WorksheetsCHEM REGENTS PREP APRIL 2018
Total questions: 106
Worksheet time: 3hrs 33mins
Name
Class
Date
1.
Which sample of matter has a indefinite volume and indefinite shape?
a)
Hg(l)
b)
NaCl(s)
c)
H2O(l)
d)
CH4(g)
2.
Which change occurs during a nuclear fission reaction?
a)
Nuclei are split into two new nuclei
b)
Isotopes are converted to isomers.
c)
Temperature is converted to mass.
d)
Nuclei are combined to form one new nuclei
3.
The valence electrons in an atom of oxygen in the ground state are all found in
a)
1st shell
b)
2nd shell
c)
3rd shell
d)
4th shell
4.
Which substance can not be broken down by a chemical change?
a)
propanol
b)
copper
c)
benzene
d)
ammonia
5.
Which subatomic particles are found in orbitals of an atom of beryllium?
a)
electrons and protons
b)
electrons and positrons
c)
electrons only
d)
neutrons and protons
6.
Which conclusion was drawn from the results of the gold foil experiment?
a)
An atom is electrically neutral
b)
The electrons in an atom are located in specific shells
c)
The nucleus of an atom is negatively charged
d)
An atom is mostly empty space
7.
Which electron configuration represents an excited state for an atom of calcium?
a)
2-8-7-1
2-8-7-1
b)
2-8-7-2
2-8-7-2
c)
2-8-7-3
2-8-7-3
d)
2-8-8-2
8.
Which conclusion was drawn from the results of the gold foil experiment?
a)
An atom is electrically neutral
b)
The electrons in an atom are located in specific shells
c)
The nucleus of an atom is negatively charged
d)
An atom is mostly empty space
9.
What is the number of electrons in an atom of scandium?
a)
21
b)
24
c)
45
d)
66
10.
Which ion has NO electrons?
a)
H+
b)
Li+
c)
Na+
d)
Rb+
11.
Which type of reaction converts one element to another element?
a)
neutralization
b)
polymerization
c)
synthesis
d)
transmutation
12.
Which nuclear emission has no charge and no mass?
a)
alpha particle
b)
beta particle
c)
gamma ray
d)
positron
13.
The amount of energy released from a fission reaction is much greater than the energy released from a chemical reaction because in a fission reaction
a)
mass is converted into energy
b)
energy is converted into mass
c)
ionic bonds are broken
d)
covalent bonds are broken
14.
Which sample of matter sublimes at room temperature and standard pressure?
a)
Br2(l)
b)
Cl2(g)
c)
CO2(s)
d)
SO2(aq)
15.
At STP, which physical property of aluminum always remains the same from sample to sample?
a)
mass
b)
density
c)
length
d)
volume
16.
Which statement describes a chemical property of silicon?
a)
Silicon is blue-gray
b)
Silicon is a brittle solid
c)
Silicon melts at 1414 C
d)
Silicon reacts with fluorine.
17.
A compound is a substance composed of two or more elements that are
a)
physically mixed in a fixed proportion
b)
physically mixed in a variable proportion
c)
chemically combined in a fixed proportion
d)
chemically combined in a variable proportion
18.
Which substance can be decomposed by chemical means?
a)
carbon
b)
vanadium
c)
germanium
d)
methane
19.
The temperature of a sample of matter is a measure of the
a)
average potential energy of the particles of the sample
average potential energy of the particles of the sample
b)
average kinetic energy of the particles of the sample
c)
total nuclear energy of the sample
d)
total thermal energy of the sample
total thermal energy of the sample
20.
Which unit is used to express an amount of thermal energy?
a)
gram
b)
mole
c)
joule
d)
pascal
21.
Which physical change is endothermic?
a)
CO2(s) --> CO2(g)
b)
CO2(l) --> CO2(s)
c)
CO2(g) --> CO2(l)
d)
CO2(g) --> CO2(s)
22.
The graph above represents the relationship between time and temperature as heat is added at a constant rate to a sample of a substance.
