T1
1. Which of the following statements is false?
-chemistry is the science that deals with the materials of the universe
-a theory explains what happens, a law tries to explain why it happens
-quantitative observations have a number and a unit
–performing experiments is part of the scientific process
2. Write the following number in scientific notation:
249,100
2.491 x 10^5
3. Write the following number in ordinary decimal form:
4.22 x 10^-4
0.000422
4. How many significant figures are represented in the example below?
7.8100 x 10^3 g
5
5. Round off the following to 4 significant figures (record your answer in ordinary decimal
notation):
0.00886254
0.008863
6. What is the correct answer for the following:
(2.741 x 10^-2 g) ÷ (33.4 L) =
The correct answer should have correct units, the correct number of significant figures,
and be correctly rounded off.
-9.155 x 10^-1 g⋅L
-8.207 x 10^-4 g/L
-9.15 x 10^-1 g⋅L
-8.21 x 10^-4 g/L
7. Convert 6.09 x10^7 pm into m (10^12 pm = 1 m).
-6.09 x 10^-5 m
-6.09 x 10^19 m
-1.64 x 10^-9 m
-1.64 x 10^4 m
8. Convert 4.6 kilograms to grams.
4,600 g
9. If Ray Bradbury's famous novel "Fahrenheit 451" were translated into Celsius, what
would the title be?
"Celsius 233"
10. How many centimeters are in 448 miles?
Use the following EXACT conversions:
1 mile = 5280 foot
1 foot = 12 inches
1 inch = 2.54 cm
7.21 x 10^7 cm
11. Ivory soap floats on water because its density is 0.90 g/cm^3, which is less than the
density of water (water is 1.0 g/cm3). If an average bar of Ivory soap has dimensions 5.0
cm x 3.0 cm x 1.5 cm, what is the mass of the bar in grams? Don't forget your significant
figures!
20.0 g
12. The average mass of an M&M candy is 0.921 g. If you buy a 47.9 g bag of M&M's, how
many M&M's are in the bag?
52.0
13. A line of 2.31 x 10^6 atoms measures 412 micrometers. What is the diameter in
nanometers of a single atom in the line?
1 nanometer (nm) = 10^-9 m
1 micrometer (μm)= 10^-6 m
0.178 nm
14. An overdose of acetaminophen can lead to liver damage and death. The calculated dosage
for a child is 6 mg per pound based on their weight. If a child weighs 40 pounds, how
many 80 mg chewable tablets should they take?
3 Tablets
15. The boiling point of liquid hydrogen is -252.80 degrees Celsius. What is the
corresponding temperature in Kelvin? (Use 273.15 for conversion)
20.35 K
16. An ingot weighing 45.0 g is placed into a graduated cylinder containing 25.0 mL of
water. The water level subsequently rises to 28.9 mL. What is the density of the ingot in
g/cm^3 (note: 1 cm^3 = 1 mL)?
11.5 g/cm^3
17. Name whether it's a chemical or physical change.
Physical Changes: The window is broken, acetone vaporizes at 56 degrees Celsius.
Chemical Changes: Gasoline burns when a match is applied, fermentation of sugar to
alcohol.
18. Which of the following is an example of a homogeneous mixture?
-vinegar and oil salad dressing
-helium
-milk
-water
19. Which of the following is a characteristic of all types of matter?
-is rigid
-naturally occurring
-occupies space
-can be held in your hand
20. Matching elements to the element group:
Sodium: alkali metal
Ca: alkaline earth metal
Cl: halogen
Argon: noble gas
21. Write the symbol for the isotope below in A^ZX notation: An isotope of cesium that has
an atomic number of 55 and a mass number of 134.
55^134Cs
22. Which of the following is an example of an element that forms a diatomic molecule and
is a gas in its natural state?
-Hydrogen
-Iodine
-Sodium
-Neon
23. What is the formula for the neutral compound formed between the aluminum cation and
the chlorine anion?
-AlCl2
-AlCl
-AlCl3
-AlCl4
24. An isotope of strontium has a charge of 2+, a mass number of 90, and an atomic number
of 38.
