TRUE/FALSE
1. There are 6.02  1023 molecules in one mole of water only when the water is in the liquid state.
ANS: F
REF: K/U
OBJ: 4.3
LOC: QC1.01
2. Helium has a mass that is one-third the mass of a carbon-12 atom.
ANS: T
REF: K/U
OBJ: 4.2
LOC: QC1.02
3. The relative proportion of stable isotopes of an element is referred to as the element's isotopic
abundance.
ANS: T
REF: K/U
OBJ: 4.2
LOC: QC1.02
4. C2H4, C3H6, C5H10, C10H20, are all possible empirical formulas for CH2.
ANS: F
REF: K/U
OBJ: 4.6
LOC: QC1.03
5. The empirical formula of a compound is the formula that yields the simplest ratio between the
atoms of the elements in a compound.
ANS: T
REF: K/U
OBJ: 4.6
LOC: QC1.03
6. The SI unit for measuring the amount of any substance is the gram.
ANS: F
REF: C
OBJ: 4.3
LOC: QC2.01
7. One mole of ammonia, NH3, is made up one atom of nitrogen and three atoms of hydrogen.
ANS: F
REF: K/U
OBJ: 4.3
LOC: QC1.01
8. The formula for potassium sulphate, K2SO4, is both an empirical and a molecular formula.
ANS: T
REF: K/U
OBJ: 4.6
LOC: QC1.03
OBJ: 4.6
LOC: QC1.03
9. C2H4O2 is the empirical formula for glucose.
ANS: F
REF: K/U
10. If the percentage, by mass, of nitrogen in ammonia, NH3, is 82.4%, then 100 g of ammonia
contains 17.6 g of hydrogen.
ANS: T
REF: I
OBJ: 4.5
LOC: QC2.02
11. The percentage composition of a compound can only be calculated with knowledge of the
compound's formula.
ANS: F
REF: K/U
OBJ: 4.5
12. One mole of chlorine gas contains 6.02  1023 atoms of chlorine.
LOC: QC2.02
ANS: F
REF: K/U
OBJ: 4.3
LOC: QC1.01
13. The mass of one formula unit of sodium chloride is the sum of the mass of one sodium ion and
one chloride ion.
ANS: T
REF: K/U
OBJ: 4.3
LOC: QC2.01
14. One mole of fluoride ions has almost the same mass as one mole of fluorine atoms.
ANS: T
REF: K/U
OBJ: 4.3
LOC: QC2.01
15. The SI unit for molar mass is g/mol, while its SI symbol is mm.
ANS: F
REF: C
OBJ: 4.3
LOC: QC2.01
16. Oxygen, nitrogen, chlorine, and helium are all elements that form diatomic molecules.
ANS: F
REF: C
OBJ: 4.3
LOC: QC2.01
17. The subscripts in a molecular formula can be determined from the mole ratio of the elements in
the compound.
ANS: T
REF: K/U
OBJ: 4.7
LOC: QC1.03
18. A mass spectrometer is a device for determining the relative masses of individual atoms.
ANS: T
REF: C
OBJ: 4.7
LOC: QC2.01
19. Using percentage composition, a chemist can only deduce the ratio of atoms or ions, not the
actual number.
ANS: T
REF: K/U
OBJ: 4.7
LOC: QC1.03
20. Two compounds can have identical percentage compositions.
ANS: T
REF: K/U
OBJ: 4.6
LOC: QC2.02
TRUE/FALSE
1. Mole ratios that relate reactants to products can be constructed from the coefficients in a balanced
chemical equation.
ANS: T
REF: K/U
OBJ: 5.2
LOC: QC1.05
2. The amount of excess reagent dictates the amount of product formed in a chemical reaction.
ANS: F
REF: K/U
OBJ: 5.1
LOC: QC1.05
3. In any chemical reaction, the theoretical yield will be less than or equal to the actual yield.
ANS: F
REF: K/U
OBJ: 5.6
LOC: QC2.01
4. In a chemical reaction that involves two reactants, the limiting reagent is identified as the reactant
that is entirely consumed.
ANS: T
REF: K/U
OBJ: 5.1
LOC: QC1.05
5. The number of molecules is always conserved in a chemical reaction.
ANS: F
REF: C
OBJ: 5.2
LOC: QC2.05
6. A gamma ray has no mass and carries a negative charge.
ANS: F
REF: K/U
OBJ: 5.3
LOC: QC2.01
7. Transmutation occurs when atoms of one element are changed into another element.
ANS: T
REF: K/U
OBJ: 5.3
LOC: QC2.06
8. The percentage yield is the actual amount of a product expressed as a percentage of the calculated
theoretical yield of that product.
