Download Semester 1 Final Exam

South Pasadena • Honors Chemistry
Name
Semester 1 Final Exam
Period
PART 1
•
MULTIPLE CHOICE (PRACTICE)
1. Which measurement below shows the temperature
to the correct precision?
20
mercury thread
Date
5. The density of copper is known to be 8.96 g/mL. A
student’s experimental result shows that the density
of her copper cube is 8.79 g/mL. The percent error
in this data is ______.
(A) 0.17 %
(B) 0.98 %
(C) 1.90 %
(D) 1.93 %
30
(A) 26 °C
(B) 26.25 °C
(C) 26.3 °C
(D) 26.30 °C
2. In scientific notation, the number 3,020,000 should
be written as:
(A) 3.02 × 106
(B) 3.02 ×10–6
(C) 302 ×104
(D) 302 ×10–4
3. How should the following computation be
recorded, with the correct number of significant
figures?
(1.15)(1.50)
(0.08206)(315)
(A) 0.0667
(B) 0.06673
(C) 0.067
(D) 6620
4. Which measurement is the most precise?
(A) 4.2  .3 g
(B) 4.3  .1 g
(C) 4.5  .4 g
(D) 4.6  .2 g
6. The average temperature on Venus is 460°C. What
is this in Kelvin?
(A) 187 K
(B) –187 K
(C) 273 K
(D) 733 K
7. Which one of the following statements is true?
(A) 1000 cm = 1 m
1
(B) 1 mm = 100 meter
(C) 1 kg = 1000 g
(D) each of these statements is true
8. What conversion factor would you use to convert
milligrams to grams?
1000 mg
(A) 1 g
1g
(B) 1000 mg
1 mg
(C) 1000 g
1000 g
(D) 1 mg
9. A metal cube of metal measures 2 cm on each side.
Its mass is 90.4 grams. What is the metal?
(A) Al (density = 2.70 g/cm3)
(B) Au (density = 19.3 g/ cm3)
(C) Fe (density = 7.86 g/ cm3)
(D) Pb (density = 11.3 g/ cm3)
10. What is the volume of a 5.08 gram sample of liquid
bromine? (density of bromine = 3.10 g/mL)
(A) 0.610 mL
(B) 1.64 mL
(C) 15.7 mL
(D) 8.18 mL
16. In which of the following states of matter are the
attractive forces between molecules strongest?
(A) Solid
(B) Liquid
(C) Gas
(D) Plasma
11. A gold block and a copper block both have a mass
of 5.0 kg. Which occupies a greater volume?
(Densities in g/cm3: gold = 19.3, copper = 8.94)
(A) Copper block
(B) Gold block
(C) They have the same volume.
(D) It cannot be determined.
17. Which set consists only of elements?
(A) Na, Ca, H2
(B) H3O+, Cl–, I3–
(C) NaCl, CH4, Br2
(D) H2S, CuCl2, KI
12. The atom represented by 57Co3+ has:
(A) 27 protons, 30 neutrons, 24 electrons
(B) 27 protons, 30 neutrons, 30 electrons
(C) 27 protons, 57 neutrons, 3 electrons
(D) 30 protons, 27 neutrons, 3 electrons
13. All of the following describe a neutron EXCEPT:
(A) It determines the identity of the atom.
(B) It does not carry a charge.
(C) It is located in the nucleus.
(D) It, along with the proton, makes us most of the
atom’s mass.
14. Which of the following is an isotope of 40K?
(A) 39K
(B) 40K+
(C) 40Ar
(D) 40Ca
15. The atomic mass of aluminum is 26.98. Which of
the following is correct?
(A) One aluminum atom has a mass of 26.98 amu.
(B) One aluminum atom has a mass of 26.98
grams.
(C) One mole of aluminum contains 26.98 atoms.
(D) One mole of aluminum has a mass of 26.98
grams.
18. What do the elements phosphorous and sulfur have
in common?
(A) They are both alkali metals.
(B) They are in the same family.
(C) They are in the same period.
(D) They both form ions with the same charges.
19. Which of the following is a liquid non-metal atom
at room temperature?
(A) Barium
(B) Bromine
(C) Mercury
(D) Nitrogen
20. Which of the following compounds is ionic?
(A) AlCl3
(B) HCl
(C) SCl2
(D) SiCl4
21. What is the formula for the ionic compound formed
when sodium ions and sulfide ions are combined?
(A) Na2S
(B) Na2SO4
(C) NaS
(D) NaS2
22. An unknown element X forms a salt with the
formula XO2. Which of the following could be X?
(A) Al3+
(B) Ca2+
(C) Na+
(D) Sn4+
23. Which one of the following is the correct formula
for calcium phosphate?
