OchemTest1

• Nonpolar Covalent: 0-<.5
• Polar Covalent: .5-1.7
• Ionic: >1.7

• VBT: Valence bond theory treats every bond as the sharing of electron density between two atoms as a result of the constructive interference of their atomic orbitals
• MOT: uses a mathematical method called the linear combination of atomic orbitals (LCAO) to form molecular orbitals. Each molecular orbital is associated with the entire molecule, rather than just two atoms.
• #atomic orbitals results in # molecular orbitals (antibonding > nonbonding > bonding)

• sp3: tetrahedral (109.5), trigonal pyramidal, bent
• sp2: trigonal planar (120), bent
• sp: linear (180)

• Dipole-dipole
• H-Bonding
• London dispersion

Carbon atoms with formal charges will only hold 3 bonds

• Wedge: coming out of page
• Dash: going into page

• 1. Don't ever break single bonds
• 2. Never exceed an octet for 2nd row elements

• 1) Allylic lone pair: lone pair next to double bond.  Lone pair creates new double bond, old double bond moves to lone pair at end.
• 2) Allylic cation: Cation next to double bond. Double bond moves to positive formal charge, new positive formal charge where double bond is missing.
• 3) Lone Pair Next to cation: Lone pair creates double bond, new positive formal charge formed.
• 4) Double bond between 2 atoms of differing electronegitivity: Double bond moves toward more electronegative atom, creating a negative formal charge, positive formal charge left on other atom.
• 5) Conjugated double bonds in a ring: Each bond moves over.

• 1) Minimize the charge (>2 charges is not significant) *Nitro groups chargest aren't associated with that limit
• 2) Electronegative atoms can bear a positive charge ONLY if they have an octet (most significant resonance structures have an octet on all atoms)
• 3) 2 carbon atoms should not have opposite charges

• acid: proton donator
• base: proton acceptor
• Always takes 2 lines
• line 1: from electron on base to H on acid
• line 2: from bond between H on acid and its connected atom

• -10 (very strong acid)
• 50 (very week acid)

• Look at conjugate base to determine stability
• 1) Which ATOM is the charge on? (more electroneg OR larger)
• 2) Which has more resonance?
• 3) Induction (pulling of e to sigma bond by electroneg atom)
• 4) Orbitals (smaller/rounder = stronger acid)
• EXCEPTION: H-C=C-H + NH₂^- <-> H-C=-C:^- + NH₃
• Acetylene is stronger acid!

It favors the weaker acid / more stable conj base

Large/bulky bases have less interaction with solute, and are less stable (weaker acid) 

• Acid: electron acceptor
• Base: electron donator