Some more Regents Chemistry practice

1
Some more Regents Chemistry practice
2
What is the empirical formula of C3H6?
A CH
C CH3
D CH6
B CH2
3
Empirical formula is the simplified version of a
molecular formulaC3H6 divide by greatest
common factor (3) to get CH2
B
4
The name of the compound KClO2, is potassium
A chlorine oxide
C chlorate
D perchlorate
B chlorite
5
ClO2 is a polyatomic ion since there is more
than one capital lettergo to Table E and keep
it as is
B
6
What is the percent by mass of carbon in HC2H3O2
(gram-formula mass is 60)?
A 12 / 60 100
C 24 / 60 100
D 60 / 12 100
B 60 / 24 100
7
Table T comp by mass part /
whole 100Since there are TWO carbon atomsit
is 24 / 60 100
C
8
What is the total volume occupied by 6.5 moles of
CO2 (g)?
A 146 L
C 22.4 L
D 6.5 L
B 3.4 L
9
For ANY gas1 mole occupies 22.4 L6.5 mol
22.4 (L/mol) 146 L
A
10
The measure of the attraction for electrons in a
chemical bond is
C attractivity
A ionization energy
D electronegativity
B atomic radius
11
Electronegativityyou can look up those values
in Table S.Ionization energy is energy required
to remove an electron.
D
12
Given the equationH2 Cl2 ? 2 HClHow
many moles of HCl will be produced when 3 moles
of H2 is completely consumed?
A 3 moles
C 6 moles
D 0.7 moles
B 2 moles
13
H2 Cl2 ? 2 HClSet up a
ratioeqn 1 2
? 3 x
C
14
What type of bond exists between an atom of
carbon and an atom of fluorine?
A ionic
C polar cov.
D nonpolar cov.
B metallic
15
Has to be covalent because two nonmetalsLook
up electronegativity values in Table S to see to
that the difference is greater than 1.Polar
e- shared UNequallyNonpolar e- shared
equally
C
16
Which is held together by metallic bonds?
A NaCl
C CO
D Br2
B Fe
17
Metallic bonding look for the metalFe
B
18
The primary forces of attraction between water
molecules in H2O are
A ionic
C molecule-ion
D van der Waals
B hydrogen
19
Water molecules held together by hydrogen
bondingremember surface tension?floating a
razor blade?
B
20
Which substance contains nonpolar covalent bonds?
A H2
C Ca(OH)2
D CaO
B H2O
21
Covalent must be two NONMETALSNonpolar
electrons shared equallyelectronegativity
difference less than 1.
A
22
What describes the electron dot structure of
CaCl2?
A brackets without charges
C brackets with charges
D no brackets, but charges
B no brackets, no charges
23
CaCl2 is ionic (metal and nonmetal) so needs
brackets AND charges
C
2
-1
-1






Ca
Cl
Cl
(gained 1 e-)
(gained 1 e-)
(lost 2 e-)
24
Which statement best describes the following
reaction?Cl Cl ? Cl2 energy
A bond formed energy released
C bond formed energy absorbed
B bond broken energy released
D bond broken energy absorbed
25
Two reactants become one productbond is
formedEnergy is on the product sideenergy is
released
A
26
The modern model of the atom shows that electrons
are
A orbiting nucleus in fixed paths
C found in regions called orbitals
D located in a solid sphere covering nucleus
B combined with neutrons in the nucleus
27
Modern model of atom wave-mechanical model
ORelectron cloud modelorbital probable
locations of e-
C
28
What is atomic number of an element that has 6
protons and 8 neutrons?
A 6
C 8
D 14
B 2
29
Atomic number number of protons
A
30
What is the total number of protons contained in
the nucleus of a carbon-14 atom?
A 6
C 12
D 14
B 8
31
The 14 in carbon-14 represents the mass number
(protons neutrons). If the atom is
carbonlook up its atomic number.
A
32
Which of these elements has an atom with the most
stable outer electron configuration?
