Honors Chemistry
Study Guide – Chapter 4 (Sections 4.1-4.4): Aqueous Reactions
Test Date: Friday, January 8th
On test day you will receive:
Chapter Four:
-
solubility rules
activity series of metals & halogens
periodic table

Solubility
o Define aqueous, soluble, and insoluble
o Be able to determine if an ionic compound is soluble or insoluble using the solubility
rules

Electrolytes
o Define electrolyte (what is required for a compound to be electrolytic?)
o Be able to determine if a compound is ionic, covalent, an acid or base
o Identify compounds as either strong, weak, or nonelectrolytes
 If ionic compound:
 Soluble = Strong electrolyte
 Insoluble = Nonelectrolyte (cannot form ions b/c they cannot dissolve,
so they cannot be electrolytes)
 If covalent compound:
 All Nonelectrolytes (they have no ions, so they cannot be electrolytes)
 If acid/base:
 If strong acid/base = Strong electrolyte
 If base is insoluble = nonelectrolyte
 Any acid not listed as one of the 7 strong = Weak electrolyte
 Must know the strong acids and strong bases
o Strong Acids = HCl, HI, HBr, HNO3, H2SO4, HClO3, HClO4
o Strong Bases = any SOLUBLE metal hydroxides (ex: NaOH)

Double Replacement Precipitation Rxns
o Define (and identify in rxns) precipitate
o Define (and identify in rxns) spectator ion(s)
o Predict the products formed in a double replacement rxn (cations switch partners) and
determine the states of matter.
 Use solubility rules:
 insoluble = (s) = precipitate formed
 soluble = (aq)
o A precipitation rxn ONLY occurs if a solid is formed [if all products are (aq) = No rxn]
 Ex: Na3PO4 (aq) + AgNO3 (aq)
 Products:  NaNO3 (aq) + Ag3PO4 (s)
 Precipitate = silver phosphate
o Write complete ionic equations (CIE) and net ionic equations (NIE)
 IMPORTANT: only (aq) compounds are broken up into ions, every other state
of matter remains unchanged in CIE and NIE
 NIE = no spectators allowed!!!

Single Replacement Redox Rxns
o Define oxidation (OIL/LEO = oxidation is loss of electrions/lose electrons oxidation)
o Define reduction (RIG/GER = reduction is gain of electrons/gain electrons reduction)
o When using the activity series, be able to tell which metals are the most reactive (at the
top)
 The more reactive the metal, the easier it is to oxidize and the more metals it
can replace below it
 Also know what it means to be a noble metal and where they are on the activity
series
o Determine if a single replacement rxn will occur and predict the products if it does
 Metal that is by itself must be ABOVE the cation in the 2nd reactant in order for
these rxns to occur
 Ex: Na (s) + Cu(NO3)2 (aq)
o Na is above Cu  this rxn does occur
o Products:  NaNO3 (aq) + Cu (s)
 If metal + acid and the rxn occurs, one product is always H2 (g)
 When the element alone is a HALOGEN gas (F2, Br2, Cl2, I2)
 Must use the halogen activity series  halogen that is alone must be
more reactive (listed above) the halogen in the 2nd reactant in order to
replace it
 Ex: F2 (g) + KCl (aq)
o Fluorine above iodine  this rxn does occur
o Products:  KF (aq) + I2 (g)
o Write complete ionic equations (CIE) and net ionic equations (NIE)
 IMPORTANT: only (aq) compounds are broken up into ions, every other state
of matter remains unchanged in CIE and NIE
 NIE = no spectators allowed!!!