FORMIILAS AND NAMES OF COMMON IONS: Simpte Anions
Group 1A
hydride ion
H'-
Group
6.4'
Oz'' peroxide ion
O?t- superoxide ion
S2-
Se2-
Te2'
sulfide ion
selenide ion
telluride ion
Group 44
L
Cr''
CarDlde ron
acetylide ion
G.roup 5A
N"
P3'
nitride ion
phosphide ion
Group 7A
F'- fluonde ion
Cl'- chloride ion
Br''
lr'
At'-
bromide ion
iodide ion
astatide ion
FORMULAS AND NAMES OF COMMON POLYATOMIC IONS:
Group 34
BO:'-
borate ion
Group 4.A
COr''
carbonate ion
HCO3I- hydrogen carbonate ion
CrOr'-
oxalate ion
HC2Oar- hydrogen oxalate ion
CzH:Ozr-acetate ion
CN''
CNO!'
SrUr
cyanide ion
cyanate ion
slllcate lon
Group 5A
Ml4- ammonium ion
NO'' nitite ion
No:'-
nitate ion
Por'' - phosphite ion
HPO:'' monohydrogen phosphite ion
H2PO3'' dihydrogen phosphite ion
phosphate ion
POI-^
HPOr'' monohydrogen phosphate ion
HrPO-a'- dihydrogen phosphate ion
arsenate ion
HAsOo2- monohydrogen arsenate ion
AsOa'
HrAsOa''dihydrogen arsenate ion
Group 6A
hydroxide ion
hydrogen sulfide ion
SO3'' sulfite ion
HSor'- hy&ogen sulfite ion
SO '- sulfate ion
HSO.rr- hydrogen sulfate ion
S2O3'' thiosulfate ion
SCNr' thiocyanate ion
HSe'- hydrogen selenide ion
SeOr'- selenate ion
HSeOrt- hydrogen selenat€ ion
HTe'- hydrogen telluride ion
TeOr'' telhnate ion
IITeOTI- hy&ogen t€llurate ion
Oq'
HS'-
9:i'p1o
Lru_
nypocruonte
ton
BrO'- hypobromite ion
hypoiodite ion
ClOzr- clrlorite ion
CIOrr' chlorate ion
BrOs!- bromate ion
iodate ion
ClO.r- perchlorate ion
BrOrr' perbromate ion
IOo'- periodate ion
IO'-
Ior'-
Transition Metals
CrOr2' chromate ion
Cr2O?2- dichromate ion
MlOa2- manganate ion
MnOr'- permanganate ion
Hg2'- mercury@ ion
(mercurous ion)
FORMLILAS AI\ID NAMES OF COMMON IONS: ,,A,,
Group Cations
Group lA (all +l ions)
Group 2A
Li'- lithium ion
Nar. sodium ion
K'] . pokssiun ion
Rb'- rubidium ion
Cst* cesium ion
Fr't tancium ion
-(all
B.'^
Mg"
Ca'Sf
Ba2'
Ra''
+2 ions)
Group 3A (+1 ard.+3 iong
beryllium ion
aluminum ion
magnesium ion
gallrum ion
calcium ion
Al'Ua-
stontium ion
barium ion
radium ion
thaltium(I) ion (thallous ion)
thallium(Itr) ion (thallic ionj
l]]
Tl'-
Gr;un aA (j2 end +4 ions) Group 5A (+3 and +5
ions)
nn(I) ron (stannous ion)
Br.- bismurh(Ill) ion
:n,.
Sn]- irnflV) ion (srannic ion)
lb:,
Pb*
lead(tr) ion (plumbous ion)
lead(IV) ion (plumbic ion)
FORMULAS AI\ID N,{MES OF COMMON IONS:
Transition Metal Cations
Gr.oup
Sc'-
38
scandium(Ill) ion
Group 68
Cr'- chromium(Il) ion
- (chromous ion)
Cr"
chromium(1l11 ion
(chronuc ion)
Gr-oup 8 (Cobalt Familv)
cobaltftr) ion
(cobaltous ion)
Co't
.
Co'-
cobalt(flI) ion
(cobalfic ion)
Group 28
Zn'
Cd?-
H&'Hgt-
zinc ion
cadmium ion
mercury(I) ion
(mercurous ion)
mercury(I! ion
(mercuric ion)
Group 48
titanium(@ ion
(titanous ion)
titanium(Iv) ion
(trranic ion)
Ti.
Ti-
Group 78
Mn.
Mn'-
manganese(Il) ion
(manganous ion)
manganese(Ill)ion
(manganic ion)
Group 8 (Nickel Famitr,)
nickel(tr) ion
. (nickelous ion)
Ni" nickel(Itr) ion
(nickelic ion)
- palladium(tr)
Pd"
ion
(palladous ion)
Pd"* palladium(I\.f ion
(palladic ion)
- platinum(Il)
ft1ion
(platinous
ion)
_
Pr" platinum(IV) ion
(platinic ion)
Ni'?*
Group 58
vanadium(tr) ion
(vanadous ion)
vanadium(III) ion
(vanadic ion)
(Iron Famirl)
iron(Il) ion
(ferrous ion)
iron(III) ion
(ferric ion)
9lgup
Fe.
