Download How to Make a Collage

Ms. Brasington [email protected]
Welcome to AP Chemistry! AP Chemistry is probably the most difficult AP course offered in
high school. By signing up for this class, you are agreeing to (1) have a solid work ethic, (2) put in
1 – 2 hours per day on chemistry outside of the classroom, (3) have a secure working knowledge base
of general chemistry prior to taking the course, (4) stay after school for help where your knowledge
base is weak or the subject area is difficult, (5) minimize absences (whether they are an approved
school activity, vacation or illness) as they will greatly affect your work load and understanding, (6)
take the AP Chemistry exam, (7) go into the AP Chemistry exam with the expectation of passing with
a 3 or higher, and (8) respect that this is a college level course and will be taught as such. Much is
expected of you; much is expected of me. With this mutual respect, these expectations can be
accomplished.
The use of a calculator will be kept to a minimum. The AP exam only allows you to use the
calculator on certain sections. Thus, your expertise in math is a necessity. You can expect to utilize
basic math skills that you began to learn in elementary school. Addition, subtraction, multiplication
and division should be second nature when you walk into the room and you should be able to do these
in your head. Practice these skills using simple flash cards. Build the numbers as you go. Do not just
stick to the basics. Expand your horizons and work with larger numbers. You also need to be
competent with using scientific notation in the above mathematical applications. Utilize the internet to
help you find ways to improve your skills. If you do not practice these skills you lose the ability to
perform them quickly, confidently and competently. Flash cards will help you throughout this course.
It is good practice to begin using now with these basic math skills.
Supplemental Text
We will be utilizing the following book along with our text. Please purchase this before the new school
year begins! I found mine on Amazon for $8.51! There are many different books
out there that appear similar. This is the specific one you need.
5 Steps to a 5 AP Chemistry
by John T. Moore, Richard H. Langley
Published by McGraw/Hill
1
Memorization of Polyatomic Ions
Many of these you already know. Many of these you do not. Be sure to have the following
polyatomic ions given in the table below memorized by day 1.
Common Polyatomic Ions
+1 CHARGE
ion
-1 CHARGE
name
ion
-2 CHARGE
name
ion
name
-3 CHARGE
ion
name
NH4+ ammonium H2PO3-
dihydrogen
phosphite
HPO32-
hydrogen
phosphite
H3O+ hydronium H2PO4-
dihydrogen
phosphate
HPO42-
hydrogen
PO43- phosphate
phosphate
Hg22+ mercury(I) HCO3-
hydrogen
carbonate
CO32-
carbonate
PO23- hypophosphite
HSO3-
hydrogen
sulfite
SO32-
sulfite
AsO33- arsenite
HSO4-
hydrogen
sulfate
SO42-
sulfate
AsO43- arsenate
NO2-
nitrite
S2O32-
thiosulfate
NO3
nitrate
SiO3
2-
OH-
hydroxide
C22-
-
-
CH3COO acetate
CrO2
-
oxalate
2-
C2O4
chromate
CN
cyanide
Cr2O72-
dichromate
CNO-
cyanate
C4H4O62- tartrate
CNS-
thiocyanate
MoO42-
O2
superoxide
2-
peroxide
MnO4-
permanganate S22-
disulfide
-
ClO
chlorite
ClO3-
chlorate
ClO4
-
-
BrO
molybdate
perchlorate
hypobromite
-
bromite
BrO3-
bromate
BrO2
BrO4
-
-
IO
perbromate
hypoiodite
IO2-
iodite
-
iodate
IO3
-
IO4
AlO2
N3-
P2O74- pyrophosphate
hypochlorite
-
ClO2
O2
name
carbide
2-
CrO4
-
ion
silicate
chromite
-
PO33- phosphite
-4 CHARGE
periodate
-
aluminate
azide
2
A bit of creativity before you get to the nitty gritty: Create a collage that shows what success means
to you regarding AP Chemistry. These are to be on ( 14in x 22 in ) poster board only. The board
needs to be completely covered. Write an explanation on the back of your collage. They will be
displayed.
Remember that success is different for each individual. No two people should have the
same collage with the same explanation.
