Conductivity of Heat
Conductivity of Electricity
Phase at Room Temperature
Ion Formation (Positive or Negative)
Number of Electrons in outermost Energy Level
10
Honors Chemistry
Final Exam Review
Problems and Essays: Set #1
Solve the following problems using Factor Label Method.
1.
In a primitive barter society the following rates of exchange exist: 1 fot = 5 vum, 2 sop = 3 tuz, 4 bef = 3 tuz,
and 9 fot = 2 bef. A man has 4 sop and wants to convert all his possessions into vum. How mnay vum can he
trade for?
2.
The food that the average American consumes in a day provides 2.0 x 103 kcal of energy. How many
calories/sec is this?
3.
A cheetah has been clocked at 112 km/hr over a 100-m distance. What is this speed in m/s?
4.
How many micrometers is 0.073 cm?
5.
How many seconds are in one day?
Solve the following problems using any method of your choice.
6.
What is the density of a cough syrup medication if 53.623 cm3 of the syrup has a mass of 50.0g?
7.
A small piece of gold has a volume of 0.87 cm3.
a. What is the mass if the density of gold is 19.3 g/cm3?
b. What is the value of this piece of gold if the market value of gold is $12 per gram?
8.
The density of silicon is 2.33 g/cm3. What is the volume of a piece of silicon that weighs 62.9 g?
9.
Nitrogen-13 emits beta radiation and decays to carbon-13 with a half-life of 10 minutes. Assume a starting
mass of 2.0 g of nitrogen-13. How many grams of that isotope will remain after four half lives?
10.
A patient is administered 20 mg of iodine-131. How much of this isotope will remain in the body after 40
days if the half-life of iodine-131 is 8 days?
11.
The mass of cobalt-60 in a sample is found to have decreased from 0.8 g to 0.2 g in a period of 10.5 years.
From this information, calculate the half-life of cobalt-60.
12.
Complete and balance the equations for the following nuclear reactions:
a.
27
13 Al
b.
214
83
+
2
4
He →
4
2
Bi →
27
14 Si
→
0
1 e
d.
66
29 Cu
→
66
30
e.
9
4
4
2
+ ?
He + ?
c.
Be +
30
14 Si
+ ?
Zn + ?
He →
12
6C
+ ?
11
Honors Chemistry
13.
Final Exam Review
Write formulas for the following compounds:
a.
b.
c.
d.
e.
f.
g.
h.
i
j.
potassium nitride______________
magnesium sulfate______________
cobalt(III) oxide______________
calcium carbonate______________
sodium phosphate______________
potassium fluoride______________
zinc hydrogen carbonate______________
barium nitrate______________
ammonium hydroxide______________
dinitrogen pentoxide______________
k. dichloro heptoxide______________
l. copper(II) bromide______________
m. nitrogen monoxide______________
n. carbon monoxide______________
o. dihydrogen monoxide______________
p. gold(I) sulfide______________
q. dihydrogen dioxide______________
r. nickel(II) phosphate ______________
s. diphosphorus pentoxide______________
t. sodium oxide______________
Balance each of the following equations:
14.
15.
16
17.
18.
19.
20.
21.
22.
23.
24.
25.
_____Cl2 + _____KI  _____ KCl
+
_____I2
_____HNO3
+ _____ LiOH  _____ H2O + _____ LiNO3
_____HCl + _____K2CO3  _____ KCl + _____ H2O + _____CO2
_____NaCl + _____ H2SO4  _____ Na2SO4 + _____HCl
_____Al +
_____ CuSO4  _____Al2(SO4)3 + _____Cu
_____P
+ _____ O2 
_____P2O5
_____Pb(NO3)2
+ _____K2CrO4 
_____PbCrO4 + _____ KNO3
_____C3H6
+ _____O2  _____CO2
+ _____ H2O
_____Zn(OH)2
+ _____H3PO4 
_____Zn3(PO4)2 + _____ H2O
_____CO + _____ Fe2O3  _____ Fe + _____CO2
_____Ca(ClO3)2  _____ CaCl2 + _____O2
_____Na2SO3 + _____ HCl
 _____ NaCl + _____ H2O + _____ SO2
ESSAYS:
1.
