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WorksheetsChem Final Review Low Stress
Total questions: 141
Worksheet time: 35hrs 15mins
Name
Class
Date
1.
Which of the following can be used to identify the equivalence point
a)
indicator
b)
temperature
c)
molarity
d)
density
2.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
3.
True/False: Both fission and fusion reactions release large amounts of energy.
a)
True
b)
False
4.
The time it takes for half of the atoms in a radioactive sample to decay
a)
radioactive dating
b)
gamma decay
c)
half life
d)
double life
5.
Subatomic particle with a positive charge found in the nucleus of an atom.
a)
neutrons
b)
electron
c)
nucleus
d)
proton
6.
A neutral subatomic particle found in the nucleus of an atom.
a)
neutron
b)
electron
c)
nucleus
d)
proton
7.
Atoms of the same element with the same number of protons but different numbers of neutrons.
a)
carbon
b)
electron
c)
isotoners
d)
isotope
8.
Why is the following chemical equation not balanced?
H2 + O2 --> H2O
H2 + O2 --> H2O
a)
each side of the equation has a different number of oxygen atoms
b)
each side of the equation has a different number of hydrogen atoms
c)
each side has the same mass
9.
What is the trend/pattern with the atomic radius (size) as you move down a column?
a)
it decreases
b)
it increases
c)
it stays the same size
d)
there is no pattern
10.
When a substance is dissolved in water, that compound is said to be ___________.
a)
Aqueous
b)
Solution
c)
Non-polar
d)
Liquid
11.
A chemical with a pH of 8 could be described as...
a)
Basic
b)
H+ donor
c)
Neutral
d)
Acidic
12.
An exothermic reaction _____ heat, so it feels ________.
a)
absorbs, cold
b)
releases, cold
c)
absorbs, warm
d)
releases, warm
13.
The neutralization reaction between HNO3 and NaOH creates water and...
a)
NaNO3
b)
Na2NO3
c)
Na(NO3)2
d)
NaH3
14.
How do you calculate the molarity of a solution?
a)
By tasting it.
b)
Dividing the moles of solute by the L of solution
c)
Dividing the moles of solute by the kg of solvent
d)
By adding the sum of the molecular weight of the elements in the substance.
15.
A solution of NaOH would most likely have a pH _____ 7
a)
less than
b)
more than
c)
equal to
16.
Tastes Sour
a)
Acids
b)
Bases
c)
Salts
d)
All
17.
pH greater than 7.
a)
Acids
b)
Bases
c)
All
18.
Anything that has mass and takes up space is called
a)
matter
b)
energy
c)
hetrogeneous
d)
homogeneous
19.
Soil, a salad, and sugar water are all examples of
a)
elements
b)
compounds
c)
mixtures
d)
atoms
20.
The volume of an irregular object can be measured by
a)
multiplying the object's length, width, height
b)
multiplying density by mass
c)
submerging the object in water in a graduated cylinder
d)
placing object on triple beam balance
21.
One example of a physical change is
a)
burning paper
b)
baking cookies
c)
toasting marshmallows
d)
dissolving salt in water
22.
One example of a chemical change is
a)
filtering a mixture
b)
burning wood
c)
boiling water
d)
crushing a can
23.
Fireworks exploding in the sky and giving off light are an example of an
a)
endothermic change
b)
chemical change
c)
physical change
d)
change is mass
24.
The measurement of how much mass is in a given volume is called
a)
weight
b)
melting point
c)
boiling point
d)
density
25.
All elements are made of basic particle called
a)
compounds
b)
mixtures
c)
atoms
d)
molecules
26.
If you describe methane as a gas that easily catches fire, you are describing a
a)
state of matter
b)
physical property
c)
chemical property
d)
chemical formula
27.
A change that produces one of more new substance is called a PHYSICAL change
a)
True
b)
False, Property
c)
False, Chemical
28.
In a ____________________ mixture, like a salad, you can see the different parts.
a)
Homogeneous
b)
Heterogeneous
c)
Snyder
d)
Cedar Hollow
29.
