http://www.wisegorilla.com/images/chemstry/0-Periodic%20table.gif

http://www.wisegorilla.com/images/chemstry/0-Periodic%20table.gif14/03/2007 14.52.49

NOMENCLATURE REQUIREMENTS FOR INTRODUCTORY CHEMISTRY

Elements

aluminum Al indium In rubidium Rbantimony Sb iodine I ruthenium Ruargon Ar iridium Ir rhodium Rharsenic As iron Fe scandium Scbarium Ba krypton Kr selenium Seberyllium Be lanthanum La silicon Sibismuth Bi lead Pb silver Agboron B lithium Li sodium Nabromine Br magnesium Mg strontium Srcadmium Cd manganese Mn sulfur Scalcium Ca mercury Hg technetium Tccarbon C molybdenum Mo tellurium Tecesium Cs neon Ne thallium Tlchlorine Cl nickel Ni tin Snchromium Cr niobium Nb titanium Ticobalt Co nitrogen N tungsten Wcopper Cu osmium Os uranium Ufluorine F oxygen O vanadium Vgallium Ga palladium Pd xenon Xegermanium Ge phosphorus P yttrium Ygold Au platinum Pt zinc Znhafnium Hf potassium K zirconium Zrhelium He radon Rnhydrogen H rhenium Re

Naturally Occurring Multiatomic Elements

bromine Br2 iodine I2 sulfur S8

chlorine Cl2 nitrogen N2

fluorine F2 oxygen O2

hydrogen H2 phosphorus P4

Monoatomic Anions

hydride H- oxide O2-

fluoride F- sulfide S2-

chloride Cl- nitride N3-

bromide Br- phosphide P3-

iodide I- carbide C4-

Polyatomic Anions

ammonium NH4+

nitrate NO3-

acetate C2H3O2-

nitrite NO2-

carbonate CO32-

chromate CrO42-

hydrogen carbonate HCO3-

dichromate Cr2O72-

perchlorate ClO4-

cyanide CN-

chlorate ClO3-

hydrogen sulfate HSO4-

chlorite ClO2-

sulfate SO42-

hypochlorite ClO-

sulfite SO32-

perbromate BrO4-

hydrogen sulfite HSO3-

bromate BrO3-

hydroxide OH-

bromite BrO2-

phosphate PO43-

hypobromite BrO-

hydrogen phosphate HPO42-

periodate IO4-

dihydrogen phosphate H2PO4-

iodate IO3-

phosphite PO33-

iodite IO2-

hydrogen phosphite HPO32-

hypoiodite IO-

dihydrogen phosphite H2PO3-

permanganate MnO4-

Binary Acids

hydrofluoric acid HF hydroiodic acid HIhydrochloric acid HCl hydrosulfuric acid H2Shydrobromic acid HBr

Oxyacids

acetic acid HC2H3O2 permanganic acid HMnO4

carbonic acid H2CO3 chromic acid H2CrO4

nitric acid HNO3 phosphoric acid H3PO4

nitrous acid HNO2 phosphorous acid H3PO3

perchloric acid HClO4 sulfuric acid H2SO4

chloric acid HClO3 sulfurous acid H2SO3

chlorous acid HClO2 hydrocyanic acid HCNhypochlorous acid HClO

Also include all other halogen acids in this list.

Greek Prefixes

1 mono 4 tetra 7 hepta 10 deca2 di 5 penta 8 octa3 tri 6 hexa 9 nona

Oxides of the Main Group Elements

dinitrogen monoxide N2O sulfur trioxide SO3

nitrogen monoxide NO diphosphorus pentoxide P2O5

dinitrogen trioxide N2O3 carbon monoxide COnitrogen dioxide NO2 carbon dioxide CO2

dinitrogen tetraoxide N2O4 silicon dioxide SiO2

dinitrogen pentoxide N2O5 chlorine dioxide ClO2

This is only a representation of this type of nomenclature.

Metals with fixed oxidation states

aluminum Al3+

Al

cadmium Cd2+

Cd

calcium Ca2+

Ca

lithium Li+

Li

magnesium Mg2+

Mg

potassium K+

K

silver Ag+

Ag

sodium Na+

Na

zinc Zn2+

Zn

Metals with variable oxidation states

chromium Cr2+

Cr3+

Cr6+

Cr(II) Cr(III) Cr(VI)

cobalt Co2+

Co3+

Co(II) Co(III)

copper Cu+ Cu

2+Cu(I) Cu(II)

gold Au+

Au3+

Au(I) Au(III)

iron Fe2+

Fe3+

Fe(II) Fe(III)

lead Pb2+

Pb4+

Pb(II) Pb(IV)

manganese Mn2+

Mn3+

Mn4+

Mn7+

Mn(II) Mn(III) Mn(IV) Mn(VII)

mercury Hg22+

Hg2+

Hg(I) Hg(II)

nickel Ni2+

Ni3+

Ni(II) Ni(III)

tin Sn2+

Sn4+

Sn(II) Sn(IV)

uranium U3+

U4+

U5+

U6+

U(III) U(IV) U(V) U(VI)

Hydrates

Use the Greek prefixes when naming hydrates to indicate the number of water moleculesassociated with each compound.