Protons: 38
Neutrons: 52
Electrons: 36
25. An ion of a given element has 34 protons and 36 electrons.
Element: Se
Charge: -2
T2
1. Which of the following is an example of a binary ionic compound?
-dichlorine trioxide
-sulfur dioxide
-boron trifluoride
-aluminum chloride
2. What are the correct names for the following substances?
PbSO3: lead (II) sulfite
NaClO2: sodium chlorite
3. Indicate subscripts for the ionic solid formed by the pairs of cations and anions below:
iron(III) cation + sulfide anion --> Fe(x)S(y)
x= 2; y=3
magnesium cation + hydrogen carbonate anion --> Mg(x)(HCO3)(y)
x= 1; y= 2
4. What are the correct names for the following aqueous acids?
HNO3: nitric acid
HI: hydroiodic acid
5. Match the name of the following ions with the appropriate charge:
Ammonium: 1+
Hydrogen Phosphate: 2Aluminum: 3+
Peroxide: 26. Which of the following is an indication that a chemical reaction has occurred?
-reaction of cobalt(II) nitrate with hydrochloric acid results in a color change
-adding red food coloring to frosting causes a color change
-heating water to 100°C produces bubbles
-heating air in a balloon causes the balloon to rise
7. Which of the following statements about chemical equations is FALSE?
-subscripts are not used to balance chemical equations
-when writing a chemical equation, the products appear on the right and the
reactants on the left
-when writing an UNBALANCED chemical equation, the number and types of
atoms on the left side of the equation must be the same as on the right.
-when the coefficients on the left side of a BALANCED chemical equation are
doubled, the coefficients on the right side must also be doubled
8. Indicate the appropriate coefficients to balance the equation below. Please indicate a
numerical value for each blank as an integer, even if that value is "1"
_1__ Mn2O3 + __6__ HCl —--> __2___ MnCl3 + __3___ H2O
9. Which of the following corresponds to the correct UNBALANCED equation from the
reaction of solid calcium carbonate with aqueous hydrochloric acid to produce gaseous
carbon dioxide, liquid water, and aqueous calcium chloride.
-Ca(HCO3)2 (s) + HCl (aq) --> CO2 (g) + H2O (l) + CaCl2 (aq)
-CaCO3 (s) + HCl (aq) -->CO2 (g) + H2O (l) + CaCl2 (aq)
-CaCO3 (s) + HCl (aq) --> CO (g) + H2O (l) + CaCl2 (aq)
-CaCO3 (s) + H2SO4 (aq) --> CO2 (g) + H2O (l) + CaSO4 (s)
10. Balance the following chemical equation. Please indicate a numerical value for each
blank as an integer, even if that value is "1"
__4__ HCl (g) + _1_ O2 (g) -->__2__ H2O (g) + __2__ Cl2 (g)
11. Balance the equation below and sum the coefficients of the species:
iron (III) oxide reacts with hydrofluoric acid to produce iron (III) fluoride and water
The sum of the coefficients is: 12
12. Which of the following corresponds to the BALANCED total ionic equation for the
following UNBALANCED reaction:
CaCl2 (aq) + (NH4)2SO4 (aq) --> CaSO4 (s) + NH4Cl (aq)
-Ca^2+ (aq) + SO4^2- (aq) --> CaSO4 (s)
-Ba^2+ (aq) + 2 NO^3- (aq) + 2 NH^4+ (aq) + SO4^2- (aq) --> BaSO4(s) +
2NH^4+ (aq) + 2NO^3- (aq)
-Ca^2+ (aq) + 2 Cl^- (aq) + 2 NH^4 +(aq) + SO4^2- (aq) --> CaSO4 (s) +
2NH4Cl (aq)
-Ca^2+ (aq) + 2 Cl^- (aq) + 2 NH^4+ (aq) + SO4^2- (aq) --> CaSO4 (s) +
2NH^4+ (aq) + 2Cl^- (aq)
-Ca^2+ (aq) + Cl^- (aq) + NH^4+ (aq) + SO4^2- (aq) --> CaSO4(s) + NH^4+ (aq)
+ Cl^- (aq)
13. For the following molecular equation, which species are the spectator ions?
Pb(NO3)2 (aq) + K2HPO4 (aq) --> PbHPO4 (s) + 2 KNO3 (aq)
K^+ and NO3^14. You have three test tubes in front of you containing aqueous solutions of
MgCl2
Na2SO4
Pb(NO3)2
How many different compounds do you expect will precipitate when you combine the
three test tubes together? 2
15. What is the correct net ionic equation for the reaction of lead (II) nitrate and sodium
chloride?
