CP Chemistry Semester Two Exam

CP Chemistry Semester Two Exam

CP Chemistry Semester Two Exam

  1. Students can prepare a both sides of a 3” X 5” HANDWRITTEN note card (no Xeroxed cards will be allowed), which will be collected when exam is finished, please include your NAME.
  2. Student should bring their own calculator to the exam. All calculators will have the memory erased prior to the exam, and again after the exam is finished.
  3. Teacher will provide a periodic table, polyatomic ion table and molecular shape and polarity sheet.
  4. The exam will be composed of 70 multiple choice questions worth 140 points.
  5. No equations, constants, conversions will be given on the exam. That information should be included on the note card.
  6. The student must decide what information to include on the note card.
  7. Below is a list of topics for the exam. The student should go through each topic and write down any needed information.

Topics may include:

Bonding and Naming

Ionic bond/Metal & Nonmetal/ Cation & Anion Charges/ Electrostatic attraction/

Naming Ionic Compounds / Roman Numerals / Polyatomic Ions

Covalent Bond/ Nonmetal + Non Metal/ naming Molecular Compounds

Electronegativity difference to determine Nonpolar covalent bond/Polar covalent bond

Valence electrons – outermost S & P electrons

Stable Octet

Single bond /Double bond/Triple bond

Electron dot structures/Shared electron pairs/Unshared electron pairs

Valence Shell Electron Pair Repulsion Theory (VSEPR)

Predicting shapes - Tetrahedral / trigonal pyramidal/ trigonal planar/ bent / linear

Reactions

energy change-endothermic/exothermic

atom rearrangement

precipitate/precipitation

solute/solvent

Writing reactions

conservation of atoms

conservation of mass

balancing equations

reactants/ products

balancing compounds

diatomic elements

subscripts/parentheses/coefficients

symbols used in equations (g, l , s , aq ), ,  , etc.

Reaction types

combustion CxHy + O2  CO2 + H2O

synthesis A + B  AB

decomposition AB  A + B

single displacement (check activity series table) AB + C  CB + A or XY + Z  XZ + Y

double displacement (check solubility table) AB + CD  AD + CB

Moles

Finding Molar Masses - H2O is 18.015 g/mol

Avogadro’s Number - 6.02 x 1023 particles/ 1 mole

Individual atoms ratio

Mole ratios in a chemical substance

Energy (in kJ)

Percent composition

Empirical formula

Molecular formula

Stoichiometry (See Stoichiometry Quiz)

Finding Molar Masses - H2O is 18.015 g/mol

Avogadro’s Number - 6.02 x 1023 particles/ 1 mole

Steps required to solve stoichiometry problems

conversion factors g x mol ; L x mol ; mol x g__

g 22.4 L mol

Ratios - mole ratios, molar mass, coefficient ratios

Reactants – excess/ limiting

Yield – actual/theoretical x 100 = % yield (how well a reaction proceeds)

Be able to:

determine the mass or moles of a product from the mass or moles of a reactant

determine the mass of a product from the limiting reactant

% yield from the theoretical yield and the actual yield

actual yield from the theoretical yield and the % yield

determine the mass or moles from volume of the reactant or product at STP

Gases

Properties of gases

Avogadro’s Law (22.4 L / mol) - a direct relationship of volume to number of moles(n) at STP

Standard Temperature and Pressure (STP) 0oC (or 273K) & 1 atm (= 760 mmHg or torr = 101.3 kPa = 14.7psi )

Convert pressures (atm to kPa to mmHg & torr) and temperatures (oC to K)

Relationship of pressure to volume -  pressure =  volume

Relationship of pressure to temperature -  pressure =  temp

Relationship of volume to temperature -  volume =  temp

Boyle, Charles, Gay-Lussac, Avogadro, Combined Gas Law

Ideal Gas Law – PV = nRT R = 0.0821 L atm

Gas Stoichiometry mol K

Solutions

Molarity

Molality

Dilution

Solubility

Solubility Table and Solubility Calculations

FINAL EXAM TIPS

Keep these tips in mind when preparing for final exams.

  • Begin studying 10 days to a week before finals to avoid ineffective cramming at the last minute.
  • Rather than reviewing the material chapter by chapter, make a list of general topics that are certain to be covered. Review well-known concepts quickly; spend more time on problem areas.
  • If you choose to listen to music while studying, choose something light that is not distracting.
  • Take brief breaks as a reward for completing different sections of material. Avoid allowing the breaks to become longer than the time spent studying. Instead of a break, use candy or a snack as an incentive.
  • After a week of preparation, relax the night before the final. Review a little, then watch television or read a good book.
  • Eat a good breakfast the day of the test to improve concentration and provide fuel for the brain.
  • RELAX. The more tense you are, the harder it will be to remember the material.

Topics May Also Include Items I Missed In the Topics Mentioned Above

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