WorksheetsChemistry Final Review
Total questions: 89
Worksheet time: 2hrs 30mins
Name
Class
Date
1.
Ionic bonds form between two ions that have...
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
2.
Which is most likely to form a negative ion...
a)
an element from Group 17
b)
a metal
c)
an element from Group 1
d)
an element with atoms that have eight valence electrons
3.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
4.
In covalent bonding, electrons are
a)
shared
b)
transferred
c)
wiped out
5.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
6.
Atoms want
a)
A full outer shell of electrons
b)
One electron short of a full shell
c)
kit kats
7.
What is a product?
a)
What's left of the chemical reaction.
b)
The beginning formulas.
8.
Which problem is balanced?
a)
PbO2 + 2H2
b)
So2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
9.
What is a coefficient?
a)
The small number on the right of the chemical symbol.
b)
The large number to the left of a formula.
10.
Solve the problem: N2 + O2 --> 2NO
a)
N2 + O2 --> 2NO
b)
2N2 + O2 --> 2NO
11.
Is this equation balanced?: CS2 + 202 --> CO2 +2SO2
a)
Yes
b)
No
12.
What is a reactant?
a)
The chemical substances that begin the reaction.
b)
What comes from the reaction.
13.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
14.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
15.
The substances at the beginning of a chemical reaction are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
16.
What is the part of the chemical equation in green called?
Fe + S --> FeS
Fe + S --> FeS
a)
products
b)
reactants
c)
yield
d)
chemical formula
17.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
18.
What does the Law of Conservation of Mass state?
a)
Matter cannot be gained or lost in a chemical reaction.
b)
Matter can only be lost in a chemical reaction.
c)
Matter can only be gained in a chemical reaction.
d)
Matter can be gained and lost in a chemical reaction.
19.
What is the little number after an element in a chemical equation called.
Example: H2
Example: H2
a)
Coefficient
b)
Subscript
c)
Atom
d)
Equation
20.
How many Elements are in this compound?
CuSO4
CuSO4
a)
3
b)
1
c)
4
d)
5
21.
Is water an element?
a)
NO
b)
yes
c)
maybe
d)
I am not sure
22.
Which of the following is NOT a classification of elements?
a)
metalloid
b)
compound
c)
metal
d)
nonmetal
23.
True or False: An element can be broken down into a simpler substance.
a)
TRUE
b)
FALSE
24.
In an atom, protons and neutrons are found where?
a)
The electron cloud
b)
The nucleus
25.
How are elements ordered on the Periodic Table?
a)
Alphabetical Order
b)
By their color.
c)
By their atomic mass.
d)
By their atomic number.
26.
The building blocks of all matter are called:
a)
atoms
b)
elements
c)
compounds
d)
mixtures
27.
A substance that is made up for one type of atom is called an:
a)
atom
b)
element
c)
compound
d)
mixture
28.
The subatomic particle with a neutral charge is:
a)
protons
b)
electrons
c)
neutrons
d)
cloud
29.
How REACTIVE an element is is based on
a)
protons
b)
atomic number
c)
electrons
d)
valence electrons
30.
Which two subatomic particles are found in the NUCLEUS of at atom?
a)
protons & nuetrons
b)
protons & electrons
c)
neutrons & electrons
d)
electrons & protons
31.
What type of subatomic particles are found in the cloud?
a)
neutrons
b)
electrons
c)
protons
d)
reactions
32.
If an element has 6 protons, 7 neutrons, and 6 electrons, what type of charge does the element have?
a)
positive
b)
negative
c)
neutral
d)
imaginary
33.
Which type of subatomic particles have the LEAST amount of mass?
a)
protons
b)
electrons
c)
neutrons
d)
nucleus
34.
If an atom has 24 protons and 24 electrons, what is the atomic number of this element?
a)
24
b)
48
c)
0
d)
42
35.
How are elements distinguished from one another?
a)
The number of valence electrons
b)
The number of neutrons
c)
The number of protons
d)
How they react with other elements
36.
Hydrochloric acid reacts with magnesium to produce hydrogen gas
a)
Physical change
b)
Chemical change
37.
Salt dissolves in water
a)
Physical change
b)
Chemical change
38.
