Remove O
(charge SAME)
Groups of FOUR
Elements whose names and symbols you should memorize (you do NOT need to know position).
H
Li
Na
K
Cs
Mg
Ca
Sr
Ba
Ra
B
Al
Ti
Cr
Mn
Fe
Chlorate, bromate, and iodate
(halogen-containing “ate”
oxoanions) are analogous to
nitrate:
NO3-, ClO3-, BrO3-, IO3-
HSO4- hydrogen sulfate
Ni
Cu
Ag
Au
N
P
Zn
Hg
“Core Ions”*
O
S
Se
Sn
Pb
F
Cl
Br
I
He
Ne
ClO4- perchlorate
ClO3chlorate
ClO2
chlorite
ClO hypochlorite
Remove O
(charge SAME)
NO3-
nitrate
NO2- nitrite
SO42-
sulfate
SO32- sulfite
PO43-
phosphate
PO33- phosphite
BrO4- perbromate
BrO3bromate
BrO2
bromite
BrO hypobromite
add H+
(charge changes)
HPO42- hydrogen phosphate
HCO3- hydrogen carbonate
add H+
Co
C
Si
H2PO4- dihydrogen
phosphate
Also learn the other common monatomic “–ides”
as well (use periodic table to determine charge
for all monatomic –ides): oxide (O2-) , the first
four halides (F-, Cl-, Br-, I-), and hydride (H-)
2-
CO3
Miscellaneous Other Ions to Know
Don’t confuse –ates with –ides!!
HSO3- hydrogen sulfite
N3- nitride
HPO32- hydrogen phosphite
P3- phosphide
*POCONOSO Mnemonic, Core Ions
periodate
iodate
iodite
hypoiodite
Add
H+
carbonate
S2- sulfide
IO4IO3IO2IO-
Add
H+
H2PO3- dihydrogen phosphite
OHhydroxide
CN
cyanide
MnO4 permanganate
C2H3O2- acetate
CrO42- chromate
Cr2O72- dichromate
NH4+
ammonium (the
only common
non-metal cation!)
List of Ions and Elements to Know (Tabular Format)‡
Anion formulas and their names
N3-
nitride
NO3-
nitrate
NO2-
nitrite
S2-
sulfide
SO42-
sulfate
SO32-
Element Symbol, Name, and Monatomic Cation Formed
common
nonmetals found
in organic
compounds (and
elsewhere!)
sulfite
HSO4
-
hydrogen sulfate
HSO3-
hydrogen sulfite
P3-
phosphide
PO4
3-
phosphate
PO33-
phosphite
HPO42-
hydrogen phosphate
-
H2PO4
dihydrogen phosphate
2-
HPO3
hydrogen phosphite
H2PO3-
dihydrogen phosphite
C4-
carbide
CO32-
carbonate
-
HCO3
hydrogen carbonate
O2-
oxide
F-
fluoride (u before o!!)
Cl-
chloride
Br-
bromide
I-
iodide
ClO4-, BrO4-, IO4-,
-
chlorate, bromate, iodate
-,
-,
ClO2 BrO2 IO2
-
chlorite, bromite, iodite
ClO-,
hypochlorite, hypobrom..etc
ClO3 BrO3 IO3
BrO-,
IO-
OH-
hydroxide
CNC2H3O2- (or CH3COO)
MnO4-
cyanide
2-
acetate
permanganate
CrO4
chromate
Cr2O72-
dichromate
NH4+
ammonium
hydrogen
carbon
H+
nitrogen
phosphorus
oxygen
sulfur
F
Cl
Br
I
chlorine
bromine
iodine
He
Ne
helium
neon
other
nonmetals or
metalloids
B
Si
Se
boron
silicon
selenium
main group
metals
Al
Sn
Pb
aluminum
tin
lead
Al3+
Type II
Type II
Li
Na
K
Cs
lithium
sodium
potassium
cesium
Li+
Na+
K+
Cs+
Mg
Ca
Sr
Ba
Ra
magnesium
calcium
strontium
barium
radium
Mg2+
Ca2+
Sr2+
Ba2+
Ra2+
Ti
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ag
Au
Hg
titanium
chromium
manganese
iron
Type II
Type II
Type II
Type II
cobalt
nickel
copper
zinc
silver
gold
mercury
Type II
Type II
Type II
Zn2+
Ag+
Type II
Type II
halogens
inert
gases
alkali metals
(also main
group)
alkaline earth
(metals) (also
main group)
perchlorate, perbromate, etc.
-,
H
C
N
P
O
S
transition
metals
fluorine
‡
NOTE1: The only metal elements outside of Group 1A and Group 2A that have only one common ion that you should memorize
for this class are: Al, Zn, Ag. The ions they tend to form are Al3+, Zn2+, and Ag+. All other transition metal elements (and lead
and tin) should be assumed to form at least two stable cations (i.e., they are Type II metals or cations) and therefore when
writing a compound with one of them in it, you need to use a Roman numeral inside of parentheses to specify its charge.
‡
NOTE2: The list of elements on the right is there to indicate the ones whose NAMES I expect you to learn. The charges of "Type
I" cations' should be memorized (see note above). The charges of "Type II" cations varies so you need not memorize them;
however, you must be able to figure out the charge of these cations from a given compound formula (from the charges on the anions).