2.
Devise a way to separate sand from a mixture of charcoal, sand, sugar, and water.
How do you know that each of the following is a chemical change?
a. Food spoils.
b. A foaming antacid tablet fizzes in water.
c. A ring of scum forms around your bathtub.
d. Iron rusts.
e. A firecracker explodes.
3.
When a small amount of a red powder is heated, it darkens and then changes into a shiny, silvery liquid. Is the
red powder a compound, an element, or a mixture/ Explain. Can you classify the shiny liquid with certainty?
Explain.
4.
Astronauts in space are weightless. Explain why it is incorrect to say that they are massless.
5.
Compare and contrast the properties of the three subatomic particles that are found in the nucleus.
6.
State the main ideas of Dalton’s atomic theory.
12
Honors Chemistry
Final Exam Review
7.
How are the three isotopes of hydrogen alike? How are they different?
8.
What parts of Dalton’s atomic theory no longer agree with our current picture of the atom?
9.
How do you test for the presence of
a. oxygen?
b. hydrogen?
c. carbon dioxide?
10.
Compare and contrast physical change and chemical change. Give at least two to three examples for each.
11.
What criterion did Mendeleyev use in arranging his periodic table? What criterion was used in constructing
the modern periodic table?
12.
How do the terms group and period relate to the periodic table?
13.
How is a representative (main group) element’s outer electron configuration related to its position in the
periodic table?
14.
Explain why atoms form chemical bonds and describe the difference between an ionic and covalent bond.
15.
Why is the possible to bend metals but not ionic crystals?
16.
Explain briefly why metals are good conductors of electricity.
17.
Describe the process of nuclear fission.
Problem Set #1: Answers
1)180 vum
6) 0.950 g/cm3
11) 5.25 years
2) 2.3 x 101 cal/sec
7) 17 g, $204
12) a.
1
1 H,
b.
210
81 Tl,
4) 7.3 x 102 μm
9) 0.125 g
3) 31 m/s
8) 27.0 cm3
c.
27
15 P,
d.
0
1
e, e.
5) 86 400 seconds
10) 6.3 x 10-1 mg
1
0n
13. a. K3N, b. MgSO4, c. Co2O3, d. CaCO3, e. Na3PO4, f. KF, g Zn(HCO3)2, h. Ba(NO3)2, i. NH4OH
j. N2O5, k. Cl2O7, l. CuBr2, m. NO, n. CO, o. H2O, p. Au2S, q. H2O2, r. Ni3(SO4)3, s. P2O5, t. Na2O
Problem Set #2:
1.
(a) 15.0 g of solid has a volume of 2.5 cm 3. What is its density?
(b) 67.2 L of SO2(g) at STP has what mass?
( c) what is the density of CO2(g) at STP?
15.0 g of NaOH = ? moles
2.5 moles of FeCl3 = ? g
33.6 L of NH3(g) at STP = ? moles
11.2 L of H2(g) = ? grams
3.
a) What is the % of oxygen in NaClO3
b) What is the % of N in Ca(NO3)2
13
Honors Chemistry
4.
5.
6.
7.
What is the molecular formula of :
(a) Molar mass 160
(b) molar mass 229
Fe 70.0 %
P = 26.6 %
O 30.0%
Mg = 31.4%
O = 42.0 %
(c) molar mass 146
Cd = 22.4 g
O = 6.4 g
H = 0.4 g
Name the following or write the formula for the following:
KOH
__________________
tin(IV) chlorate
CuSO4 __________________
zinc hydroxide
Fe2S3
__________________
ammonium phosphate
NiCO3 __________________
sodium oxide
Pb(NO3)2 __________________
magnesium bromide
__________________
__________________
__________________
__________________
__________________
What is the oxidation state of underlined atom?
K2Cr2O7
H2SO4
LiClO4
Fe(NO3)3
Balance the following
1.
2.
3.
4.
5.
6.
Al + NaOH → Na3AlO3 + H2
Ca3(PO4)2 + H2SO4 → CaSO4 + H3PO4
HCl + Ca(ClO)2 → CaCl2 + Cl2 + H2O
K + H2O → KOH + H2
Fe2O3 + C → Fe3O4 + CO2
C4H10 + O2 → CO2 + H2O
7.