Pb^2+ (aq) + 2Cl^- (aq) --> PbCl2 (s)
16. Which statement about strong electrolytes is TRUE?
-PbCl2 is an example of a strong electrolyte
-strong electrolytes form a precipitate in water
-strong acids and strong bases are strong electrolytes
-most carbonate salts are strong electrolytes
17. Which statement correctly describes the following equation?
2 Al (s) + 3Cl2 (g) --> 2AlCl3 (s)
this is an oxidation-reduction reaction in which each Al atom loses 3 electrons and each
Cl atom gains 1 electron.
18. Which of the following is the correct balanced equation for the combustion reaction of
acetylene (C2H2)?
2 C2H2 (g) +5 O2 (g) --> 4 CO2 (g) + 2 H2O (g)
19. Which of the following is an example of an oxidation-reduction reaction?
2 Al (s) + Fe2O3 (s) --> 2 Fe (s) + Al2O3 (s)
20. Which classification(s) correctly describe the following chemical equation:
2Li3N (s) --> 6Li (s) + N2 (g)
oxidation-reduction reaction, decomposition reaction
21. What salt is produced from the reaction of nitrous acid with calcium hydroxide?
Ca(NO2)2
22. Which of the options below correspond to the net ionic equation for the following
reaction:
HCl (aq) + KOH (aq) --> H2O (l) + KCl (aq)
H+ (aq) + OH- (aq) --> H2O (l)
23. Nomenclature is an important tool to learn to understand chemistry.
True.
T3
1. If you have 2.24 x 1022 atoms of Ba, how many moles of Ba do you have?
0.0372
2. How many molecules are in 1.28 grams of selenium dioxide?
6.95 x 10^21
3. Chemical analysis shows a molecule to be composed of 37.8% P, 58.5% O, and 3.7 % H.
What is the empirical formula? Fill in the blanks below.
P____O____H_____
4. A molecule with an empirical formula of HBO2 is known to have a molar mass of 175.3
g/mol. What is the molecular formula? Fill in the subscripts below.
H_4__B_4__O_8__
5. If 1.75 moles of oxygen are produced from the decomposition of NaBrO4 according to
the equation below, what was the starting mass of NaBrO4?
Molar masses: NaBrO4 = 166.89 g/mol; NaBr = 102.89 g/mol; O2 = 32.00 g/mol
NaBrO4 (s) --> NaBr (s) + 2O2 (g)
-146g
-73.0g
-292g
-260.0g
-90.0g
6. Consider the reaction:
2C2H6 (g) + 5O2 (g) + 4NH3 (g) --> 4HCN (g) + 5H2O (g)
If 76.10 g C2H6 is reacted with excess NH3 and O2, what mass of H2O can be
produced?
Molar masses: C2H6 = 30.07 g/mol; O2 = 32.00 g/mol; NH3 = 17.03 g/mol; HCN =
27.03 g/mol; H2O = 18.02g/mol
-172.6g
-114.0g
-45.60g
-228.0g
-18.24g
7. Consider the reaction:
3 CuO + 2Al --> 3Cu + Al2O3
Calculate the number of moles of Al2O3 that can form when 4.37 moles of Al reacts with
6.04 moles CuO.
2.01 moles
8. Refer to the following equation:
H2S (g) + 3F2 (g) --> SF4 (g)+ 2HF (g)
If you react 2.12 moles of F2 with excess H2S, what is the theoretical yield of SF4 in
grams?
If your actual yield of SF4 is 30.2 g, what is the percentage yield for this reaction?
Molar masses: H2S = 34.09 g/mol; F2 = 38.00 g/mol, SF4 = 108.07 g/mol, HF = 20.008
g/mol
9. How much heat is required to raise the temperature of an aluminum pan weighing 125 g
from -18.0 oC (freezer temperature) to 180.0 °C (oven temperature)?
Al specific heat capacity: s = 0.89 J/g° C
-3.45 x 10^4 J
-1.14 J
-2.20 x 10^4 J
-1.80 x 10^4 J
-2.48 x 10^4 J
10. A 50.0 g sample of water at 150 oC is added to a 50.0 g sample of water at 22.0°C. What
will be the final temperature of the water mixture?
86.0°C
11. A system absorbs 324 kJ of heat and performs 221 kJ of work. What is the DE for this
system?
+103 kJ
12. Combustion of C occurs according to the reaction below, for which DH = -394 kJ/mol of
carbon. What is the enthalpy change for a 47.5 g sample of carbon?
