S.O.L. Review

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S.O.L. Review

• Down to the wire!

2
What do you need to do now?

• Eat a good dinner, go to bed at a decent hour.
• Be on time for school tomorrow.
• Eat a good breakfast and avoid excess caffeine.
• I will be serving snacks in my room from
  815-850
• Your SOL is in the library at 905

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What do I need to study?

• Review with your flashcards, but remember they do
  not cover everything
• Review the chapter summaries in your textbook
• Look over your notes and old tests
• Look at the ppt on my website
• USA Test Preps J-Labs ARE NOT ENOUGH!!!!!

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Gas Laws

• P?, V?
• P?, T?
• V?, T?
• What law does this graph represent?

5
Chemical or Physical Change?

• A banana turns brown
• Water boils
• Licking a lollipop
• Baking bread
• Soda explodes when you shake it up

6
Safety

• What do you do with waste chemicals?
• Where do you find information on a chemical?
• What equipment protects you from toxic vapors?
• Where does broken glass go?
• What do you do when you get splashed with a
  chemical?

7
Name these chemicals!

• NaF
• sodium fluoride
• K2CO3
• potassium carbonate
• MgCl2
• magnesium chloride
• Be(OH)2
• beryllium hydroxide

• Ca3(PO4)2
• calcium phosphate
• (NH4)2SO4
• ammonium sulfate
• Mn(NO3)3
• manganese (III) nitrate
• FePO4
• iron (III) phosphate

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Write these formulas!

• potassium fluoride
• KF
• ammonium nitrate
• NH4NO3
• magnesium iodide
• MgI2
• copper (II) sulfate
• CuSO4
• aluminum phosphate
• AlPO4

• lead (II) nitrate
• Pb(NO3)2
• cobalt (II) selenide
• CoSe
• silver cyanide
• AgCN
• copper (II) carbonate
• CuCO3
• iron (II) oxide
• FeO

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These are covalent, why?

• SiF4
• silicon tetrafluoride
• N2S3
• dinitrogen trisulfide
• HBr
• hydrogen bromide (or hydrobromic acid)
• Br2
• bromine

10
Write these covalent compounds?

• diboron hexahydride
• B2H6
• nitrogen tribromide
• NBr3
• sulfur hexafluoride
• SF6
• diphosphorus pentoxide
• P2O5

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What is the empirical formula?

• C2H4O2
• CH2O
• methane
• CH4
• C6H12O6
• CH2O

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What do these look like?

• carbon disulfide
• CS2 is linear and non-polar
• boron trifluoride
• BF3 is trigonal planar and non-polar
• difluoromethane
• CH2F2 is tetrahedral and polar

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Conversions . . . YEA!

• 30 grams of H3PO4
• 0.31 moles
• 25 grams of HF
• 1.25 moles
• 110 grams of NaHCO3
• 1.31 moles
• 1.1 grams of FeCl3
• 0.0068 moles

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Moles to mass . . .

• 4 moles of Cu(CN)2
• 462 grams
• 5.6 moles of C6H6
• 436.8 grams
• 21.3 moles of BaCO3
• 4202.5 grams
• 1.2 moles of (NH4)3PO3
• 159.6 grams

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Moles ? gas volume . . .

• 25 Liters of O2
• 1.12 moles
• 10 moles of N2
• 224 L
• 1.0 x 105 Liters NH3
• 4460 moles
• 2.35 x 10-2 moles H2O(g)
• 0.527 L

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Percent Error

• If you measured 23 out of 90
• 74.4 error
• If you measured 78 out of 85
• 8.23 error
• If you start with 100g but only recover 43.
• 57 error

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Balancing Equations

• Balance equations because of the Law of
  Conservation of Matter the mass of the
  reactants mass of products
• __N2 __H2 ? __NH3
• __C6H12O6 __O2? __H2O __CO2
• __Ca3(PO4)2 __ZnCl2 ? __CaCl2 __Zn3(PO4)2

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Percent Yield

• My theoretical yield is 500g but actual recovery
  was only 327g
• 65.4 recovery
• If the recipe is written to yield 24 muffins, but
  you only got 21 out of them,
• 87.5 recovery

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Molarity!!!!!!!!!!!!!!!!!!!!!!!!