What determines an elements identity?
a)
electrons
b)
periodic table
c)
protons
d)
mass
30.
How do the following two elements bond together?
Al3+ O2-
Al3+ O2-
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
31.
The total amount of matter (atoms) before and after a chemical reaction (change), remains the same.
a)
True
b)
False
32.
The compound NaCl (Sodium Chloride) is commonly known as ______
a)
bleach
b)
fertiliser
c)
table salt
d)
window cleaner
33.
A Ph reading of 3 would be ______
a)
basic
b)
acidic
c)
alkaline
d)
neutral
34.
Which of the following is correct?
a)
Proton = positive, neutron = negative, electron = neutral
b)
Proton = positive, neutron = neutral, electron = negative
c)
electron = positive, neutron = neutral, proton = negative
d)
neutron = negative, proton = neutral, electron = positive
35.
Decomposition occurs when...
a)
Two formulas combine.
b)
A formula breaks apart.
c)
An atom is replaced during a reaction.
36.
What coefficients are needed to balance the equation?
_Al + _HF --> _H2 + _AlF3
_Al + _HF --> _H2 + _AlF3
a)
1, 1, 1, 1
b)
2, 6, 3, 2
c)
2, 3, 3, 1
d)
1, 6, 3, 2
37.
The covalent compound N2O5 would be named
a)
nitrogen oxide.
b)
dinitrogen oxide.
c)
nitrogen pentoxide.
d)
dinitrogen pentoxide.
38.
What kind of bond forms when atoms share electrons?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
39.
Cu+combines with O-2 to form
a)
Cu2O
b)
Cu2O2
c)
Cu+2O
d)
CU+1O3
40.
Ca+2 combines with Br- to form
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
41.
Find the percentage composition of Mg in Mg3(PO4)2.
a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
42.
Which element gets LARGER when it becomes an ion?
*Hint: It gets LARGER because it gains an Electron*
*Hint: It gets LARGER because it gains an Electron*
a)
Barium
b)
Lithium
c)
Strontium
d)
Bromine
43.
Salt is a/an
a)
Compound
b)
Homogeneous mixture
c)
Element
d)
Vapor
44.
Aluminum is a/an
a)
Compound
b)
Homogeneous mixture
c)
Element
45.
A form of matter with a constant volume that takes the shape of its container
a)
solid
b)
liquid
c)
gas
d)
plasma
46.
A form of matter with definite shape and volume
a)
solid
b)
liquid
c)
gas
d)
plasma
47.
Honey has a density of 15g/cm3 and dishsoap has a density of 10g/cm3 if they are both poured in a cylinder which will be on the bottom?
a)
soap
b)
honey
48.
Which property is the most useful in identifying a certain chemical?
a)
mass
b)
density
c)
color.
d)
flexibility
49.
What is the mass of 2.50 mol of Helium gas He?
a)
40 g
b)
10 g
c)
16 g
d)
32 g
50.
4Si + S8 --> 2Si2S4
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
51.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
52.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
53.
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Combustion
54.
A sample contains 27.1 g of calcium oxide. How many moles of calcium oxide are in the sample?
a)
0.520 mol CaO
b)
1.3 mol CaO
c)
0.483 mol CaO
d)
None of the above
55.
A solution of NaCl has a molarity of 0.549 M. How many moles are in 350 mL of this solution?
a)
0.193 mol NaCl
b)
0.524 mol NaCl
c)
0.234 mol NaCl
d)
None of the above
56.
Particles (molecules) in a ______________________ have more energy than the other states of matter.
a)
gas
b)
solid
c)
liquid
57.
__________ are made up of solutes and solvents.
a)
Solutions
b)
Suspension
c)
Colloid
58.
Substance dissolved in a solution
a)
concentration
b)
solute
c)
solvent
d)
solution
59.
Which of the following usually makes a substance dissolve faster in a solvent?
a)
agitating the solution
b)
increasing the particle size of the solute
c)
lowering the temperature
d)
decreasing the number of particles
60.
