Final Review

• Hydrocarbons


  Carbon atoms filled with hydrogen compounds
• Hydrocarbon types

  • Alkane
  • Alkene
  • Alkyne
• Alkane


  Saturated; single carbon bonding and the weakest bonds
• Alkene


  Unsaturated; Double carbon bonding
• Alkyne


  Unsaturated; a Triple carbon bonding with the strongest bonds
• Cyclic hydrocarbons

  • Cycloalkane
  • Cycloalkene
  • Cycloalkyne
• Aromatic Hydrocarbon


  Cyclic, planar compounds that resemble benzene (C6H6)
• Alkyl Halide


  Hydrocarbon attached with a halogen (F, Cl, Br, I, At, Ts)
• Derivatives of Water (C,HO)

  • Alcohol
  • Phenol
  • Ether
• Carbonyl Family

  • Aldehyde
  • Ketone
  • Carboxylic Acid
  • Esters
  • Acid Anhydride
  • Amides
  • Acyl Halides
• Sulfur Based (C, H, S)

  • Thiol/Mercaptan
  • Thioether/Sulfides
• Nitrogen Based (C, H, N)

  • Amine
  • Nitriles
• Amine


  Any members of a family of nitrogen-containing compounds that is derived from ammonia (NH3)
• Nitriles


  Also called Cyano compounds, it contains cyanide (CN) as the functional group with the formula RC≡N
• Acid


  Electrophiles, they love negative (-), pH<7
• Acids


  • HF
  • HCl
  • NH4+
  • H3O+
  • CH3COOH
• Bases


  Nucleophiles, they love positive (+), pH>7
• Bases

  • OH-
  • F-
  • NH3
  • CH3COO-
• pKa


  Ionization Constant of an acid, indication of the strength of the acid, weak or strong acid
• pKb


  Ionization constant of Base, used to indicate the alkalinity of a molecule/base
• Strong Acid = Weak conjugate Base, Strong Base = Weak conjugate Acid, Weak Acid = Strong conjugate Base, Weak Base = Strong conjugate Acid
• Bronsted-Lowry (Protonic Theory)


  Acid - proton donor, Base - proton acceptor
• Acidity based on electronegativity

  • H-F
  • H-Cl
  • H-Br
  • H-I
• 1. I is the least electronegative, meaning it can easily give up hydrogen, making it the strongest acid of the 4 compounds
• Acidity based on oxygen content

  • HClO
  • HClO2
  • HClO3
  • HClO4
• Acidity based on carbon content

  • CH3OH
  • CH3CH2OH
  • CH3CH3CH2OH
• Electronic Effects


  Electron withdrawal = Higher acidity, Electron Release = Lesser acidity, Electron Release through Resonance: Ortho & Para = less acidic, Meta = high acidic
• Sigma Electron delocalization / C-H Hyperconjugation

  Associated with alkyl groups, More carbon, less acidic
• Inductive Effect


  Electronegative element will pull more electron toward itself (positive) making the other side of the chain negative
• Electronegative elements


  • -F, -O,-N,-Cl, Br, -NO2, -NH2, -OH
• Groups with excess charge

  • -Nno2, -NH3,-R3+
  • -O-, -COO-
  • Alkyl groups: Tertiary>secondary> primary > methyl
• Stearic Effects


  Associated with the presence of bulky groups resulting to crowding in a molecule, How much group is attached in a molecule
• Lewis Acid


  Electron Acceptor, Molecule that wants to borrow a pair of electrons from another molecule
• Lewis Base


  Electron Donor, Molecule that has an extra lone pairs and willing to share to other molecule
• Isomers


  • Constitutional Isomers
  • Functional Isomers
  • Positional Isomers
  • Metamers
  • Tautomers
• Constitutional Isomerism


  Compounds of the same chemical formula but different structures and properties
• Chain/Skeletal Isomers


  Different carbon skeletons
• Functional Isomers


  Different Functional Groups
• Positional Isomers


  Different Location of functional groups
• Metamers


  In polyvalent functional groups, if both alkyl group's around functional group are different