# CHEMISTRY SOL REVIEW DAY 4 SOLs 1 & 5 by hcj

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```									CHEM SOL REVIEW
DAY 4
SOLS 1 & 5
SCIENTIFIC INVESTIGATIONS
A ___________________ is an
explanation that might be true and
can be tested.
Hypothesis
The factor that is changed in the
experimental group is the _____
variable. It is plotted on the x-axis.
Independent
SCIENTIFIC INVESTIGATIONS
What  you measure in an
experiment is called the
________________ variable. It is
plotted on the y-axis.
Dependent
Name 3 good safety rules for a
Chemistry lab.
UNIT 1 – SCIENTIFIC MEASUREMENT
Write  the following numbers in
scientific notation.
52, 300
 5.23 x 104
0.035
3.5 x 10-2
UNIT 1 – SCIENTIFIC MEASUREMENT
The measure of how close a
measurement is to what it
should be is called the ____
Accuracy
The repeatability of a
measurement is called ____
Precision
UNIT 1 – SCIENTIFIC MEASUREMENT
Which of the following is both
accurate and precise?
UNIT 1 – SCIENTIFIC MEASUREMENT
I conduct an experiment and
measure the mass of a substance
as 7.31 g. The accepted value is
7.5 g. What is the percent error?
(7.5-7.31) / 7.5 x 100
2.5%
2009 SOL QUESTION
A  student determined that the density of
a sample of tin is 8.00 g/mL, when the
actual density is 7.28 g/mL. What is the
percent error?
 F 0.72%
 G 9.0%
 H 9.9%
 J 91%
UNIT 1 – SCIENTIFIC MEASUREMENT
How   many significant figures are in
each of the following numbers?
 2.03
 0.00860
 78,000
 5001
 4.0 x 104
2009 SOL QUESTION
A  compound has a mass of
2.6632 x 102 g/mol. The number
of sig figs in this mass is –
F 2
G 4
H 5
J 7
UNIT 1 – SCIENTIFIC MEASUREMENT
 When   measuring volume with a
graduated cylinder, be sure to measure
at the bottom of the ________________
 Meniscus
 When measuring temperature, do not
allow the thermometer to touch the
_______________ of a beaker or other
container.
 Bottom or sides
 Mass is typically measured in _________
 Grams
UNIT 11 - SOLUTIONS
Label   this graph
UNIT 11 - SOLUTIONS
Label the phases in the phase
diagram below.
UNIT 11 - SOLUTIONS
Label the triple point in the phase
diagram below.
Critical
point
UNIT 11 - SOLUTIONS
Label  the normal melting point in
the phase diagram below.
Normal
boiling
point
2009 SOL QUESTION
When   1 g of NaCl is placed in
100g of water, a solution results.
Once the solution is prepared,
water is now considered what
part of the solution?
F Solute
G Solvent
UNIT 13 – EVERYTHING ELSE
Vaporization  is an _____ process.
 Endothermic
Freezing is an ______process.
 Exothermic
Heat (q) is the ________ of energy
between objects at different
temperatures.
Transfer
UNIT 13 – EVERYTHING ELSE
Heat  is an ________ property ---
it depends on the amount of the
substance present.
 Extensive
The total energy content of a
sample is called its __________.
Enthalpy
UNIT 13 – EVERYTHING ELSE
What  kind of reaction is shown
in the graph below?
UNIT 13 – EVERYTHING ELSE
 The  measure of disorder or randomness in
a system is called the
______________________.
 Entropy
 A catalyst is a substance that speeds up
the reaction by ___ the activation energy.
 Lowering
 Increasing the temperature,
concentration, pressure, or surface area of
a substance will ______ the reaction rate.
 Increase
UNIT 13 – EVERYTHING ELSE
Label   this graph
B

D
C
A
UNIT 13 – EVERYTHING ELSE
 When   the forward and reverse reactions
happen at the same rate, it is called ___
 Chemical equilibrium
 Give an example of a completion
reaction.
 Le Chatelier’s principle states that when
a system is at equilibrium is disturbed,
the system adjusts in a way to
______________ the change.
 Reduce
UNIT 13 – EVERYTHING ELSE
 Increasing  the concentration of the
reactants will make the ______
reaction faster than the reverse.
 Forward
 This is called a shift __________.
 Right
 An oxidation reaction is one in which
electrons are __________.
 Lost
UNIT 13 – EVERYTHING ELSE
 Assign oxidation numbers to each
element in each of the following.
 K+
 1+
 O2
0
 CaH2
 Ca = 2+, H =1-
 NH4-
 H = 1+, N = 5-

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