The atomic number tells you the
a)
number of neutrons in the nucleus
b)
number of protons in the atom
c)
number of its electrons if the atom is negatively charged
d)
atomic mass of the atom
61.
Isotopes differ in their
a)
number of protons
b)
atomic number
c)
number of nuetrons
d)
number of electrons
62.
one mole of argon resembles one mole of magnesium they have the same
a)
mass
b)
volume
c)
number of protons
d)
number of atoms
63.
in one mole of ammonia molecules there are approximately
a)
3x10^23 molecules
b)
6.02x10^23 molecules
c)
1.2x10^23 molecules
d)
2.4x10^24 molecules
64.
knowing the mass of hydrogen only, to calculate the mass of water formed, according to the following reaction:
2H2 + O2 --> 2H2O
the process that needs to be followed is:
2H2 + O2 --> 2H2O
the process that needs to be followed is:
a)
moles of H2-->Mol Ratio--> mass of H2 --> moles of H2O --> mass of H2O
b)
mass of H2 --> moles of H2 -->Mol Ratio--> moles of H2O --> mass of H2O
c)
Mass of H2O --> moles of H2O --> Mol Ratio-->moles of H2 --> mass of H2
d)
mass of H2 + mass of O2--> Mol Ratio-->mass of H2O
65.
the products formed by the complete combustion of hydrocarbons are
a)
carbon dioxide and water
b)
carbon monoxide and hydrogen
c)
carbon monoxide and water
d)
carbon dioxide and hydrogen
66.
Which of the following is the most electronegative?
a)
Na
b)
S
c)
Cl
d)
I
67.
Which of the following is a covalent compound?
a)
NaCl
b)
Mg(OH)2
c)
NO2
d)
K3PO4
68.
What is the name of the compound PCl5?
a)
Phosphorus pentachloride
b)
Phosphorus chloride
c)
Phosphorus (V) chloride
d)
Monophosphorus pentachloride
69.
What is the name of the compound Fe(OH)2
a)
Iron hydroxide
b)
Iron (I) hydroxide
c)
Iron (II) hydroxide
d)
Iron dihydroxide
70.
Dancer named the compound Ni2SO4 as "nickel sulfate." Why is Dancer wrong?
a)
There should be prefixes.
b)
There should be Roman numerals.
c)
It should be "nickel sulfide."
d)
Dancer is right.
71.
How many centimeters are in 1 meter:
a)
They are equal
b)
10
c)
100
d)
1000
72.
Which one of the following compounds would have the highest solubility in water?
a)
I2
b)
O2
c)
N2
d)
NH3
73.
What holds atoms together in a molecule
a)
density
b)
gravity
c)
physical bonds
d)
chemical bonds
74.
In the lab, volumes of liquids are usually measured using
a)
electrode
b)
scale
c)
triple-beam balance
d)
graduated cylinder
75.
If you heat a liquid and measure the temperature at which it boils, you are measuring a/an
a)
atomic property
b)
physical property
c)
chemical property
d)
molecular property
76.
Classify Stainless Steel
a)
Homogeneous
b)
Heterogeneous
77.
Classify Air
a)
Homogeneous
b)
Heterogeneous
78.
Classify oil and water
a)
Homogeneous
b)
Heterogeneous
79.
Determine the molar mass for CCl4
a)
153.8 g/mol
b)
47.54 g/mol
c)
189.35 g/mol
d)
82.9 g/mol
80.
What is the mass in grams of 5.90 mol C8H18?
a)
.0512 g
b)
19.4 g
c)
673 g
d)
389 g
81.
Which of the following is likely to be a gas?
a)
Iron
b)
Mercury
c)
Argon
d)
Carbon
82.
How many neutrons does this element have:
a)
11
b)
12
c)
23
d)
32
83.
Which of the following reactions is a combustion reaction ?
a)
MgCO3 + O2 → MgO + CO2
b)
C3H8 + 5O2 → 3CO2 + 4H2O
c)
6CO2 + 6H2O → C6H12O6 + 6O2
84.
