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Chemical Nomenclature
Written by Y. Deng, J. Bazzi and D. BandyopadhyayProduced by the Science Learning Center (SLC)
University of Michigan -Dearborn
2013
What is Chemical Nomenclature?
A set of rules to generate systematic names for chemical substancesLanguage of chemistryUsed by scientists, particularly chemists, to communicate and discuss the issues related to chemistry
?
Purpose
To introduce the systems of chemical nomenclature used to name inorganic compounds and to write chemical formulas of inorganic compounds.
Inorganic vs. Organic CompoundsInorganic compounds are referred traditionally to those
extracted from non-living things (e.g., rocks) and viewed as being synthesized by geological systems.Examples: calcium carbonate (a major compound found in rocks): CaCO3
Sodium chloride (a major compound found in table salt): NaClOrganic compounds, on the other hand, are referred
traditionally to those found in living things (e.g., plants and animals) and mainly contain carbon-hydrogen chain and ring structures. Examples: Ethanol (one of the fermentation products of grapes): CH3CH2OH
Caffeine (one of the components found in coffee beans):
Specific Objectives:1. Write correct chemical formulas
for inorganic compounds.
2. Name inorganic compounds.
3. Determine the electric charges of ions involved in ionic compounds.
The Periodic Table of the Elements is a tabular arrangement of the chemical elements, organized on the basis of their atomic numbers (i.e., the number of protons in their nuclei) and recurring chemical properties.
There are 118 elements currently listed on the periodic table. About 90 elements are found in nature. The remaining ones have been produced artificially using high energy particle accelerators.
Each element has its name and symbol. The symbol can be up to three letters. The first letter must be capitalized and the second and third, if any, are in a lower case.
Examples:Name SymbolNitrogen NChlorine ClUnun pentium Uup
The symbols of the elements are derived from:
English nameshydrogen – Hcalcium– Caphosphorus – P
Latin namesFerrum (iron) – FeAurum (gold) – Au
Chemical Symbols Derived from Their English Names
Symbol English Name Symbol English Name
H hydrogen S sulfur
C carbon Cl chlorine
N nitrogen Ca calcium
O oxygen Mg magnesium
F fluorine Mn manganese
Al aluminum Co cobalt
Si silicon Ni nickel
P phosphorous Zn zinc
Ba barium Cr chromium
Chemical Symbols Derived from Their Latin NamesSymbol English
NameLatin Name
Meaning
Ag silver argentum silver
Au gold aurum shining dawn
Fe iron ferrum iron
Hg mercury hydrargyrum liquid silver
K potassium kalium potash silver
Na sodium natrium soda
Pb lead plumbum heavy
Cu copper cuprum “from Cyprus” where the Romans found copper.
alkali metals
Noble gases
1IA alkaline
earth metals halogens
18VIIIA
or 0
HHydrogen
2IIA
13IIIA
14IVA
15VA
16VIA
17VIIA
HeHelium
LiLithium
BeBeryllium
Transition Metals
BBoron
CCarbon
NNitrogen
OOxygen
FFluorine
NeNeon
NaSodium
MgMagnesium
AlAluminum
SiSilicon
PPhosphorus
SSulfur
ClChlorine
ArArgon
KPotassium
CaCalcium
BrBromine
RbRubidium
SrStrontium
SnTin
IIodine
XeXenon
CsCesium
BaBarium
PbLead
The main group elements that must be memorized, indicated in green color for their symbols and names
4IVB
5VB
6VIB
7VIIB
8 9 1011IB
12IIB
←VIIIB→
TiTitanium
VVanadium
CrChromium
MnManganese
FeIron
CoCobalt
NiNickel
CuCopper
ZnZinc
AgSilver
PtPlatinum
AuGold
HgMercury
The transition metal elements that must be memorized, indicated in red color of their symbols and names
Exercise 1
Write names or symbols of the following elements.
1. Ca 8 . tin2. K 9. silicon3. Co 10. gold4. Mn 11. copper5. Cr 12. carbon6. Fe 13. neon7. P 14. bromine
Naming Binary Ionic Compounds
An ionic compound is a chemical compound in which ions are held together by the electrostatic forces between oppositely charged bodies.