How to Make a Collage
A collage (From the French: coller, to glue) is a work of
formal art, primarily in the visual arts, made from an
assemblage of different forms, thus creating a new whole.
A collage may include newspaper clippings, ribbons, bits of
colored or hand-made papers, portions of other artwork,
photographs and other found objects, glued to a piece of paper
or canvas.
The term collage derives from the French "coller" meaning "glue".This term was coined by both
Georges Braque and Pablo Picasso in the beginning of the 20th century when collage became a
distinctive part of modern art. Making a collage is fun, easy, and creative! You are going to make a
collage
to
represent
who
you
are.
The
following link
gives
step
by step
details:
http://www.wikihow.com/Make-a-Collage
The following problems should be review. Please complete and turn in the first day of school.
3
Kellam High School • AP Chemistry
Name_____________________________________
Period _____
Date ___/___/___
1•Matter and Measurement
PRACTICE TEST
Which physical state of matter exhibits the greatest change in volume with changes in temperature or pressure?
1.
a)
2.
solid
b) liquid
c) gas
According to the Kinetic Molecular Theory particles of a solid
a)
are bound in a regular array and do not move.
b) float freely within an array occupying various positions relative to neighbors.
c)
have no relationship to the microscopic structure of the solid.
d) vibrate back and forth but do not move past immediate neighbors.
e)
3.
float freely in the inside but do not move on the surface.
What volume of a liquid having a density of 1.48 g/cm3 is needed to supply 5.00 grams of the liquid?
a)
0.296 cm3
b) 1.48 cm3
c)
4.
d) 3.38 cm3
e)
7.40 cm3
2.26 cm3
The density of aluminum is 2.70 g/cm3. If a cube of aluminum weighs 13.5 grams, what is the length of the edge of
the cube?
a)
5.00 cm
b) 1.71 cm
c)
5.
e)
0.200 cm
1.25 cm
Which temperature change is the smallest?
a)
10°C to 20°C
b) 10 K to 20°C
c)
6.
d) 0.312 cm
d) 10°F to 20°C
e)
10°F to 20°F
10 K to 20 K
The number of significant figures in 0.06060 x 10 -5 is
a)
2
b) 3
c)
d) 5
e)
6
4
4
7.
The number, three hundred and fifty thousand, written in scientific notation is best written as
a)
350
b) 3.5 x 106
c)
8.
d) 3.50 x 105
e)
3.50 x 10-5
3.5 x 105
The mass of a sample weighted on an electronic balance that is sensitive to ±0.3 mg is 1.2300 g. The number of
significant figures in this measurement is
a)
1
b) 2
c)
9.
d) 4
e)
5
3
What is the numerical value of: 1.5 cm – 7.222 x 10-1 cm?
a)
0.7778 cm
b) 0.778 cm
c)
d) 0.8 cm
e)
7.072 x 10-1 cm
0.78 cm
10. Four samples were weighed using three different balances. (All are as accurate as the precision below indicates.) The
masses are 0.94 kg, 58.2 g, 1.55 g, and 250 mg. This total mass should be reported as
a)
1000.000 g
b) 1000.0 g
c)
d) 1.00 x 103 g
e)
1.0 x 103 g
1.000 x 103 g
11. The temperature of the room is 75°F. What is its temperature in Celsius degrees?
a)
24°C
b) 27°C
c)
d) 43°C
e)
43°C
30°C
12. The symbols for a metal, a non-metal and a noble gas in that order are
a)
Ag, Ga, Xe
b) Ce, Ge, Ne
c)
d) Ba, P, Ar
e)
P, Pb, Kr
Ca, Sn, Ks
13. Which of the following elements is a non-metal?
a)
Ca
b) Cr
c)
d) Cl
e)
Cs
Co
5
14. A good example of an ionic compound is
a)
water
b) sugar
c)
d) sodium chloride
e)
natural gas
dry ice
15. When a pure solid substance was heated, a student obtained another solid and a gas, each of which was a pure
substance. From this information which of the following statements is ALWAYS a correct conclusion?
a)
The original solid is not an element.
b) Both products are elements.
c)
The original solid is a compound and the gas is an element.
d) The original solid is an element and the gas is a compound.
e)
Both products are compounds.