What is the law of Conservation of Mass?
a)
A measure of how much mass is created or destroyed.
b)
Mass can neither be created nor destroyed during a chemical reaction.
85.
Magnesium + Hydrogen Chloride -->
a)
Magnesium hydride
b)
Sodium chloride+ Hydrogen
c)
Magnesium chloride + Hydrogen
d)
Magnesium sulfate+ Hydrogen
86.
What is the general word equation for a metal and acid reaction?
a)
metal + acid --> salt
b)
metal + acid --> salt + hydrogen
c)
metal + acid --> oxygen + hydrogen
d)
metal + acid --> oxygen + water
87.
Metal and water word equation...
a)
metal + water --> metal oxide + oxygen
b)
metal + water --> metal hydroxide + hydrogen
c)
metal + water --> metal hydride + hydrogen
d)
metal + water --> carbon dioxide + water
88.
When a more reactive metal takes the place of a less reactive metal in a compound...
a)
oxidation
b)
reduction
c)
single Replacement
d)
Double Replacement
89.
Which of the following is the correct name for MgCl2?
a)
magnesium II chloride
b)
magnesium chlorine
c)
magnesium chloride
d)
magnesium dichloride
90.
A group on the periodic table is arranged ________ where as, a period is arranged ________.
a)
horizontally, vertically
b)
vertically, horizontally
91.
Is the equation balanced?: 2H2O + O2 --> 2H2O2
a)
Yes
b)
No
92.
2H2O(g) + O2(g) <--> 2H2O2(g) what direction would the equilibrium shift if oxygen was removed?
a)
Left
b)
Right
93.
2H2O(g) + O2(g) <--> 2H2O2(g) what direction would the equilibrium shift if water was added?
a)
Left
b)
Right
94.
2H2O(g) + O2(g) <--> 2H2O2(g) what direction would the equilibrium shift if pressure was increased?
a)
Left
b)
Right
95.
Balance this equation: H2 + N2 → NH3
a)
H2 + 4N2 → NH3
b)
H2 + 3N2 → 2NH3
c)
3H2 + N2 → 2NH3
d)
2H2 + 2N2 → 2NH3
96.
In the equation,
2Mg + O2 ---> 2MgO,
which are the reactants?
2Mg + O2 ---> 2MgO,
which are the reactants?
a)
Mg and O2
b)
MgO
c)
Mg and MgO
d)
O2 and MgO
97.
2Mg + O2 ---> 2MgO how many moles of MgO can be made from 7 moles of O2?
a)
7
b)
3.5
c)
14
d)
2
98.
2Mg + O2 ---> 2MgO Given 5 moles of Mg and 3 moles of O2 which is the limiting reagent?
a)
O2
b)
Mg
99.
Name the compound MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
100.
Name this compound:
CuS
CuS
a)
Copper (IV) sulfate
b)
Copper (II) sulfite
c)
Copper (III) sulfide
d)
Copper (II) sulfide
101.
Covalent naming uses _____________ to denote the number of atoms
a)
suffixes
b)
prefixes
c)
Roman numerals
102.
Give the formula for Disulfur Monoxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
103.
Name the compound CO
a)
Carbon Oxide
b)
Carbon Oxygen
c)
Dicarbon dioxide
d)
Carbon Monoxide
104.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
105.
What kind of bond forms when one atom gives electrons to another atom?
a)
Mettalic bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
106.
An atom that has two electrons in the outer shell, such as magnesium, would most likely
a)
share to acquire a completed outer shell
b)
lose these two electrons and become a positively charged ion
c)
bind with carbon by way of hydrogen bonds
d)
bind with another calcium atom to satisfy its energy needs
107.
The density of a block of wood with a volume of 50 cubic centimeters and a mass of 100 grams is
a)
2
b)
.5
c)
500
d)
5000
108.
The smallest particle of an element is called an atom.
a)
Truee
b)
Trrue
c)
Ttrue
d)
True
109.
