Name: 
 

8th Grade 2009-2010 Miterm Practice Test


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
When particles in a closed container are heated, they
a.
lose volume
c.
lose energy
b.
move faster
d.
move closer together
 

 2. 
The electron was discovered by
a.
Ernest Rutherford
c.
John Dalton
b.
Niels Bohr.
d.
J.J. Thomson
 

 3. 
According to the Rutherford model of the atom, electrons are held in an atom
a.
scattered among the positive charges.
c.
in the nucleus
b.
by the attraction of the positively charged nucleus.
d.
by the attraction of the negatively charged nucleus.
 

 4. 
The substances in a mixture can be separated by physical means because
a.
the physical and chemical properties of the substances change.
c.
the physical, but not the chemical, properties of the substances change
b.
the chemical, but not the physical, properties of the substances change.
d.
no chemical change occurs when the substances are combined.
 

 5. 
Structural formulas have an advantage over molecular formulas because they show the
           
a.
geometric arrangement of the atoms.
c.
percent composition of the compound.
b.
number of atoms of each element present.
d.
bonding capacity of each carbon atom.
 

 6. 
According to the Thomson’s atomic model
a.
Atoms consist of negatively charged electrons scattered among positive charges.
c.
atoms consist of only positive electrical charges.
b.
atoms are either electrically positive or negative.
d.
atoms consist of only negative electrical charges.
 

 7. 
Elements that have 5, 6, 7, or 8 electrons in their outermost energy level are
a.
nonmetals
c.
metalloids
b.
alloys.
d.
metals
 

 8. 
In general, increasing the concentration of reactants causes the reaction to occur
a.
by absorbing energy.
c.
more slowly
b.
by giving off energy.
d.
faster
 

 9. 
Rutherford’s experiment demonstrated that
a.
atoms are positively charged.
c.
atoms are mostly empty space
b.
atoms are present in gold foil
d.
Thomson’s atomic model was correct
 

 10. 
The strong force
a.
causes the attraction between protons and electrons.
c.
causes neutrons to change into protons and electrons.
b.
holds protons in the nucleus together
d.
causes different atoms to be attracted to each other.
 

 11. 
Which of the following is a correctly balanced chemical equation?
a.
Ba(NOmc011-1.jpg)mc011-2.jpg + 2NaCl mc011-3.jpg BaClmc011-4.jpg+2NaNOmc011-5.jpg
c.
KClOmc011-9.jpgmc011-10.jpgKCl+Omc011-11.jpg
b.
K+Hmc011-6.jpgOmc011-7.jpg 2KOH + Hmc011-8.jpg
d.
Hmc011-12.jpgOmc011-13.jpg mc011-14.jpg Hmc011-15.jpgO +Omc011-16.jpg
 

 12. 
Dalton’s atomic theory was incorrect in stating that
a.
compounds form when atoms join together.
c.
atoms are indivisible.
b.
atoms of different elements are different.
d.
all elements are composed of atoms.
 

 13. 
Which of the following gives the correct symbols and formulas
a.
Mg + Omc013-1.jpg = MgOmc013-2.jpg mc013-3.jpg energy
c.
Mg + Omc013-5.jpg = MgO + energy
b.
Mg + O = MgOmc013-4.jpg + energy
d.
Mg + Omc013-6.jpg = MgO mc013-7.jpg energy
 

 14. 
Democritus concluded that matter
a.
consists of protons, neutrons and electrons.
c.
is positively charged.
b.
could be divided into indivisible atoms.
d.
could be divided into smaller and smaller pieces forever.
 

 15. 
Which is not the correct symbol for the element?
a.
Cr-chromium
c.
C-carbon
b.
Ca-calcium
d.
CO-cobalt
 

 16. 
The weakest of the four forces governing the behavior of subatomic particles is
a.
gravity.
c.
strong force.
b.
weak force.
d.
electromagnetic force.
 

