CP CHEMISTRY
FINAL EXAM REVIEW – FALL 2012
Name: _____________________________
___ period
1.
What state of matter has particles relatively far apart, takes the shape of the
container, and is compressible?
2.
Do radioactive substances stay radioactive forever?
3.
What phase (solid, liquid, gas) are the elements that compose family 8A?
4.
Is Boron a metal, nonmetal, or metalloid?
5.
What is the formula for magnesium phosphate?
6.
Which of the following contains a metal, a nonmetal, and a metalloid?
a. B, C, N
b. Li, Si, Ca
c. Cu, Na, Cl
d. Ar, P, Si
7.
What is the formula for hydrofluoric acid?
8.
What is the formula for sulfuric acid?
9.
What is the formula for pentanitrogen heptahydride?
10.
What type of bond is found in an alkene?
11.
What is the formula for the compound formed with magnesium and chorite ions?
12.
What type of ions does nitrogen form?
13.
What subatomic particle is neutral, found in the atom and has a mass of one AMU?
14.
What is the difference between a hypothesis, a theory, and a law?
15.
What pieces of lab equipment are used to measure mass, volume, and length?
16.
What is the difference between precise and accurate?
17.
What law states that the atoms in the reactants must equal the atoms in the
product?
CP CHEMISTRY, FINAL EXAM REVIEW – FALL 20120, page 2
18.
Balance and identify the following reaction:
CaOH
19.
+
HCl

CaCl2
+
H2O
Balance and identify the following reaction:
Fe
+
H2SO4

Fe2(SO4)3
+
H2
20.
What are the characteristics that indicate a chemical reaction has occurred?
21.
Give an example of a chemical reaction.
22.
How is energy related to the three states of matter?
23.
How is the motion of molecules affected by changes in temperature?
24.
How many electrons will sulfur need to be a neutral atom?
25.
Does oxygen need to gain or lose electrons to become stable? How many?
26.
What is the density of water? Will a substance with a density of 0.5 g/mL sink or
float?
27.
Which type of radiation has the weakest penetration ability and has the heaviest
mass?
28.
When two nuclei come together to form one larger nucleus the process is called:
_________________________ .
29.
Fusion is the process used to create new elements. True or False
30.
What is the formula when aluminum and oxygen combine?
31.
When Fe+3 and O-2 form a compound, what is the formula?
32.
What is the name of the compound in #31 and what kind of compound is it?
CP CHEMISTRY, FINAL EXAM REVIEW – FALL 2012, page 3
33.
What type of bond is created when a compound shares electrons evenly?
34.
What type of bond is formed by a transfer of electrons?
35.
Name an element that would have similar properties as fluorine.
36.
Why do elements in the same family/group have similar physical and chemical
properties?
37.
When chlorine bonds ionically, how many electrons does it want to become stable?
38.
An element that cannot conduct electricity, is dull, and is found on the right side of
the periodic table would be classified as a _________________.
39.
What phase of matter are the elements in Group 8A in?
40.
Using the periodic table, which elements have the highest ionization energy and
which ones have the lowest ionization energy?
41.
a.
down a group:
b.
across a period:
How many valence electrons do the following families have:
IA ___
IIA ___
VIIA ___
VIIIA ___
IIIA ___
IVA ___
VA ___
VIA ___
42.
Describe the location of metals, nonmetals and metalloids on the periodic table.
43.
Calculate how much of a 100 gram radioactive sample is left after 20 minutes if the
half-life equals 5 minutes.
44.
What separation technique would be best to separate a mixture of salt and water?
45.
Every element is unique and can be identified by ___________. In the flame test,
electrons first absorb energy, so they jump to ________________ then they
____________ back to their original starting position and give off the extra energy
they absorbed in the form of _______________.
CP CHEMISTRY, FINAL EXAM REVIEW – FALL 2012, page 4
46.
As you go across periods, electronegativity __________________, and as you go
down families, electronegativity ___________________.
47.
How many protons, neutrons, and electrons do the isotopes of C-14 and Kr-84 have?
48.
Given the following electron configuration, 1s22s22p63s2, what does this element
want to do to become stable?
49.
Calculate the average atomic mass for Lithium: Li-6 is 7.5% and Li-7 is 92.5%.
50.
Of the two isotopes listed in #49, which has the greatest effect on average atomic
mass?
51.
Calculate the density for each of these items:
a.
b.
Mass
42.3 g
Initial Volume
22 mL
Final Volume
494. mL
A cube that measures 3.0 cm for the length of one side. The cube has a
mass of 58.6 grams.
52.
If a substance has a density of 0.24 g/mL and a mass of 1250 grams, what volume
will it occupy?
53.
What element ends its electron fill sequence with:
a. 4p2
b. 2p4
CP CHEMISTRY, FINAL EXAM REVIEW – FALL 2012, page 5
54.
Which element from #53 is most stable?
55.
A student conducted a flame test on an unknown substance and the results of the
flame turned out to be blue. Using the data table, which element did the student
most likely have?
Metal
Symbol
Flame Color
Barium
Ba
yellow-green
Calcium
Ca
red
Copper
Cu
green
Lead
Pb
blue
Lithium
Li
pink
Potassium
K
lilac
Sodium
Na
orange
56.
What type of bond can conduct electricity, dissolves in water, and does not dissolve
in oil?
57.
What is the difference between a heterogeneous mixture and a homogeneous
mixture?
58.
What process created all elements heavier than helium?
59.
What is the most reactive group of metals on the periodic table?
60.
Given the following electron configurations, which is the most stable element?
a. 1s22s22p3
b. 1s22s22p4
c. 1s22s22p5
d. 1s22s22p6