Ap Test Reference Sheet
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1STUFF I SHOULD KNOW FOR THE AP TEST BUT DO NOT KNOW YET
IONS LIST
–
3+
2–
acetate
C
H
O
ferric
Fe
(yellow)
oxalate
C
O
2
3
2
2
4
3+
2+
2–
aluminum
Al
ferrous
Fe
(green)
oxide
O
–
–
+
ammonium
NH
fluoride
F
perbromate
BrO
4
4
–
2+
+
barium
Ba
hydrogen
H
perchlorate
ClO
4
–
–
+
bicarbonate
HCO
hydronium
H
O
periodate
IO
3
3
4
–
–
–
bisulfate
HSO
hydroxide
OH
permanganate
MnO
(purple)
4
4
–
–
2–
bisulfide
HS
hypobromite
BrO
peroxide
O
2
–
–
3–
bisulfite
HSO
hypochlorite
ClO
phosphate
PO
3
4
–
–
3–
bromate
BrO
hypoiodite
IO
phosphide
P
3
–
–
3–
bromide
Br
iodate
IO
phosphite
PO
3
3
–
–
+
bromite
BrO
iodide
I
potassium
K
2
–
2+
+
calcium
Ca
iodite
IO
silver
Ag
2
2–
2+
+
carbonate
CO
lead
Pb
sodium
Na
3
–
+
4+
chlorate
ClO
lithium
Li
stannic
Sn
3
–
2+
2+
chloride
Cl
magnesium
Mg
stannous
Sn
–
2+
2+
chlorite
ClO
manganese
Mn
strontium
Sr
2
2–
2+
2–
chromate
CrO
(yellow)
mercuric
Hg
sulfate
SO
4
4
3+
2+
2–
chromium
Cr
mercurous
Hg
sulfide
S
2
2+
2+
2–
cupric
Cu
(blue)
nickel
Ni
(green)
sulfite
SO
3
–
–
+
cuprous
Cu
(green)
nitrate
NO
thiocyanate
SCN
3
–
3–
2–
cyanide
CN
nitride
N
thiosulfate
S
O
2
3
–
2–
2+
dichromate
Cr
O
(orange)
nitrite
NO
zinc
Zn
2
7
2
SOLUBILITY RULES
STRONG OXIDIZERS (Oxidizing Agents)
–
Mn
2+
Always soluble:
MnO
in acid solution
+ H
O
4
2
+
+
+
+
+
+
Mn
2+
alkali metal ions (Li
, Na
, K
, Rb
, Cs
), NH
,
MnO
in acid solution
+ H
O
4
2
2
–
–
–
–
–
in neutral or basic sol’n MnO
NO
, ClO
, ClO
, C
H
O
, HCO
MnO
3
3
4
2
3
2
3
4
2
Cr
2–
3+
(mnemonics)
Cr
O
in acid solution
+ H
O
Generally soluble:
2
7
2
CrO
–
–
–
2–
2–
Soluble except Ag
(AP/H)
+
2+
2+
Cr
O
with a base
+ H
O
Cl
, Br
, I
, Pb
, Hg
2
7
4
2
2
–
CrO
–
2–
F
Soluble except Ca
2+
2+
2+
2+
2+
CrO
in basic solution
+ H
O
, Sr
, Ba
, Pb
, Mg
4
2
2
NO
(CBS-PM)
HNO
, concentrated
+ H
O
3
2
2
Soluble except Ca
(CBS/PBS)
NO + H
2–
2+
2+
2+
2+
SO
, Sr
, Ba
, Pb
HNO
, dilute (e.g. 6 M)
O
4
3
2
SO
H
SO
, hot, concentrated
+ H
O
Generally insoluble:
2
4
2
2
halide ions (Cl
–
–
2–
Insoluble except alkali metal ions and NH
+
Free halogens (e.g. Cl
)
)
O
, OH
2
4
H
(CBS) somewhat soluble
2+
2+
2+
H
O
in acid solution
O
Ca
, Sr
, Ba
2
2
2
H
Note: H
O
decomposes
O + O
2
2
2
2
2–
3–
2–
2–
2–
2–
CO
, PO
, S
, SO
, C
O
, CrO
NaOH
3
4
3
2
4
4
Na
O
Insoluble except alkali metals and NH
+
2
2
–
Cl
4
HClO
+ H
O
4
2
GASES THAT FORM
Other Oxidizers
) “-ous” ions (Sn
4+
3+
2+
2+
Metal-“ic” ions (e.g. Sn
H
CO
NH
OH NH
, Fe
, Fe
)
CO
+ H
O
+ H
O
2
3
2
2
4
3
2
H
–
H
SO
H
H
O
+ OH
SO
+ H
O
S
2
2
2
3
2
2
2
2HNO
NO + NO
HCN
+ H
O
STRONG REDUCERS (Reducing Agents)
2
2
2
WEAK ELECTROLYTES
–
Free halogen (Cl
Halide ions (e.g. Cl
)
)
2
metal ions
Free metals
Weak Acids (esp. HC
H
O
and HF)
2
3
2
–
–
“ates” SO
(Memorize the 8 strong acids… all others are weak)
“ites” SO
2–
2–
or SO
, NO
, NO
3
2
2
4
3
hypohalite ions (ClO
–
Free halogens, dil. basic sol’n
HCl
hydrochloric acid
HNO
nitric acid
)
3
Free halogens, conc. basic sol’n halate ions (ClO
–
HBr
hydrobromic acid
HIO
periodic acid
)
4
3
S
HI
hydroiodic acid
H
SO
sulfuric acid
2–
2–
S
O
O
2
4
2
3
4
6
HClO
perchloric acid
HClO
chloric acid
4
3
Other Reducers
OH NH
Ammonium Hydroxide (NH
(aq)) Water (H
O)
4
3
2
“-ic” ions (Sn
Metal-“ous” ions (e.g. Sn
2+
4+
)
)
O
+
DRIVING FORCES –– Double Replacement
H
O
+ H
2
2
Insoluble Solid (Precipitate)
Weak Electrolyte (H
O or Weak Acid)
2
Gas Formation
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