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CHEMISTRY SOL REVIEW DAY 4 SOLs 1 & 5

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CHEMISTRY SOL REVIEW DAY 4 SOLs 1 & 5 Powered By Docstoc
					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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Jun Wang Jun Wang Dr
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