CoSO4 • H2O cobalt(II) sulfate monohydrateBaI2 • 2 H2O barium iodide dihydrateAu(CN)3 • 3 H2O gold(III) cyanide trihydrateFeI2 • 4 H2O iron(II) iodide tetrahydrateMnSO4 • 5 H2O manganese(II) sulfate pentahydrateCd(MnO4)2 • 6 H2O cadmium permanganate hexahydrateZnSO4 • 7 H2O zinc sulfate heptahydrateMg3(PO4)2 • 8 H2O magnesium phosphate octahydrateAl(BrO3)3 • 9 H2O aluminum bromate nonahydratePb(C2H3O2)2 • 10 H2O lead(II) acetate decahydrate

Chem 127 Dr. Gragson

Chemical NomenclatureNomenclature is essential to our understanding and use of chemistry. Summarized below are the basic rulesyou should learn for naming chemical compounds. You should also read about this in Chapter 2 of your text.Note that this will NOT be covered in any detail in lecture, so you need to work on this on your own or ingroups. YOU MUST LEARN THESE RULES or you will find yourself lost and hurting for the entire term.See me for clarification and assistance.

Naming Ionic Compounds - Ionic compounds are formed between metal and nonmetal

Ionic compounds are named by first identifying the positive ion (the cation) and then the negative ion (theanion). You should note that the cation is always the metal and the anion the nonmetal. The positive ion takesthe same name as its element, the negative ion takes the first part of its element name plus an -ide ending. Thusgiven the following formulas, we would name the compounds accordingly:

Ca3P2 Calcium phosphideMgSe Magnesium selenideNa2O Sodium oxide

To write a formula from a given name, you simply take the symbols for the named elements and combine themin a ratio that gives you a neutral ionic compound. That means that the charges must balance, so you have to doa little figuring as to what ions the elements will form and how many of each you'll need to balance out positiveand negative charges. The number of each element present is shown as a subscript after the element symbol.Example:

Calcium bromide: Ca would form a +2 ion, and Br a -1 ion. Thus to have a neutral compound, you need 2 Br for every 1 Ca The formula would be CaBr2

You must know the names and charges of all monatomic ions listed on the separate handout!

Compounds with metals that can form more than one ionSeveral transition metals can form more than one ion. For systematically named compounds for themetals that can form more than one ion, the charge on the metal will be indicated in the given name by aRoman numeral in parentheses. Thus you can easily determine the corresponding formula. Forexample, iron can form either a +2 or a +3 ion, an example of a compound of the +3 ion is given below:

Iron(III) chloride FeCl3

If given the formula of such an ionic compound, you'll have to use your memorized knowledge of thecation's charge or use the charge on the anion to determine the charge on the cation, and then write thename. For example:

Fe2O3 If you can't remember what ions iron can form, you should atleast be able to use the periodic table to determine that O formsa -2 ion, there are 3 O present for a total of a -6 charge, thus weneed a +6 charge to balance this, there are two Fe, so each musthave a charge of +3. The name for this compound is iron(III)oxide

Chem 127 Dr. GragsonSometimes you will encounter the common name of compounds that contain metals that can form morethan one ion, so you need to be aware of these! An easy way to remember these is that the lower-charged ion will get the -ous suffix, while the higher-charged ion will get the -ic suffix. For example,you should know that iron can form a +2 ion or a +3 ion, the +2 ion will get the -ous suffix and the +3ion will get the -ic suffix. Thus FeCl3 would commonly be known as ferric chloride and FeCl2 would becommonly known as ferrous chloride. You should be able to name such compounds in this mannergiven a formula or write a formula for such compounds given a name. We will not focus on thecommon names, but its good to know them for use in lab and life, so make sure you’re aware of them.

Compounds formed from Polyatomic Ions- these are ionic compounds in whichone or both of the ions are polyatomic, meaning containing more than one atom.

Compounds formed from polyatomic ions are named in the same way as binary ionic compounds: Firstthe cation is identified and then the anion. However, now the ions involved are more complicated, andthere is no systematic way of naming polyatomic ions. This is one of the times in chemistry when youjust have to memorize. For example:

MgSO4 Mg+2 is the magnesium ion, SO4-2 is sulfate, this is

magnesium sulfate

Oxoanions - Most of the polyatomic ions you need to know are oxoanions, inwhich an element, usually a nonmetal, is bonded to one or more oxygen atoms.

There are families of oxoanions in which the nonmetal is bonded to oxygen in severalcombinations, differing only in number of oxygens. The only naming convention in thesefamilies is the following. If there are two oxoanions in the family, the ion with more oxygenstakes the nonmetal root name with an -ate suffix, while the ion with fewer oxygens takes thenonmetal root name with an -ite suffix. For example:

Sulfur combines with oxygen to form both SO3-2 and SO4

-2. Thus, accordingto the convention described above, SO3

-2 is named sulfite and SO4-2 is named

sulfate.