A Ca
C Na
D Ne
B Cl
33
Look for the noble gases in group 18They have
full valence shells. (2 e- for He, 8 e- for the
rest)
D
34
What is the nuclear charge of an iron atom?
A 30
C 56
D 82
B 26
35
Protons and neutrons are in nucleus. Protons are
positive and neutrons are neutral...making the
charge on the nucleus positive. Look up atomic
number of iron 26.
B
36
How many electrons are in the outermost principal
energy level of an atom of bromine in the ground
state?
A 35
C 2
D 8
B 7
37
Look up the number of valence e-Electron
config 2-8-18-7Valence e- are last number
7Group 17 has 7 valence e-.
B
38
Which electron configuration is correct for a
sodium ion?
A 2-7
C 2-8
D 2-8-2
B 2-8-1
39
Na electron config as an ATOM is2-8-1It is in
group 1 and will lose its 1 valence e- to become
stable.
C
40
The nucleus of which atom contains 48 neutrons?
32 A S 16
85 C Rb 37
112 D Cd 48
48 B Ti 22
41
Mass number is top number protons
neutronsAtomic number is bottom number
number of protons(protons neutrons)
(protons) NEUTRONS
C
42
When an atom loses an electron, the atom becomes
an ion that is
A () and larger
C () and smaller
D (-) and smaller
B (-) and larger
43
Losing e- () charge (look at oxidation
state)When you lose weight, for example, you
become smallerthe same goes for atoms ions.
C
44
Spectral lines of elements are caused when
electrons in an excited state move from
A low to high energy levels, absorbing energy
C low to high energy levels, releasing energy
D high to low energy levels, releasing energy
B high to low energy levels, absorbing energy
45
An atom absorbs energyelectron jumps to higher
energy level.(excited state)When the electron
falls back to a lower energy level, energy is
released in the form of light.(back to ground
state)
D
46
What happens when NaCl is dissolved in water?
A Na ions attracted to O atoms of water
C Cl- ions attracted to O atoms of water
D Cl- ions are repelled by the H atoms of water
B Na ions are repelled by the O atoms of water
47
Oxygen atoms have a partial negative charge so
the Na ions are attracted to that side of the
water molecule.
A
48
According to Table G, which solution at
equilibrium contains 50 g of solute per 100 g of
water at 75C?
A unsaturated solution of KCl
C unsaturated solution of KClO3
D saturated solution of KClO3
B saturated solution of KCl
49
Saturated solution is when falls right on the
curve.Go over to 75 degrees and up to 50 g of
solute.
B
50
Which compound is least soluble in 100 g of water
at 40C?
A SO2
C KClO3
D NH4Cl
B NaCl
51
When you go over to 40 degrees and then upSO2
is the first solute you run into,which means it
is the least soluble.
A
52
What is the total number of moles of solute in
2.0 L of 3.0 M NaOH?
A 6 moles
C 3 moles
D 1 mole
B 2 moles
53
When you see M head to Table Tmolarity
(moles) / (liters) x 3
2
A
54
Real gases are like ideal gases at
A high pressure low temp
C high pressure high temp
D low pressure high temp
B low pressure low temp
55
At high temps, particles move fast and have less
chance of attracting each otherAt low
pressure, particles wont be so squished
together and will be less likely to attract each
other.
D
56
As the temperature of a given sample of gas
decreases at constant pressure, the volume of the
gas
A decreases
C increases
D smells
B remains the same
57
Temperature and volume have a direct
relationshipthey both increaseorthey both
decrease.
A
58
2.0 L of CH4 and 2.0 L of O2 have the same
A density
C mass
D of atoms
B of molecules
59
They have the same volume sothey have the same
of molecules since they have the same of
moles.(6.02 x 1023 molecules in a mole)
B
60
Which phase is endothermic?
A gas ? solid
B gas ? liquid
C liquid ? solid
D liquid ? gas
61
Endothermicabsorb energy.A liquid must
absorb energy to become a gas.
D
62
What happens to average kinetic energy if
temperature is increased?
A increases
C remains the same
B decreases
63
Think of average kinetic energy and temperature
as the same thing
A
64
What happens to temperature as water freezes?