C (s) + O2 (g) --> CO2 (g)
–1560 kJ
13. Using the following thermochemical data:
P4(s) + 6 Cl2(g) → 4PCl3(g)
ΔH° = –2771 kJ/mol
P4(s) + 10 Cl2(g) → 4PCl5(g)
ΔH° = –3226 kJ/mol
calculate ΔH° for the following reaction:
PCl3(g) + Cl2(g) → PCl5(g)
14. Which of the following statements is true?
-The entropy of the universe is decreasing
-The total amount of energy in the universe is constant
-When spread energy is used to do work, the result is concentrated energy
-Solar energy is considered to be a non-renewable energy source
-Endothermic reactions give off heat
T4
1. The energy levels of the hydrogen atom (and all atoms) are ____, meaning that only
certain discrete energy levels are allowed.
-Quantized
2. The maximum number of electrons allowed in a single orbital is:
-2
3. The elements chlorine and iodine have similar chemical properties because they _____.
-have the same number of electrons in their outer energy levels.
4. What is the expected ground-state electron configuration for the iodide ion?
-[Kr]5s24d104f145p3
-[Ar]5s24d105p5
-[Kr]5s24d105p6
-[Kr]5s24d105p5
-[Kr]5s24d104f145p4
5. 1s22s22p63s23p64s23d10 is the electron configuration for which of the following atoms?
-Zn
6. Which of the following lists the elements in order of the smallest to the largest atomic
radius?
Cl < Si < Ge < Fe < Sr
7. In a nitrogen-chlorine bond, the bond is _____ and the _____ atoms bear _____ charge.
-nonpolar; Cl; no partial
-polar; N; a partial negative
-nonpolar; N; no partial
-polar; N; a partial positive
-polar; Cl; a partial positive
8. Which of the following statements is a correct description of the following reaction:
Ca (s) + Br2 (l) --> CaBr2 (s)
-Calcium gains two electrons to form Ca2+ and achieve the noble gas configuration [Ar];
Bromine loses two electrons to form 2Br- and achieve the noble gas configuration [Kr].
-Calcium gains two electron to form Ca2- and achieve the noble gas configuration [Ar];
Bromine loses two electrons to form Br22+ and achieve the noble gas configuration [Kr].
-Calcium gives up two electrons to form Ca2+ and achieve the noble gas configuration
[Ar]; Bromine gains two electrons to form 2Br- and achieve the noble gas configuration
[Ar].
-Calcium gives up two electrons to form Ca2+ and achieve the noble gas configuration
[Ar]; Bromine gains two electrons to form 2Br- and achieve the noble gas configuration
[Kr]
-Calcium gives up two electrons to form Ca2+ and achieve the noble gas configuration
[Ne]; Bromine gains two electrons to form Br22- and achieve the noble gas configuration
[Ar]
9. Which species is larger in each pair? i) Na+ or K+ ii) Ca2+ or Ca iii) F or F-K+, Ca, F10. Consider the Lewis dot structures for the following compounds and ions and
choose the best answer to the questions below (refer to the compound or ion by
its number in the drop-down list)
1. BH3
2. CO32-
3. NH3
4. CN-
Which of the following have multiple bonds?
Which of the following have resonance structures?
Which of the following violates the octet rule?
Which of the following is trigonal pyramid in shape?
11. Arrange the following elements in order of their increasing electronegativity.
-Rb< Ge< P < O
12. A 4.21 L sample of argon gas at 380. torr is compressed to a volume of 3.72 L at a
constant temperature. What is the final pressure in torr?
-430 torr
13. A balloon containing 847 mL helium gas at 25.0 oC is placed in a liquid nitrogen bath
and cooled to -196 oC at a constant pressure of 1.00 atm. What is the final volume of the
helium balloon?
-219mL
14. At constant temperature and pressure, a balloon containing 3.40 moles of hydrogen gas
has a volume of 2.07 L. If an additional 1.25 moles of hydrogen gas is added to the
balloon, what will the final volume be?
-0.761 L
-7.64 L
-1.51 L
-2.83 L
-0.353 L
15. A gas originally occupying 10.1 L at 0.925 atm and 25.0 °C is changed to 14.3 L at 100.
oC. What is the new pressure?
-0.818 atm
16. You combine 3.20 g of helium gas with 36.40 g of argon gas in a balloon at a pressure of
1.14 atm and a temperature of 29.7 C. What is the volume of the balloon in Liters?
-37.3 L
17. One of the most important characteristics of the water molecule is its ______________,
which allows it to surround and attract both positive and negative ions.
-Polarity