Fe'-
S
Group
lB
Cu'- copper(t) ion
. lcuprous ion)
Cu'- copper(Il) ion
. (cupric ion)
Ag'- silver(I) ion
. largentous ion)
Ag" silver(Ill) ion
. (argentic ion)
Au'- gold(I) ion
(aurous ion)
- gold(@
Au'ion
(auric ion)
Classes of Inorganic Compounds
Icnic Compounds
binary metal-nonmetal compounds
temary metal-nonmetal compounds
quatemary metal-nonmetal compounds
Ulolecular Compounds
binary nonmetal-nonmetai
sali
sait
acid salt
compounds
NaCl
Na2SO4
NaHSO,r
rnolecule
network covalent
CO
SiO,
Acids (substances that dissociate to produce H'(aq.) when dissolved in water)
binary hydrogen-nonmetal compounds
temary hydrogen-radical ion compounds
Bases (substances that yield
metal hydroxides
Olf(aq.) when dissolved
(ternary)
il
acid
acid
HCl(aq.)
ffzsor(aq)
water)
base
NaOH
Ilydrates (substances that contain molecular HzO in their structure)
^^..-^..-t^
-ur
^a:^-t
rurlL^ u..,urpvuuu,>
salt hydrate
-of molecular
compomds
molecular
hydrate
NazCOr o10 HzO
COz oHzO
Ionic Compounds
Writing Their Names
1.
2.
Write the cation name frst.
Write the anion name last.
Writing Their Formulas
l.
2.
3.
4.
Wnte the cation formula irrst, complete with charge.
Write the anion formuia second, complete with charge .
Balance total cation charge with total anion charge by choosing subscripts to multiply the number ofcations
and./or anions in the formula.
Erase all charges
Molecular Compounds
Writing Their Names
1.
2.
Wnte the compiete name of the more metallic element first. Use a prefx to indicate the number of this type
of atom.
Write the stem word of the more nonmetallic element second. Add "ide" to form the anion name. Use a
prefix to itdicate the number of this Rpe of atom.
Writing Their Formulas
1.
2.
3.
Write the symbol of the more ;netallic element first.
Write the symbol of the more nonmetallic element last.
Translate prefixes into the number of each atom present. Write this number as a subscript to the element
symbol.
Pre{ix No.
mono t
di
2
tri
3
tella 4
penta 5
Prefi-res
Prefir No.
hexa 6
hepta 7
octa 8
nona 9
deca 10
Stenn
B
bor
carb
Si silic
C
Words
nitr
phosph
As arsen
Sb stibn
N
P
O ox
S sulf
selen
Te tellur
Se
F fluor
Cl chlor
Br brom
I iod
At u.tut
Acids
lYritilg Their
1.
2.
i.
Names
Find the anion by removing all first position Ho from the fornruia.
Nanethe anion. Then finci ihe stem w'ord of the anion by removing its sul'fi-r. Special siems: S = sulfil and
P : phosphor.
Nane the acid by adding an appropriate prefix and/cr suffix to the siem lr-ord of the anion aad by adding the
word. "acid."
Aniol
Acid
hyCro- -ic acid
-ide
hlpo- -ite
-ite
-ate
per- -ate
hlpo-
per-
-ous acid
-ous acid
-ic acid
-rc acid
lYriting Their Formulas
1.
2.
3.
4.
Wnte H- first.
Translate the acid name into an anion formuia. Wnte the anion fon:nulaiast.
Use a subscript to H'to balance aaion cha:ge with cation charge.
Erase ali charges.
Bases
Writing Their Names
1.
2.
Write the name of the cation first.
Write hydroxide last.
Writing Their Formulas
1.
2.
3.
b.
Wriie the cation rymbol hrst, complete with charge.
Write Otf last.
Use a subscript to (OH-) to balance cation and anion charge.
E:ase aiJ charges.
E[ydrates
Writing Their Narnes
1.
2.
3.
Write the name of the compound, ignoring associated water molecules.
Add "hy&ate":.to the name of the compound.
Use a prefi-r to "hydrate" to indicate the number ofwater molecules.
lYriting Their Formulas
1.
2.
J.
Write the formula of the compound, igoring,'(orefix)hydrate."
Add HzO to the formula of the compound.
trse a prefix number to HzO to indicate the number of water molecuies.
B:Ho
CIl4
SiIi4
GeH+
Srllr
Common Names of Some Plolecller Comoounds
diborane
methane
silane
gel..nane
starrrane
NH-,l
amtnonia
PHr
AsH:
Sbtlj
phosphrne
HrO
HuS
\,vater
arshe
slbme
hy&ogen sulf;de