A decreases
C remains the same
B increases
65
Temperature (average kinetic energy) remains the
same during a phase changeonly potential
energy changes during a phase change.
C
66
Elements in a given period contain the same
number of
A protons
C valence e-
D of energy levels
B neutrons
67
Going across period 4every element has 4 energy
levels.Examples 2-8-8-1 2-8-18-6
D
68
Atoms of metals tend to
A lose e- and form (-) ions
C gain e- and form (-) ions
D gain e- and form () ions
B lose e- and form () ions
69
Metals only have a few valence e- and want to
lose e-.Look at the oxidation for metalsthey
are positive.
B
70
Which two elements have chemical properties that
are most similar?
A Cl and Ar
C K and Ca
D C and N
B Li and Na
71
Elements in the same group have the same of
valence e-.Elements with the same of valence
e- have similar chemical properties.
B
72
If M represents an alkali metal, what is the
formula for the compound formed by M and oxygen?

A MO2
C M2O3
D M3O2
B M2O
73
Alkali metals Group 1Group 1 form 1
ionsM1O-2criss-crossM2O
B
74
As elements of Group 15 are considered from top
to bottom, the metallic character of the atoms
A increases
C remains the same
B decreases
75
Metallic character increases as you go down a
group.
A
76
Which Group 15 element exists as a diatomic
molecule at STP?
A phosphorus
C nitrogen
D arsenic
B bismuth
77
Remember HOF BrINCl?Hydrogen, oxygen,
fluorine, bromine, iodine, nitrogen, chlorine
C
78
Properties of nonmetal atoms include
A low ionization energy and low
electronegativity
C high ionization energy and low
electronegativity
D high ionization energy and high
electronegativity
B low ionization energy and high
electronegativity
79
Ionization energy energy required to remove
e-.High ionization energy because nonmetals
want to GAIN, not lose e-. Electronegativity
attraction for e- when in a bond.High
electronegativity because nonmetals pull harder
on e-.JUST USE TABLE S!!!
D
80
A redox reaction always demonstrates the
conservation of
A mass
C charge
D both mass and charge
B neither mass or charge
81
Both mass and charge will be conserved.
D
82
What occurs when an atom is oxidized?
A loss of e- and an increase in oxidation number
C gain of e- and an increase in oxidation number
D gain of e- and a decrease in oxidation number
B loss of e- and a decrease in oxidation number
83
GGGRRRRR.Gain reduction(charge
reduced)Lose oxidation(charge icnreases
think of when metals lose e-)
A
84
An electrochemical setup consists of two
half-cells, an anode, a cathode, an external
circuit, and a salt bridge. When a rxn occurs,
ion migration takes place through the?
A anode
C salt bridge
D external circuit
B cathode
85
Ions pass through salt bridgeElectrons pass
through external circuit.
C
86
The decomposition of water is forced to occur by
use of an externally applied electric current.
This procedure is called
A neutralization
C esterification
D hydrolysis
B electrolysis
87
If an outside power source is needed to get a
chemical reaction to occur, it must be an
electrolytic cell. Decomposing water is called
electrolysis.
B
88
Which description is correct for a voltaic cell?

A spontaneous anode is (-)
C spontaneous anode is ()
D nonspontaneous anode is ()
B nonspontaneous anode is (-)
89
Voltaic cells do NOT need an outside power
source, which means they are spontaneous.VANvol
taic anode is negative.(opposite for
electrolytic)
A
90
Given the reaction Zn HCl ? ZnCl2 H2
The oxidation number of H1
decreases because it
A loses protons
C loses electrons
D gains electrons
B gains protons
91
If charge decreases, H1 must have been
reduced.Remember gaining negative electrons
makes it more negative.
D
92
Which reaction occurs when equivalent quantities
of H and OH- are mixed?
A oxidation
C neutralization
D hydrolysis
B reduction
93
Equal amounts of hydrogen ions and hydroxide ions
makes a solution neutralpH 7.
C
94
What is the pH of a 0.01 M solution of KOH?
