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Honors Chemistry FINAL Prep
Honors Chemistry FINAL Prep
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Honors Chemistry FINAL Prep
Flashcards
100 cards
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Practice quiz
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Questions
100
Answers
1
Solve: (5.6 × 10
7
m) x (3.60 x 10
–2
m) =
2.016 x 106 m2
3.157 x 106 m
2.189 x 103 m2
4.222 x 109 m
2
An increase in particle size speeds up a reaction.
True
False
3
Hess’s law allows you to determine the______ by using the known heats of two or more equations.
heat of formation
volume
mass
heat of reaction
4
Water has low specific heat, while metals generally have high specific heat.
False
True
5
What's the relationship between the 3 units of pressure? 1 atm = _____ mm Hg = _____ kpa
760, 101.3
720, 101.3
25, 101.5
760, 1.013
6
Which of the following ARE soluble in water?
nitrates
phosphates
sulfides
carbonates
7
92.5 g iron oxide reacts with CO. Fe
2
O
3
+ 3CO → 2Fe + 3CO
2
. What's the theoretical yield of Fe?
64.7g Fe
44.3g Fe
98.1g Fe
56.9g Fe
8
The products of a combustion reaction are:
NEVER carbon dioxide and water
ALWAYS carbon dioxide and water
ONLY produced in the absence of oxygen
SOMETIMES carbon dioxide and water
9
Place the particle size in these from smallest to largest: I.Suspension II.Colloid III.Solution
III, II, I
II, I, III
III, I, II
I, II, III
10
The following equation is balanced: C
3
H
8
+ 4O
2
→3CO
2
+ 4H
2
O.
False
True
11
In acidic soils, hydrangeas produce _________ flowers.
blue
white
pink
yellow
12
What is the proper name for the compound formed by calcium and sulfur?
calcium sulfide
dicalcium disulfide
calcium sulfite
calcium sulfur
13
A conversion factor:
all of the above
does not change the value of a measurement.
is a ratio of equivalent measurements.
is equal to 1.
14
An atom’s oxidation number is its charge if the electrons were assigned to a more _______ atom.
reduced
ionized
electronegative
oxidized
15
What is the theoretical energy that exists at absolute zero?
Zero kilopascals
Zero Kelvin
Zero degrees Celsius
Zero atmospheres
16
3NO
2
+ H
2
O → 2HNO
3
+ NO. How much NO
2
reacts with H
2
O to produce 7.48 X 10
22
molecules of NO?
12.5g NO2
22.3g NO2
19.5g NO2
17.1g NO2
17
What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL?
1.2 × 10–2 mL
86 mL
2.4 × 10–2 mL
42 mL
18
The structure of ice is a regular open framework of water molecules in a hexagonal arrangement.
False
True
19
The ______________ and ______________ points of a solid are at the same temperature.
vaporization, melting
freezing, vaporization
melting, freezing
freezing, condensation
20
Redox reactions are currently understood to involve any shift of _________ between reactants.
atoms
electrons
oxygen
protons
21
There are _______ classes of chemical reactions that refer to electron transfer.
2
4
1
3
22
A triprotic acid contains two ionizable hydrogens.
True
False
23
A _________ is a substance that speeds up a reaction, but is not used up in the reaction.
precipitate
none of the above
substrate
catalyst
24
If 4Al + 3O
2
→ 2Al
2
O
3,
how may moles of aluminum are needed to form 2.5 mol Al
2
O
3
?
5.00 mol Al
1.00 mol Al
10.00 mol Al
2.50 mol Al
25
The triple point on a phase diagram is determined by specific _________ and __________ .
None of the above
Pressure, temperature
Mass, pressure
Mass, temperature
26
The reaction in which water molecules produce ions is called the self-ionization of water.
False
True
27
Find the mass, in grams, of 5.26 x 10
-3
mol C
20
H
42
. Solve to 3 significant figures.
2.67 g
5.77 g
2.45 g
1.48 g
28
Which factor does NOT affect the rate of a chemical reaction?
concentration
temperature
particle size
molar mass
29
2C
2
H
2
+ 5O
2
→ 4CO
2
+ 2H
2
O. How much H
2
O can be produced by 2.66 mol of C
2
H
2
with 9.31 mol O
2
?
63.8g H2O
47.9g H2O
44.5g H2O
56.9g H2O
30
ALL of the Noble Gases have 8 valence electrons.
False
True
31
What was the first substance to be identified as a colloid?
mayonnaise
egg whites
glue
whipped cream
32
Which of the following is the correct scientific notation for 0.000 008 62?
8.62 x 10-6
86.2 x 10-7
8.62 x 106
86.2 x 107
33
CS
2
+ 3O
2
→ CO
2
+ 2SO
2
. Calculate the volume of SO
2
produced when 42.4 mL O
2
reacts with CS
2
.
