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CHEM 101 EXAM #2

Ch. 4-6

QuestionAnswer
2 bonding pairs, 0 lone pairs, sp hybridization, 180 bond angle linear (1)
3 bonding pairs, 0 lone pairs, sp2 hybridization, 120 bond angle trigonal planar
2 bonding pairs, 1 lone pair, sp2 hybridization, 120 bond angles bent (1)
4 bonding pairs, 0 lone pairs, sp3 hybridization, 109.5 bond angles tetrahedral
3 bonding pairs, 1 lone pair, sp3 hybridization, 109.5 bond angles trigonal pyramidal
2 bonding pairs, 2 lone pairs, sp3 hybridization, 109.5 bond angles bent (2)
5 bonding pairs, 0 lone pairs, sp3d hybridization, 90, 120, 180 bond angles trigonal bypyramidal
4 bonding pairs, 1 lone pair, sp3d hybridization, 90, 120, 180 bond angles seesaw
3 bonding pairs, 2 lone pairs, sp3d hybridization, 90, 180 bond angles t-shaped
2 bonding pairs, 3 lone pairs, sp3d hybridization, 180 bond angles linear (2)
6 bonding pairs, 0 lone pairs, sp3d2 hybridization, 90, 180 bond angles octahedral
5 bonding pairs, 1 lone pair, sp3d2 hybridization, 90, 180 bond angles square pyramidal
4 bonding pairs. 2 lone pairs, sp3d2 hybridization, 90, 180 bond angles square planar
nitrates soluble
salts with alkali metal ions (group I) are soluble
chloride, bromide, and iodide salts are soluble EXCEPT silver (I), lead (II), and mercury (I)
sulfate salts are soluble EXCEPT barium sulfate, lead (II) sulfate, mercury (I) sulfate, and calcium sulfate
hydroxides with Ba and Ca marginally soluble (kinda sorta soluble)
Most hydroxides are... slightly soluble
sulfides, carbonates, chromates, and sulfates are slightly soluble EXCEPT group I cations and ammonium
salts with ammonium are... soluble
most ionic compounds contain... 2 types of ions
in a precipitation rxn, the precipitate must have... a zero net charge
dilution equation M1V1 = M2V2
mols of solute ARE NOT... determined through dilution
molarity equation M = mols/liters
what is an electolyte a particle that transfers current, charge, etc
nonelectrolyte does not produce ions when dissolved
weak electrolytes partial dissociation; substances that produce lesser ions when dissolved (weak acids, weak bases)
strong electrolytes complete dissociation; substances produce ions when dissolved (soluble salts, strong acids, strong bases)
according to Svante Arrhenius, the conductivity of a solution... depends on the number of ions present
hydration interaction between water molecules and the ions of a salt, causing dilution
differences in solubility of ionic compounds depends on attraction of ions to one another and attraction of ions to water molecules
solute substance dissolved (minority)
solvent liquid/ water (majority)
HCl hydrochloric acid, strong acid
HBr hydrobromic acid, strong acid
HClO4 perchloric acid, strong acid
H2SO4 sulfuric acid, strong acid
HI hydroiodic acid, strong acid
HNO3 nitric acid, strong acid
KOH potassium hydroxide, strong base
NaOH sodium hydroxide, strong base
Ba(OH)2 barium hydroxide, strong base
CsOH cesium hydroxide, strong base
Sr(OH)2 strontium hydroxide, strong base
Ca(OH)2 calcium hydroxide, strong base
LiOH lithium hydroxide, strong base
RbOH rubidium hydroxide, strong base
carbonate and phosphate are not soluble EXCEPT with sodium, potassium, ammonium
sulfide is only soluble with sodium, potassium, ammonium, barium
hydroxide and oxides are only soluble with sodium, potassium, barium, group I cations
sulfate salts are soluble EXCEPT with calcium, silver, mercury (I), strontium, barium, lead (II)
nitrates, acetates, chlorates, perchlorates salts soluble
sodium, potassium, and ammonium salts are soluble
bronsted lowry acid proton donor
bronsted lowry base proton acceptor
Created by: accident_prone
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