WorksheetsChemistry Fall Semester Final Exam
Total questions: 54
Worksheet time: 14hrs 30mins
Name
Class
Date
1.
In the nuclear equation given below, calculate the mass number of the alpha particle.
a)
0
b)
4
c)
234
d)
238
2.
An atom has no net electrical charge because
a)
its subatomic particles carry no electrical charges.
b)
the positively charged protons cancel out the negatively charged neutrons.
c)
the positively charged neutrons cancel out the negatively charged electrons.
d)
the positively charged protons cancel out the negatively charged electrons.
3.
The isotope below has how many neutrons, protons, and electrons.
a)
126 neutrons, 52 protons, and 52 electrons.
b)
74 neutrons, 52 protons, and 52 electrons.
c)
52 neutrons, 74 protons, and 74 electrons.
d)
52 neutrons, 126 protons, and 126 electrons.
4.
What are the two fundamental subatomic particles found in the nucleus?
a)
proton and electron
b)
proton and neutron
c)
neutron and electron
d)
neutron and positron
5.
What is the smallest amount of energy that can be gained or lost by an atom?
a)
electromagnetic photon
b)
beta particle
c)
quanta
d)
wave-particle
6.
In the ground state, which orbital does an atom’s electrons occupy?
a)
the highest available
b)
the lowest available
c)
the n = 0 orbital
d)
the d suborbital
7.
It is impossible to know precisely both the location and velocity of an electron at the same time because of:
a)
the Pauli exclusion principle
b)
the dual nature of light
c)
how electrons travel in waves
d)
the Heisenberg uncertainty Principle
8.
How many valence electrons does boron contain?
a)
1
b)
2
c)
3
d)
4
9.
Atoms of elements in group 1A have ____________.
a)
One electron in their outermost energy level
b)
Two electrons in their outermost energy level
c)
Seven electrons in their outermost energy level
d)
Eight electrons in their outermost energy level
10.
In their elemental state, which group has a complete octet of valence electrons?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
11.
It can be predicted that carbon will experience a large jump in ionization energy after its
a)
second ionization
b)
third ionization
c)
fourth ionization
d)
fifth ionization
12.
Elements in the same group of the periodic table have the same
a)
number of valence electrons.
b)
physical properties.
c)
number of electrons.
d)
electron configuration.
13.
What is a row of elements on the periodic table called?
a)
octave
b)
period
c)
group
d)
transition
14.
Why is the calcium ion (Ca²⁺) more stable than the calcium atom (Ca)?
a)
Twenty electrons are more stable than eighteen electrons.
b)
Eighteen electrons are less stable than twenty electrons.
c)
The two electrons more than the noble gas configuration is more stable.
d)
The noble gas configuration is more stable.
15.
Cations form when atoms _______ electrons.
a)
gain
b)
lose
c)
charge
d)
delocalize
16.
Atoms that gain electrons to form negative ions are ____________.
a)
metals
b)
cations
c)
anions
d)
dogions
17.
What is the name of the compound shown below?
a)
calcium chlorine-oxygen
b)
carbon chlorate
c)
calcium perchlorate
d)
calcium chlorate
18.
What is the name of the compound shown below?
a)
lithium (II) oxide
b)
lithium oxide
c)
lithium oxygen
d)
lithide oxygen
19.
What is the name of the compound shown below?
a)
beryllium (II) chloride
b)
beryllium (I) chloride
c)
beryllium chlorate
d)
beryllium chloride
20.
What is the name of the compound shown below?
a)
manganese sulfite
b)
magnesium sulfite
c)
magnesium sulfate
d)
manganese sulfide
21.
What is the formula for aluminum hydroxide?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
22.
What is the formula for potassium oxide?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
23.
What is the formula for copper (II) phosphate?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
24.
Covalent bonds are different from ionic bonds because:
a)
atoms in a covalent bond lose electrons to another atom
b)
atoms in a covalent bond do not have noble-gas electron configurations
c)
atoms in a covalent bond share electrons with another atom
d)
atoms in covalent bonds gain electrons from another atom
25.
Which of the following diatomic gases has the shortest bond between its two atoms?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
26.
Identify the name of the following covalent compounds or acid shown below.
a)
boron bisilicide
b)
monoboron disilicide
c)
diboron monosilicide
d)
diboride disilicide
27.
Identify the name of the following covalent compounds or acid shown below.
a)
monosulfur tetrachloride
b)
sulfide tetrachlorine
c)
tetrasulfur chloride
d)
sulfur tetrachloride
28.
Identify the formula for the following covalent compound: dinitrogen trioxide
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
29.
Identify the formula for the following covalent compound: tetraphosphorus decaoxide
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
30.