16. Classify each observation as a physical or a chemical property and tally them.
Observation 1: Bubbles form on a piece of metal when it is dropped into acid.
Observation 2: The color of a crystalline substance is yellow.
Observation 3: A shiny metal melts at 650°C.
Observation 4: The density of a solution is 1.84 g/cm3
a)
2 chemical properties and 2 physical properties
b) 3 chemical properties and 1 physical properties.
c)
1 chemical properties and 3 physical properties
d) 4 chemical properties
e)
4 physical properties
17. To convert a value in kilograms to centigrams one should
a)
multiply by 105
b) multiply by 103
c)
d) divide by 105
e)
divide by 10-1
multiply by 10-3
18. How many cm2 are in an area of 4.21 in2?
a)
10.7 cm2
b) 114 cm2
c)
d) 1.66 cm2
e)
1.14 cm2
27.2 cm2
19. When the prefix micro (µ) is used in the metric system, a fundamental unit of measurement is multiplied by a factor of
a)
10-9
b) 10-6
c)
d) 103
e)
109
10-3
6
20. Of the masses 86.30 g, 0.0863 kg and 8.630 x 10 5 mg, which (if any) is the largest?
a)
86.30
d) they are the same
b) 0.0863 kg
c)
e)
5
8.630 x 10 mg
two are the same,
one is smaller
21. The element chlorine is obtained for commercial use by the following method:
a)
Isolation from gas pockets in the earth’s crust.
b) Separation from air by a high pressure technique.
c)
Filtration of brine (NaCl) solutions.
d) Electrolysis of aqueous NaCl solutions.
e)
Mixing sulfur and argon in equal quantities.
22. Consider a brass alloy which contains 66% copper and 34% zinc. How many grams of zinc are present in 125 kg of
the alloy?
a)
d) 2.4 x 104 g
2.4 g
b) 42 g
c)
e)
4.2 x 104 g
83 g
23. The density of a sodium sulfate solution is 1.07 g/cm3. The solution is 8.00% sodium sulfate by mass. How many
cm3 of the solution are needed to supply 4.28 g of sodium sulfate?
a)
30.0 cm3
b) 35.0 cm3
c)
d) 45.0 cm3
e)
50.0 cm3
40.0 cm3
24. Which of the following is NOT an SI base unit?
a)
mass
d) time
b) volume
c)
e)
temperature
length
2  Atoms and Elements
1.
Certain properties are characteristic of metals. Which property means that you can pound the substance into a foil?
a)
ductility
b) conductivity
2.
c)
sectility
d) malleability
Which of the following is a metalloid?
a) As
b) Ag
c) S
d) Pb
e) He
7
3.
Which of the following is a transition metal?
a) Cl
4.
e) C
b) Kr
c) K
d) Al
e) H
b) Eu
c) Cd
d) P
e) W
Which element has the highest melting point?
a) Pb
7.
d) Ca
Which of the following is an lanthanide?
a) Xe
6.
c) P
Which of the following is an alkali metal?
a) Mg
5.
b) Ni
b) Au
c) Os
d) W
e) Hg
Pictured below is a schematic of the Rutherford experiment. Which scattered -particle gives the best evidence for
the nuclear atom?
a
b

c
e
a) a
8.
b) b
c) c
d) d
e) e
Which of the following is an isotope of the element with 20 protons (p=20) and 22 neutrons (n=22)?
a)
titanium-22
b) zirconium-40
9.
d
c)
calcium-40
d) titanium-48
The imaginary element X has the following natural abundances and isotopic masses. What is the atomic weight of X?
24
24.02 amu
40.0%
12 X
26
26.10 amu
60.0%
12 X
For questions 13 - 16, use the following key:
(each answer may be used once, more than once, or not at all.)
a)
John Dalton
b) Ernest Rutherford
c)
J.J. Thomson
d) Democritus
13. His model of the atom has been called the “billiard ball” model.
14. He studied matter in cathode ray tubes.
8
15. His philosophical idea included the term “atomos”.
16. He added to the atomic theory the idea that atoms had positive and negative parts.
220
17. Consider the following notation: 86 Rn
Which statement below is correct?
a)
This particle contains 86 protons
b) This particle has a mass number of 86
c)
This particle has an atomic number of 220
d) This particle contains 220 neutrons
18. If copper metal is a mixture two isotopes, Cu-63, mass = 62.9298 u and Cu-65, mass = 64.9278 u. The molar mass
of copper is 64.546 g/mole. Calculate the % abundances of the two isotopes of copper.