Usually, the positively charged portion consists of metal cations (e.g., Na+) and the negatively charged portion consists of anions (e.g., Cl-).
Formation of An Ionic Compound
Cl
Cl-
e -
A sodium atom loses an electron to form a positive ion (cation): Na+.A chlorine atom gains an electron to form a negative ion (anion): Cl-.The cation and the anion are held together by the electrostatic forces (ionic bond) to form an ionic compound.
Na
Na+
Rules for Naming Binary Ionic Compounds
1. When naming cations, the name of the element is used.
2. When naming anions that are derived from an atom of the element, the name of the element is modified with the suffix –ide added.
3. Write the symbol of the cation first, and then the symbol of the anion.
For example: Chlorine (Cl) is the name of the element. When a chlorine atom gains an electron, it becomes an anion, chloride (Cl-).
NaCl
Formation of Magnesium Chloride
MgCl
e- e-
Write the formula with the positive & negative charges balanced. Mg 2+ + 2 Cl- MgCl2
Mg2+
Cl
Cl- Cl-
A subscript “2” is used to indicate number of chloride ion present in a magnesium chloride compound.
4. Compounds are electrically neutral, thus the total number of cations and anions must be such that positive and negative charges balance to zero.
5. The number of each ion present in the compound is designated by a subscript following its chemical symbols. For example, an aluminum oxide compound consists of 2 aluminum cation (Al3+) and 3 oxide anions (O2-).
Rules for Naming Binary Ionic Compounds(Continued)
MgCl2
Al2O3
15VA
16VIA
17VIIA
18VIIIA
1IA
2IIA
13IIIA
3 2 1 0 +1 +2 +3
1H
2He
3Li
4Be
7N
8O
9F
10Ne
11Na
12Mg
13Al
15P
16S
17Cl
18Ar
19K
20Ca
Transition Metal
Elements
31Ga
35Br
36Kr
37Rb
38Sr
53I
54Xe
55Cs
56Ba
A modified periodic table useful for writing formulas for binary ionic compounds. The numbers in blue indicate the common charges of cations and anions after these atoms gain or lose electrons.
Metals Non-metals
Examples of Binary Ionic Compounds
Full Name Name of Cation Name of Anion Chemical Formula
sodium chloride sodium (Na+) chloride (Cl-) NaCl
lithium bromide lithium (Li+) bromide (Br-) LiBr
calcium iodide calcium (Ca 2+) Iodide (I-) CaI2
aluminum sulfide aluminum (Al3+) sulfide (S2-) Al2S3
potassium oxide potassium (K+) oxide (O2-) K2O
lithium hydride lithium (Li+) hydride (H-1) LiH
barium nitride barium (Ba2+) nitride (N3-) Ba3N2
strontium phosphide strontium (Sr2+) phosphide (P3-) Sr3P2
Some metals can form cations with different charges. These cations can be named using two systems:
(a) Stock System:The charges of cations can be described by using Roman numerals.