ANS: T
REF: K/U
OBJ: 5.6
LOC: QC2.01
9. If 165.0 g of silver iodide was produced in a reaction for which the theoretical yield was 192.0 g,
the percentage yield is 85.94%.
ANS: T
REF: I
OBJ: 5.6
LOC: QC2.08
10. Producing sodium carbonate using the Leblanc process was proven to be very expensive,
inefficient, and harmful to the environment.
ANS: T
REF: MC
OBJ: 5.7
LOC: QC3.01
11. The following is an example of a balanced chemical equation:
2AgNO3 + CaCl2
2AgCl + Ca(NO3)2
ANS: T
REF: K/U
OBJ: 5.2
LOC: QC2.05
12. Consider the following chemical equation: Mg + H3PO4
H2 + Mg3(PO4)2
When this equation is properly balanced, the coefficient of hydrogen phosphate, H3PO4, will be 2.
ANS: T
REF: K/U
OBJ: 5.2
LOC: QC2.05
13. The following is an example of a balanced chemical equation:
Na2SO3 + H2SO4
Na2SO4 + H2O + 2SO2
ANS: F
REF: K/U
OBJ: 5.2
LOC: QC2.05
14. A balanced chemical equation has the same number of each type of atom on each side of the
equation.
ANS: T
REF: C
OBJ: 5.2
LOC: QC2.05
15. Consider the following chemical equation: KClO3 + HCl
KCl + ClO2 + Cl2 + H2O
When this equation is properly balanced, the coefficient of potassium chloride, KCl, will be 4.
ANS: F
REF: K/U
OBJ: 5.2
LOC: QC2.05
16. An alpha particle can be stopped by 4 cm of air or by a sheet of paper.
ANS: T
REF: K/U
OBJ: 5.3
LOC: QC2.01
17. The following represents a properly balanced nuclear equation:
+
ANS: T
REF: K/U
OBJ: 5.3
LOC: QC2.06
18. The following represents a properly balanced nuclear equation:
+
+
ANS: T
REF: K/U
OBJ: 5.3
19. The symbol used to represent a beta particle is
ANS: T
REF: K/U
LOC: QC2.06
.
OBJ: 5.3
LOC: QC2.01
20. Alpha decay is properly illustrated in the following nuclear equation:
+
ANS: T
COMPLETION
REF:
K/U
OBJ:
5.3
1. The law of definite proportions was initially stated by ____________________.
ANS: Joseph Proust
LOC: QC1.04
REF: K/U
OBJ: 4.1
2. A(n) ____________________ formula shows the ratio between the number of atoms in a
substance in its simplest terms.
ANS: empirical
LOC: QC1.03
REF: K/U
OBJ: 4.6
3. _________________________ describes the proportion of stable isotopes of an element.
ANS: Isotopic abundance
LOC: QC1.02
REF: K/U
OBJ: 4.2
4. The actual number of atoms that make up a molecule is shown by a(n) ____________________
formula.
ANS: molecular
LOC: QC1.03
REF: K/U
OBJ: 4.6
5. A(n) ____________________ is the standard unit used to represent the chemical quantity of any
substance.
ANS: mole
LOC: QC2.01
REF: C
OBJ: 4.3
6. CH2O is the ____________________ formula of C6H12O6.
ANS: empirical
LOC: QC1.03
REF: K/U
OBJ: 4.6
7. Bromine, Br2, iodine, I2, and hydrogen, H2, are examples of ____________________ elements.
ANS: diatomic
LOC: QC2.01
REF: C
OBJ: 4.3
8. The empirical formula for acetic acid, CH3COOH, is ____________________.
ANS: CH2O
LOC: QC1.03
REF: K/U
OBJ: 4.6
9. The symbol used to represent Avogadro's constant is ____________________.
ANS: NA
LOC: QC2.01
REF: C
OBJ: 4.3
10. The mass of an element in a compound divided by the total mass of that compound, then
multiplied by 100 is known as ______________________________.
ANS: percentage composition
LOC: QC2.01
REF: K/U
OBJ: 4.5
11. The number of particles found in 12 g of carbon, 40 g of sodium hydroxide, or 18.0 g of water is
equivalent to ____________________.
ANS: 6.02  1023
LOC: QC1.01
12. One atomic mass unit is defined as exactly
ANS: C-12 atom
REF: C
OBJ: 4.3
the mass of a(n) ____________________.