If there are four oxoanions in the family, the ion with the most oxygen atoms has the prefix per-,the nonmetal root and the suffix -ate. Ion with one fewer oxygen has just the root and the suffix-ate. Ion with two fewer oxygens has just the root and the suffix -ite. Ion with fewest oxygenshas the prefix hypo-, the root, and suffix -ite. For example Cl forms four oxoanions:

ClO4- is perchlorate, ClO3

- is chlorate, ClO2- is chlorite, ClO- is hypochlorite.

The polyatomic ions you need to know the names, formulas and charges for are on a separate handout.Commit them to memory now as you’ll need them throughout the term and following terms.

Hydrated Ionic Compounds - these are ionic compounds that have a specificnumber of water molecules associated with each formula unit.

Hydrates are named by attaching the word hydrate with a Greek numerical prefix to the systematic nameof the ionic compound. The Greek prefix tells how many waters are associated with each formula unitof the compound. For example:

MgSO4 •7H2O Magnesium sulfate heptahydrate

Chem 127 Dr. GragsonNaming Acids - Acids are important hydrogen containing compounds

When naming acids, we consider them as anions connected to the number of hydrogen ions (H+) needed tomake the compound neutral. There are two major types of acids to consider.

Binary acids - these are formed when certain gaseous compounds dissolve in water.There are only two elements present as the name implies.

These are basically a single nonmetal, combined with hydrogen. To name such compounds, you attachthe prefix hydro- to the nonmetal root, add an -ic suffix and end with separate word acid. For example:

HCl When hydrogen chloride dissolves in water, hydrochloric acid isformed.

Oxoacids - These are formed between hydrogen and an oxoanion.

The names of oxoacids are similar to those for the corresponding oxoanion, except for the suffixes. Ifyour anion has the -ate suffix, the corresponding acid has an -ic suffix. If your anion has the -ite suffix,the corresponding acid has an -ous suffix. You keep any prefixes to the anions like hypo- and per-. Sofor example:

HClO4 ClO4- is the perchlorate anion, need only one H+ ion to make a neutral

compound.This is perchloric acid.

Naming Covalent Compounds - Covlanet compounds are formed between twononmetals

These compounds are named by giving the element name to the first species listed in the formula, and by givingthe other species the beginning of the element name plus an -ide ending. Essentially, we're treating one speciesas more cation-like and the other as more anion-like, and naming as we did with ionic compounds. Sincenonmetals often combine in different proportions to form a number of different compounds, we have to includeprefixes in the names to indicate the numbers of each kind of atom present. NOTE that neither species in acovalent compound forms an ion, electrons are shared here, so the formula or name is your explicit guide toarriving at the name or formula. For example, given the following formulas we name these two compounds ofcarbon and oxygen as follows:

CO Carbon monoxideCO2 Carbon dioxide

The mono- in front of the first atom present is omitted from the name.

With this type of compound its MUCH easier to write the formula from the name, since the numbers of eachatom present are indicated in the name. For example

Dinitrogen tetroxide N2O4

Sulfur tetrafluorideSF4

You need to memorize the prefixes mono through deca.

Nomenclature Information

There is one really major rule to remember when trying to write a formula. Here it is:

The sum of all positive and negative charges in the formula MUST equal zero.

You can't write a correct formula without following this rule. That's pretty clear, isn't it?

Recommended Skills for Naming Compounds1. Using the periodic table, identify any element as a metal, nonmetal, or metalloid. (Metals are elements which donate electrons assuming a positive charge in compounds. Nonmetals are elements which accept electrons taking on a negative charge in compounds. Metalloids are elements which accept or donate electrons, depending on the circumstances. Hydrogen acts as a postive, but all other properties label it a non-metal. It can also form a –1 charge, so most do not even categorize it with others. Think of it as a category of one.2. Learn the correct spelling of names and symbols of selected elements. (1 - 20, 24 - 30, 35, 47, 50, 53, 56, 79, 80, 82 are recommended for your study.)3. Learn the names, formulas, and oxidation numbers of selected polyatomic ions. Note that a compound which has a polyatomic ion must have more than two elements (examples: sulfate, nitrate, carbonate, acetate, phosphate, chlorate, hydroxide, ammonium, cyanide, iodate).4. Learn the rules for deriving the names and oxidation numbers of related polyatomic ions which differ in the number of oxygen atoms. Learn the connection between the polyatomics and their related acids. Most common to learn are sulfate, nitrate, chlorate, phosphate.

Acid with one more MOST Acid with one less Acid with two lessoxygen atom than COMMON oxygen atom than oxygen atoms thanmost common acid ACID most common acid most common acid HClO4 HClO3 HClO2 HClOPER+ stem+ IC+ ACID stem + IC + ACID stem + OUS + ACID HYPO+ stem +OUS+ACID perchloric acid chloric acid chlorous acid hypochlorous acid

Salt of an acid with Salt of most Salt of acid with Salt of an acid withone more oxygen common one less oxygen two less oxygensthan most common acid than most common than most common acid. acid. acid. NaClO4 NaClO3 NaClO2 NaClOPER + stem + ATE stem + ATE stem + ITE HYPO + stem + ITEsodium perchlorate sodium chlorate sodium chlorite sodium hypochlorite

5. Using the periodic table, determine the most probable charge of non-transition elements.6. Learn a list of selected common metals which have more than one oxidation number. (Fe, Cu, Sn, Hg, Pb, Co, Cr, Au are commonly used in introductory classes like this one.)7. Determine the oxidation number of the elements from the formula of the compound.