(A) Ca2(PO4)3
(B) Ca3(PO4)2
(C) CaPO4
(D) PO4Ca3
24. What is the name of the compound N2O3?
(A) dinitride trioxide
(B) dinitrogen trioxide
(C) nitrate
(D) nitrogen oxide
25. The formula for hydrosulfuric acid is:
(A) H2S
(B) H2SO4
(C) HS
(D) HSO4
26. Which of the following is incorrect?
(A) 1 mole of O2 molecules has 6.02 × 1023 oxygen
atoms.
(B) 1 mole of O2 molecules has a mass of 32
grams.
(C) 1 mole of O2 molecules occupy 22.4 liters at
STP.
(D) All of the above statements are correct.
27. How many molecules are in 2.00 × 10–2 moles of
carbon tetrachloride, CCl4? (molar mass = 154
g/mol)
(A) 1.20 × 1023
(B) 3.01 × 1023
(C) 6.02 × 1023
(D) 1.20 × 1022
28. What is the percent of carbon in barium carbonate,
BaCO3?
(molar mass = 197.3 g/mol)
(A) 3.04%
(B) 6.09%
(C) 14.0%
(D) 20.0%
29. The general formula CnH2n describes the molecular
composition of the hydrocarbon family known as
the
(A) alkadienes
(B) alkanes
(C) alkenes
(D) alkynes
30. Structural formulas have advantages over
molecular formulas because they show the
(A) bonding arrangement of each carbon atom.
(B) geometric arrangement of the atoms.
(C) number of atoms of each element present.
(D) percentage composition of the compound.
31. How many carbons make up the “parent chain” in
the following molecule?
(A) 4
(B) 5
(C) 6
(D) 7
32. The number of isomers of bromopropane, C3H7Br,
is
(A) 2
(B) 3
(C) 4
(D) 7
33. Which of the following is an isomer of the
compound below:
F
H
C
(A)
F
F
H
H
F
H
F
F
C
C
H
(D)
H
F
F
H
C
C
H
F
H
34. Which of the following is the correct name for the
following compound:
H
H
H
Br
C
C
C
H
H
Br
H
(A) 1,1-dibromobutane
(B) 1,1-dibromopropane
(C) 2-bromopropane
(D) 3,3-dibromopropane
35. Which functional group is found in the following
compound?
H
H
H
C
C
H
H
O
H
37. When the equation for the combustion of propene,
C3H6, is balanced with the lowest whole-number
coefficients, what is the coefficient of oxygen, O2?
(A) 6
(B) 9
(C) 12
(D) 18
C
F
H
(A) Grain alcohol (ethanol)
(B) Isopropyl alcohol (2-propanol)
(C) Nail polish remover (acetone, or propanone)
(D) Vinegar (ethanoic acid)
C
C
(C)
F
H
C
(B)
H
C
H
36. The structure of which compound is given below?
H H
C
C
O
(A) Aldehyde
(B) Carboxylic Acid
(C) Ether
(D) Ketone
H
C
H
38. When an alcohol reacts with a carboxylic acid,
which of the following is formed?
(A) A ketone
(B) An ester
(C) An ether
(D) CO2
39. In a sample of salt water, the salt is called the
(A) Precipitate
(B) Solute
(C) Solution
(D) Solvent
40. Which of the following compounds is expected to
be soluble in water?
(A) CaSO4
(B) FeS
(C) PbCl2
(D) SrBr2
41. How many grams of sodium hydroxide pellets,
NaOH, are required to prepare 50.0 mL of a 0.150
M solution? [molar mass NaOH = 40.0 g/mol]
(A) 0.300
(B) 2.00
(C) 3.00
(D) 200.
42. If 50 mL of a 200 mL sample of 0.10 M sodium
chloride solution is spilled, what is the
concentration of the remaining solution?
(A) 0.025 M
(B) 0.075 M
(C) 0.10 M
(D) 0.20 M
43. List the following solutions prepared with the same
solute in order of increasing concentration:
I. 30.0 g solute in a 240 mL solution
II. 30.0 g solute in a 120 mL solution
III. 60.0 g solute in a 120 mL solution
(A) I < II < III
(B) II < I < III
(C) II < III <I
(D) III < II < I
44. A 100 mL sample of a solution with a
concentration of 5.00 M is diluted to a new volume
of 400 mL with distilled water. The new
concentration will be
(A) 1.25 M
(B) 1.66 M
(C) 15.0 M
(D) 20.0 M
45. A property of acids are that they
(A) are caustic
(B) feel slippery
(C) neutralize water
(D) taste sour
46. Which of the following represents the dissociation
of CaI2 in solution?
