This packet goes in order with PP2. Fill out all of the examples and then go back to the front and do the worksheet to see if you retained any of the information.

1. 1
Exam 2 Naming Worksheet
Formula Name Ionic or Covalent?
C2H3O2-
sodium sulfide
NO3-
bromate
HCO3-
cuprous oxide
Na3PO4
magnesium sulfate
heptahydrate
CuO
chromium (III) bromide
P2O5
HCl
nitrous acid
NaNO2
iron (III) sulfide

2. 2
Monoatomic Ions
Metals: Nonmetals:
Polyatomic Ions: covalently bonded compounds made of two
or more atoms that are considered as a single unit.
Ammonia: ____________
Ammonium: __________
Acetate: _______________
Cyanide:_______________
Hydroxide:____________
Peroxide:______________
Oxyanions: type of polyatomic ions with added oxygen atom
BO33- borate CO32- carbonate
Two Ions in Series Four Ions in Series
Compound more oxygen atoms ends
with ________
Compound with less oxygen atoms
ends with ________
NO3- ____________ NO2- ____________
SO42- ____________ SO3-2 ____________
SeO42-___________ SeO32- ____________
SO42-____________ SO3-2_____________
TeO42-___________ TeO32-____________
AsO43-___________ AsO33-___________
PO43-____________ PO33-____________
Oxyanion with more oxygen atoms
than the “-ate”, now also begins
with _______
Oxyanion with less oxygen atoms
than the “-ite”, now also begins
with ________
ClO4- ___________ IO4-____________
ClO3- ___________ IO3- ____________
ClO2- ___________ IO2-____________
ClO- ____________ IO- ____________
BrO4-____________
BrO3- ____________
BrO2- ____________
BrO- ___________

3. 3
Oxyanions with H+ added
Current Version: (-prefix hydrogen OR dihyrogen)+(anion)
PO43- phosphate ion = HPO42- hydrogen phosphate ion
= H2PO4- dihydrogen phosphate ion
Older Version: (-prefix bi)+(anion)
HCO3- _______________________ HPO42- _______________________
Binary Ionic Compounds
Metals forming a single ion: ________________________________________
KCl ____________________ Na2S ____________________
Metals forming multiple ions
Current: ______________________________________________
CuO _________________ Cu2O ___________________
________ iron (III) sulfate ________ copper (II) chloride
Older Version: ____________________________________________
FeS ___________________ Fe2S3 _____________________
________ copper (I) chloride _______ mercury (II) oxide

4. 4
Ionic Compounds containing polyatomic Ions
Since we should have the polyatomic ions charge memorized,
we do not need to indicate how many of each ion there will be.
MgSO4 _______________________
__________ aluminum chromate
Na3PO4 _______________________
Hydrates: Ionic compounds with water molecules added
We use prefixes to indicate the number of water molecules
1=mono 2=di 3=tri 4=tetra 5=penta
6=hexa 7=hepta 8=octa 9=nona 10=deca
MgSO4  7H2O  magnesium sulfate ________hydrate
CoCl2  6H2O  cobalt (II) chloride ________hydrate
(Barely Ever seen on Exams)
Covalent Compounds
Formula:(prefix)+(1st non-metal)+(prefix)+(2nd non-metal)
(same prefixes as the hydrates)
1=mono 2=di 3=tri 4=tetra 5=penta
6=hexa 7=hepta 8=octa 9=nona 10=deca
NCl3  nitrogen trichloride
P2O5 diphosphorous pentoxide
________  disulfur dichloride
Cl2O7 __________________________

5. 5
Binary Acids: Hydrogen + non-metal
Formula: (hydro)+(nonmetal+ic)+(acid)
HBr hydrobromic acid
_______  hydrochloric acid
H2S ____________________________
HF ____________________________
Oxyacids: Hydrogen + polyatomic ion
If polyatomic ion ended in –ate, it changes to –ic acid
If polyatomic ion ended in –ite, it changes to –ous acid
EX: chloratechloric acid chlorite chlorous acid
HNO4 pernitric acid
HNO3 __________________
HNO2 __________________
________  hyponitrous acid
H2CO4 _______________________
H2CO3 ______________________
__________  carbonous acid
H2CO________________________