8. Learn the seven diatomic gases, sometimes called diatomic elements. They are:Names hydrogen oxygen nitrogen chlorine bromine iodine fluorineFormulas H2 O2 N2 Cl2 Br2 I2 F2On the periodic table, six of them are located in the upper right portion of the table. N O F Notice that these six make a block number 7 and that the top bar Cl of the 7 points (sort-of) in the direction of the seventh diatomic Br element, hydrogen. I

Others like to use the mnemonic HONClBrIF and pretend it is the name of a famous chemist. Whenever you see the name of one of there, write its formula as above. “Bromine” or “bromine gas” means Br2. However “bromide” means Br–1, NOT Br2. Br–1 is also called “bromide ion.”

Common Misconceptions1. Because a given element is diatomic, that the same element will always be diatomic when combined with some other element in a compound. Notice that the number of oxygens is not limited to two in these compounds: CO NO2 HNO3 H2SO4 P2O5Note that the 2 in NO2 DOES NOT mean that there is a diatomic oxygen molecule involved, it means that there are two oxygen atoms. Or in H2SO4, there are not two oxygen molecules, but 4 distinct oxygen atoms.2. Because some of the diatomic elements are gases that all gaseous elements (or even molecules) must be diatomic. Only five of the diatomic molecules are gases at room temperature. Bromine is liquid and iodine is a solid at room temperature. All noble gases are monoatomic. Also greater than diatomic gases exist, P4 and S8.

Symbols and Charges for Monoatomic IonsSymbol Name Symbol NameH+ hydrogen ion H¯ hydrideLi+ lithium ion F¯ fluoride Note that theNa+ sodium ion Cl¯ chloride letters in an ion’sK+ potassium ion Br¯ bromide name before theRb+ rubidium ion I ¯ iodide -ide ending isCs+ cesium ion O2¯ oxide the stem. ForBe2+ beryllium ion S2¯ sulfide example, the stemMg2+ magnesium ion Se2¯ selenide for bromide isCa2+ calcium ion Te2¯ telluride brom-.Sr2+ strontium ionBa2+ barium ion Ag+ silver ion N3¯ nitrideRa2+ radium ion Ni2+ nickel ion P3¯ phosphideZn2+ zinc ion Al3+ aluminum ion As3¯ arsenide

Systematic name Common Systematic name CommonSymbol (Stock system) name Symbol (Stock system) nameCu+ copper(I) cuprous Hg22+ mercury(I) mercurousCu2+ copper(II) cupric Hg2+ mercury(II) mercuricFe2+ iron(II) ferrous Pb2+ lead(II) plumbousFe3+ iron(III) ferric Pb4+ lead(IV) plumbicSn2+ tin(II) stannous Co2+ cobalt(II) cobaltousSn4+ tin(IV) stannic Co3+ cobalt(III) cobalticCr2+ chromium(II) chromous Au+ gold(I) aurousCr3+ chromium(III) chromic Au3+ gold(III) auricMn2+ manganese(II) manganousMn3+ manganese(III) manganic

Symbols and Charges for Polyatomic IonsFormula Name Formula NameNO3¯ nitrate ClO4¯ perchlorateNO2¯ nitrite ClO3¯ chlorateCrO42¯ chromate ClO2¯ chloriteCr2O72¯ dichromate ClO¯ hypochloriteCN¯ cyanide IO4¯ periodateMnO4¯ permanganate IO3¯ iodateOH¯ hydroxide IO¯ hypoioditeO22¯ peroxide BrO3¯ bromateNH2¯ amide BrO¯ hypobromiteCO32¯ carbonate HCO3¯ hydrogen carbonate (bicarbonate)

SO42¯ sulfate HSO4¯ hydrogen sulfate (bisulfate)SO32¯ sulfite HSO3¯ hydrogen sulfite (bisulfite)C2O42¯ oxalate HC2O4¯ hydrogen oxalate (binoxalate)PO43¯ phosphate HPO42¯ hydrogen phosphatePO33¯ phosphite H2PO4¯ dihydrogen phosphate

More Symbols and Charges for Polyatomic IonsS2O32¯ thiosulfate HS¯ hydrogen sulfideAsO43¯ arsenate BO33¯ borateSeO42¯ selenate B4O72¯ tetraborateSiO32¯ silicate SiF62¯ hexafluorosilicateC4H4O62¯ tartrate SCN¯ thiocyanate

C2H3O2¯ acetate (an alternate way to write acetate is CH3COO¯)

There is one positive polyatomic ion. It is NH4+ and is called the ammonium ion.