(A) CaI2  Ca + I2
(B) CaI2  Ca2+ + 2 I–
(C) CaI2 Ca2+ + 2 I–
(D) CaI2 is insoluble so it does not dissociate.
47. A solution that conducts electricity very well is
called a:
(A) liquid conductor
(B) metallic solution
(C) strong electrolyte
(D) weak electrolyte
48. Which chemical is the conjugate base?
NH3 + H2O  NH4+ + OH–
(A) H2O
(B) NH3
(C) NH4+
(D) OH–
49. If a solution has [OH–] = 1.0 × 10–3 M, what is the
pH?
(A) 3
(B) 7
(C) 11
(D) 14
50. What is the [OH–] in a solution in which [H+] is
1.0 × 10–6 M?
(A) 1.0 × 10–6 M
(B) 1.0 × 10–7 M
(C) 1.0 × 10–8 M
(D) 1.0 × 10–9 M
51. A solution tested with cabbage juice turns green.
Which of the following could be its pH?
(A) 1
(B) 4
(C) 7
(D) 10
52. A substance that turns cabbage juice blue and
slightly lights up a light bulb is a:
(A) strong acid
(B) strong base
(C) weak acid
(D) weak base
53. Which reaction below would be classified as a
single replacement reaction?
(A) 2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag
(B) 2 H2 + O2  2 H2O
(C) Ba(OH)2 + H2SO4  BaSO4 + 2 H2O
(D) NaHCO3  NaOH + CO2
54.
… H3PO3  … H3PO4 + …PH3
When the equation above is balanced, the
coefficient for H3PO4 is:
(A) 1
(B) 2
(C) 3
(D) 4
55. When solutions of potassium sulfate and calcium
bromide are combined, which of the following
precipitates?
(A) KBr
(B) CaS
(C) CaSO4
(D) There is no precipitate.
56. Which of the following are products when
magnesium metal is placed in hydrochloric acid?
(A) H
(B) H+
(C) Mg
(D) MgCl2
57.
Zn  Zn2+ + 2e–
In the half reaction above:
(A) Zn is oxidized because it is gaining electrons.
(B) Zn is oxidized because it is losing electrons.
(C) Zn is reduced because it is gaining electrons.
(D) Zn is reduced because it is losing electrons.
58. When we reacted AgNO3 and K2CrO4 to form
Ag2CrO4 and KNO3, ________ was oxidized.
(A) chromate ion
(B) nitrate ion
(C) silver ion
(D) nothing (it wasn’t a redox reaction)
59. During the “ornament lab,” hydrogen gas was
produced according to the following equation:
Zn + 2 HCl  ZnCl2 + H2
Which chemical was oxidized?
(A) H2
(B) HCl
(C) Zn
(D) ZnCl2
60. What mass of sulfur dioxide, SO2 (64.0 g/mole), is
produced when 245 g of sulfuric acid, H2SO4 (98.0
g/mole) reacts completely with zinc metal
according to the balanced equation below?
Zn + 2 H2SO4  ZnSO4 + SO2 + 2 H2O
(A) 64.0 g
(B) 80.0 g
(C) 128 g
(D) 160 g
South Pasadena • Honors Chemistry
Name
Semester 1 Final Exam
Period
PART B
Date
SHORT ANSWER
•
(PRACTICE)
Only answers will be graded. Unless otherwise stated, no partial credit will be awarded with the work. Numerical
answers should be reported with the correct number of significant digits and with appropriate units.
1.
1
2
3
The length and width of a
rectangular sheet of
aluminum foil are measured
as shown. Record the
dimensions of the foil with
correct number of significant
figures.
4
1
2
3
4
5
cm
5
cm
2.
Chlorine naturally exists in two isotopes: Cl-35 (isotopic mass 34.9689
amu) and Cl-37 (36.9659 amu). If chlorine has a molar mass of 35.453
g/mol, find the % abundance of each isotope.
Abundance of Cl-35:
Abundance of Cl-37:
3.
4.
Name the following compounds.
NH4ClO3
CuO
H3PO3
IF7
A 12.3 g sample of a gas occupies 6.28 L
at STP. Find the number of molecules in
this sample.
(Show your work using dimensional analysis.)
Find the molar mass of this gas.
(Show work here.)
5.
Convert the density of copper, 8.96 g/cm3,
to lb/in3.
(Show your work using dimensional analysis.)
[1 kg = 2.2046 lb, 1 in = 2.54 cm]
6.
7.
Draw two isomers for C3H6I2.
Draw two isomers for C2H2Cl2.
8.
Identify the functional groups in the
compound MMDA.
9.
