Term
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Definition
| Orbitals fill in order of increasing energy, from lowest to highest. |
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Term
| Pauli Exclusion Principle |
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Definition
| Only two electrons can occupy an orbital. Their spins must be paired(i.e., they must be in the opposite direction). |
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Term
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Definition
1. When orbitals of equal energy [degenerate] are available but there are not enough electrons to fill all of them completely, then one electron is added to each orbital before a second electron is added to any of them.
2. The spins of single electrons in the degenerate orbintals must be aligned |
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Term
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Definition
the measure of an atom's attraction for electrons that is shares in a chemical bond with another atom
Increases to top and right of periodic table |
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Term
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Definition
| the energy released upon additino of an electron. Increases down and left. |
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Term
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Definition
| formed by sharing of one or more pairs of electrons between two atoms to give a noble gas configutration at each atom |
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Term
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Definition
| a covalent bond with a electronegativity difference of 0.5 to 1.9 |
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Term
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Definition
| a covalent bond with an electronegativity difference of less than 0.5 |
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Term
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Definition
the product of the charge e on one of a molecules atoms times the distance d seperating the two atoms
μ=e*d |
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Term
| Steps for determing lews structures for polyatomic ions |
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Definition
1. determine number of valence electrons (add valence electrons by each atom +/- ions)
2. Determine connectivity
3. Connect atoms with a single bond
4. If two atoms share only a single pair of electrons: single bond. If two: double. If three: triple. |
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| formaldehyde (Methyl aldehyde) |
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Term
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Definition
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Term
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Definition
| FC=#valence in neutral atom - (unshared + (1/2)*shared) |
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Term
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Definition
| -OH (hydroxyl) group bonded to a tetrahedral carbon atom. |
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Term
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Definition
a molecule with a nitrogen bondeed to one, two, or three carbon atoms by single bonds
primary -> C+NH2
secondary-> C+NH1
tertiary -> C+N
Notice this classification system of 1, 2, 3rd order is different than other fxnl groups
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Term
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Definition
A compound containing -CHO group
[alternatively written -CH=O] |
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Term
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Definition
| a compound containing a carbonyl group (=O) bonded to two atoms |
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Term
| Carboxylic Acid/Carboxyl Group |
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Definition
| A compound containing a craboxyl (-COOH) group. Also writeen -CO2H |
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Term
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Definition
| carbonyl adjacent to an ether linkage |
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Term
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Definition
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Term
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Definition
| any group containing an aromatic ring |
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Term
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Definition
| Also called carboxylic amide, derivative of carboxylic acid in which -OH is replaced by an amine |
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Term
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Definition
2 electron groups
2 bonding
180 degress |
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Term
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Definition
3 electron groups
3 bonding
120 Degrees |
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Term
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Definition
4 Electron groups
4 bonding
109.5 degrees |
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Term
| Tetrahedral/Trigonal pyramidal |
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Definition
4 electrong groups
3 bonding
1 lone pair
107 degrees |
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Term
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Definition
4 Electrong groups
2 Bonding
2 Lone Pairs
104.5 Degrees |
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Term
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Definition
5 Electrong Groups
5 Bonding
90/120 degrees |
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Term
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Definition
6 Electron Groups
6 Bonding
90/90 degrees |
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Term
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Definition
covalent bonds formed when two p orbitals overlap one another. Not as strong as sigma orbitals
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Term
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Definition
strongest of all chemical covalent bonds
occurs in sp overlaps (single bonds) |
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Term
| Rules for Writing Contributing Structures |
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Definition
1. Contributing Structures must have the same number of valence electrons
2. all contributing structures must obey the rules of covalent bonding (no more than 2 electrons in the valence shell of 2nd order, etc)
3. Positions of all nuclei must be the same in all contributing structures; contributing structures differ only in distribution of valence electrons
4. All structures have same # of pair/unpaired electrons |
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Term
| Estimating the relative importance of Contributing stuctures |
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Definition
Preference 1. Filled Valence Shells
Preference 2. Maximum Number of Covalent Bonds
Preference 3. Least separation of Unlike Charges
Preference 4. Negative Charge on a More electronegative atom |
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