238
92
8.
90
38
9.
235
92
10.
8.
Final Exam Review
2
2
He
Sr → _____ +
0
1
U → ____ +
U + 01 n →
248
98
Cf
+
12
6
143
56
C →
e
Ba +
1
0
90
36
Kr + ______
n + ______-
(a) 5.0 L of SO2(g) at 27 ºC and 760 mm Hg is what volume at 23 ºC and 1520 mm Hg?
(b) What pressure is needed to hold 22.0 g of CO2(g) in 4.0 L at 27 ºC?
( c) 3.4 g NH3 has what volume at STP?
(d) What is the comparative rate of diffusion between CO2 and O2?
9.
Note: balance the equation before proceeding to solve the problems.
(a) How many moles of O2 are needed to burn 112 g of CO into CO2?
CO + O2 → CO2
(b) How many grams of HCl will be produced from 7.1 g of Cl2?
C10H16 + Cl2 → C + HCl
( c) How many liters of NH3 are needed to make 72 g H2O at STP?
NH3 + O2 → NO + H2O
(d) How many liters of O2 are needed to burn 40.0 L of C2H6(g) at STP?
(e) How many grams of N2 can be made from 3.4 g NH3 and 6.4 g O2?
14
Honors Chemistry
Final Exam Review
4NH3(g) + O2(g) → 2N2(g) + 6H2O(l)
10.
(a) How many calories are needed to raise the temperature of 25 g of H2O from 20.0 ºC to 65.0 ºC?
(b) 0.50 g of C2H6 burns in a calorimeter. 200.0 g of water changes from 20.0 ºC to 57.0 ºC. What is the
molar heat of combustion?
( c) 10.0 g of ice is placed in H2O. How many calories of heat will it gain to become 10.0 g of H2O(l) at 0.0
ºC?
11.
What is net ionic equation (Balance equations first)?
(a) Ag+(aq) + NO3- (aq) + Ca+2(aq) + Cl- (aq) → AgCl(s) + Ca+2(aq) + NO3- (aq)
(b) KOH (s) + 2H+1 (aq) + SO4-2(aq) → H2O(l) + K+1(aq) + SO4-2 (aq)
12.
(a) What is the molarity of 10.0 g NaOH in 250 ml solution?
(b) How many grams of AgNO3 are needed to make 6.0 L of 2.0 M solution?
*( c) What is the mole fraction of 50.0 g of CCl4 in 50.0 g of C6H6?
(d) 40.0 g of CH3OH in 200.0 g of H2O has what freezing point? Kf = 1.86 ºC/mol/kg; FP pure water = 0.0 ºC.
13.
(a) 0.001 M HCl = ? pH
0.0001 M HCl = ? pH
0.01 M NaOH = ? pH
pH = 1 [H+] = ?
0.1 M NaOH = ? pH
pH = 10 [OH-] = ?
(b) How many ml of 2M HCl are needed to neutralize 60.0 mL of 0.5 M NaOH?
*( c) 0.1 M C2H3O2 ( acetic acid) ionizes 1.34 %. What is the Ka? 0.2 M does the same. Calculate the Ka.
(d) What is the molarity of Ag+1(aq) dissolved if the Ksp of AgCl = 1.2 x 10-10? AgCl → Ag+(aq) + Cl-(aq)
(e) the concentration of Ca+2(aq) = 6.9 x 10-5 mol/L. What is the Ksp?
CaCO3(s) ↔ Ca+2(aq) + CO3-2 (aq)
ANSWERS TO THE PROBLEM SETS:
1a) 6.9 g/cm3
b) 192 g
2. 0.375 mol NaOH
406.3 g FeCl3
c) 1.96 g/L
1.5 mol NH3
2 grams He
3. 45 % NaClO3 17 % Ca(NO3)2
4a) Fe2O3
5.
6.