Write the structural formulas for the
products when the following compounds
are combined:
Structure:
Name:
Structure:
Name:
Structure:
Name:
Structure:
Name:
H
H
H
C
C
C
C
H
10.
C
C
O
H
O
H
H
C
O
H
Consider a solution in which
pH
[OH–] = 6.5 × 10–7 M. Find its pH, pOH,
and [H+], and determine whether the
[H+]
solution is acidic, basic, or neutral.
pOH
Acidic/Basic/Neutral
11.
Write the balanced equations for the
following reactions. States are not
required.
Propanol (C3H7OH) is burned in air.
A sample of solid aluminum oxide is strongly heated.
12.
Write the balanced equations for the
following reactions. States are not
required.
Aluminum metal is placed in a solution of cupric chloride.
Solid ammonium acetate is placed in water.
Useful Formulas and Constants
1 mole = 6.022 × 1023 particles = 22.4 L gas at STP
K = °C + 273
m
D=V
m
Molar Mass = n
n
M=V
Mc · V c = Md · V d
[H+][OH–] = 1.0 × 10–14
pH + pOH = 14
pH = – log [H+]
pOH = – log [OH–]
Solubility Rules for Salts
Always soluble:
 alkali ions, NH4+, NO3−, ClO3−, ClO4−, C2H3O2−, HCO3−
Generally soluble:
 Cl−, Br−, I−
Soluble except with Ag+, Pb2+, Hg22+
 F−
Soluble except with Pb2+, Ca2+, Ba2+, Sr2+, Mg2+
2−
 SO4
Soluble except with Pb2+, Ca2+, Ba2+, Sr2+
Generally insoluble:
 O2−, OH−
Insoluble except with Ca2+, Ba2+, Sr2+,
alkali ions, NH4+
 CO32−, PO43−, S2−, SO32−, CrO42−, C2O42−
Insoluble except with alkali ions and NH4+
Strong Acids
HCl, HBr, HI, HNO3, H2SO4, HClO3,
HClO4, HIO4
Strong Bases
LiOH, NaOH, KOH, RbOH, CsOH,
Ca(OH)2, Sr(OH)2, Ba(OH)2
Gases that Form
 H2S (g)
 H2CO3 (aq)  CO2 (g) + H2O (ℓ)
 H2SO3 (aq)  SO2 (g) + H2O (ℓ)
 NH4OH (aq)  NH3 (g) + H2O (ℓ)
South Pasadena • Honors Chemistry
Name
Semester 1 Final Exam
Period
PART C
•
Date
FREE RESPONSE (PRACTICE)
For each question, write your response in the space provided. If the problem requires mathematical computation,
show your work (steps) neatly, reporting your answer with the correct number of significant digits and units.
Partial credit is given only when the process taken is clearly shown. Place a box around or circle your final
answer.
 Unit conversions should be shown using dimensional analysis, showing how all units cancel out.
 Work for problems involving formulas should follow the I.E.S.A. form.
1. A particular compound containing only chlorine and oxygen is 52.56% chlorine by mass. The molar mass of
the compound is found to be between 60 and 70 g/mol.
a. Find the empirical formula for this compound. (4 points)
b. Find the molecular formula for this compound. (2 points)
2. Samples of the HBr, Mg(OH)2, and NH3 are obtained.
a. Complete the table for aqueous samples of each compound, predicting its color in cabbage juice and its
conductivity with a light bulb, and writing its dissociation equation. (12 points)
Compound
(i)
Cabbage Juice Color
[red | green | purple]
Conductivity
[bright | dim | dark]
Dissociation Equation
HBr
(ii) Mg(OH)2
(iii)
NH3
b. How many mL of a 7.00 M HBr solution is required to prepare 250 mL of 0.140 M HBr? (4 points)
c. The solubility of Mg(OH)2 at 20°C is 0.0014 g/100 g water. How many grams of water are needed to
dissolve 0.0112 g Mg(OH)2? (2 points)
3. Consider the following balanced reaction for the combustion of isopropyl alcohol, or 2-propanol, C3H8O (ℓ)
2 C3H8O (ℓ) + 9 O2 (g) → 6 CO2 (g) + 8 H2O (ℓ)
a. 4.05 g C3H8O is burned in air.
i. What volume (in L) of CO2 at STP can be produced? (4 points)
ii. If 4.25 L of CO2 was actually produced above, what was the percent yield of CO2? (2 points)
b. Suppose 50.0 g C3H8O and 50.0 g O2 are combined?
i. What is the theoretical yield of H2O in grams? (4 points)
ii. Identify the limiting and excess reactants. (2 points)
iii. How much (in grams) of the excess reactant remains if the reaction goes to completion? (4 points)