 17. 
Mendeleev’s original periodic table of the elements contained many “missing” elements. Using his periodic table, he was able to
a.
correctly predict the properties of the missing elements
c.
find the missing elements.
b.
change the location of the missing elements so there would be no blank spaces.
d.
form the missing elements as a result of chemical reactions
 

 18. 
According to the chemical formula for ammonia, NHmc018-1.jpg, one molecule consists of
a.
3 nitrogen atoms and 1 hydrogen atom
c.
3 nitrogen atoms and 3 hydrogen atoms
b.
1 nitrogen atom and 1 hydrogen atom
d.
1 nitrogen atom and 3 hydrogen atoms
 

 19. 
When substances go directly from the solid phase to the gas phase, the phase change is called
a.
evaporation
c.
vaporization
b.
sublimation
d.
condensation
 

 20. 
In an exothermic reaction,
a.
energy is released.
c.
some energy is destroyed.
b.
energy is taken from the surroundings.
d.
energy is stored in one or more of the products.
 

 21. 
A unit of mass is the
a.
newton
c.
gram
b.
liter
d.
kilometer
 

 22. 
Mendeleev’s periodic table arranged all the known elements in order of
a.
increasing atomic mass.
c.
increasing valence.
b.
decreasing atomic mass
d.
decreasing valence.
 

 23. 
Which is true for all the members of the halogen family?
a.
They have 7 valence electrons.
c.
They are all metals.
b.
They are very inactive.
d.
They may be found free, or chemically uncombined, in nature.
 

 24. 
The chemical reaction between an acid and a base is called
           
a.
dissociation
c.
neutralization
b.
emulsification
d.
ionization
 

 25. 
Carbon atoms
a.
 may form either covalent or ionic bonds.
c.
form covalent bonds.
b.
form ionic bonds.
d.
never form bonds with other carbon atoms.
 

 26. 
Elements on the left side of the periodic table tend to be
a.
active solids
c.
active gases.
b.
inactive gases
d.
inactive solids
 

 27. 
A substance that dissolves in water is
a.
insoluble
c.
soluble
b.
a solvent
d.
a colloid
 

 28. 
Elements on the right side of the periodic table tend to be
a.
active solids
c.
inactive gases
b.
inactive solids
d.
active gases.
 

 29. 
Valence electrons are found
a.
throughout the electron cloud.
c.
in the nucleus.
b.
in the outermost energy level.
d.
in the energy level closest to the nucleus
 

 30. 
Which of the following is a correctly balanced equation describing a synthesis reaction?
a.
Hmc030-1.jpgCOmc030-2.jpg mc030-3.jpg Hmc030-4.jpgO+COmc030-5.jpg
c.
2Hmc030-10.jpg+Omc030-11.jpgmc030-12.jpg 2Hmc030-13.jpgO
b.
3Fe+Omc030-6.jpgmc030-7.jpg Femc030-8.jpgOmc030-9.jpg
d.
KClOmc030-14.jpgmc030-15.jpg KCl+Omc030-16.jpg
 

 31. 
Bohr’s atomic model placed the electrons
a.
in the nucleus.
c.
scattered among the positive charges.
b.
in definite orbits around the nucleus.
d.
in no definite position.
 

 32. 
Which is not a characteristic of a metal?
a.
good conductor of heat and electricity
c.
malleable
b.
found on the far right of the periodic table
d.
ductile
 

 33. 
The mathematical formula for density is
a.
D=m/v
c.
D=m x v
b.
D- m + v
d.
D-v/m
 

 34. 
Which of the following represents a correctly balanced double - replacement reaction?
a.
MgCOmc034-1.jpg +HCl mc034-2.jpg  MgClmc034-3.jpg + H2COmc034-4.jpg
c.
Cmc034-8.jpgH8 + Omc034-9.jpgmc034-10.jpg   3COmc034-11.jpg + 4Hmc034-12.jpgO
b.
Zn+2HCl mc034-5.jpg  ZnClmc034-6.jpg + Hmc034-7.jpg
d.
Ba(NOmc034-13.jpg)mc034-14.jpg + Kmc034-15.jpgSO4mc034-16.jpgBaSOmc034-17.jpg + 2KNOmc034-18.jpg
 

 35. 
In a structural formula, each dash (—) represents a(an)
           
a.
electron
c.
negative charge.
b.
pair of electrons.
d.
bond between 2 carbon atoms.
 

