January 21, 2013
Semester Review: You can bring to the semester final a handwritten 3x5 card with any
information you wish to help you on the exam. The following ideas and words may be
helpful to you. Any or all of the following could be on your flashcards, however
remember that you may not use your flashcards on the semester final. Review your
notes, section
All Material from first semester. Safety, Unit 1, Unit 2, and all class activities.
For Unit 2:
Identify all functional groups by molecular formula and structural formula. Recognize
there may be isomers of these)
Relate smell to functional group.
R-C-O-O-H etc.
Relate different smells to functional group.
Classifying molecules. (shape, types of bonds, types of compound, polarity etc.)
Carbon Hydrogen Oxygen Nitrogen Sulfur relationships within compounds
Functional group type and characteristics such as:
Carboxylic acids and names
Ketone and name of substance
Ether and name of substance
Alcohol and name of substance
Amine and name of substance
Ester and name of substance
Reaction of an acid and alcohol forming an ester
Synthesis, synthesis reaction
Prefixes in names telling how many carbons including but not limited to:
Meth, Eth, Prop, But, Pent, Hex, Hept/Sept, Oct
Smell such as:
Iso
Putrid, sweet, mint, medicinal, fishy, fruity, floral and proper usage.
Sweet smelling include esters, ketones, and alcohols (be able to distinguish between
shape and molecule)
Minty smelling include ketones, alcohols (be able to distinguish between shape of
molecule).
ethanol, butanol, hexanol, isopentanol are examples of alcohols
ethy alcohol, butyl alcohol, hexyl alcohol, methyl hexanol are another naming type of
alcohols
acetic acid, ethanoic acid, propanoic acid, butric acid, butanoic acid, heptanoic acid
are examples of acids given in this unit
Catalyst
Lewis Structures, Lewis Dot two ways to show how electrons are being shared.
HONC 1234 bond types/bond strengths in polar and nonpolar compounds
How many functional groups have one oxygen and have no smell?
Sharing of electrons vs giving taking of electrons (electronegativity and
electronegativity difference)
How many functional groups have one oxygen and have more than one smell?
Shape of molecule, bond angles, unbonded electrons, bonded electrons
Give the structural formula of Citronellol, L and D Carvone, Fenchol
Single bonds, double bonds, triple bonds resonating bonds, symmetry,
equivalence
Covalent, Polar covalent
To process the type/characteristics of a compound, determine/ask yourself
questions such as:
molecular shape--- long, stringy, pan shaped etc.
molecular formula--- one oxygen, two oxygen, no oxygen, nitrogen, etc.
functional group--- ester, carboxylic, amine, ether, alcohol, etc.
smell--- putrid is carboxylic, fishy is amine, etc.
Electron domains
Receptor sites: what they do, size, shape, polarity
Tetrahedral, Pyramidal, Trigonal Planar, Bent, Linear, Point
Smells come from gases. What substances provide gases, Do not be fooled,
solid substances such as D-carvone smells like caraway seeds (caraway seeds
are solid), like rye bread and L-carvone is minty. Also liquids that are highly
volatile have smell
Polarity (nonpolar or polar) intermolecular force partial charges
Number of carbons, numbers of hydrogens, long, stringy, frying pan, ball shaped
5-19 carbons long and stringy is sweet smelling, including fruity, floral smells
5 or less carbon alcohols are medicinal, 6 carbon chains that are flat are minty smell
6 carbon chains and ball shaped have camphor smell
More than one carbon chain and one oxygen ball shaped is camphor smelling.
Ethyl butyrate which is an acid and a liquid, smells like pineapple. You have
other examples on your flashcards.
January 21, 2013
Some diatomic elements that are small nonpolar gases, have a smell. So realize
there are not solid rules or characteristics to go by.
Water is polar and like most polar substances is an exception by not having a
smell. Could this be why receptor sites dissolve in moisture to work?
For Unit 1:
Know all lab equipment and how to safely use.
Know the safety rules. Review the Lab Safety Contract. Review notes of the
material and placement of the safety material in the lab area.
Know/recommend compound types from last semester and examples. (Ionic,
Molecular Covalent, Metallic, and Network Covalent.
Be able to define and write a hypothesis for an experiment.
Mirror images, Mirror image isomers
Understand the difference between physical, chemical and nuclear properties.
Right/Left handed
Definition of Chemistry
Hydrophobic vs. Hydrophillic
What is matter?
Amino Acids
Accuracy vs. precision and measuring of volume, length and mass.
Proteins: shape, peptide bonds, chains of amino acids
Define and work with equation for Density.
Intensive vs Extensive properties
Reactivity
Writing Chemical equations. Reactants, states, balancing, yields, products
Know the steps of the copper cycle used in the text.
Handling of chemical substances including disposal by MSDS.
Disposal of strong acids. Disposal strong bases.
Reactions of Zinc, Copper, Nitric Acid, Nitrogen Dioxide, Copper II Nitrate,
Sodium Hydroxide, Copper II Hydroxide, Copper II Oxide, Sulfuric Acid.
Observations in the lab and class include qualifying, quantifying, safe use of
senses and time.
Oxidation states
Writing lab reports. Lab report format. Data tables, conclusions based on data
written in data table and observations.
Atomic mass and amu. Be able to take a sample and determine amu.
Protons, neutrons, electrons. Atomic Number.
Trends and patterns that the periodic table is built upon.
Electronegativity, Reactivity,
Atomic number, alkali metals, alkaline earth metals, metalloids, metals nonmetals,
actinides, lanthanides, main group elements, halogens periods, groups, families,
noble gasses, transition metals, rare earth metals
Naming of Ionic Compounds. Use of oxidation states, roman numerals for metals
with multiple oxidation states. Rule of Zero
Naming of nonmetal compounds. Use of prefixes
Knowing/Using the polyatomic ions given in class to make "Happy" compounds.
January 21, 2013
Atomic models and scientist: Solid Sphere (John DaltonP,
Plum Pudding (J.J. Thomson), Nuclear Model (Ernest Rutherford), Solar System
(Niels Bohr), Proton model (Ernest Rutherford), Electron Cloud (James Chadwick
and Werner Heisenberg).
Main ideas/theories accepted in each model.
Isotopes
Electron Configurations
Energy levels, Principal Quantum levels
Subshell
Oribitals
Electron directions or rotation
Valence electrons
Stable vs. Unstable
Aufbau Principle
Hunds rule
Pauli Exclusion Principle
Heisenburg Uncertainty Principle
Alpha, Beta, Gamma Decay
Cations compared to Anions
Fission vs. Fusion
Characteristics of Ionic compounds. (Solid vs. Aqueous)
Half Life. Know Carbon 12 Dating and half life of Carbon 12.
Conductivity
Flame Tests. Know colors learned in lab and compounds given in text. Know
procedure for doing this type of lab.
Ionic, Molecular Covalent, Network Covalent, Metallic Compounds
Nuclear Reactions, Chain reactions. Natural Decay
Electroplating