Summer Assignment Memorization Flashcards
(50 cards)
When the name of the anion ends in –ide
the acid name begins with the prefix hydro-, the stem of the anion has the suffix –ic and it is followed by the word “acid”. For example: HCl: Cl- is chloride, so HCl = hydrochloric acid
When the anion name ends in –ite
the acid name is the stem of the anion with the suffix –ous, followed by the word “acid”. For example: ClO2- is the chlorite ion, so HClO2 = chlorous acid
When the anion name ends in –ate
the acid name is the stem of the anion with the suffix –ic, followed by the word “acid”. For example: ClO3- is the chlorate ion, so HClO3 = chloric acid
When the anion name begins with per-
the acid name begins with per- and the stem of the anion has the suffix –ic and it is followed by the word “acid”. For example: ClO4- is the perchlorate ion, so HClO4 = perchloric acid
Rules for Naming Ionic Compounds
- Balance charges – charges should always = 0
- Cation is always written first (in name and in formula)
- Change the ending of the anion (if an element) to –ide. If a polyatomic ion, the ion name does not change.
Solubility Rules
- All compounds containing alkali metal cations or the ammonium ion are soluble.
- All compounds containing NO3-, ClO4-, ClO3-, and C2H3O2- anions are soluble.
- All chlorides, bromides, and iodides are soluble except those containing Ag+, Pb2+, or Hg2+.
- All sulfates are soluble except those containing Hg2+, Pb2+, Sr2+, Ca2+, or Ba2+.
- All hydroxides are insoluble, except compounds of the alkali metals, ammonium, Ca2+, Sr2+, or Ba2+.
- All compounds containing PO43-, S2-, CO32-, and SO32- are insoluble, except compounds of the alkali metals or ammonium.
Oxidation Number
a number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms
Rules for Determining Oxidation Number
- The oxidation number of any uncombined element is zero (0).
- The oxidation number of a monatomic ion is equal to the charge on the ion.
- The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.
- The oxidation number of fluorine in a compound is always -1.
- Oxygen has an oxidation number of -2 unless it is combined with fluorine (where it will be +2) or it is in a peroxide (where it will be -1).
- The oxidation state of hydrogen in most of its compounds is +1 unless it is combined with a metal, in which case it will be -1.
- In compounds, the elements of Groups 1 and 2, as well as aluminum have oxidation numbers of +1, +2, and +3, respectively.
- The sum of the oxidation numbers of all atoms in a neutral compound is 0.
- The sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion.
Chromium
Cr; +2, +3; Chromium (II), Chromium (III)
Manganese
Mn; +2, +3; Manganese (II), Manganese (III)
Iron
Fe; +2, +3; Iron (II), Iron (III); Ferrous, Ferric
Cobalt
Co; +2, +3, Cobalt (II), Cobalt (III)
Copper
Cu; +1, +2; Copper (I), Copper (II); Cuprous, Cupric
Lead
Pb; +2, +4; Lead (II), Lead (IV); Plumbous, Plumbic
Mercury
Hg; +1, +2; Mercury (I), Mercury (II); Mercurous, Mercuric
Tin
Sn; +2, +4; Tin (II), Tin (IV); Stannous, Stannic
Gold
Au; +1, +3; Gold (I), Gold (III)
Silver
Ag; +1, +2 (rare); Silver, Silver (II)
Bismuth
Bi; +3, +5; Bismuth (III), Bismuth (V)
Antimony
Sb; +3, +5; Antimony (III), Antimony (V)
Cadmium
Cd; +2; Cadmium
Zinc
Zn; +2; Zinc
Ammonium
NH4+
Acetate
C2H3O2-
