Semester Two Review Packet

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Semester Two Review Packet
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Unit Nine States of matter
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• Intermolecular Forces attractive forces between
  molecules
• Surface Tension tendency of liquids to minimize
  surface area
• Viscosity resistance of a liquid to flow
• Volatile easily evaporates
• Vapor Pressure pressure exerted by a liquids
  vapor molecules
• Melting phase change from solid to liquid
• Freezing - phase change from liquid to solid
• Boiling - phase change from liquid to gas
• Condensing - phase change from gas to liquid
• Sublimation - phase change from solid to gas
• Deposition - phase change from gas to solid

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• 2. Gases would have weak intermolecular forces
  whereas solids and liquids would have strong
  intermolecular forces.
• 3. The rate of vaporization increases with
• - increase in surface area
• - increase in temperature
• - decrease in strength of IMF
• 4. Vapor pressure increases with
• - decreases in strength of IMF
• - increase in temperature
• 5. To make a liquid boil
• - increase the temperature
• - decrease the atmospheric pressure
• 6. To make a gas condense
• - decrease the temperature
• - increase the atmospheric pressure

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• 7. How much energy would be needed to vaporize
  43.0 g of water?
• 8. How much energy would be needed to melt 28.0 g
  of ice?
• 9. What quantity of heat would need to be added
  to 123.4 g of water to change its temperature
  from 52C to 86C?

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• 10. Dispersion is a temporary uneven distribution
  of electrons that increases with molar mass,
  symmetry and surface area.
• 11. Dipole Dipole is a permanent distribution
  of electrons
• 12. Hydrogen Bonding occurs when hydrogen is
  bonded to nitrogen, oxygen, or fluorine.
• 13. Molecular Solids have neutral corners, low
  melting points, are nonmetal with nonmetal or a
  metalloid with a metal or nonmetal.
• 14. Covalent Solids have neutral corners, high
  melting points, are metalloid with metalloid, or
  a metalloid with a metal or nonmetal.
• 15. Metallic Solids have positive ions and are
  metals with metals.
• 16. Ionic Solids have positive and negative ions
  at the corners and are metals with nonmetals.
• 17. Why is water unique?
• Water has a low molar mass yet is a liquid at
  room temperature, easily dissolves polar and
  ionic compounds, expands upon freezing, and its
  ice is less dense than water.

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• 18. What is the percentage of water, by mass, in
  FeSO47H2O?

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Unit Ten Gas Laws
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• 19. Standard pressure is
• 1 atm, 101.325 kPa, 760 mmHg, and 14.7 psi
• 20. Temperature must be in units of Kelvin.
• K 273 C
• 21. What are the relationships between pressure
  and volume, pressure and temperature, volume and
  temperature, and volume and the number of moles?
• - P increases V decreases
• - V increases and T increases
• - V increases and n increases
• - P increases and T increases

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• 22. A gas mixture contains helium, oxygen, and an
  unknown gas. Calculate the partial pressure (in
  atm) of the unknown gas when the partial pressure
  of helium is 503 mmHg, oxygen is 214 mmHg, and
  the total pressure is 1.13 atm.
• 23. If a balloon occupies 1.49 L at room
  temperature (25.0C), what temperature in C
  would you need to increase the volume to
  3.07L?
• 24. If there is a pressure of 536 mmHg in a
  container and it is heated from 20.0C to
  100.0C, what is the new pressure?
• 25. A hand pump with a moveable piston has an
  applied pressure of 3.08 atm and a volume of
  3.25L. What is the volume if the applied
  pressure is decreased to 1.18 atm?

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• 26. If you transfer a gas at room temperature
  (25.0C ) from a 5.89 L cylinder to a 2.41 L
  container and the pressure increases from 0.653
  atm to 1.36 atm, what is the final temperature in
  C?
• 27. If you blow up a balloon with helium gas and
  the volume increases from 56.3 mL to 1006 mL and
  there are initially 0.163 moles, how many moles
  need to be added?
• 28. If 28.4 L of Cl2 react with an unlimited
  supply of H2 at STP, how many moles of HCl would
  be produced?
• 29. If helium effuses 3.60 times faster than an
  unknown gas sample, what is the molar mass of the
  unknown gas?

