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• The first electron domain consists only of linear bonding with 180 bond angle and no lone pairs (s)
• The second electron domain consists of only linear bonding with bond angles of 180 for both 2 bonds, and 1 bond with 1 lone pair (sp)
• The third electron domain consists of three bonding types all of the trigonal planar formation and with a bond angle of 120 (sp2)

  1. Trigonal planar with 3 bonds, no lone pairs
  2. Bent with 2 bonds, 1 lone pair
  3. Linear with 1 bond, 2 lone pairs
• The fourth electron domain consists of four bonding types all of the tetrahedral formation and with a bond angle of 109.5 (sp4)

  1. Tetrahedral with 4 bonds, no lone pairs
  2. Trigonal pyramid with 3 bonds, 1 lone pairs
  3. Bent with 2 bond, 2 lone pairs
  4. Linear with 1 bond and 3 lone pairs
• The fifth electron domain consists of four bonding types all of the Trigonal bipyramidal formation and with a bond angle of 90 and 120 (sp3d)

  1. Trigonal bipyramid with 5 bonds, no lone pairs
  2. See Saw with 4 bonds, 1 lone pair
  3. T-shape with 3 bond, 2 lone pairs
  4. Linear with 2 bonds, 3 lone pairs
• The sixth electron domain consists of three bonding types all of the Octahedral formation with a bond angle of 90 (sp3d2)

  1. Octahedral with 6 bonds and no lone pairs
  2. Square pyramid with 5 bonds and 1 lone pair
  3. Square planar with 4 bonds and 2 lone pairs
• atomic radius increases down a group and decreases across a period
• Doubly filled orbitals are easier to ionize as they have higher electron shielding/is repelled by opposing electron
• Electron affinity increases across a period of decreases down a group
• 1st Ionization energy generally increases across a period and decreases down a group
• Electronegativity increase across a period and decreases down a group
• Metallic character increases diagonally from Helium to Francium
• Non-metallic character increases from Francium to Helium
• Basic metal oxides form metal hydroxides
• The negatively charges ions of the reactants of acidic non-metal oxides can contribute to acid rain and ocean acidification
• Oxidation indicated by +/- number
• Charge indicated by number +/-
• For positive oxidation states, after ionization, they're all isoelectronic. Hence, the one with more protons will have higher effective nuclear charge and pull electrons closer, making radii smaller
• EDTA ^4- is hexadentate ligand that uses 6 lone pairs to form 6 coordinate covalent bonds- it preserves foods as it binds to metal ions in enzymes catalyzing chemical reactions
• H has oxidation of -1 in metal halides
• Acid rain equation (sulfurous acid)

  S(s)+O2(g)->SO2(g)

  SO2(g)+H2O(l)->H2SO3(aq)
• Ocean acidification equation:

  N(g)+O2(g)->2NO(g)

  2NO(g)+O2(g)->2NO2(g)

  2NO2(g)+H2O(l)->HNO3(aq)+HNO2(aq)
• Acid rain equation (sulfuric acid)

  2SO2(s)+O2(g)->2SO3(g)

  SO3(g)+H2O(l)->H2SO4(aq)
• Because 4s and 3d are so close in energy, there is no distinct jump in ionization energies between the two levels, allowing for variable oxidation states
• Crystal field theory proposes that at ligands with lone pairs approach the metal ion, the electrons in its 3d sub-shell are repelled and split unequally into different energies (3<2).
• Crystal field theory allows for the formation of colored complexes as because the d-orbitals are not filled, the ones at lower energy can absorb energy and be "promoted" this causes the absorption of certain wavelenghts of light and release of its complimentary colors
• The energy needed to promote an electron from lower to higher energy in split orbitals depend on the oxidation state, bonded ligands, and transition metal in question
• Most transition metals are diamagnetic or paramagnetic, diamagnetic with no magnetic reaction when they have no unpaired electrons and paramagnetic when they have increasing numbers of unpaired electrons that affect the magnetic field and make them slightly magnetic
• Transition metals that are ferromagnetic include iron, nickel, and cobalt as they have the strongest magnet interactions
• Boiling point increase with increased molar mass as more electrons are present, making the molecule more polarizable and making the London Dispersion forces stronger with more surface area to act on
• Boiling point increases when molecules and straight-chained as in branched chains, there is less surface-area contact for the London dispersion forces to act on
• Alcohols, amines, amides, and carboxylic acids have the highest boiling point due to their hydrogen bonds
• Aldehydes, ketones, esters, ethers, and nitriles have the second highest boiling point as they have dipole-dipole forces
• Functional groups are arranged by importance in order unless its a halogen alkane where its alphabetically organized
• Esterification, or nucleophilic substitution between carboxylic acids and alcohols create esters when catalyzed by concentrated acids like H2SO4
• With increases mass, esters have higher boiling points
• Esters become progressively less soluble as the lenght of the hydrophobic C-H chain grows
• Esters are named as follows;

  alcohol (prefix+"yl") and carboxylic acid (prefix+"noate")
• Ester IUPAC names present the alcohol first, then the acid. The structural formula presents the acid first and then the alcohol
• H from the acid and the OH from the alcohol is taken to form the H2O along with the ester