3 • Molecules and Compounds
1.
What is the formula of the ionic compound formed between Mg and Br?
a)
MgBr
b) Mg2Br
c)
2.
e)
Mg2Br3
MgBr2
What is the formula of the ionic compound formed between Ca and P?
a)
Ca2P3
b) CaP
c)
3.
d) Mg2Br2
d) Ca2P
e)
Ca3P2
Ca5P10
What is the name of the SO32– ion?
a)
sulfate
b) nitrate
c)
d) sulfur trioxide
e)
hydrogen sulfate
sulfite
4.
What is the correct formula and charge for the chromate ion?
a) CrO42–
d) Cr2O7–
b) CrO4–
e) Cr3+
c) Cr2O72–
5.
Which one of the following elements forms ions with two different valences?
a)
calcium
b) arsenic
c)
iron
d) fluorine
9
6.
The correct name for CCl4 is
a)
carbon(I) chloride
b) carbon chloride
c)
carbon tetrachloride
d) monocarbon chloride(IV)
e)
7.
carbochlorinate
The correct formula for hydrogen telluride is
a)
HTe
b) H2Te
8.
H3Te
d) HTe2
The correct formula for dinitrogen tetroxide is
a) NO2
d) NO3–
b) N2O4
c)
9.
c)
e)
(N2O)4
N2 O 5
The correct name for S2Cl2 is
a)
sulfur dichloride
b) sulfur(I) chloride
c)
sulfur(II) chloride
d) disulfur dichloride
e)
sulfur chloride
10. The correct name for H3P is
a)
hydrogen phosphide
b) trihydrogen phosphide
c)
hydrogen phosphate
d) phosphorus trihydride
e)
hydrogen triphosphate
11. The molar mass of (NH4)2S is closest to:
a)
50 g/mol
b) 82 g/mol
c)
68 g/mol
d) 100 g/mol
12. How many atoms are in 12 molecules of glucose, C6H12O6?
a)
24
b) 288
c)
2160
d) 7.22 x 1024
10
13. Calculate the number of atoms in 4.0 x 10-5 g of aluminum.
a)
8.9 x 1017
b) 4.6 x 1019
c)
6.5 x 1020
d) 3.8 x 1023
14. Which of the following samples contains the smallest number of atoms?
a)
1 g H2
b) 1 g O2
c)
1 g O3
d) 1 g Cl2
15. What is the mass of one molecule of octane, C8H18?
a)
114 g
b) 1.89 x 10-22 g
c)
1.10 x 10-22 g
d) 4.32 x 10-23 g
16. What is the percent nitrogen (by mass) in ammonium carbonate, (NH 4)2CO3?
a)
14.53%
b) 27.83%
c)
29.16%
d) 33.34%
17. Of the following, the only empirical formula is
a)
N2F2
b) N2F4
c)
H2C2
d) HNF2
18. A compound consists of the following elements by weight percent:
carbon - 40.0%
oxygen - 53.3%
hydrogen - 6.7%
The ratio of carbon : oxygen : hydrogen in the empirical formula is
a)
1:2:1
b) 1:1:1
c)
1:1:2
d) 2:1:2
19. An organic compound which has the empirical formula CHO has a molar mass of 232. Its molecular formula is:
a)
CHO
b) C2H2O2
c)
C4H4O4
d) C8H8O8
20. When CaSO4·y H2O is heated, all of the water is driven off. If 34.0 g of CaSO4 [molar mass = 136] is formed from
43.0 g of CaSO4·y H2O, what is the value of y?
a)
1
b) 2
c)
3
d) 4
11
4 • Chemical Equations and Stoichiometry
1.