Ex. Iron can form two cations: Fe2+ & Fe3+ FeCl2: iron(II) chlorideFeCl3: iron(III) chloride(pronounce: iron-two chloride; iron-three chloride)(b) Classical system:Assign the ending “ous” to the cations with fewer positive charges and the ending “ic” to the cations with more positive charges
Ex. Iron can form two cations: Fe2+ & Fe3+ FeCl2: ferrous chlorideFeCl3: ferric chloride
Element CationsNames, Charges
chromium, Cr chromium(II)(chromous) +2 chromium(III)
(chromic) +3
cobalt, Co cobalt(II)(cobaltous) +2 cobalt(III)
(cobaltic) +3
copper, Cu copper(I)(cuprous) +1 copper(II)
(cupric) +2
iron, Fe iron(II)(ferrous) +2 iron(III)
(ferric) +3
lead, Pb lead(II)(plumbous) +2 lead(IV)
(plumbic) +4
manganese, Mn manganese(II)(manganous) +2 manganese(III)
(manganic) +3
mercury, Hg mercury(I)(mercurous) +1 mercury(II)
(mercuric) +2
nickel, Ni nickel(II)(nickelous) +2 nickel(III)
(nickelic) +3
tin, Sn tin (II)(stannous) +2 tin(IV)
(stannic) +4
Naming of Cations Using the Classical and Stock Systems:
Additional Examples of Binary Ionic Compounds
Chemical Formula Name of Cation Name of
AnionName
(Stock System)Name
(Classical System)
FeF2(Fe2+)
iron(II), ferrous fluoride (F-) iron(II) fluoride ferrous fluoride
FeF3(Fe3+)
iron(III), ferric fluoride (F-) iron(III) fluoride ferric fluoride
Cu2O (Cu+)
copper(I), cuprous oxide (O2-) copper(I) oxide cuprous oxide
CuO (Cu2+)copper(II), cupric oxide (O2-) copper(II) oxide cupric oxide
PbBr2(Pb2+)
lead(II), plumbousbromide
(Br-)lead(II)
bromideplumbousbromide
PbBr4(Pb4+)
lead(IV), plumbicbromide
(Br-)lead(IV)bromide
plumbicbromide
Exercise 2Give the names or formulas of the following binary
ionic compounds. If a compound can be named by both the Stock and the Classical systems, provide both names.
1. CaO2 8. aluminum chloride
2. NaH 9. calcium phosphide3. Mg3N2 10. stannous oxide
4. FeI3 11. ferric bromide
5. CuCl 12. ferrous bromide6. CuCl2 13. barium nitride
7. Ba3P2 14. nickel(III) chloride
IIIA IVA VA VIA VIIA
VIB VIIB
BBO3
3-
borate
CCO3
2-
carbonate
NNO3
-
nitrate{NO2
-}{nitrite}
O F
SiSiO4
4-
silicate
PPO4
3-
phosphate{PO3
3-}{phosphite}
SSO4
2-
sulfate{SO3
2-}{sulfite}
ClClO3
-
chlorate {ClO2
-}{chlorite}
CrCrO4
2-
chromateCr2O7
2-
dichromate
MnMnO4
2-
manganateMnO4
-
permanganate
BrBrO3
-
bromate
IIO3
-
iodate
An oxo-anion usually contains two elements in which one of them must be oxygen. The oxo-anions of some elements (in blue) can have either a suffix -ate or -ite added to the root names of the elements. For example, SO4
2- and SO32- are oxo-anions of sulfur
element. Their names are sulfate and sulfite, respectively.
Names of Some Oxo-Anions
Names of Common Polyatomic Ions
Formula of Ion Name of Ion Formula
of Ion Name of ion Formula of Ion Name of Ion
NO2- nitrite NO3
- nitrate SCN- thiocyanate
SO42- sulfate HSO4
- hydrogen sulfate bisulfate BrO3
- bromate
SO32- sulfite HSO3
- hydrogen sulfitebisulfite AsO3
3- arsenite
CO32- carbonate HCO3
- bicarbonatehydrogen carbonate AsO4
3- arsenate
MnO4- permanganate CrO4
2- chromate Cr2O72- dichromate
PO43- phosphate HPO4
2- hydrogen phosphate H2PO42- dihydrogen
phosphate
ClO2- chlorite ClO3
- chlorate ClO4- perchlorate
ClO- hypochlorite IO3- iodate IO4
- periodate
Names of Common Polyatomic Ions (cont.)Formula Ion
NH4+ ammonium
Hg22+ mercury(I)
(mercurous)CN cyanideOH hydroxideO2
2 peroxide
SCN thiocyanateC2H3O2
(or CH3COO-) acetateCHO2
- (or HCOO-) formateC2O4
2- (or -OOC-COO-) oxalate
Examples of Ionic Compounds with Polyatomic Ions
Formula Name of Cation Name of Anion Stock System
Classical System
NiSO4(Ni2+)
nickel(II), nickelous sulfate(SO42-) nickel(II)
sulfatenickelous
sulfate
Ni2(SO4)3(Ni3+)
nickel(III), nickelic sulfate(SO42-) nickel(III)
sulfatenickelicsulfate
(NH4)2HPO4 (NH4+), ammonium hydrogen
phosphate(HPO42-)
ammoniumhydrogen
phosphate
ammonium hydrogen
phosphate
Al(CH3COO)3 Al3+, aluminum acetate(CH3COO -) aluminum acetate
aluminum acetate
Hg2(NO2)2
(Hg22+)
mercury(I) mercurous
nitrite(NO2-) mercury(I)
nitritemercurous
nitrite
Hg(NO2)2
(Hg2+)mercury(II)
mercuricnitrite(NO2
-) mercury(II)nitrite
mercuricnitrite
Exercise 3
Give the names or formulas of the following ionic compounds with polyatomic ions. If a compound can be named by both the Stock and the Classical systems, provide both names.
