Term
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Definition
electron is transferred from one atom to another
generally occurs between metal cation and nonmetal anion |
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Term
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Definition
electrons are shared between 2 atoms in a bond
generally occurs between 2 non metal atoms |
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Term
electronegativity
increases up/down? left/right? |
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Definition
measure of the ability of an atom in a bond to attract the bonding electrons
increases right and up |
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Term
| what is difference in electronegativity used for? |
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Definition
| determine how ionic or covalent a bond is |
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Term
ΔEN 50%
ΔEN ionic
ΔEN covalent
ΔEN totally covalent |
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Definition
ΔEN 50% 1.7
ΔEN ionic >1.7
ΔEN covalent <1.7
ΔEN totally covalent ≤0.4 |
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Term
bond polarity
due to __________________
in _____ bond |
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Definition
due to difference in electronegativity
in covalent bond |
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Term
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Definition
| occurs when you have a polar bond |
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Term
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Definition
| measure of the bond dipole (amount of polarity) |
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Term
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Definition
more polar
larger the bond dipole
greater the dipole moment |
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Term
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Definition
| first bond between any 2 atoms |
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Term
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Definition
| second or third bond between any 2 atoms |
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Term
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Definition
| different forms of a lewis structure that differ only in the placement of electrons |
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Term
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Definition
| placement of sigma bonding electrons and one pair electrons around the central atom |
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Term
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Definition
| arrangement of attached atoms around the central atom |
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Term
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Definition
| relationship of the net distribution of electrons in the bonds around the central atom |
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Term
AX2
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: linear
molecular geometry: linear
polarity: NP
hybridization: sp |
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Term
AX3
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal planar
molecular geometry: trigonal planar
polarity: NP
hybridization: sp2 |
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Term
EAX2
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal planar
molecular geometry: bent
polarity: P
hybridization: sp2 |
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Term
AX4
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: tetrahedral
molecular geometry: tetrahedral
polarity: NP
hybridization: sp3 |
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Term
EAX3
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: tetrahedral
molecular geometry: pyramidal
polarity: P
hybridization: sp3 |
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Term
E2AX2
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: tetrahedral
molecular geometry: bent
polarity: polar
hybridization: sp3 |
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Term
AX5
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal bipyramid
molecular geometry: trigonal bipyramid
polarity: NP
hybridization: sp3d |
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Term
EAX4
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal bipyramid
molecular geometry: seesaw
polarity: P
hybridization: sp3d |
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Term
E2AX3
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal bipyramid
molecular geometry: t-shaped
polarity: P
hybridization: sp3d |
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Term
E3AX2
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: trigonal bipyramid
molecular geometry: linear
polarity: NP
hybridization: sp3d |
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Term
AX6
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: octahedral
molecular geometry: octahedral
polarity: NP
hybridization: sp3d2
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Term
EAX5
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: octahedral
molecular geometry: square pyramid
polarity: P
hybridization: sp3d2 |
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Term
E2AX4
electron pair geometry
molecular geometry
polarity
hybridization |
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Definition
electron pair geometry: octahedral
molecular geometry: square planar
polarity: NP
hybridization: sp3d2 |
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Term
| exceptions in lewis structures |
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Definition
electron deficient molecules
BF3
BeF2
odd number of electrons
NO2 |
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Term
formal charge
definition and formula |
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Definition
charge and atom would have if the electrons in a bond are shared equally between the two atoms
FC = # valence electrons - # lone pair electrons on the atom - # bonds to the atom |
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Term
oxidation number
definition and formula |
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Definition
charge an atom would have if the electrons in the bond belong solely to the more electronegative atom
ON = # valence electrons - # lone pair electrons on the atom - # bonding electrons that belong to the atom |
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Term
| determine best resonance form (2) |
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Definition
- magnitude of formal charge should be as small as possible
- negative charge should be on the more negative atom
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Term
| determine group number of unknown central atom |
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Definition
- determine shape of molecule
- determine total number of valence electrons
- subtract out the valence electrons associated with the attached atoms
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Term
| s + s overlap gives a ____ bond |
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Definition
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Term
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Definition
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Term
| p + p end gives a ____ bond |
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Definition
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Term
| p + p sideways overlap gives a ____ bond |
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Definition
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Term
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Definition
| mathematical combination of different energy atomic orbitals to form an equivalent number of equal energy orbitals that are needed to form equal energy bonds |
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Term
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Definition
puts electron density outside the two nucleii (antibonding orbitals)
higher energy than original s orbitals |
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Term
| constructive interference |
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Definition
electron density is on the internuclear axis between the two centers (bonding orbitals)
lower energy than original s orbitals |
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Term
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Definition
(# of bonding electron) - (# of antibonding electrons)
2 |
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Term
zero order
rate of a zero order reaction is _____
equation
half life equation |
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Definition
rate of a zero order reaction is constant
[A] = -kt + [A]o
t= time of the reaction
[A] = concentration at any time, t
[A]o = initial concentration
k = rate constant
t1/2 = [A]o/(2k) |
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Term
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Definition
| time needed for half the initial material to react |
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Term
first order reaction
equation
half life reaction
half life of a first order reaction is _____ of the concentration |
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Definition
ln[A] = -kt + ln[A]o
t1/2 = .693/k
half life of a first order reaction is independent of the concentration |
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Term
| rate order for third order is faster/slower than rate order for second order |
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Definition
| rate order for third order is slower than rate order for second order |
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Term
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Definition
| rate depends on the number of collisions and the number of molecules with enough energy (Ea) to react |
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Term
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Definition
| (# of collisions)(# molecules with E>Ea) |
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