Balance the following equation:
___NH3 + ___O2  ___NO2 + ___H2O
The balanced equation shows that 1.00 mole of NH3 requires ___ mole(s) of O2.
a) 0.57
c) 1.33
b) 1.25
d) 1.75
2.
Write a balanced equation for the combustion of acetaldehyde, CH 3CHO.
When properly balanced, the equation indicates that ___ mole(s) of O 2 are required for each mole of CH3CHO.
a) 1
c) 2.5
b) 2
d) 3
3.
Balance the following equation with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. Select the
number that is the sum of the coefficients in the balanced equation:
___KClO3  ___KCl + ___O2
a) 5
b) 6
c) 7
d) 8
4.
Write a balanced equation for the combustion of propane, C3H8.
When properly balanced, the equation indicates that ___ moles of O 2 are required for each mole of C3H8.
a) 3
b) 3.5
c) 5
d) 8
5.
What is the total mass of products formed when 16 grams of CH4 is burned with excess oxygen?
a) 80 g
c) 36 g
b) 44 g
d) 32 g
6.
Calculate the mass of hydrogen formed when 25 g of aluminum reacts with excess hydrochloric acid.
2Al + 6HCl  2 AlCl3 + 3 H2
a) 0.41 g
c) 1.2 g
b) 0.92 g
d) 2.8 g
7.
How many grams of the mixed oxide, Fe3O4, are formed when 6.00 g of O2 react with Fe according to
3Fe + 2O2  Fe3O4
a)
b)
8.
43.4
86.8
c)
d)
174
21.7
For the reaction:
2MnO2 + 4KOH + O2 + Cl2 2KMnO4 + 2KCl + 2H2O
there is 100. g of each reactant available. Which reagent is the limiting reagent?
[Molar Masses: MnO2=86.9; KOH=56.1; O2=32.0; Cl2=70.9]
a) MnO2
c) O2
b) KOH
d) Cl2
12
9.
How many grams of nitric acid, HNO3, can be prepared from the reaction of 92.0 g of NO 2 with 36.0 g H2O?
3NO2 + H2O  2HNO3 + NO
a)
b)
10.
64
76
c)
d)
84
116
The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage
yield?
C6H6 + HNO3  C6H5NO2 + H2O
a) 100%
c) 54.3%
b) 27.4%
d) 85.6%
5 • Reactions In Aqueous Solution
1.
When H2SO4 and Ba(OH)2 are reacted in a double replacement reaction, one of the products of the reaction is…
a)
H2
d) BaH2
b) H2O
c)
2.
e)
BaS
Which of the following is a base?
a)
KOH
d) CH3OH
b) C2H5OH
c)
3.
e)
Br–
H2CO3
d) HClO3
b) HF
c)
e)
H3PO4
HNO3
d) H2S
b) H2SO3
c)
e)
HNO2
H2SO4
What is the oxidation number of C in CO32–?
a)
+6
d) +1
b) +4
c)
6.
HNO3
SO2 turns into which acid in solution?
a)
5.
CO2
Which of the following is a strong acid?
a)
4.
SO2
e)
–1
+2
What is the oxidation number of Br in KBrO4?
a) +1
b) –1
c) +5
d) +7
e) +8
13
7. For each change below, label the change of the underlined element as Oxidation, Reduction, or Neither
___ Cu2+  Cu
___ CH4  CO2
___ H2O2  H2O
___ CO2  H2CO3
8.
How many milliliters of 0.123 M NaOH solution contain 25.0 g of NaOH (molar mass = 40.00 g/mol)?
a)
5.08 mL
b) 50.8 mL
c)
9.
d) 625 mL
e)
5080 mL
508 mL
If you need 1.00 L of 0.125 M H2SO4, how would you prepare this solution?
a)
Add 950. mL of water to 50.0 mL of 3.00 M H2SO4.
b) Add 500. mL of water to 500. mL of 0.500 M H2SO4.
c)
Add 750 mL of water to 250 mL of 0.375 M H2SO4.
d) Dilute 36.0 mL of 1.25 M H2SO4 to a volume of 1.00 L.
e)
Dilute 20.8 mL of 6.00 M H2SO4 to a volume of 1.00 L.
