Download Chemistry Exam Review Sheet

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Chemistry Exam Review Sheet
The final exam will consist of multiple choice questions to be answered on a scantron answer sheet.
The following is a list of topics discussed in class this year to ass you in reviewing for the exam. Since the entire
year cannot be repeated in a few review sessions, it would be most beneficial to you if you bring questions
and/or areas of concern that you would like to have discussed in class. Please come to me before June 8th if
you feel that you need more help with a topic.
Measurement of Matter
Metric system [How many liters is 200 ml?]
Big Mass, Volume, Density (D = M/V)
Calculate the density of an object with a mass of 700 g and a volume of 35 cm3? in mg/L?
Graphing
Lab Equipment (Uses and Names)
Lab Safety
Confirming Test: Reference vs. Control (water testing lab)
How do you separate different mixtures?
Water Unit:
Physical and Chemical Properties
appearance vs. how it reacts?
chemically similar?
List the physical properties of water.
boiling point/ freezing point/ surface tension
solids/ liquids/ gases
(s/l/g/aq)
temperature ? and scales used?
Mixtures:
SOLUTIONS:
solute? solvent?
Example
Solution
Suspension
colloid
Elements- symbols, Compounds-formulas
define?
examples?
Municipal water treatment vs. Mother Nature
List the steps involved in water treatment.
Tyndall effect?
Settle out?
2
Write formulas of compounds with the help of the periodic table or the oxidation numbers. (charges)
a. sodium chloride
b. sodium hydroxide
c. sulfur dioxide
d. Cu (II) and SO4
e. Na and NO3
f. carbon monoxide
Ionic compounds (tooth & notch)
Solubility Curves
solids vs. gases
How do I know if a solution is….
Unsaturated?
Acid vs. Base
Which is the acid? Base?
pH scale litmus paper?
DO
Saturated?
NaOH
Supersaturated?
HCl, how did you know?
Ions: Gain or lose electrons.
How is a cation or an anion formed?
Electron configurations: valence electrons, energy levels
Octet Rule? Stable configuration
Use valence shell to predict ion formed.
Review the 2 handouts from electron configurations.
Use this information to predict the formula given two elements. (remember X & Z?)
Z has 1s22s22p1 and X has 1s22s22p4 what will be the formula of the compound formed?
Like dissolves Like? What does this mean?
Polar
Non-Polar
Ionic
RESOURCES:
Balance Equations
Law of conservation of Matter
Renewable vs. Non-renewable
Physical and Chemical Changes
Has the identity of the substance changed?
Physical
examples?
Observations?
Phase changes such as evaporation/condensation?
Chemical
melting/freezing? Belong in physical or chemical?
Metals, Nonmetals, Metalloids (semi-metals)
Location and Properties on the periodic table:
Do they conduct?
Recall lab experience
Are they malleable or brittle?
Do they react w/ acid?
3
Arrangement of Periodic Table
Families (Groups)
Rows (Periods)
Mendeleev vs. Modern Form
Noble Gases
Periodic Trends
Number of outermost or valence electrons in groups/families and trends in periods
Energy level of electrons in outermost shell related to the periods
Relate to group characteristics
Relate to rows of elements
Relate to ion formation
(most common ionic charge of families)
Chemical properties / Physical properties
Predicting bonds formed using the locations of elements on periodic table
What trends exist as we go left to right in a period or down a group on the periodic table?
Covalent vs. Ionic
Example: Use the following chemical formulas and the periodic table to predict chemical formulas for compounds
containing the pairs of elements.
Na2O
BC13
CaC12
A1F3
K and Se
Sr and I
Ga and Br
Al and Br
Balancing Equations
Coefficients
Subscripts
Counting atoms
CO2 + 2NH3  CON2H4 + H2O
Symbols
Formulas
Moles:
Molar Mass = GFM
Calculate molar mass for:
CaOH
Ca3(PO4)2
Mg(OH)2
FeCl3
6.02 x 1023 particles = 1 mole
given grams convert to moles?
Percent Composition:
Given moles convert to grams?
mass of solute
X 100%
= % composition by
(mass of solute + solvent)
Metal Reactivity: Use of the activity series, significance of location within the series?
Will the following reaction happen?
Mg + AgCl  ?
mass
4
Redox Reactions:
LEO  GER
oxidation
reduction
Oxidizing agent vs. reducing agent
examples?
Half-reactions
Anode vs. cathode
PETROLEUM UNIT:
Organic vs. Inorganic
to build and burn
Refining/fractional distillation
Viscosity Lab: Calculate D = m/v
Relate the # of carbon atoms
Hydrocarbons:
carbon  - hydrogen bonds
Alkane
vs.