3.71 mL SO2
45.7 mL SO2
28.3 mL SO2
63.55 mL SO2
34
Which of these measurements is expressed to three significant figures?
0.007m
7007 mg
0.070 mm
7.30 × 10–7 km
35
At STP, how many moles are in the volume of 89.6 L of SO
2
?
2,007.04 mol SO2
67.2 mol SO2
4.00 mol SO2
112 mol SO2
36
In collision theory, atoms, ions, and molecules can form products w/ enough SPONTANEOUS energy.
True
False
37
Any aqueous solution in which hydrogen ions and hydroxide ions are equal is a(n) ____________ .
acidic solution
basic solution
neutral solution
All of the above
38
Which of these statements is INCORRECT?
I. a strong acid and a weak base yield a neutral solution
III. a weak acid and a strong base yield a basic solution
II. a strong acid and a weak base yield an acidic solution
None of the above
39
Acids and bases are classified as strong or weak based on the degree they ionize in water.
False
True
40
A___ will form if the product of 2 ___ in the mixture is greater than the Ksp for the compound.
intermediate, ions
intermediate, reactants
precipitate, ions
catalyst, reactants
41
According to Lewis, _____ accepts pairs of electrons and _____ donates electrons in a reaction.
a base, an acid
hydrogen, hydroxide
an acid, a base
hydroxide, hydrogen
42
The equation H
3
PO
4
+ 3KOH →K
3
PO
4
+ 3H
2
O is an example of which type of reaction?
decomposition
single-replacement
combination
double-replacement
43
The numbers placed in front of formulas in an equation in order to balance it is called a ____.
subscript
all of the above
coefficient
reactant
44
Which of the following is NOT considered a colloid?
milk
marshmallow
blood
salt water
45
The quantity of heat absorbed by a ________ liquid is = the heat released when vapor condenses.
liquefying
condensing
solidifying
vaporizing
46
The actual order of a reaction must be determined by _______________ .
a reaction mechanism
collision theory
experiment
Le Chatelier’s principle
47
ALL chemical reactions consist of two or more elementary reactions.
False
True
48
Ionic compounds melt at a lower temperature than molecular compounds.
True
False
49
Solve: (1.7 × 10
–5
m) + (3.72 x 10
–4
m) =
4.96 m
3.11 x 104 m2
3.89 x 10-4 m
2.072 x 10-5 m
50
According to Le Chatelier’s principle, which stress would NOT upset equilibrium?
change in temperature
use of an intermediate
change in pressure
change in concentration
51
In Bronsted-Lowry Acid Base Theory, an acid is a H ion ____ and a base is a hydrogen ion ____ ?
acceptor, donor
neutralizer, donor
donor, neutralizer
donor, acceptor
52
The conversion of a gas to a solid is called _____ and from a solid to a gas is called _____ .
deposition, vaporization
deposition, sublimation
evaporation, sublimation
vaporization, condensation
53
The number of seconds in a 40-hour work week can be calculated as follows:
40 h x 60 min / 40 h x 60 s / 60 min
40 h x 60 min / 1 h x 60 s / 1 min =
60 s x 1 min / 60 sec x 1 h / 60 min =
1 s x 1 min / 60 s x 40 h / 60 min =
54
The ionic charge of all metals in group 1A is:
2
1
-1
0
55
The particles of atoms or molecules at any given temp. have a NARROW range of kinetic energy.
False
True
56
CaC
2
+ 2H
2
O → C
2
H
2
+ Ca(OH)
2
. How many moles of CaC
2
are needed to fully react with 57.1 g H
2
O?
3.88 mol CaC2
3.45 mol CaC2
1.96 mol CaC2
1.59 mol CaC2
57
Adding heat to a reaction BOTH increases entropy AND shifts reactions toward reactants.
False
True
58
A single-replacement reaction can be identified by:
an element and a compound on the right side of the equation
both a and b
an element and compound on the left side of the equation
none of the above
59
The Roman numeral in iron(II) ion refers to:
the specific positive charge of the ion
the group number
the number of atoms
the number of possible ionic charges it could have
60
H bonds in ice hold H
2
O molecules farther apart, in more ordered arrangements, than liquid H
2
O.
False
True
61
For reactions occurring at standard conditions, calculate the heat of reaction using ________ .
Hess’s Law
standard heats of formation
standard heats of reaction
molar heat of solution
62
A hydronium ion contains three hydrogens.
False
True
63
Substances that MOST READILY dissolve in H
2
O include molecular and nonpolar covalent compounds.
True
False
64
During any chemical or physical process, the energy of the universe
remains unchanged.
fluctuates consistently.
decreases.
increases.
65
Which of these equalities is
NOT
correct?
1000 mm = 1 m
1 cm3 = 1 mL
100 cg = 1 g
1 kg = 100 g
66
The quantity of heat absorbed by melting is the same as the heat released when the liquid ___.
liquefies
vaporizes
condenses
solidifies
67
How many zeros in the measurement 0.000 050 700m are significant?