10. What is the molarity of the solution that results when 60.0 g NaOH is added to enough water to make 500. mL
solution?
a)
1.33 M
b) 12.0 M
c)
d) 8.0 M
e)
1.50 M
3.00 M
11. What is the molarity of the solution that results when 45.0 g HCl is dissolved in enough water to make 250. mL
solution?
a)
4.94 M
b) 4.50 M
c)
d) 1.80 M
e)
1.46 M
3.24 M
12. How many grams of Na2CO3 (molar mass = 106.0 g/mol) are required for complete reaction with 25.0 mL of 0.155
M HNO3?
Na2CO3 + 2HNO3  2NaNO3 + CO2 + H2O
a)
0.122 g
b) 0.205 g
c)
d) 20.5 g
e)
205 g
0.410 g
14
13. What volume of 0.150 M NaOH is needed to react completely with 3.45 g iodine according to the equation:
3 I2 + 6 NaOH  5 NaI + NaIO3 + 3 H2O
a)
181 mL
b) 45.3 mL
c)
d) 2.04 mL
e)
1.02 mL
4.08 mL
14. What is the concentration of an NaOH solution if it takes 16.25 mL of a 0.100 M HCl solution to titrate 25.00 mL of
the NaOH solution?
a)
0.0165 M
b) 0.151 M
c)
d) 0.100 M
e)
0.413 M
0.0650 M
15. A 4.00 M solution of H3PO4 will contain ___g of H3PO4 in 0.250 L of solution.
a)
196 g
b) 98.0 g
c)
d) 24.0 g
e)
12.0 g
49.0 g
6 • Energy and Chemical Reactions
1.
How many joules are equivalent to 37.7 cal?
a)
9.01 J
b) 4.184 J
2.
1.51 J
d) 158 J
The quantity of heat that is needed to raise the temperature of a sample of a substance 1.00 degree is called its
a)
heat capacity
b) specific heat
3.
c)
c)
enthalpy
d) kinetic energy
If 25 J are required to change the temperature of 5.0 g of substance A by 2.0C, what is the specific heat of substance
A?
a)
250 J/gC
b) 63 J/gC
4.
c)
10. J/gC
d) 2.5 J/gC
How much energy is required to change the temperature of 2.00 g aluminum from 20.0C to 25.0C? The specific
heat of aluminum is 0.902 J/gC.
a)
2.3 J
b) 9.0 J
c)
0.36 J
d) 0.090 J
15
5.
Consider the thermal energy transfer during a chemical process. When heat is transferred to the system, the process is
said to be _______ and the sign of H is ________.
a)
exothermic, positive
b) endothermic, negative
c)
exothermic, negative
d) endothermic, positive
6.
When two solutions react the container “feels hot.” Thus,
a)
the reaction is endothermic.
b) the reaction is exothermic.
c)
the energy of the universe is increased.
d) the energy of both the system and the surroundings is decreased.
7.
Which one of the following would have an enthalpy of formation value (Hf) of zero?
a)
H2O(g)
c)
b) O(g)
8.
H2O(l)
d) O2(g)
Calculate the standard enthalpy of the reaction for the process
3NO(g)  N2O(g) + NO2(g)
using the standard enthalpies of formation (in kJ/mol): NO = 90; N2O = 82.1; NO2 = 34.0
a)
-153.9 kJ
c)
b) 206 kJ
-26.1 kJ
d) 386 kJ
19. Calculate the amount of heat needed to change 25.0 g ice at 0C to water at 0C.
The heat of fusion of H2O = 333 J/g;
a)
56.5 kJ
c)
b) 8.33 kJ
7.06 kJ
d) 463 kJ
7&8 • Atomic Structure & Periodicity
9.