• What is the formula for molarity?
• Molarity moles solute/L of solution
• How do you find moles if you are given mass?
• Moles mass / molar mass (periodic chart)
• What is the formula for a dilution?
• M1V1 M2V2

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Calculate it

• You have 4.5L of a solution that you added 3.15
  moles of NaCl to.
• 0.7M
• How many moles of CuBr do you need to make 10.0L
  of a 3M solution?
• 30 moles
• What is the volume of a 6.3M solution made from
  3.22moles of AgNO3
• 0.511 L or 511 mL

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What are these?

• Isotopes?
• Atomic Number?
• Ions?
• Trend in electronegativity?
• Trend in ionization energy?
• Trend in atomic mass?

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Random

• Formula for density?
• D m/V
• Kelvin conversion?
• K C 273
• Ideal Gas Law?
• PV nRT
• Specific Heat?
• cp q / m x ?T
• pH
• -log10H3O

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What is . . .

• Standard temperature and pressure?
• Oxidation?
• Reduction?
• Arrhenius Acid/Base?
• Bronsted-Lowry Acid/Base?

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Who is?

• Thomsson?
• Rutherford?
• Bohr?
• Mendeleev?
• Moseley?

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What type of reaction is this?

• Na Cl NaCl
• Synthesis
• H2O H2 O2
• Decomposition
• CxHyOz O2 H2O CO2
• Combustion
• A BX AX B
• Single Replacement
• AX BY AY BX
• Double Replacement

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What are these rules?

• Aufbau
• Hunds Rule
• Heisenberg Uncertainty Principle
• Periodic Law
• Paulis Exclusion Principle

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Which forces hold these atoms and molecules
together?

• H2O
• Intramolecular Covalent Bond
• Intermolecular Hydrogen Bonding
• NaCl
• Intramolecular Ionic
• Intermolecular Ionic
• NH3
• Intramolecular Covalent
• Intermolecular Dipole-dipole

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Organic Compounds

• Men Meth-
• Eat Eth-
• Popcorn Prop-
• Butter But-
• Single is ane
• Double is ene
• Triple is -yne

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SOL Review

• Speed Round

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Read each question carefully and choose the best
answer.

• 1. The average kinetic energy of a sample of
  water molecules is
• Increased as the temperature is increased
• Increased as the temperature is decreased
• Unaffected by temperature changes
• Always equal to zero

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• 2. The element chlorine exists as two naturally
  occurring isotopes. Cl-35 occurs 75 of the time
  and Cl-37 occurs 25 of the time. Which of the
  following calculations should be used to
  calculate the correct average atomic mass of
  chlorine?
• A. (35 amu x .75) (37 amu x .25)
• B. (35 amu x 3) 37 amu
• 2
• (35 amu x 3) 37 amu
• 3
• 35 amu 37 amu
• 2

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• 3. The mass of an object was recorded as 9.93 g,
  9.90 g, and 10.02 g, using an electronic
  analytical balance. What is the average of these
  three masses expressed to the correct number of
  significant figures?
• 9.9 g B. 9.95 g C. 10.0 g D. 10.00 g

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• 4. Which of these shows a volume of 1.25 liters
  expressed in milliliters?
• A. 125 mL
• B. 12.5 x 101 mL
• C. 1.25 x 102 mL
• D. 1.25 x 103 mL

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• 5. How does the radioactive isotope C-14 differ
  from its
• stable counterpart C-12?
• It has a different number of protons and two less
  neutrons than C-12
• It has the same number of protons and two more
  electrons than C-12
• It has the same number of protons but two more
  neutrons than C-12
• It has a different number of protons and two more
  neutrons than C-12

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• 6. What is the first step that should be taken
  when a caustic chemical gets into a persons
  eyes?
• Identify the chemical
• Call for an ambulance
• Flush the affected area with water
• Apply a neutralizing agent

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• 7. Which of these conclusions can be drawn from
  Rutherfords experiment?
• Each atom contains electrons.
• The nucleus of an atom can be split.
• Each atom contains protons.
• Atoms are mostly empty space.