3
2
8
7
68
Liquids and gases are BOTH known as condensed states of matter.
False
True
69
In a chemical equation, the _________ for a reaction can be written as a reactant or a product.
solution
enthalpy change
pressure constant
catalyst
70
Which name in the old system represents the copper ion with the highest charge?
copper(II) ion
cuprous ion
copper(III) ion
cupric ion
71
H's electronegative value is 2.1, O is 3.5, F is 4.0, Na is 0.9 and Cl is 3.0. Which is true?
All of the above
The bond between fluorine and fluorine is nonpolar
The bond between hydrogen and oxygen is very polar
The bond between sodium and chlorine is ionic
72
What two types of reactions are NOT redox-reactions?
double-replacement, acid-base
acid-base, single-replacement
combustion, decomposition
combination, double-replacement
73
There are a total of fourteen crystal structures and seven corresponding unit cells.
False
True
74
How can we name an ion of magnesium?
None of the above
Magnesium ion
Magneside ion
Magnesium anion
75
A double-replacement reaction takes place when K
2
SO
4
reacts with Pb(NO
3
)
2.
1 of the products is
PbSO4
CNO3
K2S
NaPb
76
How can you quantify the amount of a substance?
By mass.
By count.
By volume.
All of the above.
77
Catalysts permit reactions to proceed _______________
along a lower energy path.
along a higher energy path.
and decrease reactants needed.
and increase product yield.
78
What's the formula of a compound with the empirical formula CClN and molar mass of 184.5 g/mol?
C4Cl4N4
C3Cl3N3
C2ClN2
CClN2
79
Lowering temperature USUALLY slows down a reaction.
False
True
80
What is the oxidation number of carbon in the polyatomic ion CO
3
2-
?
-4
-3
+3
+4
81
How many atoms are in 1.14 mol of sulfur trioxide (SO
3
)?
2.75 x 1024 atoms
6.86 x 1023 atoms
1.89 x 1022 atoms
7.57 x 1022 atoms
82
The larger the solubility product constant, the larger the solubility of the compound.
True
False
83
What is the correct name for Cl
2
O
8
?
dichlorine octoxide
dichloride octoxide
dichlorine octaoxide
dichlorine nonoxide
84
Who was the chemist responsible for standardizing the way compounds are named?
Constantine Fahlberg
Fritz Haber
John Dalton
Antoine-Laurent Lavoisier
85
Early chemists saw oxidation as the combining of an element with ______ to produce a(n) ______.
oxygen, acid
hydrogen, acid
hydrogen, oxide
oxygen, oxide
86
Salts and acids accelerate corrosion by producing ______ that make(s) electron transfer easier.
conductive solutions
oxides
oxygen
ions
87
About what percent of Earth’s surface is covered in water?
75%
70%
80%
85%
88
Which of these statements is correct?
Increasing pressure shifts a reaction towards the reactants
Adding products shifts reactions towards the reactants
Spontaneous and nonspontaneous refer to rates of a reaction
All of the above
89
According to Arrhenius, ___ are compounds that yield H ions ___ are compounds yielding OH ions.
conjugate acids, conjugate bases
acids, bases
conjugate bases, conjugate acids
bases, acids
90
A __________ consists of two ions or molecules related by the loss or gain of one hydrogen ion.
Lewis acid
Arrhenius acid
Bronsted-Lowry base
conjugate acid-base pair
91
The volume of a gas varies with a change in ____________ or a change in __________ .
Pressure, temperature
Mass, pressure
Mass, temperature
None of the Above
92
Chemists use________to calculate how much reactant or how much product is formed in a reaction.
Avogadro’s number
stoichiometry
balanced chemical equations
percent yield
93
Ba(s) + HCl(aq) →BaCl
2
(aq) + H
2
(g) When balanced, the coefficient in front of HCl should be:
1
2
6
3
94
Which suffix is used to represent the polyatomic ion with the greater number of oxygen atoms?
Sulfide
Sulfic
Sulfate
Sulfite
95
Mg + 2HCL → MgCl
2
+ H
2
. Identify the excess reagent when 6.21 g HCl reacts with 5.13 g Mg.
H2
HCl
MgCl2
Mg
96
Rubber, plastic, asphalt, and glass are known as ________________ solids.
analogous
autotrophic
amorphous
allotropic
97
Gold and platinum are called _________ because they resist losing their electrons by corrosion.
alloys
alkali metals
noble metals
metal hydrides
98
A buffer solution is better able to resist drastic changes in pH than is pure water.
False
True
99
Binary molecular compounds are formed from
two nonmetallic elements.
two metals.
polyatomic ions.
a positively charged cation and a negatively charged anion.
100
What unique and important property of water results from hydrogen bonding?
high boiling point
high surface tension
low vapor pressure
all of the above