Which quantum number determines the subshell occupied by an electron (s, p, d, f, etc.)?
a)
n
c)
b) l
ml
d) ms
10. What position on the standing wave shown below corresponds to a crest?
a) A
b) B
c) C
d) D
e) E
16
11. How many orbitals make up the 4d subshell?
a) 0
b) 1
c) 3
d) 5
e) 7
12. The value of l that is related to the following orbital is:
a) 0
b) 1
c) 2
d) 3
e) 4
13. The correct electron configuration for nitrogen is
a)
1s2 2s2 2p6 3s2 3p2
b) 1s2 2s2 2p6 2d4
c)
1s2 2s2 2p3
d) 1s2 2s2 3s2 4s1
e)
1s2 1p5
14. The electron configuration of the indicated atom in the ground state is correctly written for which atom?
a)
Ga
[Ar] 3d12 4s2
b) Ni
[Ar] 3d10
c)
[Ar] 3s2 3p8
Ni
d) Cu
[Ar] 3d10 4s1
15. Which of the following sets of quantum numbers is possible for a 3d electron?
1
a) n = 3, l = 3, ml = –2, ms = +
2
1
b) n = 2, l = 1, ml = +1, ms = –
2
1
c) n = 3, l = 1, ml = 0, ms = –
2
1
d) n = 3, l = 2, ml = –2, ms = +
2
1
e) n = 4, l = 1, ml = +1, ms = +
2
16. In what section of the periodic table is the 4f subshell being filled?
a)
period 4
b) transition elements Y to Cd
c)
noble gases
d) group IA
e)
lanthanides
17
17. Which one of the following elements has 3 electrons in a p subshell?
a) Sb
b) Na
c) Sc
d) V
e) Nd
18. Which of the following distributions of electrons is correct for three electrons in p-subshell?
a)


b)


c)


d)


e)




20. Which of the following correctly represents the ionization of an atom?
a)
Cl(g) + e–  Cl–(g)
b) Na(g)  Na+(g) + e–
c)
Na(s) – e–  Na+(g)
d) Cl2(g)  2 Cl(g)
21. Which of the following is likely to have the largest atomic radius?
a) H
b) Mn
c) Cl
d) Rb
e) Ag
23. Which of the following has the greatest ionization energy?
a) K
b) Ca
c) Fe
d) Ga
e) Br
24. Which of the following has the lowest ionization energy?
a) Li
b) Na
c) K
d) Rb
e) Cs
26. Draw the orbital diagram for a neutral Ag atom:
5s
4s
3s
2s
1s
18
Write the electron configuration for silver:
27. Long form:
28. Short form using noble gases:
9  Bonding & Molecular Structure
1.
The correct Lewis symbol for ground state carbon is
a)
2.
b)
b)
c)
d)
e)
b) P
c) S
d) B
e) F
How many electrons are shown in the Lewis structure of perchlorate ion, ClO4–?
a) 30
5.
e)
Which of the atoms below is least likely to violate the octet rule?
a) Be
4.
d)
The correct Lewis symbol for ground state aluminum is
a)
3.
c)
b) 31
c) 32
d) 50
e) 51
Which of the following is the correct Lewis structure for SOCl2? (Consider formal charge)
a)
d)
b)
e)
c)
6.
In which of the following is the actual compound a resonance hybrid of Lewis structures?
a)
NO2
b) H2O
c)
7.
d) CCl4
e) none of these
O3
Which of the following bonds is most polar?
a)
N – Cl
b) C – N
c)
d) Br – Br
e)
S–O
S–S
19
8.
9.
Which one of the following molecules is a polar molecule?
a)
c)
b)
d)
Which molecular shape has bond angles which are not all the same?
a)
linear
d) planar triangular
b) tetrahedral
c)
e)
trigonal bipyramid
octahedral
10. The molecule BrF3 has how many lone pairs of electrons on the central atom?
a)
0
b) 1
c)
2
d) 3
11. What is the geometrical arrangement of electron pairs in H2O?
a)
linear
b) bent
c)
d) trigonal bipyramidal
e)
tetrahedral
octahedral
12. What is the shape of BrI3?
a)
square planar
b) T-shaped
c)
d) pyramidal
e)
bent
distorted tetrahedral
13. Which of the following is a polar species?
a)
CO2
b) PCl5
c) ICl2–
d) TeCl4
e)