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8.
Group Mass Data for Sample X (g) Displacement Data for Sample X (mL)
1 2.7 3.4
2 1.20 1.5
3 6.2 7.40
According to the above data, which of the
following represents the average density for
sample X using the correct number of significant
figures? A. 1 g/mL B. 0.8 g/mL C. 0.81
g/mL D. 0.821 g/mL
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• 1. Which is the correct formula for iron (III)
  sulfate?
• Fe3(SO4)2 B. FeSO4
• C. Fe2(SO4)3 D. Fe2(SO3)3

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• 2. Which of these represents the empirical
  formula and the molecular formula, respectively,
  for a given organic compound?
• CH and C2H2
• CH and CH4
• CH2 and C2H2
• CH3 and C3H12

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• 3. Which of these describes a tendency for atomic
  radii as displayed on the periodic chart?
• Atomic radii decrease left to right across a
  period.
• Atomic radii increase left to right across a
  period.
• Atomic radii decrease top to bottom down a group.
• Atomic radii increase, then decrease from top to
  bottom down a group.

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4. Chlorine forms a 1- ion. How many electrons
does a chloride ion have? A. 1 B. 16
C. 17 D. 18
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• 5. Which of the groups below has the electron dot
  structure shown above?
• Noble gases
• Halogens
• Alkali metals
• Transition elements

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• 6. An element has an electron configuration of
• 1s22s22p63s2. Which of these will be in the
  same group as this element?
• 1s22s22p6
• 1s22s22p63s23p64s2
• 1s22s22p63s1
• 1s22s22p63s23p6

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• 7. Which of these elements is the most chemically
  active?
• A. F B. Cl C. Br D. I

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1. What is the percentage of aluminum in
aluminum oxide (Al2O3)? A. 47 B. 48
C. 53 D. 54
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• 2. A student wanted to calculate the formula for
  hydrated copper sulfate. After careful massing,
  she heated the compound to remove the water. She
  calculated the formula to be CuSO4 . 4H2O. The
  actual formula was CuSO4 . 5H2O. What is the most
  likely source of analytical error in the
  students experiment?
• The water was not completely evaporated from the
  compound.
• The actual mass of the anhydrous CuSO4 was less
  than the measurement.
• The CuSO4 reacted with elemental copper.
• The atmospheric pressure prevented complete
  reaction.

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• 5. Which is an example of a synthesis reaction?
• HCl KOH ? KCl H2O
• Pb(NO3)2 2HBr ? PbBr2 2HNO3
• Mg H2SO4 ? MgSO4 H2
• C O2 ? CO2

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(No Transcript)
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7. Using the chart above, which of these
combinations will probably form a
precipitate? A. Ammonium chloride B. Barium
bromide C. Calcium chromate D. Copper (II)
carbonate
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• 8.
• Very Active Metal Water ? Metal hydroxide ?
• Which of these completes this reaction?
• Oxygen
• Hydrogen
• Metal oxide
• Air

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• 9. A compound is composed of 58.8 C, 9.8 H,
  and 31.4 O, and the molar mass is 102 g/mol.
  What is the molecular formula for this compound?
• C2H10O3
• C5H5O3
• C5H10O2
• CH3O3

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10. NaHCO3(s) HCl(aq) ? NaCl(aq) CO2(g)
H2O(g)
Data Table
Evaporating dish watch glass 42.70
g Evaporating dish watch glass 45.20
g NaHCO3 Evaporating dish watch glass
44.45 g NaCl
A student conducted an experiment and was
interested in the mass of the product of the
chemical reaction. Some results of the experiment
are shown above. What is the mass of the
NaCl? A. 0.75 g B. 1.75 g C. 2.25 g D.
2.50 g
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• 11. A compound is 50 sulfur and 50 oxygen. What
  is the empirical formula?
• SO4
• S2O4
• SO3
• SO2

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A(s) B(s) ? D(g) heat

• 12. The reaction shown above is
• An endothermic reaction
• An exothermic reaction
• A decomposition reaction
• A double-replacement reaction

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• 13. Which compound contains both ionic and
  covalent bonds?
• NH4Cl
• MgBr2
• CH4
• NH3

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• One of the main assumptions of the kinetic
  molecular theory of gases is that the particles
  of an ideal gas
• must be single atoms instead of molecules
• are in constant motion
• must be maintained at very high pressures
• must be highly chemically reactive

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2. A sample of oxygen gas is collected over
water at 220C and 98.67 kPa pressure. If the
partial pressure of the water is 2.67 kPa, the
partial pressure of the oxygen is
A. 93.3 kPa B. 96.00 kPa C. 98.66 kPa D. 101.33
kPa
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3. If the pressure exerted on a confined gas is
doubled, then the volume of the gas --

1. increases four times
2. decreases by one-fourth
3. is doubled
4. is halved

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• 4. Water can be made to boil above its normal
  boiling point of 100oC by
• a. decreasing the air pressure
• b. increasing the air pressure
• c. increasing the heat being applied
• d. decreasing the volume of the
• container

