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30 Cards in this Set
- Front
- Back
Schrodinger N
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Shell of electron orbital
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Schrodinger L=0
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s orbital
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Schrodinger L=1
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p orbital
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Schrodinger L=2
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d orbital
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Schrodinger L=3
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f orbital
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Order of filling Schrodinger orbitals
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1s, 2s, 2p, 3s, 3p, 4s, 3d
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Schrodinger m1
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orbital in space (-1, 0 or 1)
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Oxidation
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loses electron
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Reduction
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Gains e-
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Electronegativity
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how strongly atttoms attract e-
Top right most electronegative, bottom left least |
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Ionic Bonds
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Electroneg dif > 2.1
Mutual attraction of cation for several sourrounding anions or opposite Atom forms cation by giving up one or more e- to atom(s) forming anion |
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Non-polar Covalent Bond
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= electronegativities
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Polar Covalent Bonds
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Different electronegativity (significant dipoles)
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Coordinate covalent bonds
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Atom donates both e- for the shared pair and the other uses a vacant orbital for bonding
H..N+H3 |
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Covalent Bonds
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Nonmentals usually form the,
Dif of electroneg <1.7 Atoms share one or more pairs or e- Alpha bonds are symmetrical about axis of rotation |
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How many covalent bonds formed from C, H, N, P, O, S and hologens? What if they have +1 charge?
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C-4, H-1 N-3, P-3, O-2, S-2, halogens-1
If +1 charge then they form one more bond |
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Lewis dot structures for representative (A) groups
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Given by group number of periodic table
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Lewis Dot Structures for covalent molecules
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Determine correct # of Ve- for each atom
if - charge add extra e-, if + take one away Write symbols and form single bonds between them put other e-'s as lone pairs check to see that each atom has octet if not use dbl or triple bonds |
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Resonance
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2 or more lewis dot structures made by only moving electrong
Lower E structures are major |
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What Makes a Major Resonance Structure
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All atoms have complete Octet
More bonds= more stability No unnecessary seperation (causes high enery structures) It is better to have a negative charge on a highly electronegative element like O than C Dispersal of charge = higher stability |
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Formal Charge
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FC= group # - nonbonding electrons - 1/2 shared electrons
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Arrhenius Acid
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Gives proton (H+)
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Arrhenius Base
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Gives up hydroxide
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Arrhenius conjugates
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Acids and bases neutralize each other to form conjugate base and acid
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Bronsted-Lowry acid
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gives up proton (H+)
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Bronsted-Lowry Base
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Accepts proton
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Lewis Acid
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Accepts electron pair to form covalent bond and have a positive charge (like H+ or hydronium) or have available vacant orbitals (BF3)
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Lewis Base
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Donates electron pair to form covalent bond and has a negative or neutral charge with lone pair(s) of electrons
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Ka
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([H3O+][A+])/[HA]
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Acid Strength
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The more elctronegative an anion, the more acidic (most acidic bottom right, least top left)
Stability of Acid increases down a group Dispersal of charge over a larger atom stabilizes anions The more anion on a central atom the more acidic |