 36. 
An example of a substance that sublimes is
a.
dry ice
c.
regular ice
b.
ice cream
d.
ice water
 

 37. 
As a result of an endothermic reaction
a.
the reactants have more energy than the products.
c.
the products have more energy than the reactants.
b.
no energy change occurs.
d.
the reactants and the products have the same amounts of energy.
 

 38. 
In attempting to group elements, Mendeleev used their
a.
physical properties only
c.
chemical properties only
b.
physical and chemical properties
d.
melting point only.
 

 39. 
The type of bond that forms between sulfur and oxygen is
a.
ionic
c.
none of these since the two atoms cannot combine.
b.
metallic
d.
covalent
 

 40. 
Which of the following has a definite volume, but not a definite shape?
a.
plasma
c.
liquid
b.
solid
d.
gas
 

 41. 
In chemical combinations, nonmetals tend to
a.
lose electrons
c.
gain, lose, or share 1 electron
b.
gain, lose, or share 4 electrons.
d.
gain electrons
 

 42. 
A catalyst is a
a.
substance that is changed as a result of a chemical reaction
c.
substance that lowers the activation energy needed for a reaction.
b.
products that speeds up the rate of a reaction
d.
reactant that speeds up the rate of a reaction.
 

 43. 
Which of the following is a correctly balanced equation describing a decomposition reaction?
a.
Cu+AgNOmc043-1.jpgmc043-2.jpg CuNOmc043-3.jpg+Ag
c.
Hmc043-8.jpgCOmc043-9.jpgmc043-10.jpg Hmc043-11.jpgO+COmc043-12.jpg
b.
Femc043-4.jpgOmc043-5.jpgmc043-6.jpg 2Fe+Omc043-7.jpg
d.
KClOmc043-13.jpgmc043-14.jpg KCl+Omc043-15.jpg
 

 44. 
An example of a chemical property is
a.
mass
c.
the ability to rust
b.
density
d.
color
 

 45. 
The smallest particle of a compound that retains the properties of the compound is called a(an)
a.
atom
c.
element
b.
molecule
d.
proton
 

 46. 
The formation of a chemical bond involves
a.
only the electrons.
c.
protons and electrons.
b.
electrons and neutrons.
d.
only the protons.
 

 47. 
Which of the following is a correctly balanced chemical equation?
a.
2Hmc047-1.jpg+Omc047-2.jpgmc047-3.jpg 2Hmc047-4.jpgO
c.
Zn+2AgNOmc047-9.jpgmc047-10.jpg Zn(NOmc047-11.jpg)mc047-12.jpg
b.
Nmc047-5.jpg+3Hmc047-6.jpgmc047-7.jpg NHmc047-8.jpg
d.
Cu+Omc047-13.jpg Cumc047-14.jpgO
 

 48. 
Which part of the atom is involved in chemical bonding.
a.
only the electrons
c.
only the valence electrons.
b.
only the nucleus
d.
only the protons
 

 49. 
An example of a crystalline solid is
a.
glass
c.
table salt
b.
tar
d.
candle wax
 

 50. 
An example of a chemical reaction is the
a.
shattering of a glass
c.
freezing of ice
b.
explosion of fireworks
d.
drying of wet laundry
 

 51. 
Which of the following is a metalloid?
a.
iron
c.
silicon
b.
copper
d.
sodium
 

 52. 
According to Charles’s Law
a.
pressure of a gas increases if volume decreases
c.
volume of a gas increases if temperature increases
b.
pressure of a gas decreases if volume decreases
d.
volume of a gas decreases if temperature increases
 

 53. 
When an atom loses electrons, it
a.
becomes negatively charged.
c.
becomes positively charged.
b.
will form a metallic bond.
d.
obtains a neutral charge
 

 54. 
Atoms with a low ionization energy
a.
tend to form negative ions.
c.
gain electrons easily.
b.
tend to remain neutral.
d.
lose electrons easily.
 

