Electron configuration for cations - Subtract 1 from exponent of highest n-value orbital (ex. remove from 4s before 3d)
Ag+ = [Kr]5s^1 4d^9
Electron configuration for anions - Add 1 to closest orbital
Cl- = [Ne]3s^2 3p^6
Atomic orbitals - s, p, d, f
Primary vs secondary structures of...
Semmelweis Entrance Exam Electron configuration for cations - Subtract 1 from exponent of highest n -value orbital (ex. remove from 4s before 3d) Ag+ = [Kr]5s^1 4d^9 Electron configuration for anions - Add 1 to closest orbital Cl- = [Ne]3s^2 3p^6 Atomic orbitals - s, p, d, f Primary vs secondary structures of proteins - Primary - AA chain (linked by peptide bonds) Secondary - stabilized by non -covalent bonds (alpha helices & beta sheets) Most bonds in organic compounds are - covalent Properties of water - 1. polar 2. capable of adhesion and cohesion 3. high heat capacity (so it's hard to raise its temp) 4. great solvent 5. high heat of vaporization (allows humans to cool off via sweat) 6. water is less dense as a solid than a liquid Intermolecular forces of water - hydrogen bonding Solution components - 1. solvent (product being dissolved) 2. solute (medium for dissolving solvent) Molarity - the number of moles of solute per liter of solution Solubility rules - SOLUBLE 1. alkali metals (group 1) & NH4+ cations 2. NO3 - or CH3COO - anions 3. Cl, Br, I (except when bonded to Ag+, Pb2+ or Hg2+) 4. sulfate ions (except when with Ca2+, Sr2+, Ba2+, Pb2+) INSOLUBLE 1. Metal oxides (except CaO, SrO, BaO) 2. Hydroxides (except when with Ca2+, Sr2+, Ba2+) 3. Carbonates, phosphates, sulfides, and sulfites (unless bound to alkali metal or NH4+) Solubility product - Ksp = [A]^a[B]^b **only products because we don't include solids in the equilibrium expression for NaCl - Ksp = x^2 for PbCl2 - Ksp = 4x^3 for Cr(OH)3 - Ksp = 27x^4 Large Ksp means - strong electrolyte (more soluble) Strong acids - So I brought no clean clothes 1. H2SO4 2. HI 3. HBr 4. HNO3 5. HCl 6. HClO4 7. HClO3 Strong bases - 1. NaOH 2. LiOH 3. KOH 4. CsOH 5. RbOH 6. Ba(OH)2 7. Ca(OH)2 8. Sr(OH)2 Bases can certainly look pleasing (K), really something strong (Na) Le Chatlier's principle: pressure - pressure applied (or volume reduced) --> equilibrium proceeds in direction with fewer moles pressure removed (or volume increased) --> equilibrium proceeds in direction with more moles Le Chatlier's principle: temperature - increasing temperature - toward products (if endothermic) - toward reactants (if exothermic) decreasing temperature - toward products (if exothermic) - toward reactants (if endothermic) Le Chatlier's principle: concentration - increase concentration of reactants - reaction shifts toward products decrease concentration of reactants - reaction shifts toward reactants **the goal is to restore equilibrium
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