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Unit Eleven Solutions
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• 30. Terms
• Solution a homogeneous mixture of two or more
  substances
• Solute the minority component
• Solvent the majority component
• Suspension a mixture from which the particles
  settle out upon standing
• Colloid a permanent mixture whose particles are
  smaller than a suspension and larger than a
  solution
• Tyndall Effect a way to differentiate solutions
  from colloids and suspensions based on the
  scattering of light
• Electrolyte aqueous solutions containing a
  solute that dissociates into ions and conducts
  electricity
• Solubility the amount of component that will
  dissolve in a certain amount of liquid
• Saturated holds the maximum amount of solute
  under the solution conditions

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• Unsaturated holds less than the maximum amount
  of solute under the solution conditions
• Supersaturated holds more than the normal
  maximum amount of solute
• Concentration the amount of solute in a
  solution
• Mass Percent the number of grams of solute per
  100 grams of solution
• Molarity the number of moles of solute per
  liter of solution
• Molality the number of moles of solute per
  kilogram of solvent
• Colligative Properties a property that depends
  on the number of solute particles and not the
  type of solute particle (how much you have not
  what you have)
• Freezing Point Depression difference in
  temperature between the freezing point of a
  solution and the freezing point of the pure
  solvent
• Boiling Point Depression difference in
  temperature between the boiling point of a
  solution and the boiling point of the pure
  solvent

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• 31. Which of the following will scatter light?
• - colloid and suspension
• 32. What would happen to the following if more
  solute is added to the solution
• - Saturated nothing will happen
• - Unsaturated solute will dissolve
• - Supersaturated extra solute will disrupt the
  solution and precipitate out
• 33. Solubility depends on
• - identity of solute and solvent
• - temperature
• - pressure (only gases)
• 34. Factors that increase the rate of solution
  are
• - decreasing the particle size
• - stirring
• - increasing temperature (except for gases)

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• 35. Solubility Curve
• a. Pb(NO3)2 at 30C
• - 66 g
• b. 12 g of KClO3
• - 35C
• c. 70 g of CaCl2 at 16C
• - saturated
• 36. A soft drink contains 85.2 grams of sucrose
  (C12H22O11) in a 741 mL solution. What is the
  percent mass if the density of the solution is
  1.00 g/mL?
• 37. What is the molarity of a solution that
  contains 98.5 grams of MgBr2 dissolved to produce
  a 1.00 L solution?

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• 38. What volume of 12 M HCl do you need to make
  500.0 mL of a 3.0 M solution?
• 39. Determine the volume in milliliters of 0.225
  M KOH solution required to neutralize 185 mL of
  0.125 M HCl. The neutralization reaction is
• KOH(aq) HCl(aq) ? H2O(l) KCl(aq)
• 40. Calculate the molality of a solution
  containing 225 grams of glucose (C6H12O6)
  dissolved in 1.25 L of water. (Assume the
  density of 1.00 g/mL for water).

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• 41. What is the freezing point depression and the
  boiling point elevation of a 2.43 m solution of
  Al2(SO4)3 in water?