Prefixes Used to Indicate Number in a Name Involving Two Non-Metalsmono– 1 hexa– 6di– 2 hepta– 7tri– 3 octa– 8tetra– 4 nona– 9penta– 5 deca– 10These prefixes are used in naming binary compounds involving two non–metals. Example include P2O5, Cl2O, NO, N2O, NO2, N2O5, PCl3, PCl5, SO2, SO3, SiO2. Sometimes metal ions are involved in a Greek prefix name, but these are less common. Examples include UF6, SbCl3, SbCl5, OsO4, BiCl3.

There is a preferred order of the nonmetals when writing them in a formula. It is:Rn, Xe, Kr, B, Si, C, Sb, As, P, N, H, Te, Se, S, I, Br, Cl, O, F.

CO is carbon monoxide, NOT carbon monooxide. As4O6 is tetrarsenic hexoxide, NOT tetraarsenic hexaoxide.

Acid Names – add the word acid to each name when saying or writing.Non–oxygen containing Oxygen containing (oxyacids)

Name when dis- Name when a pureFormula solved in water compound Formula NameHF hydrofluoric acid hydrogen fluoride HNO3 nitric acidHCl hydrochloric acid hydrogen chloride HNO2 nitrous acidHBr hydrobromic acid hydrogen bromide H2SO4 sulfuric acidHI hydroiodic acid hydrogen iodide H2SO3 sulfurous acidHCN hydrocyanic acid hydrogen cyanide H3PO4 phosphoric acidH2S hydrosulfuic acid hydrogen sulfide H2CO3 carbonic acid

HC2H3O2 acetic acid(Note that it is hydrogen sulfide, NOT hydrogen sulfuride.) (also written CH3COOH)

Cations (Positive Ions)

Monoatomic Polyatomic

Only One More Than OneIon Possible Ion Possible

Rule: Rule: Rule: ??Name of element + "ion" (a) newer rule - positive charges

indicated by a Roman numeral Examples:Examples: NH4+ ammoniumNa+ sodium ion Examples: Hg22+ mercury(I) ionMg2+ magnesium ion Fe2+ iron(II) ion or mercurous ionH+ hydrogen ion Fe3+ iron(III) ionK+ potassium ion Cu+ copper(I) ion Comment:Sr2+ strontium ion Cu2+ copper(II) ion Hg22+ is two Hg+ ions bonded together,Cs+ cesium ion like this: Hg+—Hg+ Ca2+ calcium ion (b) older rule (but still used) - Latin

stem + "ous" for the lesser charge. However, Hg+ by itself does not exist,Comment: Latin stem + "ic" for the greater therefore mercury(I) ion is Hg22+

The number of positive charges charge.is NOT indictated in the name (Also, Hg2+ is mercury(II), but that is abecause it is not necessary. Examples: monoatomic ion.)These ions NEVER take on Fe2+ ferrous iontwo possible positive charges. Fe3+ ferric ion

Cu+ cuprous ionComment: Cu2+ cupric ionHydrogen will take on a Sn2+ stannous ionnegative one charge (see Sn4+ stannic ionmonoatomic anions fornaming.

Anions (negative ions)

Monoatomic Oxyanions Others and Oxyanions which(containing oxygen) Exceptions contain hydrogen

Rule: Rule: Rule: Rule:Stem of the element least oxygen hypo ___ ite ion These items do not follow any H plus oxyanion:name + "ide" less oxygen ___ ite ion rules; they must be memorized. "hydrogen" + name of

more oxygen ___ ate ion The rules referred to are those oxyanionExamples: most oxygen per ___ ate ion in the box just to the left.H¯ hydride ion H2 plus oxyanion:F¯ fluoride ion Examples: Examples: "dihydrogen" + nameO2¯ oxide ion ClO¯ hypochlorite ion OH¯ hydroxide ion of oxyanionN3¯ nitride ion ClO2¯ chlorite ion CN¯ cyanide ionC4¯ carbide ion ClO3¯ chlorate ion SCN¯ thiocyanate ion Examples:

ClO4¯ perchlorate ion OCN¯ cyanate ion HCO3¯ hydrogenSO32¯ sulfite ion O22¯ peroxide ion carbonate ion orSO42¯ sulfate ion O2¯ superoxide ion bicarbonate ion

MnO42¯ manganate ionComment: MnO4¯ permanganate ion HSO4¯ hydrogenHalogens (except F) form all four C2H3O2¯ acetate ion sulfate ion or bisulfateions. When only two of the four Cr2O72¯ dicromate ion ionexist, they are the -ite and -ate ions. C2O42¯ oxalate ion

HPO42¯ hydrogenphosphate ion orbiphosphate ion

H2PO4¯ dihydrogenComment: phosphate ionH2CO3 is not named using thisrule because it is a compound see comment just toand not an ion. the left.

