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WorksheetsChemistry Middle School Review
Total questions: 63
Worksheet time: 1hrs 18mins
Name
Class
Date
1.
When a scientist mixed two chemicals, an exothermic reaction takes place. Which of the following would be proof that the reaction was exothermic?
a)
a change of color
b)
a change of state
c)
a temperature decrease
d)
a temperature increase
2.
Which of the following is a chemical change?
a)
water freezes to form ice
b)
sugar dissolves in water
c)
gasoline burns in a car engine
d)
a piece of metal expands when it is heated
3.
In the reaction methane + oxygen turns into carbon dioxide + water, the methane and oxygen are called _______________.
a)
reactants
b)
products
c)
neutrals
d)
energizers
4.
A change in the shape of an object is an example of _________________.
a)
a chemical change
b)
energy
c)
an endothermic change
d)
a physical change
5.
Increasing the concentration of a reactant in a chemical reaction will _____________.
a)
decrease the rate of the reaction
b)
stop the reaction from happening
c)
increase the rate of the reaction
d)
have no effect on the rate of the reacion
6.
In any chemical reaction, the mass of the products is always:
a)
slightly less than the mass of the reactants
b)
much less than the mass of the reactants
c)
the same as the mass of the reactants
d)
greater than the mass of the reactants
7.
Raising the temperature of a chemical reaction would make the reaction __________________.
a)
happen slower
b)
happen faster
c)
stop completely
d)
proceed as normal
8.
What are substances on the left side of a chemical equation called?
a)
electrons
b)
groups
c)
products
d)
reactants
9.
What is a chemical equation?
a)
a diatomic molecule
b)
a shorthand representation of a chemical bond
c)
a shorthand representation of a chemical reaction
d)
a substance
10.
What does the number in front of the molecular symbol mean?
a)
It shows that there is only one molecule present in a reaction
b)
It shows the number of molecules in the reaction
c)
It shows the number of reactions that took place
d)
All of the choices
11.
When this equation (C3H8 + O2 -> CO2 + H2O ) is balanced, the coefficient in front of carbon dioxide is:
a)
1
b)
12
c)
3
d)
6
12.
An element plus additional element reacts to form one product is an example of which type of chemical reaction?
a)
combustion
b)
decomposition
c)
synthesis
d)
single replacement
13.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement
b)
decomposition
c)
combustion
d)
single replacement
14.
Provides evidence that a chemical reaction has occurred.
a)
dissolving
b)
melting
c)
formation of a gas
d)
bending
15.
What type of chemical reaction takes place when fluorine reacts with sodium bromide?
a)
single replacement
b)
double replacement
c)
combustion
d)
synthesis
16.
What are the correct coefficients when this equation is balanced?
KClO3 --> KCl + O2
KClO3 --> KCl + O2
a)
2,2,2
b)
2,2,3
c)
1,2,3
d)
3,3,3
17.
_P4+_O2 → _P2O3
a)
3 P4+1 O2 → 2 P2O3
b)
1 P4+1 O2 → 2 P2O3
c)
1 P4+ 3 O2 → 2 P2O3
d)
1 P4+ 2 O2 → 3 P2O3
18.
_BaS + _PtF2 → _BaF2 + _PtS
a)
1 BaS + 1 PtF2 → 1 BaF2 + 1 PtS
b)
4 BaS + 2 PtF2 → 1 BaF2 + 1 PtS
c)
1 BaS + 2 PtF2→ 2 BaF2 + 2 PtS
d)
1 BaS + 3 PtF2 →1 BaF2 + 2 PtS
19.
How many total atoms are represented? 4Al2O3
a)
2
b)
8
c)
5
d)
20
20.
Substances that enter into a chemical reaction (found to the left side of the arrow)
a)
product
b)
reactant
c)
chemical
d)
balanced equation
21.
In every balanced chemical equation, each side of the equation has the same number of ____.
a)
coefficients
b)
moles
c)
molecules
d)
atoms of each element
22.
When balancing equations what does
-->
mean?
-->
mean?
a)
subscript
b)
equals
c)
it is just an arrow
d)
yield
23.
Is the following equation balanced or unbalanced?
Fe + S --> FeS
Fe + S --> FeS
a)
balanced
b)
unbalanced
24.
___________________ are the elements or compounds that are formed in a chemical
reaction.
reaction.
a)
Polymers
b)
Bonds
c)
Reactants
d)
Products
25.
Subatomic particles with a negative charge
a)
Electrons
b)
Neutrons
c)
Protons
d)
Quarks
26.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Proton Number
d)
Atomic Number
27.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus
d)
Electrons
28.
Atoms of the same element with a different number of neutrons
a)
Ion
b)
Gluons
c)
Isotope
d)
Quarks
29.
A charged atom (positive OR negative)
a)
Ion
b)
Isotope
c)
Electron Cloud
d)
Quark
30.