7.
b) Cd(OH)2
Potassium hydroxide
Sn(ClO3)4
copper(II) sulfate
Zn(OH)2
iron(III) sulfide
(NH4)PO4
nickel (II) carbonate
Na2O
lead (II) nitrate
MgBr2
Cr: +6
S: +6
Cl: +7
N: +5
1) 2, 6, 2, 3
2) 1, 3, 3, 2
3) 4, 1, 1, 2
5) 6, 1, 4, 1
6) 2, 9, 8, 10
7)
10)
236
90
Th
4) 2, 2, 2, 1
8)
90
39
Y
1
9) 2 0 n
259
104
Unp
15
Honors Chemistry
Final Exam Review
8. a) 2.5 l
b)
c) 4.5 l
d) 1.25
9. a) 2 mol O2
b) 16.7 g HCl
c) 59.7 L NH3
d) 140 L O2
e) 2.8 g N2
10. Omit
11. a) Ag+(aq) + Cl- (aq) → AgCl(s)
12. a) 1.0 M
b) 2028 g
13. a) pH = 3
pH = 12 [H+] =
b) 15 mL
c) omit
10-1
c) omit
d) 11.635 ºC
M
d) 1.09 x 10-5 M
e) Ksp = 4.76 x 10-9
Multiple Choice: Answers:
1-a
2-d
3-b
4-c
5-d
6-b
7-c
8-d
9-c
10-d
11-d
12-c
13-c
14-a
15-b
16-b
17-d
18-a
19-c
20-d
21-d
22-a
23-d
24-b
25-c
26-a
27-b
28-b
29-b
30-a
31-d
32-c
33-b
34-b
35-d
36-d
37-b
38-b
39-c
40-c
41-e
42-c
43-d
44-a
45-d
46-d
47-d
48-e
49-b
50-d
51-c
52-d
53-b
54-c
55-d
56-d
57-a
58-b
59-c
60-b
61-b
62-c
63-c
64-a
65-c
66-c
67-a
68-d
69-a
70b
71-a
72-d
73-d
74-d
75-d
76-d
77-d
78-d
79-d
80-c
81-b
82-a
83-d
84-b
85-a
86-e
87-b
88-b
89-c
90-d
91-b
92-d
93-d
94-c
95-c
96-b
97-a
98-b
99-c
100-d
101-a
102-c
103-d
104-d
105-c
106-a
107-b
108 - 1 109:a-2; b—8; c-18; d-32; e-50
110:a- 2nd; b- 2s; c- 2p; d-4d
111:a-s; b-p; c-d; d-f
112:a-2; b-6; c-10; d-14
113:a-2; b- s; c-6; d-2; e-18
116: a- 3; 3s, 3p, 3d
117: a-1; b-3; c-5; d-7; 118: a- 1; b—4; c-9; d-16
119: c – ns2np5; d- ns2np6; e- ns2np1;
122: a-2; b- 15; c-16
120: a-2; b-14; c- 17
124: a- Al; b- K; c- At; d- Te
126: a-15; b- 1s22s22p63s23p3; c- P
127: a-1; b-6; c- 6; d-0; e- 6; f- 6; g-6; h-6; I-6; j- 0; 128: 8, 7
131- atomic mass
115- 1s, 2s, 2p, 3s, 3p
121: a-1; b-3; c-4; d-6; e-7
123:
125:a-Li; b- C; c- Mn; d- Ti
130: p+n
114: b, c, e;
129: # of p; charge and # of p
132: period 1-2; period 2-8; period 3-8; period 4-18
133-18
134: complete outermost energy level and very stable;
135: s sublevel: group 1, and 2; p-sublevel – groups 13-18
137- same number of valence electrons
136-d
138 – charged particle
139-losing or gaining electrons
140- by losing electrons
141- by gaining electrons
142: groups 1-12 (metals)
143 – nonmetals in groups 15-17
16
Honors Chemistry
145: +1; +2, -1; 0
Final Exam Review
146: a- Rb; b- I; c- Rb; d- Mg; e- P; f- Ac; g- Al; h- Ba
147: a-lost 1; b- gained 2; c- lost 3; d- gained 3; e- lost 4; f- gained 1; g- lost 2; h- lost 3
148: a-N; b- Sn; c- F; d- Ge; e- I; f- Ca; g- Sb; h- Al 149- increase
150-decrease
151: a- Na; b- K; c- Al; d- Br; e- N; f- Ar
153 – decrease
152- decrease
17