Nomenclature Learn to name binary compounds of a metal and a nonmetal. Learn how to name binary compounds containing only nonmetals. Learn the names of common polyatomic ions and how to use them in naming compounds. Learn names for common acids and how the anion composition determines the acids name. Learn to write the formula of a compound, given its name.
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Nomenclature Learn to name binary compounds of a metal and a nonmetal. Learn how to name binary compounds containing only nonmetals. Learn the names of.
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Nomenclature
Learn to name binary compounds of a metal and a nonmetal.
Learn how to name binary compounds containing only nonmetals.
Learn the names of common polyatomic ions and how to use them in naming compounds.
Learn names for common acids and how the anion composition determines the acids name.
Learn to write the formula of a compound, given its name.
Naming compounds
Common names are Epsom salts, milk of magnesia, laughing gas, and many more
There are over 4 million different compounds and more are discovered all the time
Memorizing the common names would be impossible so we have a system
Binary compounds
Compounds composed of 2 elements Two types:
Compounds that contain a metal and nonmetal
Compounds that contain 2 nonmetals
Naming Compounds That Contain a Metal
and a NonmetalTo learn to name binary
compounds of a metal and a nonmetal.
Binary Ionic Compound
Contain a positive ion (cation) and a negative ion (anion)
Two types of binary ionic compounds Type I: contain elements with only one
ion Na+, Cs+, Ca+2, etc
Type II: contain elements with 2 or more ions
Cr+2 or Cr+3, Cu+ or Cu+2
Type I Binary Ionic Compounds
The cation is always named 1st
The cation is named as the element name Na+ is sodium
The anion is named by taking the 1st part of the element name and adding –ide Cl- is chloride
Type I Binary Ionic Compounds
NaI sodium iodide
CaO calcium oxide
NaCl sodium chloride
KI potassium iodide
CaS calcium sulfide
CsBr cesium bromide
MgO magnesium oxide
CsF cesium fluoride
AlCl3 aluminum chloride
MgI2 magnesium iodide
Rb2O rubidium oxide
SrI2 strontium iodide
K2S potassium sulfide
Type II Binary Ionic Compounds
Some metals can produce 2+ ions When this happens, we use Roman
Numerals The Roman numerals only tell us the
charge, not how many of that ion there are in the compound
You do not need to use Roman numeral for metals that form only 1 cation
Type II Binary Ionic Compounds
What is FeCl2 made of? Fe+2 and two Cl-
What would we name it? Iron (II) chloride
What is PbO2 made of and what is its name? Pb+4 and 2 O-2 called lead (IV) oxide
Type II Binary Ionic Compounds
Write out the following and give their name CuCl
copper (I) chloride HgO
mercury (II) oxide Fe2O3
iron (III) oxide MnO2
manganese (IV) oxide PbCl4
lead (IV) chloride
Review Type I and II
CoBr2
Co+2 + Br- cobalt (II) bromide CaCl2
Ca+2 + Cl- calcium chloride Al2O3
Al+3 + O-2 aluminum oxide CrCl3
Cr+3 + Cl- chromium (III) chloride
Naming Binary Compounds That
Contain Only Nonmetals (Type III)
To learn how to name binary compounds containing only
nonmetals.
Rules for naming Type III The 1st element in the formula is named 1st and
the full element name is used. The 2nd element is named as though it were an
anion. Prefixes are used to indicate the # of atoms
present The prefix mono- is never used for the 1st
element
Prefixes for Type III mono- 1 di- 2 tri- 3 tetra- 4 penta- 5 hexa- 6 hepta- 7 octa- 8
Type III
BF3
notice they are both nonmetals Name the 1st element – boron Name the 2nd as an anion – fluoride Add prefixes
boron trifluoride
Practice Problems
NO nitrogen monoxide
N2O3 dinitrogen trioxide
CCl4 carbon tetrachloride
NO2 nitrogen dioxide
IF3 iodine trifluoride
I2O7 diiodine heptoxide
CO2 carbon dioxide
CF4 carbon tetrafluoride
NH3 nitrogen trihydride
PCl3 phosphorous trichloride
Naming Binary Compounds: A
ReviewTo review the naming of Type
I, II, and III binary compounds.
Naming binary compounds
Binary Compound?
Yes
Metal Present?
YesNo
Type III: Use prefixes Does the metal form more than one cation?
