Chemical
Nomenclature
Naming compounds and writing
chemical formulas.
Canton South Chemistry!
Predicting Charges on Monatomic Ions
+1 +2
+3 +4 +5
+2 +3
-4 -3 -2 -1 0
Understanding Nomenclature
Nomenclature refers to the process of naming chemicals.
Initially the focus is on the most basic rules and ideas involved in
the naming of compounds.
I. Binary Compounds
A binary compound contains just two element
1. The element with the positive
charge ( more metallic ), is written
first.
2. The element with the negative
charge( more non-metallic) is written
second
Understanding Nomenclature
The first
•
word (metal or positive ion) remains the same word
The second word (negative ion) is formed by changing the ending
of the element name to “ide”.
For example:
ex:
fluorine changes to fluoride,
NaCl
KBr
and
oxygen to oxide
sodium chloride
potassium bromide
1. Using the rules given , name the compounds listed below.
1. MgO
____________________ 2. CaI2
__________________
3. BaS
____________________ 4. ZnI2 ______________________
5. CaO
____________________ 6. Ag2O_____________________
7. K3P
____________________ 8. AlBr3_____________________
9. Na3N ____________________ 10. MgS_____________________
Writing proper Chemical formulas.
The net charge of the formula must be zero
potassium
and
chlorine
= potassium chloride
1+
1-
=
0
K
Cl
=
KCl
Crisscross Method
simplified method for writing these formulas
Calcium
Ca2+
Ca2+
1
2+
Ca2+
1
and
bromide
Br1-
=
=
calcium bromide
0
Br12
Subscripts
2Br1-
=
0
Ca1Br2
2
**But we don’t write ones!!!
CaBr2
Crisscross Method
simplified method for writing these formulas
aluminum
Al3+
Al3+
2
6+
Al3+
2
and
sulfide
S2-
=
=
aluminum sulfide
0
S23
Subscripts
6S2-
=
0
Al2S3
3
Al2S3
Using the rule given , give the formula for these compounds
12. sodium chloride ____________13. potassium iodide __________
14. magnesium sulfide __________15. aluminum bromide__________
16. strontium oxide ____________ 17. sodium sulfide
__________
18. rubidium phosphide _________19. barium nitride
__________
Groups/Families
VIIIA
IA
IIA
• 23, 24, 23, 23, 23, 12, 2
•
1, 2
•
24, 13, 12
Cr
+1
+2
Mn
+2
+3
+2
+4
Fe
+2
+3
Co
Ni
+2
+3
+2
+3
Cu
+1
+2
VIIA
I-VIIIB
+1
+2
+4
-4
-3
-2
+2
+4
+3
+5
+2
Cd
+2
multiple
charges
Pt
VIA
Zn
+3
Ag
VA
Au
Hg
+1
+3
+1
+2
-1
0
Type II Binary Compounds
(Stock System)
Some metallic element are capable of more than one
positive charge. We will indicated these with a
roman numeral in parenthesis following the name of
the positive element.
Roman numeral = the + charge
iron (II) = 2+
and
iron (III) = 3+
***Used only when:***
MORE THAN 1 POSITIVE CHARGE
Type II Binary Compounds
(Stock System)
Compare
iron
FeCl2
&
and
chloride
2+
FeCl3
2-
Fe
1
Cl 12
iron
chloride
3+
Fe
1
3Cl13
=
iron(II) chloride
=
0
iron(III) chloride
=
0
***Used only when:***
MORE THAN
1 POSITIVE CHARGE
Type II Binary Compounds
4. Name the following compounds.
21. CuO ______________________ 22. PbS
lead (II) sulfide
________________________
23. HgCl ______________________ 24. MnO2 _________________________
25. Fe2S3 ______________________ 26. SnBr2 ________________________
27. BiCl3 ______________________ 28. PbCl4 ________________________
Classical
or
“Old School”
The "ous"-"ic" System
Another method of indicating metallic ions with
more than one charge is:
a suffix
The suffix -ous is used for the lower charge.
while the suffix -ic is used for the higher ionic charge
* Chemistry trivia time:
In the James Bond movie Goldfinger who was the villian?
Auric Goldfinger
What was the license plate number on Goldfinger's Rolls Royce?
AU3
What was the name of Goldfinger's business establishment?