Compounds

Ionic Compounds with Covalent(Cation–Anion) hydrogen (Two Nonmetals)

H–metal H–nonmetal H–oxyanion

Rule: Rule 1: Rule 1: Rule:Name of cation + name of anion (without the presence of H2O) (without the presence a) Less electronegative(word ion dropped) hydrogen _____ide of H2O) element first.

like ionic compounds: exception: when one ofExamples: Examples: cation + anion the elements isNaCl sodium chloride HCl hydrogen chloride hydrogen hypo ___ite hydrogen.MgCl2 magnesium chloride HBr hydrogen bromide hydrogen ___ite b) Number of atoms ofFe3N2 iron(II) nitride HF hydrogen fluoride hydrogen ___ate each kind specified by(NH4)2S ammonium sulfide H2S hydrogen sulfide hydrogen per ___ate Greek prefixes.Na2CO3 sodium carbonate c) The prefix mono- atNaClO4 sodium perchlorate Rule 2: Rule 2: beginning is dropped.NaH sodium hydride (when dissolved in H2O) (when dissolved in H2O)CaH2 calcium hydride hydro _____ic acid hypo ___ous acid Prefixes:

___ous acid 1 = mono 6 = hexaComment: Examples: ___ic acid 2 = di 7 = heptaThe name does not indicate HCl(aq) hydrochloric acid per ___ic acid 3 = tri 8 = octathe numbers of cations and HF(aq) hydrofluoric acid 4 = tetra 9 = nonaanions because there is only H2S(aq) hydrosulfuric acid Examples: 5 = penta 10 = decaone possibility for the ions to HClO hypochlorous acidcombine to form a compound. Comment: HClO2 chlorous acid Examples:

a) These H-containing compounds HClO3 chloric acid N2O4 dinitrogen tetroxide

Covalent Comment: are named as if they were ionic HClO4 perchloric acid CO carbon monoxide

Tetraoxide becomes tetroxide, compounds. HNO2 nitrous acid CO2 carbon dioxide

monooxide becomes monoxide, etc. b) The (aq) in the formulas of the HNO3 nitric acid PCl3 phosphorous trichloride

so that the name sounds better. acids is often omitted when it is H2SO3 sulfurous acid N2O dinitrogen monoxide

H-containing compounds do not obvious from the context that H2SO4 sulfuric acidfollow a rule concerning the order they are acids. See covalent commentin which the elements are written in the far left corner ofand should be memorized (H2O, NH3, etc.). the page.

Flow Chart for Naming Simple Inorganic CompoundsThe flowchart is adapted from p. 131-132 of the February 1983 issue of the Journal of Chemical Education.

Does the formula Are there twobegin with H? atoms, both It is an Does the acid contain No Yes the same? acid. a polyatomic ion?

Yes No (More than two elements.) Yes No

It is the diatomic gas hydrogen.

Does it begin with a metal Does the polyatomicwhich has more than one end in -ate or -ite?oxidation number? Fe, Ni, -ate -iteCu, Sn, Hg, Pb, Co, Cr, Au Name the first No Yes element followed by

its oxidation number. Name the(Roman numeral) polyatomic

ion, replacing-ate with -ic.

Does the formula contain Add the worda polyatomic ion? (More acid.than two elements.) Is the polyatomic No Yes written first? Name the

No Yes polyatomicion, replacing-ite with -ous.

Name the first element, Add the wordthen the polyatomic ion. acid.

(If two elements are present,name both, then the Write the prefixpolyatomic ion.) hydro, then the

name of theName the polyatomic first, second element

Are both elements then name the element second. with the -icnonmetals? If there are two polyatomics, ending. Add the No Yes name the first, then the second. word acid.

Name the first Are both elementselement, then the the same?second element No Yeswith -ide ending.

Name the first element using the It is a diatomicproper prefix (di, tri, etc.), but never element. Themono. Name the second element with compound has thethe proper prefix (including mono) same name as theand the -ide ending. element.

PREPCHEM Writing Formulas and Naming Compounds

1. Write the formulas for the binary ionic compounds formed between the following elements: a) potassium and iodine: ans d) aluminum and sulfur: ans b) magnesium and chlorine: ans c) sodium and sulfur: ans 2. Name the binary ionic compounds indicated by the following formulas: a) AgCl: ans b) ZnO: ans c) CaBr22: ans d) SrF2 ans

e) BaO: ans f) CaCl2: ans

3. Write the formula and give the name for the compounds formed between the following ions: a) Cu2+and Br1-: ans ans b) Fe2+and O2-: ans ans c) Pb2+ and Cl1-: ans ans d) Hg2+ and S2-: ans ans e) Sn2+ and F1-: ans ans f) Fe3+ and O2- : ans ans 4. Write formulas for the following ionic compounds: a) sodium iodide: ans e) copper (II) sulfate: ans b) calcium chloride: ans f) sodium carbonate: ans c) potassium sulfide: ans g) calcium nitrite: ans d) lithium nitrate: ans h) potassium perchlorate ans 5. Give the names for the following compounds:

http://www.prepchem.org/formulasandnamesofcpds.html (1 of 4)14/09/2006 12.34.48

PREPCHEM Writing Formulas and Naming Compounds

a) Ag2O: ans b) Ca(OH)2: ans

c) KClO3: ans d) NH4OH: ans

e) FeCrO4: ans f) KClO: ans

6. Name the following binary molecular compounds: a) SO3: ans b) ICl3: ans

c) PBr5: ans

7. Write the formulas for the following compounds: a) carbon tetraiodide:ans b) phosphorus trichloride: ans c) dinitrogen trioxide: ans 8. Write formula for the compounds formed between the following: a) aluminum and bromine: ans b) sodium and oxygen: ans c) magnesium and iodine: ans d) Pb2+ and O2-:ans e) Sn2+ and I1-:ans f) Fe3+ and S2-: ans g) Cu2+ and NO3