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50 25 0 -25




Temperature (oC)
5 10 15 20 25
Time (min)
5. An experiment yielded the above temperature
and time information. What is the freezing point
of the material in this experiment if the
material is a solid at time zero? a. 25oC b.
0oC c. 25oC d. 50oC
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2H2S (g) 3O2 (g) ? 2H2O (g) 2SO2 (g)

• 6. If 3.50 g of H2S are used in the above
  reaction, what will be the theoretical yield of
  water in grams?
• 0.102 g
• 0.185 g
• 1.85 g
• 185 g

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CH4 2O2 ? CO2 2H2O

• 7. The number of grams of oxygen required for the
  complete combustion of 4.00 grams of methane
  (CH4) is
• 4.00 g
• 8.00 g
• 16.0 g
• 32.0 g

63
Read each question carefully and choose the best
answer.

• A solution contains 225 g of glucose, C6H12O6,
  dissolved in enough water to make 0.825 L of
  solution. What is the molarity of the solution?
• A. 0.66 M B. 0.97 M C. 1.03 M D.
  1.52 M

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2. Which volume will be occupied by a gas
containing 6.02 x 1023 atoms at STP? A. 1.0
L B. 11.2 L C. 22.4 L D. 44.8 L
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• 3. How many milliliters of 2.00 M H2SO4 are
  needed to provide 0.250 mole of H2SO4?
• 125 mL
• 1.25 x 101 mL
• 8.00 x 103 mL
• 8.00 mL

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• 4. A catalyst accelerates a chemical reaction
  because the
• catalyst decreases the number of collisions in a
  reaction
• activation energy of the reaction is lowered in
  the presence of a catalyst
• catalyst decreases the concentration of the
  reactants
• temperature of the reaction increases due to the
  catalyst

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• 5. In the reaction 2SO2 (g) O2 (g) ? 2SO3 (g),
  which change would cause the greatest increase in
  the concentration of SO3?
• Decrease the concentration of SO2
• Decrease the concentration of O2
• Increase the concentration of SO2
• Increase the concentration of O2

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• 6. The hydrogen ion concentration is 1 x 10-7.
  What is the pH of this solution?
• 1
• 7
• 10
• 14

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• 7. Each beaker shown above contains 2.2 grams of
  iron and 1 liter of 3M H2SO4. Which reaction will
  go to completion first and why?
• Beaker A because of increased surface area.
• Beaker B because of increased surface area.
• Beaker A because of a higher concentration level.
• Beaker B because of a higher concentration level.

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8. Four aqueous solutions and their
concentrations are shown in the above
illustration. Which of the solutions is most
likely to be the strongest conductor of
electricity? a. I b. II c. III d. IV
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• 9. If the temperature of a reaction is increased,
  the reaction proceeds at a much quicker rate
  because the
• Activation energy increases
• Energy of the products increases
• Frequency of collisions between reactants
  increases
• Energy of the activated complex increases

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• 10. The formula H2SO4 is representative of which
  of the following?
• A catalyst
• A base
• An acid
• An organic compound

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11. To remove the sand first and then the salt
from a mixture of sand and salt water, one
combination of techniques you could use would be
to first A. evaporate and then distill B.
evaporate and then condense C. filter and then
evaporate D. filter and then condense
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• 12. A student must make a 3M acid solution using
  a 5M acid solution. Which of these is the safest
  way to make the solution?
• Slowly pour the 5M acid into water.
• Slowly add water to the 5M acid solution.
• Mix half the acid with water then add the
  remaining water.
• Mix half the water with acid, then add the
  remaining acid.

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First 6 Weeks SOL Answers

1. A
2. A
3. B
4. D
5. C
6. C
7. D
8. C

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Second 6 Weeks SOL Answers

1. C
2. A
3. A
4. D
5. B
6. B
7. A

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Third 6 Weeks SOL Answers

1. C
2. A
3. B
4. C
5. D
6. D
7. D
8. B

9. C 10. B 11. D 12. B 13. A
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Fourth 6 Weeks SOL Answers

1. B
2. B
3. D
4. B
5. B
6. C
7. C

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Fifth 6 Weeks SOL Answers

• D 6. B 11. C
• C 7. B 12. A
• A 8. B
• B 9. C
• D 10. C