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Unit Twelve Acids and Bases
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• 42. Determine whether the following are acids
  (A), bases(B), or both (X).
• a. ____ pHgt7 b. ____ Tastes bitter
• c. ____ Tastes sour d. ____ pHlt7
• e. ____ Corrosive to skin f. ____ Blue litmus
  red
• g. ____ Feels slippery h. ____ Electrical
  Conductor
• i. ____ Red litmus blue
• 43. Name the following formulas
• a. CsOH
• - cesium hydroxide
• b. H2S
• - hydrosulfuric acid
• c. HNO3
• - nitric acid
• d. HNO2
• - nitrous acid

B
B
A
A
A
A
B
X
B
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• 44. Write the formulas of the following names
• a. hydrobromic acid
• - HBr
• b. iron (II) hydroxide
• - Fe(OH)2
• c. phosphoric acid
• - H3PO4
• d. chlorous acid
• - HClO2
• 45. Explain how water is amphoteric.
• Water can act as an acid and a base. It is able
  to accept and donate protons.
• 46. List the six strong acids HCl, HBr, HI,
  HClO4, H2SO4, HNO3
• 47. List the eight strong bases LiOH, NaOH, KOH,
  RbOH, CsOH, Ca(OH)2, Ba(OH)2, Sr(OH)2
• 48. The ion product constant for water is Kw
  1.0 x 10-14

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• 49. Calculate the pH, pOH, H, and OH-.
  Identify the type of solution as acidic, basic,
  or neutral.

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• 50. What are the reactants and products in an
  acid base reaction?
• - reactants acid and base
• - products water and salt (ionic compound)
• 51. What is the purpose of titrations?
• A titration is an experimental technique used to
  determine the concentration of an unknown
  acid/base by comparing it to an acid/base
  solution of known concentration
• 52. H2SO4 (aq) Ba(OH)2 (aq) ?
  BaSO4(aq) 2 H2O(l)
• 53. 2 Al(OH)3(aq) 3 H2SO4(aq) ?
  Al2(SO4)3 (aq) 6 H2O(l)
• 54. What is the molarity of a solution of NaOH if
  34.2 mL of the solution is used to neutralize
  25.3 mL of 0.50 M HCl?

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• 55. How many milliliters of 1.25 M HCl must be
  added to 50.0 mL of 2.50 M LiOH to make a neutral
  solution?
• 56. What is a buffer? What do they consist of?
• A buffer is a solution that resists a change in
  pH. Buffers contain a weak acid and its conjugate
  base.
• 57. For the following questions label each part
  of the following chemical reactions with acid
  (A), base (B), conjugate acid (CA) and conjugate
  base (CB).

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Unit Thirteen Equilibrium
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• 58. Terms
• Activation Energy - amount of energy that must be
  absorbed by reactants before a reaction can occur
• Catalyst - a substance that increases the rate of
  a chemical reaction but is not consumed by the
  reaction
• Equilibrium - when forward and reverse reactions
  are occurring under the same conditions and at
  the same rate
• Enthalpy - the energy difference between the
  reactants and products another word for energy
• Entropy - randomness, disorder
• Equilibrium constant - product of concentrations
  of products divided by the product of the
  concentrations of reactants
• Free Energy - the net balance or difference
  between energy (enthalpy) and entropy

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• Le Châteliers Principle - when a chemical system
  at equilibrium is disturbed, the system shifts in
  a direction that minimizes the disturbance
• Reversible Reaction - a reaction where the
  products can re-form reactants
• Solubility Product Constant - is an equilibrium
  expression for a chemical equation that
  represents the dissolving of an ionic compound
• Spontaneous - happens on its own, does not have
  to be forces
• Static - at rest not changing
• Steady State - constant change but unlike
  equilibrium there is no reverse reaction
• Thermodynamic - the study of energy relationships

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• 59. Describe each of the following situations as
  either equilibrium or steady state. a. Lake
  Wissota Dam and the water behind it. The level
  in the lake is constant. Steady State b. The
  liquid in a sealed container and the vapor above
  it at constant temperature Equilibrium c. The
  solid solute remaining in a sealed container of
  solution Equilibrium
• 60. For the reaction below, Keq 0.39. If the
  equilibrium concentration of HC2H3O2 is 2.3 M,
  what are the equilibrium concentrations for the
  two ions below? HC2H3O2 (aq) H2O (l) ?
  H3O(aq) C2H3O2 (aq)
• 61. Calculate the value of Keq for the reaction
  below, using the given equilibrium
  concentrations CH4 (g) 3 Br2 (l) ?
  CHBr3 (aq) 3 HBr (aq)