1-: ans

h) NH4

1+ and SO42-: ans

9. Name the following compounds using the Stock system where appropriate: a) NaI:ans b) MgS: ans c) CaO: ans d) K2S: ans

http://www.prepchem.org/formulasandnamesofcpds.html (2 of 4)14/09/2006 12.34.48

PREPCHEM Writing Formulas and Naming Compounds

e) CuBr: ans f) FeCl2: ans

10. Write the formulas for each of the following compounds: a) barium sulfide: ans b) sodium hydroxide: ans c) lead (II) nitrate: ans d) potassium permanganate: ans e) iron (II) sulfate: ans f) diphosphorus trioxide: ans g) disulfur dichloride: ans h) carbon diselenide: ans **********Physical Science students may stop at this point. ********** i) acetic acid: __________ j) chloric acid: __________ k) sulfurous acid: __________ l) phosphoric acid: __________ 11. Assign oxidation numbers to each atom in the following compounds or ions: a) HCl: H: _____; Cl: _____ b) CF4 C: _____; F: _____

c) PCl3 P: _____; Cl: _____

d) SO2 S: _____; O: _____

e) HNO3 H: _____; N: _____; O: _____

f) KH K: _____; H: _____ g) P4O10 P: _____; O: _____

h) HClO3 H: _____; Cl: _____; O: _____

i) N2O5 N: _____; O: _____

j) GeCl2 Ge: _____; Cl: _____

12. Assign oxidation numbers to each atom in the following compounds or ions:

http://www.prepchem.org/formulasandnamesofcpds.html (3 of 4)14/09/2006 12.34.48

PREPCHEM Writing Formulas and Naming Compounds

a) HF H: _____; F: _____ b) CI4 C: _____; I: _____

c) H2O H: _____; O: _____

d) PI3 P: _____; I: ______

e) CS2 C: _____; S: ______

f) Na2O2 Na: _____; O: _____

g) H2CO3 H: _____; C: _____; O: _____

h) NO2

1-N: _____; O: _____

i) SO4

2- S: _____; O: _____

j) ClO2

1-Cl: _____; O: _____

k) IO3

1-I: _____; O: _____

http://www.prepchem.org/formulasandnamesofcpds.html (4 of 4)14/09/2006 12.34.48

Inorganic Nomenclature Worksheet1. ammonium sulfide 51. aluminum acetate 101. sodium acetate2. sodium nitrate 52. calcium chloride dihydrate 102. zinc sulfite3. cupric bromide 53. barium chromate 103. silver bicarbonate4. aluminum sulfate 54. cobaltic chloride 104. potassium iodide5. potassium nitrate 55. barium chloride dihydrate 105. lead(IV) chlorite6. ferrous carbonate 56. sulfurous acid 106. mercurous chromate 7. lead(II) phosphate 57. potassium hydroxide 107. lead(II) nitrite 8. diphosphorus pentoxide 58. zinc bisulfite 108. potassium dichromate 9. cupric hydroxide 59. sodium sulfite 109. magnesium carbonate 10. calcium fluoride 60. cobaltous sulfate 110. calcium bicarbonate 11. nickel nitrate 61. ferric oxide 111. aluminum hydroxide 12. silver cyanide 62. silver phosphate 112. cobaltous oxide 13. ammonium sulfite 63. sodium hypochlorite 113. ferric permanganate 14. zinc sulfate 64. ammonium chromate 114. ammonium chromate 15. tin(II) chloride 65. barium carbonate 115. nitrogen triiodide 16. antimony(III) chloride 66. calcium iodide 116. sulfur trioxide 17. silver sulfide 67. cupric sulfate 117. ammonium dichromate 18. magnesium hydroxide 68. cuprous chloride 118. iron(III) bicarbonate19. ammonium carbonate 69. ferric carbonate 119. ammonium perchlorate 20. nickel acetate 70. zinc phosphate 120. cobaltic acetate 21. sodium chromate 71. sodium nitrite 121. cobaltous hydroxide 22. chromic bisulfate 72. silver oxide 122. iron(II) chromate 23. potassium permanganate 73. nickel bromide 123. ferric bromide24. silver perchlorate 74. magnesium oxide 124. zinc sulfate25. potassium phosphate 75. mercuric perchlorate 125. boron phosphide26. nickel iodide 76. lithium hypochlorite 126. ferric bicarbonate27. mercurous oxide 77. oxygen difluoride 127. cupric bisulfate28. lead(II) chlorite 78. cobalt(II) hydrogen sulfate 128. acetic acid (diff. from 79)29. hydrogen iodide 79. acetic acid (see #128) 129. barium bisulfite30. iron(II) bisulfite 80. barium hypochlorite 130. nitric acid31. magnesium nitrate 81. ammonium hydroxide 131. calcium sulfide32. iron(III) chromate 82. cobalt(II) iodide 132. copper(I) bisulfate33. iron(II) chromate 83. chromium(II) bicarbonate 133. zinc permanganate34. copper(II) hydroxide 84. sodium hydroxide 134. ferric carbonate35. cuprous carbonate 85. silver nitrate 135. hydrobromic acid36. chromic acetate 86. mercury(II) nitrate 136. hydrocyanic acid37. calcium chlorate 87. hydrochloric acid 137. hydrogen cyanide38. ammonium oxide 88. aluminum bisulfite 138. sulfuric acid39. aluminum perchlorate 89. cobalt(III) hydrogen sulfate 139. copper(I) sulfate40. zinc bicarbonate 90. ferric hydrogen carbonate 140. chromium(III) oxide41. sodium phosphate 91. phosphorus pentabromide 141. aluminum oxide42. silver hypochlorite 92. nickel chloride hexahydrate 142. cobaltous bisulfate43. ammonium phosphate 93. ammonium aluminum sulfate 143. barium carbonate44. ferrous chlorite 94. iron(III) hydrogen carbonate 144. mercuric chloride45. potassium sulfide 95. mercury(I) hydrogen phosphate 145. ferrous chromate46. tin(IV) bromide 96. plumbic hydrogen carbonate 146. cupric hydroxide47. lithium chromate 97. mercuric hydrogen carbonate 147. perchloric acid48. magnesium bisulfate 98. mercurous hydrogen phosphate 148. ferric phosphate49. ferrous phosphate 99. copper(II) sulfate pentahydrate 149. lead(II) oxide50. calcium sulfate dihydrate 100. chromic dihydrogen phosphate 150. cobaltic chlorate