Identify the formulas for the following acid: phosphorous acid
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
31.
Identify the name of the following acid:
a)
hydrocaarbonic acid
b)
carbonic acid
c)
carbonous acid
d)
All of the above.
32.
What is the probable product of a double-replacement reaction?
a)
A new compound and the replaced metal
b)
A new compound and the replaced nonmetal
c)
Two different compounds
d)
A single compound
33.
The equation shown below is what type of reaction?
a)
deconstructive
b)
synthesis
c)
single replacement
d)
double replacement
34.
Determine the balanced chemical equations for the following reaction. Sodium phosphate (Na₃PO₄) and calcium chloride (CaCl₂) react to form sodium chloride (NaCl) and calcium phosphate (Ca₃(PO₄)₂).
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
35.
Determine the balanced chemical equations for the following reaction: Potassium metal (K) and chlorine (Cl₂) gas combine to form potassium chloride (KCl).
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
36.
Determine the appropriate coefficients to balance the chemical equation below.
a)
1, 2, 1, 2
b)
2, 1, 2, 1
c)
2, 1, 1, 2
d)
1, 2, 2, 1
37.
Determine the appropriate coefficients to balance the chemical equation below.
a)
2, 3, 6, 1
b)
1, 6, 3, 2
c)
3, 2, 1, 6
d)
6, 1, 2, 3
38.
Which of the following is a correct mole ratio for the following equation shown below?
a)
2 mol Al : 3 mol Br
b)
3 mol Br2 : 2 mol Al
c)
2 mol AlBr3 : 1 mol Br2
d)
2 mol Br : 2 mol Al
39.
A chemical reaction equation must be ____ in order to make stoichiometric calculations.
a)
measured
b)
controlled
c)
balanced
d)
produced
40.
How many moles of carbon dioxide is produced when 10.4 mol of propane (C₃H₈) gas is burned in excess oxygen?Use the equation below.
a)
0.288 mol
b)
3.46 mol
c)
31.2 mol
d)
52.0 mol
41.
You calculate the theoretical yield of a chemical reaction starting with 50.0g of reactant is 25.0g of product. What is the percent yield if the actual yield is 22.0g of product?
a)
88%
b)
44%
c)
50%
d)
Option 4
42.
The amount of product formed during a reaction depends on the
a)
limiting reactant
b)
excess reactant
c)
reaction rate
d)
None of the above
43.
In the following reaction, how many moles of NaCN are required to react with 5 mol of Au?
a)
3
b)
5
c)
8
d)
10
44.
Stoichiometry is the study of quantitative relationships between amounts of —
a)
the reactants and products of a chemical reaction relative to time
b)
the products of a chemical reaction only
c)
the reactants and products of a chemical reaction
d)
the reactants of a chemical reaction only
45.
The amount of product that can be produced from a given amount of reactants based on stoichiometric calculations is:
a)
actual yield
b)
percent yield
c)
theoretical yield
d)
stoichiometric yield
46.
What law are all stoichiometric calculations based on?
a)
law of definite proportions
b)
law of conservation of mass
c)
law of conservation of energy
d)
none of the above
47.
What is the ratio between the coefficients of any two substances in a balanced equation?
a)
Molar mass balanced equation
b)
Mole ratio
c)
Quadratic equation
d)
Chemical formula
48.
The substance that limits the extent of a chemical reaction has a special name. What is this substance called?
a)
Limiting reactant
b)
Limiting product
c)
Excess reactant
d)
Excess product
49.
The mass of the final product in a chemical reaction is based on what?
a)
the amount of excess reactant
b)
the amount of limiting reactant
c)
the presence of a catalyst
d)
the amount of oxygen present
50.
A(n) ______________________ is a reactant that has a portion remaining after the reaction has stopped.
a)
excess reactant
b)
actual yield
c)
percent yield
d)
stoichiometry
e)
mole ratio
51.
The ratio of the actual yield to the theoretical yield expressed as a percent is called the ______________________.
a)
percent yield
b)
actual yield
c)
stoichiometry
d)
excess reactant
e)
mole ratio
52.
The study of the quantitative relationships among the amounts of reactants used and the amounts of products formed by a chemical reaction is called ______________________.
a)
stoichiometry
b)
actual yield
c)
percent yield
d)
excess reactant
e)
mole ratio
53.
The reactant that limits the extent of the reaction is called the ______________________.
a)
limiting reactant
b)
actual yield
c)
percent yield
d)
stoichiometry
e)
excess reactant
54.
The ______________________ is the maximum amount of product that can be produced from a given amount of reactant.
a)
theoretical yield
b)
actual yield
c)
percent yield
d)
stoichiometry
e)
excess reactant
100 %