Arrangement of the elements organized by atomic number
a)
Electron Cloud
b)
Periodic Table
c)
Electron Configuration
d)
None of these
31.
Discovered the electron within the atom
a)
Thomson
b)
Chadwick
c)
Schrodinger & Heisenberg
d)
Dalton
32.
Believed that atoms of the same element are identical to each other
a)
Bohr
b)
Rutherford
c)
Dalton
d)
Thomson
33.
Calculation used to find the number of neutrons in an atom
a)
Atomic Mass - Atomic Number
b)
Atomic Number - Atomic Mass
c)
Atomic Mass - Electrons
d)
none of these
34.
Elements which are shiny, conduct electricity and heat are called
a)
metals
b)
nonmetals
c)
metalloids
d)
nonexistent
35.
The group NOBLE GASES is located where on the periodic table?
a)
Right Side
b)
Left Side
c)
Middle
d)
Only the last column on the right
36.
The most reactive metals on the periodic table are called
a)
Noble Gases
b)
Halogens
c)
Alkali Metals
d)
Alkaline-earth Metals
37.
Most of the elements on the periodic table are
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Liquids
38.
Elements that have properties of both metals and nonmetals are called
a)
Groups
b)
Periods
c)
Metalloids
d)
Zigzags
39.
What is the meaning of atom?
a)
"dividable"
b)
"invisible"
c)
"hard particles"
d)
"not able to be divided"
40.
Which of the following describes RADIOACTIVE ISOTOPES?
a)
they are stable
b)
they never change
c)
they are unstable
d)
they don't produce energy
41.
Sodium (Na), Rubidium (Rb), and Francium (Fr) are all metals with high reactivity to water. Based on the Periodic Table, which of the following is true?
a)
Magnesium (Mg) is a metal with high reactivity to water.
b)
Rhodium (Rh) is a metal with high reactivity to water.
c)
Xenon (Xe) is a metal with high reactivity to water.
d)
Potassium (K) is a metal with high reactivity to water.
42.
Which of the following is a representation of Bohr's model of the atom?
a)
Model A
b)
Model B
c)
Model C
d)
Model D
43.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
44.
What does the nucleus of an atom contain?
a)
Electrons and neutrons
b)
Protons and neutrons
c)
Neutrinos and positrons
d)
DNA and RN
45.
An atom's overall charge is ________.
a)
positive
b)
depends
c)
neutral
d)
negative
46.
Neon has an atomic number of 10 and an atomic mass of 20.180. How many protons, electrons, and neutrons will it have?
a)
P=10 E=10 N=11
b)
P=5 E=5 N=10
c)
P=10 E=10 N=10
d)
P=10 E=5 N=5
47.
When naming ionic compounds you always write the name of the positive element _______ .
a)
first
b)
second
c)
with "ide"
d)
with a prefix
48.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
49.
MgF2
a)
magnesium fluoride
b)
manganese Phosphide
c)
magnesium(III) fluoride
d)
magnesium fluoride(II)
50.
How many sodium atoms can bond with one bromine atom?
a)
1
b)
2
c)
3
d)
4
51.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
52.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
53.
What kind of bond forms when atoms share electrons?
a)
Chemical bond
b)
Ionic bond
c)
Covalent bond
d)
Electron bond
54.
Fe+3 combines with S-2 to form
a)
Fe+4(S)=3
b)
Fe2S4
c)
Fe2S3
d)
Fe3S2
55.
AlBr3
a)
aluminum bromide
b)
aluminum tribromide
c)
aluminum bromine
d)
monoaluminum tribromide
56.
What is the correct term for "bond that forms when electrons are shared equally"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
57.
What is the correct term for "bond that forms between a metal and a nonmetal"?
a)
ionic bond
b)
metallic bond
c)
nonpolar covalent bond
d)
polar covalent bond
58.
What is the correct term for "atom with a full valence shell"?
a)
positive ion (cation)
b)
negative ion (anion)
c)
neutral atom
d)
stable atom
59.
Carbon has four electrons in its valence shell. How many nore electrons does carbon need to have a full valence shell?
a)
2 more
b)
4 more
c)
8 more
d)
0 more, it is already full
60.
The correct formula for the diagram is _________.
a)
K2O
b)
2KO
c)
KOK2
d)
KO2
61.
The correct formula for the diagram is _________.
a)
K2O
b)
2KO
c)
KOK2
d)
KO2
62.
Which of the following is a property of all covalent compounds?
a)
They are formed froma metal and a nonmetal.
b)
They are solids.
c)
They share electrons.
d)
They conduct electricity.
63.
Because the overall charge in a compound must be ____________, the charge of iron in Fe2O3 can be calculated as 3+.
a)
2+
b)
1+
c)
0
d)
1-
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