During interval AB which energy change occurs for the particles in this sample?
a)
The potential energy of the particles increases.
b)
The potential energy of the particles decreases.
c)
The average kinetic energy of the particles increases.
The average kinetic energy of the particles increases.
d)
The average kinetic energy of the particles decreases.
23.
A beaker with water and the surrounding air are all at 24°C. After ice cubes are placed in the water, heat is transferred from
a)
the ice cubes to the air
b)
the beaker to the air
c)
the water to the ice cubes
d)
the water to the beaker
24.
Which list of elements consists of a metal, a metalloid, and a nonmetal?
a)
Li, Na, Rb
b)
Cr, Mo, W
c)
C, Si, Sn
d)
O, S, P
25.
Why does the ion Na+ have a smaller radius than the atom Na?
a)
Na+ has one less electron shell than Na
b)
Na+ has one more electron shell than Na
c)
Na+ has more electrons than Na
d)
Na+ has more protons than Na
26.
Which formula represents sodium sulfate?
a)
NaSO4
b)
NaSO3
c)
Na2SO4
d)
Na2SO3
27.
The correct formula for calcium phosphate
a)
Ca3PO4
b)
Ca6PO4
c)
Ca3(PO4)2
d)
Ca2 (PO4)3
28.
How much Iodine-125 will remain after 100 years if the original sample had a mass of 80 grams and the half-life of I-125 is 25 years?
a)
20 grams
b)
2.5 grams
c)
5 grams
d)
10 grams
29.
An atom's mass number equals the number of...
a)
protons plus the number of electrons
b)
protons plus the number of neutrons
c)
protons
d)
neutrons
30.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
31.
As you move down the periodic table atoms get bigger. This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
32.
Two naturally occurring isotopes of an element have masses and abundance as follows: 54.00 amu (20.0%) and 56.00 amu ( 80.0%). What is the relative atomic mass of the element?
a)
54.20
b)
54.40
c)
54.80
d)
55.60
33.
Atoms of 38 Ca and 40 Ca differ with respect to number of
a)
protons
b)
electrons
c)
neutrons
d)
orbitals
34.
Arrange in order of increasing ability to penetrate matter.
a)
Beta, gamma, alpha
b)
Alpha, gamma, beta
c)
Gamma, beta, alpha
d)
Alpha, beta, gamma
35.
Classify this process.
a)
Nuclear fission
b)
Nuclear fusion
c)
Alpha decay
d)
Beta decay
36.
Which process involves the splitting of large nuclei?
a)
Beta decay
b)
Alpha decay
c)
Nuclear fission
d)
Nuclear fusion
37.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
38.
How many moles of Na2SO4 is needed to make 2.5 L of 2.0 M solution?
a)
5 moles
b)
1 moles
c)
1.25 moles
d)
0.80 moles
39.
N2 + 3H2 → 2NH3
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
a)
6 mol H2
b)
2 mol H2
c)
3 mol H2
d)
15 mol H2
40.
How many neutrons would Potassium-41 (K) have?
a)
22
b)
19
c)
41
d)
1
41.
What bonds to make an ionic bonds?
a)
metals and metals
b)
metals and nonmetals
c)
nonmetals and metalloids
d)
nonmetals and nonmetals
42.
The general formula for a synthesis reaction
a)
A + B--> AB
b)
AB--> A + B
c)
A + BX--> AX + B
d)
AX + BY --> AY+ BX
43.
Elements in the same group have the same ____.
a)
number of protons
b)
number number of neutrons
c)
# valence electrons
d)
color
44.
All atoms of the same element have the same ____.
a)
number of neutrons
b)
number of protons
c)
number of electrons
d)
mom and dad
45.
Isotopes of the same element have different ____.
a)
hair
b)
protons
c)
neutrons
d)
electrons
46.
When the solution is holding more solute than its maximum (by raising the temperature saturating the solution and then lowering the temperature) it is said to be
a)
Supersaturated
b)
Saturated
c)
Unsaturated
d)
Undefined
47.
What is a solution called where more amount of solute CAN BE dissolved at a specific temperature and pressure?
a)
Supersaturated
b)
Saturated
c)
Unsaturated
d)
Undefined
48.