1. CaSO3 8. calcium phosphate
2. NaHCO3 9. cuprous sulfite
3.Hg2(NO3)2 10. ammonium nitrite
4. Hg(NO2)2 11. ferrous dihydrogen phosphate
5. Cu(CH3COO)2 12. barium cyanide
6. Ba(SCN)2 13. potassium permanganate
7. Na2Cr2O7 14. plumbous carbonate
Formula Pure Substance Aqueous SolutionHCl hydrogen chloride hydrochloric acid
HBr hydrogen bromide hydrobromic acid
HI hydrogen iodide hydroiodic acid
H2S hydrogen sulfide hydrosulfuric acid
HCN hydrogen cyanide hydrocyanic acid
A. Acids without oxygen atoms
An acid is a substance that ionizes in water to produce hydrogen ions (H+). A base is a substance that ionizes in water to produce hydroxide ions (OH-).
The following compounds are named depending on whether they are present as pure substances or are dissolved in water to form aqueous solutions .
B. Common oxo-anions and their corresponding oxo-acids.
Element Oxo-Anion Oxo-Acidboron BO3
3 borate H3BO3 boric acid
nitrogen NO3 nitrate HNO3 nitric acid
phosphorusPO4
3 phosphate H3PO4 phosphoric acid
PO33 phosphite H3PO3 phosphorous acid
sulfurSO4
2 sulfate H2SO4 sulfuric acid
SO32 sulfite H2SO3 sulfurous acid
chlorine
ClO hypochlorite HClO hypochlorous acid
ClO2 chlorite HClO2 chlorous acid
ClO3 chlorate HClO3 chloric acid
ClO4 perchlorate HClO4 perchloric acid
bromine BrO3 bromate HBrO3 bromic acid
iodine IO3 iodate HIO3 iodic acid
C. Common organic acids
Formula Name
HCOOH (CH2O2) formic acid
CH3COOH (C2H4O2) acetic acid
HOOCCOOH (C2H2O4) oxalic acid
D. Bases
Formula Name Formula Name
NaOH sodium hydroxide LiOH lithium hydroxide
KOH potassium hydroxide Sr(OH)2 strontium hydroxide
Mg(OH)2 magnesium hydroxide Ca(OH)2 calcium hydroxide
Ba(OH)2 barium hydroxide AgOH silver hydroxideZn(OH)2 zinc hydroxide Al(OH)3 aluminum hydroxide
Hg2(OH)2mercury(I) hydroxidemercurous hydroxide Hg(OH)2
mercury(II) hydroxidemercuric hydroxide
CuOH copper(I) hydroxidecuprous hydroxide Cu(OH)2
copper(II) hydroxidecupric hydroxide
Ni(OH)2nickel(II) hydroxidenickelous hydroxide Ni(OH)3
nickel(III) hydroxidenickelic hydroxide
Co(OH)2cobalt(II) hydroxidecobaltous hydroxide Co(OH)3
cobalt(III) hydroxidecobaltic hydroxide
Pb(OH)2lead(II) hydroxide
plumbous hydroxide Cr(OH)3chromium(III) hydroxide
chromic hydroxide
Exercise 4
Give the names or formulas of the following acids and bases. If an acid or a base can be named by both the Stock and the Classical systems, provide both names.