Auric Enterprises
** Mercury's name was changed because hydroargentous and
hydroargentic would be just to much to handle
“Old School”
The "ous"-"ic" System
(“old school”)
29. ferric chloride
(Stock)
________________________
tin (IV) oxide
30. stannic oxide ________________________
31. mercuric iodide
_____________
SnO2
_____________
________________________
32. cuprous oxide ________________________
33. plumbous sulfide
formula
_____________
_____________
________________________
_____________
34. antimonic bromide _______________________ ____________
35. aurous phosphide
________________________
_____________
Ternary Compounds
It takes “3” or more
A ternary compound contains three or more different elements.
Ternary compounds usually contain one or more polyatomic ions (
Examples:
Fe(ClO4)2
;
NaOH
:
radicals ).
NH4MnO4
When writing the formula – the basic rules apply.
Polyatomic ions ( radicals )are treated just like an ion.
Determining Names and Formulas of Ionic Compounds
Containing Polyatomic Ions
Ex: Calcium hydroxide
Calcium
Ca2+
Ca2+
1
and
hydroxide
OH1-
=
=
calcium hydroxide
0
OH12
Subscripts
CaOH2
But OH2 = H2O = water !!!
***Parentheses : need to be used whenever more than a single
polyatomic ion is needed to balance the charges
- in other words if you add a subscript put the
polyatomic radical in parentheses.
Ca(OH)2
Practice with Polyatomic Ions
NH4OH
ammonium hydroxide
Ba(OH)2
barium hydroxide
Fe(CN)3
iron (III) cyanide
Zn(C2H3O2)2
zinc acetate
ammonium sulfide
(NH4)2S
plumbous hydroxide
Pb(OH)2
... the `ate chart
Polyatomic Ions – they all contain oxygen
-3
-2
-1
PO43-
SO42-
NO3-
CrO42-
ClO3-
CO32-
MnO3-
... the `ate chart
-3
-2
Please
Study
Nomenclature
Crazy
Class
Chemistry
-1
Manana ?
... the `ate become… `ites
–
they all lose an oxygen..
-3
-2
-1
PO33-
SO32-
NO2-
CrO32-
ClO2-
CO22-
MnO2-
but the charge remains the same
... the `ate; the `ite; now the hypo–
subtract another oxygen !!
-3
-2
-1
PO23-
SO22-
NO -
CrO22-
ClO -
CO 2-
MnO -
and the charge remains the same
... the `ate; the `ite; the hypo..
–
lets add an oxygen … the Per-
-3
-2
-1
PO53-
SO52-
NO4-
CrO52-
ClO4-
CO42-
MnO4-
and the charge remains the same
`ate
ClO4-1
`ite
hypo- per-
perchlorate
ClO3-1
chlorate
ClO2-1
chlorite
ClO-1
hypochlorite
carbonate versus bicarbonate
CO3-2
carbonate
Na2CO3
sodium carbonate
HCO3-1
bicarbonate
NaHCO3
sodium bicarbonate
add H+ and drop a negative charge
Determining Names and Formulas of Ionic
Compounds Containing Polyatomic Ions
36.
AlPO4
38. __________
40.
______________________
lithium cyanide
37. (NH4)2CO3
39. ___________
KClO
______________________
42. __________
calcium phosphate
43. ___________
44. __________
ammonium acetate
45. NaMnO4
_______________________
copper(II) nitrate
41. Zn(C2H3O2)2 ______________________
ammonium sulfite
_______________________
Naming Covalent Molecular
Compounds
Nonmetal to Nonmetal ( or to the right of the zigzag red line)
Use these Prefixes:
mono - 1 di 2
penta - 5 hexa 6
nona - 9 deca – 10
Ex:
Greek prefixes to indicate number
(never use mono on first)
tri -
3
hepta - 7
BF3 boron trifluoride
tetra - 4
octa - 8
NO nitrogen monoxide
N2O5 dinitrogen pentoxide
Naming Covalent Molecular Compounds
1. CO
__________________________
8. diphosphorus pentoxide _________________
2. PBr3 ______________________________
9. carbon dioxide
_________________
3. CCl4 ______________________________ 10. selenium trioxide
_________________
4. NCl3 ______________________________
_________________
11. sulfur hexafluoride
5. SeO2 ______________________________ 12. phosphorus pentiodide ________________
6. P2O3 _____________________________
13. sulfur tribromide
________________
7. NH3 ______________________________
14. phosphorus hexachloride______________