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Chemistry Test
Form 1
Part A: Match the letter of the correct definition to the Vocabulary term.
1. Octet Rule
A. A reaction in which one substance
breaks down into its parts.
2. Ion
B. A bond that is formed by sharing
electrons.
3. Charge
C. A charged atom.
D. The number of electrons an
4. Covalent Bond
element is willing to gain, lose, or
share to form compounds.
5. Ionic Bond
E. States that all elements want
either a full outer shell or eight
6. Subscript
electrons in their outer electron
shell.
7. Polyatomic Ion
F. A multiplier. It is used to balance
equations.
8. Synthesis Reaction
G. A reaction in which two reactant
compounds switch ions.
9. Decomposition Reaction
H. This number tells the number of
atoms of one element in a
10. Single Displacement Reaction
compound.
I. Bonds formed by gaining and losing
11. Double Displacement Reaction
electrons.
J. A group of atoms that act as a
12. Reactants
single charged ion.
K. States that matter cannot be
13. Products
created or destroyed.
L. A reaction in which two or more
14. Law of Conservation of Matter
reactants combine to form one
new product.
15. Coefficient
M. What is made during a reaction
N. The chemicals that undergo a
reaction.
O. A reaction in which one element
replaces another in a compound.
Part B: True/False. You may earn extra credit by correcting false answers.
__________16. If an atom’s charge is positive, it has lost electrons.
__________17. If an atom’s charge is negative, it has lost protons.
__________18. You balance an equation by changing subscripts.
__________19. You can only put a coefficient in front of a compound.
__________20. The number of atoms on both sides of an equation must be equal
for each element.
Part C: For each of the following compounds, identify the number of atoms of each
element.
21. Na2SO4
Na= _____
S= ______
O= _____
22. 3H2CO3
H=_____
C= _____
O= _____
23. Fe(NO3)3
Fe= _____
N= _____
O= _____
Part D: Write the correct chemical formulas for the following pairs of ions.
24. Ca2+
NO3 1- _________
25. Cu2+
F1-  __________
26. Ca2+
CO32- __________
Part E: Identify each reaction as synthesis (S), decompostion (D), single
displacement (SD), or double displacement (DD).
_____27. AgNO3 + NaCl  AgCl + NaNO3
_____28. C + O2  CO2
_____29. Fe + 2HCl  Fe Cl2 + H2
_____30. H2CO3  H2O + CO2
Part F: Identify each of the folowing equations as balanced (B) or not balanced
(NB).
_____31. 2HgO + Cl2  2HgCl + O2
_____32. Na + Br2  2NaBr
_____33. AgNO3 + NaCl  AgCl + NaNO3
Part G: Balance the following equations.
34. C + H2 
CH4
35. Mg +
O2 
MgO
Part G: Multiple Choice
_____35. An atom’s atomic number is
equal to the number of
a. the total protons and
neutrons
b. protons
c. the total electrons and
neutrons
d. neutrons
_____36. The scientists who
developed the format of the
modern Periodic Table are
a. Mendeleev and Meyer
b. Darwin and Mosart
c. Mendel and Meyerson
d. Oscar and Meyer
_____37. The Periodic Table is
arranged by
a. Atomic number
b. Atomic number and properties
c. properties
d. number of electrons
**BONUS**
1. Balance: C8H18 +
O2 
CO2 +
_____39. The Mass number is equal
to the number of
a. protons
b. the total protons and
neutrons.
c. the total electrons and
neutrons
d. neutrons
_____40. Valence electrons are
a. the electrons in the outer
electron shell.
b. The electrons in the first
electron shell.
c. the total number of
electrons.
d. the number of electrons and
atom is wiling to gain, lose, or
share.
H 2O
2. What about an atom’s atomic structure determines its chemical reactivity?
3. Explain the following cartoon on the back of this page.