1. HF (aqueous solution) 8. nitric acid
2. H2SO3 9. aluminum hydroxide
3. H2CO3 10. ferric hydroxide
4. H2S (pure substance) 11. cuprous hydroxide
5. Hg2(OH)2 12. hydrocyanic acid
6. Fe(OH)2 13. nitrous acid
7. H3PO4 14. sulfuric acid
Hydrates – compounds that have a specific number of water molecules attached to them.
Examples:
(1) BaCl2·2H2O
(2) CuSO4·5H2O
(3) MgSO4·7 H2O
The First Ten Greek Prefixes
Greek Prefix Number
mono- 1di- 2tri- 3
tetra- 4penta- 5hexa- 6hepta- 7octa- 8nona- 9deca- 10
Examples of Hydrates and Their Names
(1) BaCl2·2H2O
Name: barium chloride dihydrate(2) CuSO4·5H2O
Name : copper(II) sulfate pentahydrate (Stock System)
Or cupric sulfate pentahydrate (Classical System)
(3) MgSO4·7 H2O
Name: magnesium sulfate heptahydrate
The Greek prefixes are used to indicate the number of water molecules in hydrates.
Exercise 5
Give the names or formulas for the following hydrates. If a hydrate can be named by both the Stock and the Classical systems, provide both names.
(1) LiCl·H2O (6) barium chloride dihydrate
(2) MgSO4·7H2O (7) sodium carbonate decahydrate
(3) CoCl2·6H2O (8) ferrous sulfate hexahydrate
(4) CuSO4·5H2O (9) strontium nitrate tetrahydrate
(5) Na2SO4 10H∙ 2O (10) manganese(II) nitrate tetrahydrate
NAMING BINARY MOLECULAR COMPOUNDS(CONTAINING TWO ELEMENTS, BUT DON’T CONTAIN CATIONS AND ANIONS)
Part VI
Rules for Naming Binary Molecular Compounds
1.When naming the first element, the name of the element is used.
2.Then name the second element by taking the first part of the element name and adding the suffix “ide”.
3.Use Greek prefixes to denote the number of atoms of each element present.
4.The prefix “mono” can be omitted for the first element.
5.For oxides, the ending “a” in the prefix is sometimes omitted.
Examples of binary molecular compounds: CO2, CCl4
Examples
CO: carbon monoxide (not monocarbon monoxide)
CO2: carbon dioxide
SO3: sulfur trioxide
N2O4: dinitrogen tetroxide (not tetraoxide)
PCl5: phosphorus pentachloride
S2F10: disulfur decaflouride
An exception to the use of Greek prefixes involves molecular compounds containing hydrogen
Traditionally, many of these compounds are called either by their common names or by names that do not specifically indicate the number of H atoms present.
Examples:CH4 - methane; NH3 – ammonia; PH3 –
phosphineH2O- water; H2S – hydrogen sulfide; SiH4 -silane
Exercise 6
Give the names or formulas for the following binary molecular compounds.
1. NO 8. dinitrogen monoxide
2. SO2 9. boron trichloride
3. Cl2O7 10. diarsenic pentoxide
4. PBr3 11. sulfur hexachloride
5. SF6 12. nitrogen triiodide
6. P2O5 13. carbon tetra bromide
7. CCl4 14. diphosphorus pentoxide
AcknowledgementsThe authors would like to thank Ali Bazzi, Ogie Stewart and Ruixiao Zuo for their valuable comments and suggestions that were of great help in preparing and improving this module.
The authors would like to thank Annette Sieg, Assistant Director of SLC, as well as the SLC staff for their help and technical support.
Exercise 1 – Key
Write names or symbols of the following elements
1. Ca calcium 8 . tin Sn2. K potassium 9. silicon Si3. Co cobalt 10. gold Au4. Mn manganese 11. copper Cu5. Cr chromium 12. carbon C6. Fe iron 13. neon Ne7. P phosphorus 14. bromine Br
Exercise 2 - KeyGive the names or formulas of the following binary ionic compounds. If a compound can be named by both the Stock and the Classical systems, provide both names.