CCl4
20
14. Among those listed below, which element will have the strongest tendency to form double bonds?
a)
S
b) B
H
2.1
Li
1.0
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Fr
0.7
c)
Al
d) O
Electronegativity Values
Be
1.5
Mg
1.2
Ca
1.0
Sr
1.0
Ba
0.9
B
2.0
Al
1.5
Ga
1.6
In
1.7
Tl
1.8
C
2.5
Si
1.8
Ge
1.8
Sn
1.8
Pb
1.8
N
3.0
P
2.1
As
2.0
Sb
1.9
Bi
1.9
O
3.5
S
2.5
Se
2.4
Te
2.1
Po
2.0
F
4.0
Cl
3.0
Br
2.8
I
2.5
At
2.2
He
--Ne
--Ar
--Kr
--Xe
--Rn
---
12 • Gases and Their Properties
1.
A pressure of 745 mmHg corresponds to ___ kPa.
a)
55.89 kPa
b) 0.980 kPa
2.
3.
a)
- 469 K
b)
77 K
d) 745 kPa
c)
153 K
d) 469 K
1.20 atm is the same pressure as:
1.2 mmHg
b) 760 mmHg
c)
d) 850 mmHg
e)
358 mmHg
912 mmHg
For an ideal gas, which pair of variables are inversely proportional to each other (if all other factors remain constant)?
a)
P, V
b) P, T
5.
99.3 kPa
Liquid nitrogen has a boiling point of -196 °C this corresponds to…
a)
4.
c)
c)
V, T
d) n, P
A real gas would act most ideal at
a)
1.0 atm and 273 K
b) 10 atm and 546 K
c)
10 atm and 273 K
d) 0.5 atm and 546 K
e)
0.5 atm and 273 K
21
7.
A 31.0 mL sample of gas is collected at a temperature of 37 °C and pressure of 720 mmHg. What is its volume at 17
°C and 580 mmHg.
a)
23 mL
b) 27 mL
c)
d) 41 mL
e)
58 mL
36 mL
11. What is the pressure exerted by some nitrogen gas collected in a tube filled with water on a day when the room
temperature is 18.0 °C and the room pressure is 750.0 mmHg? [The partial pressure of water at 18 °C is 15.5 mmHg.]
a)
15.5 mmHg
b) 750.0 mmHg
c)
d) 760.0 mmHg
e)
732.0 mmHg
734.5 mmHg
12. As the average kinetic energy of the molecules of a sample increases, the temperature of the sample
a)
decreases
c)
remains the same
b) increases
13. If a gas that is confined in a rigid container is heated, the pressure of the gas will…
a)
increase
c)
remain the same
b) decrease
14. A mixture of gases at 810 kPa pressure contains:
3.0 moles of oxygen gas,
2.0 moles of helium gas, and
4.0 moles of carbon dioxide gas.
What is the partial pressure of helium gas, P He.
a)
405 kPa
b) 1620 kPa
c)
d) 81.0 kPa
e)
180 kPa
810 kPa
18. At STP, it was found that 1.12 L of a gas had a mass of 2.78 g. Its molar mass is
a)
2.78 g/mol
b) 27.8 g/mol
c)
55.6 g/mol
d) 111 g/mol
17  Acid-Base Equilibria
1.
What is the [H+] when [OH-] = 8.1 x 10-5?
a)
8.1 x 10-5 M
b) 1.0 x 10-7 M
c)
d) 3.6 x 10-6 M
e)
8.1 x 10-5 M
1.2 x 10-10 M
22
2.
What is the [H+] when [OH-] = 3.3 x 10-9?
a)
3.0 x 10-6 M
b) 1.0 x 10-7 M
c)
3.
e)
3.3 x 10-9 M
3.3 x 10-5 M
What is the [H+] in a 0.0025 M HCl solution?
a)
1.0 x 10-7 M
b) 4.0 x 10-12 M
c)
4.
d) 6.6 x 10-5 M
d) 3.6 x 10-5 M
e)
need more info
-3
2.5 x 10 M
What is the [OH-] in a 0.0050 M HCl solution?
a)
5.0 x 10-3 M
b) 1.0 M
c)
d) 6.6 x 10-5 M
e)
2.0 x 10-12 M
1.0 x 10-7 M
23