Exam 2 Topics
Exam 2 may be moved until Monday (3/3).
Topics include material covered on or before 2/24/03 (today)
Atomic Theory
· Quantum Model:
o Valence electrons (outer shell, ignore d electrons), atoms ionized to get to full valence/octet, noble gas configuration
o Groups, Lewis Dot for atoms, halogen= ns2np5
Bonding
· Ionic Bonds, Covalent Bonds, Polar Covalent Bonds
· Lewis dot structure of elements & ions
· Don't worry about octet exceptions
· Electronegativity (EN) values will be given, know how to use them.
· Know EN cutoffs for bond type. Remember H is an exception
Lewis Structures
· Official Lewis steps (1-5). Know the steps.
· Extra Lewis structure rules: 2+ carbons form chains, H never in center, H on O if possible
· Similarity between ClO4- and BrO4-
Nomenclature
· Element names, symbols (remember HONClBrIF)
· Funny elements, e.g. Potassium (K)
· Prefixes (mono-, di-, tri- … up to 10)
· Naming non-metal diatomic compound:
o Prefix-1st element <space> prefix-2nd element root-ide
o Elements in alphabetical order
· Element ions
o Metals: add “ion” to name
o Group 5A – 7A (non-metals): add –ide to element root + space + ion
Unit D
· Molecular Geometry:
o 3-D repulsion idea, electron pairs or bonds are a “stick”
o Linear, Trigonal planar, Tetrahedral
· Polarity
o Bond dipoles -> molecular dipoles
o Draw H2O with bond dipoles, determine net dipole
o Bond & molecular dipoles for CH4, CH3Cl, CH2Cl2, CHCl3, CCl4
Unit N
· Oxyanions:
o 5 to know
o system {per-ate, -ate, -ite, hypo-ite, -ide}
o system for acids
· Ionic compounds: balance charge to make them neutral
· Common chemicals: familiar ones from lecture examples
· 2 non-metal compounds (N2O dinitrogen monoxide)
· Multiple charges for Cu & Fe (cuprous, cupric, copper(I), copper(II) ions, same for Fe (II, III)).
· Procedure & bottom of pg. N.18
· Complex Ions:
o Cations: NH4+ = ammonium ion
o anions: oxyanions, CN- cyanide ion, OH- hydroxide ion, CH3COO- acetate ion
Unit C
· Measurement, dimensions, metric units
· Scientific Notation
· Significant Figures
· Temperature (°C, °F, K – use formulas (given on exam) to convert)
· Density = mass/volume, will something float?
Skills
· Find # of valence electrons for an element.
· Draw Lewis dots for an atom or ion.
· Determine formula of an ionic compound (given Al & Cl, come up with AlCl3)
· Determine polarity of a bond based on electronegativity.
· Draw Lewis structure (follow the 5 steps)
· Name an element, determine the elemental formula (HONClBrIF)
· Name a diatomic compound.
· Name metal ions, non-metal ions.
· Calculations, etc.