What is the empirical formula of the following molecular formula: C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
49.
Name this reaction, Cl2 + 2KI --> I2 + 2KCl
a)
Synthesis
b)
Single Replacement
c)
Double Replacement
d)
Decomposition
50.
Balance this equation: H2 + N2 → NH3
a)
H2 + 4N2 → NH3
b)
H2 + 3N2 → 2NH3
c)
3H2 + N2 → 2NH3
d)
2H2 + 2N2 → 2NH3
51.
What is the equation for the positron emission by oxygen-16?
a)
168O + 0+1e --> 169F
b)
168O --> 42He + 126C
c)
168O --> 0-1e + 169F
d)
168O --> 0+1e + 167N
52.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma
d)
none
53.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if N2 was removed?
Which direction does the reaction shift if N2 was removed?
a)
Shift right
b)
Shift left
c)
No shift
d)
Shift both directions
54.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
55.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
56.
2NH3+22kJ↔N2+3H2
Which direction does the reaction shift if NH3 was added?
Which direction does the reaction shift if NH3 was added?
a)
Shift right
b)
Shift left
c)
No shift
d)
Shift both directions
57.
Why can ionic compounds not conduct electricity when they are solid?
a)
their electrons are not free to move
b)
their ions are free to move
c)
their ions are not free to move
d)
their electrons are free to move
58.
What would the charges be on the ions that make up Al2O3?
a)
Al2+ and O3-
b)
Al2- and O3+
c)
Al3+ and O2-
d)
Al3- and O2+
59.
Name this compound:
CuS
CuS
a)
Copper (IV) sulfate
b)
Copper (II) sulfite
c)
Copper (III) sulfide
d)
Copper (II) sulfide
60.
Write the formula for copper (I) phosphide
a)
Cu3P
b)
CuP
c)
Cu1P
d)
CuP3
61.
Polyatomic ions are
a)
ions formed from one atom
b)
ions formed from more than one atom
c)
ions formed in compounds
62.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
63.
At approximately what temperature does the solubility of sodium chloride, NaCl, match the solubility of potassium dichromate, K2Cr2O7?
a)
60 ºC
b)
30 ºC
c)
50 ºC
d)
83 ºC
64.
Which substance is MOST soluble at 0 ºC?
a)
KI
b)
NaNO3
c)
NaCl
d)
Ce2(SO4)3
65.
Calculate the number of moles in 85.3g of water.
a)
.211 g
b)
.211 moles
c)
4.73 moles
d)
4.73 g
66.
What is the percentage by mass of calcium in CaCl2?
a)
32%
b)
34%
c)
36%
d)
38%
67.
What is 0*C in Kelvin?
a)
110 *K
b)
100 *K
c)
273 *K
d)
210 *K
68.
What type of reaction is this?
a)
Exothermic
b)
Endothermic
69.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
70.
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
a)
Synthesis
b)
Decomposition
c)
Single Displacement
d)
Combustion
71.
Why must chemical equations be balanced?
a)
So that the equation doesn't explode
b)
The reaction won't happen until it is balanced
c)
Matter cannot be created or destroyed, merely rearranged
d)
None of these
72.
Which of the following elements make up the unknown sample?
a)
A and B
b)
B and C
c)
C and D
d)
B and C
73.
Light is emitted when an electron moves from the ________ state to the _________ state
a)
excited, ground
b)
ground, excited
74.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
75.
This picture represents which of the following?
a)
Element
b)
Compound
c)
Mixture
76.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
77.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture
78.
Italian Salad Dressing
a)
heterogeneous mixture
b)
homogeneous mixture
79.
Two or more substances mingled together, but not chemically combined are known as a
a)
residue
b)
solution
c)
distillate
d)
mixture
80.
Elements and compounds are always ___.
a)
pure
b)
mixed
81.
Gas particles are in _______________ motion.
a)
constant
b)
random
c)
constant and random
d)
perpetual
82.