REF: C
OBJ: 4.2
LOC: QC1.02
13. Gold and oxygen can combine to form two compounds of different combining proportions.
Resulting formulas of these compounds include Au2O and ____________________.
ANS: Au2O3
LOC: QC1.04
REF: K/U
OBJ: 4.1
14. The ratio of hydrogen to oxygen, by mass, in hydrogen peroxide is ____________________.
ANS: 1:16
LOC: QC2.01
REF: C
OBJ: 4.1
15. The total number of atoms present in 1 mol of gold is ____________________.
ANS: 6.02  1023
LOC: QC2.03
COMPLETION
REF: I
OBJ: 4.4
1. A(n) ____________________ reagent is the only reagent left over when all other reagents have
been consumed in a chemical reaction.
ANS: excess
LOC: QC1.05
REF: K/U
OBJ: 5.1
2. A(n) ____________________ reaction is a type of nuclear reaction in which lightweight nuclei
are combined to form a larger nucleus.
ANS: fusion
LOC: QC2.06
REF: C
OBJ: 5.3
3. A(n) ____________________ is a reagent that is completely consumed in a reaction and thereby
limits the amount of product(s) that is/are formed.
ANS: limiting reagent
LOC: QC1.05
REF: K/U
OBJ: 5.1
4. A(n) ____________________ ray is a quantum of energy of very high frequency and very short
wavelength.
ANS: gamma
LOC: QC2.06
REF: C
OBJ: 5.3
5. When a balanced chemical equation is used to calculate the maximum amount of product that
should form during a reaction, the value obtained is called the _________________________.
ANS: theoretical yield
LOC: QC2.01
REF: K/U
OBJ: 5.6
6. Once a chemical reaction is actually carried out, the ratio of the actual yield to the theoretical
yield is known as the _________________________.
ANS: percentage yield
LOC: QC2.01
REF: K/U
OBJ: 5.6
7. A nuclear reaction where an atom is split into two approximately equal parts is known as
____________________.
ANS: fission
LOC: QC2.06
REF: C
OBJ: 5.3
8. The most popular method used to produce sodium carbonate in industry in the 1700s and the
1800s was later proven inefficient and harmful to the environment. This method of producing
sodium carbonate was known as the _________________________.
ANS: LeBlanc process
LOC: QC3.01
REF: MC
OBJ: 5.7
9. The Solvay process was an effective and efficient method used in the late 1800s to produce
____________________.
ANS: sodium carbonate
LOC: QC3.01
REF: MC
OBJ: 5.7
10. The elementary particles located inside the nucleus are called ____________________.
ANS: nucleons
LOC: QC2.06
REF: K/U
OBJ: 5.3
11. A symbol that can be used to represent a proton in a nuclear equation is
that identifies the same particle is ____________________.
ANS:
LOC: QC2.06
REF: C
. An alternate symbol
OBJ: 5.3
12. The process whereby an element changes its identity when its nucleus is struck with other nuclear
particles or nuclei is referred to as _________________________.
ANS: artificial transmutation
LOC: QC2.06
REF: K/U
OBJ: 5.3
13. ____________________ is the calculation of the quantities of reactants and products involved in
a chemical reaction.
ANS: Stoichiometry
LOC: QC2.01
REF: K/U
OBJ: 5.4
14. To help interpret scientific data collected in the lab, scientists will use graphs and compare their
data against graphs that have been constructed using known values. A type of graph that uses
known values is called a ____________________.
ANS: standard curve
LOC: QC3.03
REF: MC
OBJ: 5.1
15. The process whereby an unstable nucleus emits a high-speed electron is called
____________________.
ANS: beta decay
LOC: QC2.06
REF: K/U
OBJ: 5.3
1.What is the significance of the mole and how does it help chemists?
2.Describe how the law of definite proportions was developed and explain its significance to the
formation of the atomic theory.
3.Outline and describe the application of chemical quantities and calculations in prescription drug
dosages.
4.The elements hydrogen and oxygen can be combined to form H20 or H2O2. Compare some of the
properties and uses of H20 and H2O2 and briefly outline the variables that determine them.
5.Identify three careers which rely on knowledge of analyzing unknown substances. For each career,
explain why their ability to analyze unknown substances is so important.
1.Identify two applications of nuclear chemistry and outline the role each application plays in society.
2.Compare and contrast a CANDU reactor with a typical nuclear fission reactor.
3.Outline the significance of stoichiometry in industry and explain how it helps chemical
manufacturers.
4. Distinguish between alpha, beta, and gamma radiation.
5.Distinguish between nuclear fission and nuclear fusion.