No Yes
Type I: Use the element name for the
cation
Type II: Determine the charge of the
cation; use a Roman numeral after the
cation
Type I, II, III
AsF3 arsenic trifluoride
Al2S3 aluminum sulfide
SnBr4 tin (IV) bromide
CS2 carbon disulfide
CdS cadmium sulfide
AgCl silver chloride
KI potassium iodide
NO nitrogen monoxide
P2O5 diphosphorous pentoxide
FeCl3 iron (III) chloride
Naming compounds with polyatomic ions
Simply write the name of the polyatomic ion No change is needed
What would NH4C2H3O2 be called? Look at the table
NH4 – ammonium C2H3O2 – acetate
Put the them together in the same order as the formula
Ammonium acetate
Naming compounds with polyatomic ions
If using a cation with more than one charge, use Roman numerals Fe(NO3)3
The 2nd 3 tells us that there are 3 NO3 in the formula
Looking on our chart we see NO3 has a charge -1
If they’re totaled, that makes our total charge -3
Fe must be +3 to cancel it out Iron (III) nitrate
Polyatomic Practice
Na2SO4
sodium sulfate
KH2PO4
potassium dihydrogen phosphate
Mn(OH)2
Manganese (II) hydroxide
Na2SO3
sodium sulfite
Cu(NO3)2
Copper (II) nitrate
PbCO3
Lead (II) carbonate
KHSO4
potassium hydrogen sulfate
NH4I ammonium iodide
NaCN sodium cyanide
Naming Chemical Compounds
Binary Compound?
Yes
Metal Present?
YesNo
Type III: Use
prefixes
Does the metal form more than one cation?
NoYes
Type I: Use the element
name for the cation
Type II: Determine the charge of the
cation; use a Roman numeral after the cation
No
Polyatomic Ion or Ions Present?
No Yes
We will learn this
procedure
later.
Name the compound similar to naming binary
compounds but use the polyatomic chart for
their names
Name the following chemical compounds to be turned in for
a grade1. Na2CO3
2. FeBr3
3. PCl3
4. CsClO4
5. CuSO4
6. NaHCO3
7. BaSO4
8. CsClO4
9. BrF5
10. NaBr11. KOCl12. Zn3(PO4)2
13. Ca(HCO3)2
14. MgI2
15. KMnO4
16. Sb2O3
17. Fe(OH)2
1. Na2CO3 sodium carbonate
2. FeBr3 iron (III) bromide
3. PCl3 phosphorous trichloride
4. CsClO4 cesium perchlorate
5. CuSO4 copper (II) sulfate
6. NaHCO3 sodium hydrogen carbonate
7. BaSO4 barium sulfate
8. CsClO4 cesium perchlorate
9. BrF5 bromine pentafluoride
10. NaBr sodium bromide
11. KOCl potassium hypochlorite
12. Zn3(PO4)2 zinc (II) phosphate
13. Ca(HCO3)2 calcium hydrogen carbonate
14. MgI2 magnesium iodide
15. KMnO4 potassium permanganate
16. Sb2O3 antimony (III) oxide
17. Fe(OH)2 iron (II) hydroxide
Naming Acids
To learn how the anion composition determines the
acid’s nameTo learn names for common
Acids
A molecule w/ one or more H+ ions attached to an anion
The rules for naming acids depend on whether it has oxygen
Rules for naming acids
If no oxygen is present Add prefix hydro- and suffix –ic to the root
word and the word acid to the end HCl
hydro + chlorine + ic + acid hydrochloric acid
Rules for naming acids
If oxygen is present Named after the anion present
When anion ends in –ate Add suffix –ic and the word acid H2SO4 sulfate becomes sulfuric acid
When anion ends in –ite Add suffix –ous and the word acid HNO2 nitrite becomes nitrous acid
Naming AcidsDoes the anion contain oxygen?
YesNo
hydro-+anion root+ -ic hydro(anion root)ic acid
Check the ending of the anion name
-ite -ate
anion or element root+ -ous(root)ous acid
anion or element root+ -ic(root)ic acid
Acid Practice HF
Hydrofluoric acid H3PO3
Phosphorous acid HNO3
Nitric acid HBrO3
Bromic acid H2S
Hydrosulfuric acid
Writing Formulas from Names
To learn to write the formula of a compound, given its
name
Formulas from names So far you were given a name and you
gave the formula A lot of times the reverse is also
necessary calcium hydroxide
Ca+2 OH-
You will need 2 hydroxide ions to cancel out the +2 charge of Ca