Alkene
PACKET
vs.
Alkyne
Saturated?
Unsaturated?
Bonds?
Ionic Bonds
Covalent Bonds – (Polar vs. Nonpolar, why is O2 non-polar?)
Diatomic (HINClBrOF)
As number of carbons increase how does the ….. change? As the number of branches increases?
Boiling Points trends
Viscosity
Surface area
Intermolecular Forces?
What is an isomer? Can you recognize isomers?
Straight-chain vs. branched
Molecular formulas vs. Structural Formulas vs. Electron-dot Diagrams
What is polymerization?
Conservation of Energy:
Exothermic vs. Endothermic
Graphs
Chemical Potential Energy of Reactants compared to the Products
5
Types of Energy (Heat, Light, Chemical, etc.)
Kinetic vs. potential energy
Heat of Combustion:
The Table and use of the table
increasing or decreasing the number of C's changes the heat of combustion (kj/gram) and
the molar heat of combustion (kj/mole) in what way?
Which is the better fuel? Why?
grams to kj? moles to kj?
Specific Heat of water
4.2 J/gC
1 Cal/gC
definition?
If higher (or lower) than water? What does this mean?
Given:
Thermal Energy needed = specific heat x change in temperature x mass of water
FOODS UNIT:
Calorimetry 1 Cal/gC
Carbohydrates
Proteins
Fats
4 Cal/g
4 Cal/g
9 Cal/g
CHO
monosaccharides/ disaccharides/polysaccharides
amino acids
peptide linkage
saturated vs. unsaturated vs. polyunsaturated?
Functional Groups: Carboxylic Acid, Alcohol, Ester, Ether, etc...
Limiting Reactants: chemical reactions
If you are given moles, what is the LR? ER? How much is left over?
If you are given grams? (remember to convert to ‘moles given’ first)
Reaction Rates:
change rates by?
concentration/surface area/temp/catalyst
relate to COLLISIONS!
AIR UNIT:
Characteristics of Gases? demos
Color?
perfume?
The Atmosphere Lab?
The Pressure’s On Lab?
balloon in flask?
marshmallow? Mass & Space
6
Gas Laws:
Boyle's
Charles
Gay-Lusacc's
Combined
Equations?
Examples?
Graphs?
Ideal vs. Real?
Postulates of the Kinetic Molecular Theory of Gases?
relate collisions?
STP:
0C and 1 atm.
Kelvin temperature scale vs. Celsius scale?
1 mole of any gas will occupy 22.4 Liters at STP
Avogadro's Law?
equal volumes of gases at the same temperature and pressure contain the same number of molecules.
moles to moles?
volume to volume? moles to volume?
Heat capacity vs. reflection?
Dynamic Equilibrium:
Rate of forward reaction = rate of reverse reaction
Properties remain constant
Does this mean you have equal amounts of product and reactant?
Shifts. . . if conditions are changed (the concentration of reactants or products). . .
Can you predict the SHIFT?
Acid and Base
pH related to the hydrogen ion concentration
Compare pH values to each other
Strong acid & Strong base vs. Weak acid & Weak base?
Ionic equations: net and total
Neutralization
Write the equation for a neutralization
Dissociation?
7
Buffers
What is a buffer? How do they work? Is it related to Dynamic Equilibrium?
H2O + CO2  H2CO3  H+ + HCO3-
Electrochemistry
Which metal loses electrons? Which loses electrons?
Use of the metal activity series, relate to oxidation and reduction.
Higher on the table means….?
Which metal will act as the cathode or the anode?
Write the half reactions for the following equation
Zn + Cu2+  Zn2+ + Cu
Use of the electronegativity table, what does a higher electronegativity mean? Lower?
Voltaic cell Lab
NUCLEAR UNIT:
Architecture of Atoms: who’s who in the discovery of the atom?
Subatomic particles:
Nucleus - protons,
charge?
mass?
neutrons
Electrons (trends?)
Given 12.011C6 and the isotope 14C6 identify and define:
Atomic Number
Mass Number
Atomic Mass
Isotopes? How do you know if two atoms are the same or just isotopes?
Isotopic Notation… review the YT’s
Molar Mass and Isotopic Abundance
Radioactive decay? alpha/beta/ gamma?
Rutherford's Gold Foil Experiment
Rutherford's experiment in magnetic fields
8
Types of Radiation
EMR
alpha
energy
effect of distance
penetrating ability
shielding effects
*compare all of the above with each other
beta
Balancing Nuclear Equations
Bombardment
Transmutation?
Half-life problems
Define Fission vs. Fusion. What is critical mass?
Conservation of Mass and Energy
Nuclear Power Plants, pros and cons. What about the waste?
gamma