Organic Chemistry (L.g. Wade, Jr Sixth Edition) Chapter 1

Front 1

Schrodinger N

Back 1

Shell of electron orbital

Front 2

Schrodinger L=0

Back 2

s orbital

Front 3

Schrodinger L=1

Back 3

p orbital

Front 4

Schrodinger L=2

Back 4

d orbital

Front 5

Schrodinger L=3

Back 5

f orbital

Front 6

Order of filling Schrodinger orbitals

Back 6

1s, 2s, 2p, 3s, 3p, 4s, 3d

Front 7

Schrodinger m1

Back 7

orbital in space (-1, 0 or 1)

Front 8

Oxidation

Back 8

loses electron

Front 9

Reduction

Back 9

Gains e-

Front 10

Electronegativity

Back 10

how strongly atttoms attract e-
Top right most electronegative, bottom left least

Front 11

Ionic Bonds

Back 11

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

Front 12

Non-polar Covalent Bond

Back 12

= electronegativities

Front 13

Polar Covalent Bonds

Back 13

Different electronegativity (significant dipoles)

Front 14

Coordinate covalent bonds

Back 14

Atom donates both e- for the shared pair and the other uses a vacant orbital for bonding

H..N+H3

Front 15

Covalent Bonds

Back 15

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

Front 16

How many covalent bonds formed from C, H, N, P, O, S and hologens? What if they have +1 charge?

Back 16

C-4, H-1 N-3, P-3, O-2, S-2, halogens-1

If +1 charge then they form one more bond

Front 17

Lewis dot structures for representative (A) groups

Back 17

Given by group number of periodic table

Front 18

Lewis Dot Structures for covalent molecules

Back 18

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

Front 19

Resonance

Back 19

2 or more lewis dot structures made by only moving electrong

Lower E structures are major

Front 20

What Makes a Major Resonance Structure

Back 20

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

Front 21

Formal Charge

Back 21

FC= group # - nonbonding electrons - 1/2 shared electrons

Front 22

Arrhenius Acid

Back 22

Gives proton (H+)

Front 23

Arrhenius Base

Back 23

Gives up hydroxide

Front 24

Arrhenius conjugates

Back 24

Acids and bases neutralize each other to form conjugate base and acid

Front 25

Bronsted-Lowry acid

Back 25

gives up proton (H+)

Front 26

Bronsted-Lowry Base

Back 26

Accepts proton

Front 27

Lewis Acid

Back 27

Accepts electron pair to form covalent bond and have a positive charge (like H+ or hydronium) or have available vacant orbitals (BF3)

Front 28

Lewis Base

Back 28

Donates electron pair to form covalent bond and has a negative or neutral charge with lone pair(s) of electrons

Front 29

Ka

Back 29

([H3O+][A+])/[HA]

Front 30

Acid Strength

Back 30

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