A piece of copper is cut in half
a)
physical change
b)
chemical change
39.
a sugar cube is ground up
a)
physical change
b)
chemical change
40.
water is heated and changed to steam
a)
physical change
b)
chemical change
41.
iron rusts.
a)
physical change
b)
chemical change
42.
ice melts
a)
physical change
b)
chemical change
43.
milk sours (goes bad)
a)
physical change
b)
chemical change
44.
Freezing Juice?
a)
Physical Change
b)
Chemical Change
45.
After you mix two substances together, a new substance forms. This is an example of:
a)
Physical Change
b)
Chemical Change
46.
Is hammering wood together to build a house a chemical or physical change?
a)
chemical
b)
physical
47.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
48.
Molecule
a)
A group of atoms bonded together
b)
Basic unit of a chemical element
c)
Coefficient
d)
Subscript
49.
Can matter be created or destroyed?
a)
Yes, it can be created.
b)
Yes, it can be destroyed.
c)
No, matter is always conserved
d)
None of these
50.
If there is no subscript, there is ______ atom(s) of that element.
a)
0
b)
2
c)
only 1
d)
1 million
51.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______.
a)
Warm
b)
Cold
52.
what is an example of exothermic?
a)
firework
b)
ice pack
c)
coal
d)
wood
53.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
54.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
55.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
56.
4. 1. What is a pure substance made of two or more elements that are chemically combined called?
a)
A. element
b)
B. compound
c)
C. mixture
d)
D. solution
57.
Spaghetti and meatballs is an example of a:
a)
compound
b)
element
c)
mixture
d)
molecule
58.
Salt water is:
a)
A Compound
b)
An element
c)
A mixture
d)
An atom
59.
Baking soda (NaHCO3)
a)
A. MIXTURE
b)
B. COMPOUND
c)
C. ELEMENT
60.
A combination of substances that are not chemically combined is called a(n)____________.
a)
mixture
b)
compound
c)
physical
61.
This picture represents which of the following?
a)
element
b)
compound
c)
mixture of elements
d)
mixture of compounds
62.
Is salt (NaCI) a compound or a element
a)
Compound
b)
element
63.
A chemical reaction is...
a)
when a substance is mixed with another substance
b)
when a substance undergoes a change to form a new substance
c)
when a substance is dissolved into another substance
d)
when a substance is heated or exposed to another substance
64.
Which of the following is not evidence of a chemical reaction?
a)
Formation of a precipitate
b)
Production of gas
c)
Change in temperature
d)
Change in state of matter
65.
Which statement explains the Law of Conservation of Matter?
a)
In a chemical
reaction, matter can only be destroyed.
b)
In a
chemical reaction, matter can only be created.
c)
Matter can neither be
created nor destroyed in a chemical reaction.
d)
Matter can be created
or destroyed in a chemical reaction.
66.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
67.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
68.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
69.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
70.
How many electrons does potassium K contain? (click to see image)
a)
19
b)
39
c)
20
d)
40
71.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
72.
How many electrons should Hydrogen have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
73.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
74.
How many electrons should Beryllium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
75.
How many electrons should Boron have around its Lewis dot model?
a)
1
b)
3
c)
5
d)
7
76.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
77.
How many electrons should Magnesium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
78.
?
a)
Boron
b)
Carbon
c)
Nitrogen
d)
Lithium
79.
?
a)
Beryllium
b)
Boron
c)
Barium
d)
Bromine
80.
What element is represented in this Bohr Model?
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
81.
an element will always have the same number of
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
82.
Which group of the periodic table is composed of inert (not reactive) gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
83.
With which group would Group 2 most likely bond?
a)
Group 1
b)
Group 2
c)
Group 16
d)
Group 17
84.
With which element will Hydrogen most likely bond?
a)
Chlorine
b)
Sulfur
c)
Argon
d)
Silicon
85.
With which element would Fluorine most likely bond?
a)
Nitrogen
b)
Lithium
c)
Sulfur
d)
Iodine
86.
With which group would Group 18 most likely bond?
a)
Group 1
b)
Group 2
c)
Group 13
d)
None
87.
Which two groups on the Periodic Table are the MOST reactive?
a)
Group 1 and Group 17
b)
Group 2 and Group 16
c)
Group 13 and Group 15
d)
Group 17 and Group 18
88.
How many valence electrons are elements trying to reach in their outer shells?
a)
1
b)
2
c)
5
d)
8
89.
What determines the reactivity of an element?
a)
Size of its nucleus
b)
Number of total electrons
c)
Number of valence electrons
d)
Number of shells
100 %