True or False? At STP, two samples of a gas will have the same number of particles if they have the same volume.
a)
True
b)
False
83.
The higher the average kinetic energy the __________________
a)
the higher the volume
b)
the higher the mass
c)
the higher the temperature
d)
the higher the density
84.
The model of the atom that scientists use today is?
a)
Billiard Ball Model
b)
Plum Pudding Model
c)
Quantum mechanical model
d)
Planetary model
85.
Where are the metalloids / semimetals located on the periodic table?
a)
Blue
b)
Red
c)
Green
86.
Where are the nonmetals located on the periodic table?
a)
Blue
b)
Red
c)
Green
87.
Which type of force is this?
a)
Intramolecular
b)
Intermolecular
88.
What letter represents the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
89.
What factors are required for a chemical reaction to occur?
a)
collision of reactant particles
b)
sufficient energy
c)
favorable orientation of particles
d)
all of these
90.
Which of the following equations represents an endothermic reaction?
a)
N2O4(g) + 59 kJ → 2NO2(g)
b)
2H2(g) + O2(g) → 2H2O(l) + 572 kJ
c)
2BrCl(g) -29.3 kJ →Br2(g) + Cl2(g
d)
2H2(g) + O2(g) → 2H2O(l) ΔH = -572 kJ
91.
An electrolyte is...
a)
The rapid, random movement of particles in colloidal dispersion.
b)
A substance that dissolves in water and conducts electric current.
c)
A substance that dissolves in water and does not conduct electric current.
d)
The solution process when water is the solvent.
92.
Which substance on Table H has the strongest intermolecular forces of attraction?
a)
propanone
b)
ethanol
c)
water
d)
ethanoic acid
93.
Which substance on Table H has the lowest normal boiling point?
a)
propanone
b)
ethanol
c)
water
d)
ethanoic acid
94.
Which substance on Table G has the lowest solubility at 70oC?
a)
NaNO3
b)
HCl
c)
NH4Cl
d)
KClO3
95.
Which substance on Table G is not a gas?
a)
HCl
b)
KCl
c)
NH3
d)
SO2
96.
If 0.002 g of PbCl2 are dissolved in 2000.0g of water, how many parts per million are dissolved? (Assume density of water is 1 g/mL)
a)
10ppm
b)
1ppm
c)
2ppm
d)
20ppm
97.
Which of the following solutions will have the highest boiling point?
a)
1M NaCl (aq)
b)
2M C6H12O6 (aq)
c)
2M CaCl2
d)
1M NaNO3
98.
Colligative properties depend on the _____ of solute particles in solution.
a)
type
b)
number
c)
pH
d)
nature
99.
Is MgS soluble or insoluble?
a)
Soluble
b)
Insoluble
c)
Neither
d)
Both
100.
Is AgCl soluble or insoluble?
a)
Soluble
b)
Insoluble
c)
Neither
d)
Both
101.
Will the following reaction take place?
AuNO3 + Li ->
AuNO3 + Li ->
a)
yes
b)
no
102.
Which term refers to how strongly an atom of an element attracts electrons in a chemical bond with an atom of a different element?
a)
entropy
b)
electronegativity
c)
activation energy
d)
first ionization energy
103.
At STP, which substance has metallic bonding?
a)
ammonium chloride
b)
iodine
c)
barium oxide
d)
silver
104.
Compared to the boiling point and the freezing point of water at 1 atmosphere, a 1.0 M CaCl2(aq) solution at 1 atmosphere has a...
a)
lower boiling point and lower freezing point
b)
lower boiling point and higher freezing point
c)
higher boiling point and lower freezing point
d)
higher boiling point and higher freezing point
105.
Which compounds are classified as electrolytes?
a)
KNO3 and H2SO4
b)
KNO3 and CH3OH
c)
CH3OCH3 and H2SO4
d)
CH3OCH3 and CH3OH
106.
What is the density of an object having a mass of 8.0 g and a volume of 25 cm3?
a)
0.32 g/cm3
b)
2.0 g/cm3
c)
3.1 g/cm3
d)
200 g/cm3
100 %