 55. 
The chemical equation Hmc055-1.jpg+Omc055-2.jpgmc055-3.jpg  Hmc055-4.jpgO is not balanced because
a.
the same numbers and kinds of atoms are not present on both sides of the equation.
c.
hydrogen and oxygen are destroyed
b.
the same substances do not appear on both sides of the equation
d.
the same numbers and kinds of molecules are not present on both sides of the equation
 

 56. 
The mass of your science textbook is approximately
a.
1600 kg.
c.
160 g.
b.
160 kg.
d.
1600 g.
 

 57. 
All acids contain the element
              
a.
nitrogen
c.
chlorine
b.
hydrogen. 
d.
oxygen.    
 

 58. 
The formula for zinc iodide is ZnImc058-1.jpg.  What is the oxidation number of zinc in zinc iodide?
a.
2-
c.
1-
b.
1+
d.
2+
 

 59. 
Acids react with active metals to produce  
a.
a. hydrogen gas.
c.
oxygen gas.
b.
different gases, depending on the acid.
d.
either hydrogen or oxygen gas.
 

 60. 
An example of a physical change is the
a.
process called photosynthesis
c.
rust on a garden tool
b.
change in the color of leaves in the autumn
d.
shredding of a piece of paper
 

 61. 
An atoms with an oxidation number of 2-
a.
has 6 valence electrons.
c.
has 2 valence electrons.
b.
will form an ion with a charge of 2+
d.
will form an ion with a charge of 6-
 

 62. 
A solution is a
a.
type of molecule
c.
heterogeneous mixture
b.
homogeneous mixture
d.
type of compound
 

 63. 
According to Boyle’s law, if the volume of a gas is decreased, the
a.
particle collisions within the gas will increase
c.
temperature of the gas will increase
b.
particle collisions within the gas will decrease
d.
pressure of the gas will decrease
 

 64. 
Which does not occur as a result of a chemical reaction?
a.
Molecules may react with other molecules.
c.
Atoms may join with other atoms or molecules.
b.
Molecules may be broken apart to become atoms.
d.
New atoms may form.
 

 65. 
The units used to measure density are
a.
grams per milliliter
c.
newtons per kilogram
b.
milliliters
d.
cubic centimeters
 

 66. 
The pH of acid rain is likely to be
           
a.
7.
c.
0.
b.
4.
d.
10.
 

 67. 
When two or more substances are combined, but each retains most of its properties, the resulting combination is called a(an)
a.
compound
c.
mixture
b.
homogeneous substance
d.
element
 

 68. 
Of the following, the strongest base would have a pH of
                                                                 
a.
6.
c.
10. 
b.
7.
d.
3.  
 

 69. 
The noble gases are inactive because
a.
they are all low-density gases.
c.
their outermost energy levels are complete.
b.
they are nonmetals.
d.
they all have 6 valence electrons.
 

 70. 
The products of any acid-base neutralization reaction always include
a.
hydronium ions.
c.
hydrogen gas
b.
hydroxide ions
d.
water.
 

 71. 
An ionic bond results from
a.
attractions between oppositely charged ions.
c.
the sharing of electrons.
b.
attraction between ions having the same charge.
d.
attractions between neutrally charged atoms.
 

 72. 
Sharing of electrons occurs in
a.
the formation of ions
c.
metallic bonding
b.
covalent bonding
d.
ionic bonding.
 

True/False
Indicate whether the sentence or statement is true or false.
 

 73. 
A reactant is formed as a result of a chemical reaction.
 

 74. 
Most of the elements of the periodic table exist naturally as solids.
 

 75. 
The nucleus makes up about 99.9 percent of the mass of the atom.
 

 76. 
An alloy is a type of heterogeneous mixture
 

 77. 
Ctf077-1.jpgHtf077-2.jpg is an example of a structural formula.
 

 78. 
The amount of matter in an object determines its weight.
 

 79. 
An atom that contains 11 protons also contains 11 electrons.
 

 80. 
An amorphous solid can be thought of as a slow-moving liquid.
 

 81. 
The nucleus of an atom is positively charged.      .
 

 82. 
Matter is always solid.
 

 83. 
Subscripts may be used to balance chemical equations.
 

 84. 
Nonmetals have relatively high melting points.
 



 
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