1. CaO2 calcium peroxide
2. NaH sodium hydride3. Mg3N2 magnesium nitride
4. FeI3 ferric/iron(III) iodide
5. CuCl cuprous/copper(I) chloride6. CuCl2 cupric/copper(II) chloride
7. Ba3P2 barium phosphide
8. aluminum chloride AlCl3
9. Calcium phosphide Ca3P2
10. Stannous oxide SnO11. Ferric bromide FeBr3
12. Ferrous bromide FeBr2
13. Barium nitride Ba3N2
14. Nickel (III) chloride NiCl3
Exercise 3 - Key Give the names or formulas of the following ionic compounds with polyatomic ions. If a compound can be named by both the Stock and the Classical systems, provide both names.
1. CaSO3 calcium sulfite
2. NaHCO3 sodium hydrogen carbonate
or sodium bicarbonate3.Hg2(NO3)2 mercurous/mercury(I) nitrate
4. Hg(NO2)2 mercuric/mercury(II) nitrite
5. Cu(CH3COO)2 cupric/copper(II) acetate
6. Ba(SCN)2 barium thiocyanate
7. Na2Cr2O7 sodium dichromate
8. calcium phosphate Ca3(PO4)2
9. cuprous sulfite Cu2SO3
10. ammonium nitrite NH4NO2
11. ferrous dihydrogen phosphate Fe(H2PO4)2
12. barium cyanide Ba(CN)2
13. potassium permanganate KMnO4
14. plumbous carbonate PbCO3
Exercise 4 - KeyGive the names or formulas of the following acids and bases. If an acid or a base can be named by both the Stock and the Classical systems, provide both names.
1. HF (aqueous solution) hydrofluoric acid
2. H2SO3 sulfurous acid
3. H2CO3 carbonic acid
4. H2S (pure substance) hydrogen sulfide
5. Hg2(OH)2 mercurous/mercury(I) hydroxide
6. Fe(OH)2 ferrous/iron (II) hydroxide
7. H3PO4 phosphoric acid
8. nitric acid HNO3
9. Aluminum hydroxide Al(OH)3
10. Ferric hydroxide Fe(OH)3
11. Cuprous hydroxide CuOH12. Hydrocyanic acid HCN13. Nitrous acid HNO2
14. Sulfuric acid H2SO4
Exercise 5 - KeyGive the names or formulas for the following hydrates. If a hydrate can be named by both the Stock and the Classical systems, provide both names.
(1) LiCl·H2O lithium chloride monohydrate
(2) MgSO4·7H2O magnesium sulfate heptahydrate
(3) CoCl2·6H2O cobaltous/cobalt (II) chloride hexahydrate
(4) CuSO4·5H2O cupric/copper (II) sulfate pentahydrate
(5) Na2SO4 10H∙ 2O sodium sulfate decahydrate
(6) barium chloride dihydrate BaCl2·2H2O
(7) sodium carbonate decahydrate Na2CO3·10H2O
(8) ferrous sulfate hexahydrate FeSO4·6H2O
(9) Strontium nitrate tetrahydrate Sr(NO3)2·4H2O
(10) manganese (II) nitrate tetrahydrate Mn(NO3)2·4H2O
Exercise 6 - KeyGive the names or formulas for the following binary molecular compounds.
1. NO nitrogen monoxide 8. dinitrogen monoxide
N2O
2. SO2 sulfur dioxide 9. boron trichloride
BCl3
3. Cl2O7 dichlorine heptoxide 10. diarsenic pentoxide
Ar2O5
4. PBr3 phosophorus tribromide 11. sulfur hexachloride SCl6
5. SF6 sulfur hexafluoride 12. nitrogen triiodide NI3
6. P2O5 diphosphorus pentoxide 13. carbon tetrabromide CBr4
7. CCl4 carbon tetrachloride 14. diphosphorus pentoxide P2O5