States that mass is neither created nor destroyed in a chemical reaction.
a)
law of multiple proportions
b)
law of conservation of mass
c)
law of definite proportions
110.
Which element has the highest first ionization energy?
a)
sodium
b)
aluminum
c)
calcium
d)
phosphorus
111.
When a metal atom combines with a nonmetal atom, the nonmetal atom will...
a)
lose electrons, decrease in size
b)
lose electrons, increase in size
c)
gain electrons, decrease in size
d)
gain electrons, increase in size
112.
When combining with nonmetallic atoms, metallic atoms generally will...
a)
lose electrons and form negative ions
b)
lose electrons and form positive ions
c)
gain electrons and form positive ions
d)
gain electrons and form negative ions
113.
Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms'...
a)
number of principal energy levels
b)
number of valence electrons
c)
atomic numbers
d)
atomic masses
114.
When the mols of acid = mols of base
a)
titration
b)
neutralization
c)
equivalence point
d)
equilibrium
115.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
116.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
117.
An element with five valence electrons is
a)
phosphorus
b)
oxygen
c)
beryllium
d)
rubidium
118.
How many significant figures does the following number have: 2.040x102
a)
6
b)
4
c)
3
d)
2
119.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
120.
Round 0.010229 to four sig figs
a)
1022
b)
1023
c)
0.01023
d)
0.01022
121.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
122.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
123.
What type of bond would be formed between Lithium and oxygen?
a)
covalent
b)
ionic
c)
metallic
d)
dispersion
124.
Which of the following is a property of metals?
a)
dull
b)
brittle
c)
good electrical and thermal conductor
d)
none of the options
125.
What is the chemical formula for Lead II bromide?
a)
PbBr
b)
Pb2Br
c)
PbBr2
d)
Not enough info
126.
What is the chemical formula for Ammonium Phosphate?
a)
NH4PO4
b)
(NH4)3PO4
c)
NH4(PO4)3
d)
(NH4)2P
127.
What is the chemical formula for Iron (III) Oxide?
a)
FeO
b)
Fe3O
c)
Fe3O2
d)
Fe2O3
128.
Positive ions are called ____________.
a)
cations
b)
anions
c)
atoms
d)
molecules
129.
What is this element?
1s22s22p63s2
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
130.
What is this element?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
131.
What is the correct Noble Gas configuration for Mg?
a)
[Ar]4s1
b)
[He]2s1
c)
[Ne]3s2
d)
[Ar]4s2
132.
A sample of matter that can be dissolved is said to be?
a)
Soluble
b)
Insolube
c)
Insatiable
d)
Unstable
133.
Which of the following is a transition metal?
a)
Magnesium
b)
Aluminium
c)
Iron
d)
Neon
134.
How many moles are needed to make 2.5 L of a 3.8 M solution?
a)
9.5 mol
b)
0.66 mol
c)
1.5 mol
d)
15 mol
135.
You have a 0.5 M MgSO4 stock solution available. Calculate the volume of the stock solution needed to make 2.0 L of 0.20 MgSO4.
a)
0.8 L
b)
5 L
c)
0.1 L
d)
0.5 L
136.
What is the concentration of a solution that has a volume of 2.5 L and contains exactly 2.125 moles of calcium phosphate? **Remember to write the chemical formula**
a)
264 M
b)
0.85 M
c)
3.7 M
d)
2.0 M
137.
How much 18 M nitric acid is need to prepare a 6.0 M solution of 250 mL?
(M1V1 = M2V2)
(M1V1 = M2V2)
a)
0.750 L
b)
75 L
c)
83.3 L
d)
0.083L
138.
If the [H3O+1] < [OH-1] the solution is...
a)
acidic
b)
basic
c)
neutral
139.
If there is the maximum amount of solute in a solution, it is said to be
a)
satured
b)
unsaturated
c)
supersaturated
d)
concentrated
140.
How much 1.50M KBr can be made from 15.6 mL of concentrated KBr with a molarity of 9.65 M?
a)
150. mL
b)
151 mL
c)
1.00 L
d)
100. mL
141.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
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