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| Species that donates electron pair |
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| Species that accpets electron pair |
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| Electron pulling power of an atom |
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| Trend of Electronegativity |
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Definition
| Increase across a period and up a group |
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Definition
| Transfer electrons from metal atom to non metal atom. Difference in electronegativity >2 |
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Definition
| Two nonmetals share electrons. Difference in electronegativity <1.5 |
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| M initial V initial = M final V final |
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| C= (wavelength in Meters)(Frequency in Hertz) |
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Definition
E= vh
frequency x Plancks constant |
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| (E=hv)- (threshold energy)= (1/2m x v^2) |
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| Combined energy of a photon |
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| Energy to different orbital for hydrogen |
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Definition
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Definition
| waves in phase. Adds to height of wave. |
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Definition
| Waves out of phase. Subtract from height. |
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| Heisenberg's uncertainty equation |
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Definition
(Δp)(Δx) > h/4Π
p=momentum
x=position |
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Definition
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Definition
l=1
Nodule plane
px, py,pz |
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Term
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Definition
| Outer e feel reduced electrostatic attraction |
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Term
| Pauli exclusion principle |
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Definition
| No more than two electrons per orbital and if 2 are in the same orbial, then spin paired |
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Definition
| Due to e repulsion, e in the same subshell will occupy differeent orbitals and with parallel spin |
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Definition
Half the distance betwerr centers of neighboring atoms
Increase down a group, decrease across a period |
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Term
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Definition
Energy needed to remove e from atom (gas phase)
Decrease down a group, Increase across a period
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| Energy released when e is added to a gas phase atom |
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Definition
indicates gain or loss of an e while forming a covalent bond
FC=V-(L+(S/2)) |
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Term
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Definition
Atoms with highly distorted e
Bigger the anion, less tightly the e are held,more likely to have covalent properties. |
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Definition
Ions that cause large distortions
Small cations like Al +3 |
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Definition
Covalent bonds where e are not equally shared.
Has electric dipole moment that does not cancel out |
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Definition
Valence-Shell Electron-Pair Repulsion Model
Bonding e pairs and lone pairs repel each other |
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Definition
Two orbitals, each with 1 e overlap end to end
Allow bound atoms to rotate
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Definition
Two orbitals, each with 1 e overlap side-by-side
Do not allow bonds to rotate
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