A 1
C 12
D 13
B 2
95
Two steps1. KOH is a baseOH- 0.01
so pOH is 2.2. 14 pOH pH
14 2 12
C
96
The H3O of a solution is 1 x 10-8. This
solution has a pH of
A 6, which is acidic
C 6, which is basic
D 8, which is acidic
B 8, which is basic
97
H3O is the hydronium ionthink of it like the
H ion. Just take the exponent and that will
be the pH8.0 7 is acidic 7 14 is
basic
B
98
How many mL of 0.20 M KOH are needed to
completely neutralize 90.0 mL of 0.10 M HCl?
A 25 mL
C 90 mL
D 180 mL
B 45 mL
99
Table Ttitration equation.MAVA MBVB
(0.1) (90) (0.2) X
B
100
If a given solution contains H 1 x 10-9,
what is the OH-?
A 1 x 10-5
C 1 x 10-14
D 1 x 10-1
B 1 x 10-9
101
The exponents need to add up to 14 1 x 10-5
A
102
Which compound is a strong Arrhenius base?
A C2H5OH
C HOH
D NaOH
B CH3OH
103
Go to Table L for bases and Table K for
acidsthey are usually in those tables.HOH is
water, both CH3OH and C2H5OH are alcohols.
D
104
Methyl orange is used to test a solution. If it
turns red, what could the pH value be?
A 3.0
C 4.4
D 8.6
B 4.0
105
Go to Table M for indicator questions.3.2 -
4.4red - orange - yellow
A
106
Which statement best describes the solution
produced when an Arrhenius acid is dissolved in
water?
C only () ion in solution is NH4
A only (-) ion in solution is OH-
D only (-) ion in solution is HCO3-
B only () ion in solution is H
107
Acids produce H ions.Bases produce OH-
ions.
B
108
Which formula represents a saturated compound?
A C2H4
C C2H2
D C3H8
B C3H6
109
Only alkanes are saturatedsaturated
hydrocarbons have the most hydrogens
possiblethe compound needs all single bonds.
D
110
What describes two isomers of a hydrocarbon?
A same formula, same structure
C same formula, different structure
D different formula, same structure
B different formula, different structure
111
Isomers have the same formula, but the atoms are
arranged differently.Two isomers of pentane
will both have 5 carbons and 12 hydrogensthey
will just be arranged differently.
C
112
What is the maximum number of covalent bonds that
can be formed by one carbon atom?
A 1
C 3
D 4
B 2
113
Carbon has 4 valence electrons and will need to
form 4 bonds to complete its valence shell.
D
114
A compound with the formula CH3CH2OH is
classified as an
A alkane
C alkene
D acid
B alcohol
115
Table Rthe OH functional group makes it an
alcohol.
B
116
How many bromine atoms are in the compound
1,1-dibromopropane?
A 1
C 3
D 4
B 2
117
Di- means 2.The 1,1 tells you location of
each of the bromine atoms. So you can count the
numbers also.
B
118
Which formula represents ethanoic acid?
A CH3CHO
C CH3COOH
D CH3CH2CHO
B CH3CH2COOH
119
Eth- means two carbons.Table R-COOH
functional group means organic acid.
C
120
What is the name of the chemical reaction when
glucose decomposes into carbon dioxide and
ethanol?
A fermentation
C substitution
D combustion
B addition
121
Fermentationdecomposition would also work.
A
122
When radium-226 undergoes natural transmutation,
it emits
A an alpha particle
C a position
D a neutron
B a beta particle
123
Table Nfind radium-226 and look for decay
mode.
A
124
Which type of radiation has zero mass and zero
charge?
A alpha
C gamma
D neutron
B beta
125
Table O...0 ? 0
C
126
What type of radiation has the weakest
penetrating power?
A alpha
C gamma
D neutron
B beta
127
Alpha particles are big and slow and wont pass
through paper.
A
128
What type of radiation has the weakest In how
many days will a 12 g sample of iodine-131 decay,
leaving 1.5 g of the original isotope?
A 8
C 20
D 24
B 16
129
Four half-lives1 12 62 6 33
3 1.5
D