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• 62. What causes a system at equilibrium to shift?
  Stress
• 63. Methyl alcohol (methanol) is made according
  to the following net equation. Predict the
  effect on the equilibrium system (shift left,
  shift right, or no effect).
• CO (g) 2 H2 (g) ? CH3OH (g)
  heat
• a. CO is added to the container RIGHT
• b. The volume is decreased RIGHT
• c. A catalyst is added NO EFFECT
• d. Temperature is increased LEFT
• e. Pressure is increased RIGHT
• f. Hydrogen gas is removed LEFT
• 64. Write the complete equation for Fe(OH)2 and
  write the Ksp expression.
• Fe(OH)2 ? Fe2 2OH- Ksp Fe2OH-2

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•  

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Unit Fourteen Redox
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• 68. Assign an oxidation number to the specified
  atom in each of the following examples.

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• 71. Will the following redox reactions be
  spontaneous?
• a. Pb(s) Sn2(aq) ? Pb2(aq) Sn(s) NO
• b. Pb(s) Ag(aq) ? Pb2(aq) Ag(s) YES
• 72. How can you pre-determine if a metal will
  dissolve in an acid?
• If the metal is below H2 on the activity series
  it will not dissolve in the acid. If the metal
  is above H2 on the activity series it will
  dissolve in an acid.
• 73. Calculate the cell voltage and give the cell
  notation for electrochemical cells made from the
  following electrodes.
• Ecell 1.05v Ni Ni2 2Ag 2Ag

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Unit Fifteen Organic
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• 80. Draw isomers of hexane.

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Unit Sixteen Biochemistry
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• 93. Dogs may eat homework but do they digest it?
  Explain why. Paper is made of cellulose which
  is indigestible so the dog cannot digest the
  paper.
• 94. The insulin protein contains 51 amino acids.
  How many DNA base pairs are required to code for
  all the amino acids in insulin? 153
• 95. When wet hair is put into curlers and allowed
  to dry, the hair tends to retain the shape of the
  curler. Why? When hair dries the hydrogen bonds
  stay in place from when wet, therefore keeping
  the shape of the curler.
• 96. Why is shape so important in the functions of
  proteins? The shape determines the function.
  Heat can denature and change shape therefore
  change function.
• 97. Name three lipids of the cell and describe
  their function. Answer will vary

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• 98. What are the different structures of
  proteins? How would you identify these
  structures? Primary amino acid sequence
• Secondary short range repeating pattern along
  protein chain Tertiary large scale bends and
  folds Quaternary arrangement of chains in
  protein
• 99. How are alpha-helix proteins different from
  beta-pleated sheet proteins? Alpha helix is a
  coil held together through hydrogen bonds of NH
  and CO. The side chains extend outward.
• For beta-pleated sheets the peptide backbones of
  the chain interacts through hydrogen bonds. The
  side chains extend above and below.
• 100. The anti-HIV medicine AZT introduces a fake
  thymine molecule into the cell. When a virus
  attempts to use the fake nucleotide in
  replicating its DNA, the fake nucleotide doesnt
  work. Below are diagrams of the fake thymine on
  the left and the real thymine on the right. How
  does AZT keep the virus from replicating when the
  virus tries to incorporate the fake thymine into
  its DNA? Azidothymidine and thymine have the
  same shape but slightly different structures.
  Thymine has an OH group and azidothymidine has an
  amine group (-NNNH). The different structure
  has a different function.

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Final Schedule

• Friday
• 1st Hour 835 1030
• 2nd Hour 1040 1235
• Lunch 1235 130
• 3rd Hour 135 335
• Monday
• 4th Hour 835 1030
• 5th Hour 1040 1235
• Lunch 1235 130
• 6th Hour 135 335