If a formula can be named more than one correct way, then give all. For example, Fe(HCO3)3 can be named four different ways. They are iron(III) bicarbonate, iron(III) hydrogen carbonate, ferric bicarbonate, and ferric hydrogen carbonate. The second way would be best.151. HgF2 191. KF 231. N2O5 271. NaOH 290. XeF4 328. Be(ClO4)2152. KCl 192. CaSO4 232. SnCrO4 272. NI3 291. Hg(OH)2 329. (NH4)2Cr2O7153. KMnO4 193. HCl 233. Al2O3 273. ClF3 292. CaH2 330. Ba(BrO3)2154. KClO4 194. SbCl3 234. CuCO3 274. P3N5 293. As4O6 331. AuCl3155. ZnO 195. As4O10 235. ClO2 275. UF6 294. BN 332. Al2S3156. Ba(OH)2 196. NH4Cl 236. CuS 276. NBr3 295. CoS 333. Na2HPO4157. NH4MnO4 197. NH4NO3 237. MgI2 277. Cl2O3 296. N2O4 334. Mg3(PO4)2158. CaCO3 198. IF5 238. CoCl3 278. CsF 297. H3BO3 335. CuSO3159. Ba3(PO4)2 199. NaHCO3 239. NaCN 279. CO 298. I2O5 336. KAl(C2O4)2160. Fe2O3 200. Ba(OH)2 240. Hg3N2 280. Cu2S 299. PbO 337. Cr2(SO3)3161. CoF3 201. FeCl3 241. BrO3 281. KHCO3 300. NaBr 338. HClO162. H2CO3 202. HF 242. SiF4 282. SbCl5 301. Li2CrO4 339. HClO2163. K2SO4 203. PbSO4 243. Sb2O5 283. CO2 302. ICl 340. HClO3164. NaHSO4 204. KrF2 244. LiH 284. HgO 303. SO3 341. HClO4165. PF5 205. NaCl 245. SF6 285. PCl3 304. Hg2O 342. Mn(IO3)2166. Ag2O 206. P2O5 246. SnI4 286. PBr5 305. NaH 343. KBrO3167. Pb(ClO2)2 207. AlBr3 247. KOH 287. IF7 306. OsO4 344. Fe(ClO4)3168. Cu2CrO4 208. Ba(NO3)2 248. K2O 288. Cl2O 307. XeF2 345. Cr(OH)3169. Ca(ClO4)2 209. BrF5 249. H2SO4 289. CCl4 308. Ca(C2H3O2)2170. HC2H3O2 210. P4O6 250. lithium oxide 309. NaC2H3O2171. LiI 211. FePO4 251. xenon trioxide 310. Al(OH)3172. Al2(SO4)3 212. Hg2SO4 252. gold(I) chloride 311. Li2HPO4173. HBr 213. KH 253. gold(I) cyanide 312. Ca(NO3)2174. Hg2(ClO)2 214. Co2(SO3)3 254. sodium oxide 313. Ni(ClO4)2175. CrCl3 215. N2O3 255. potassium chlorate 314. Mn(NO3)2176. H3PO4 216. N2O 256. mercurous nitrite 315. Au(H2PO4)3177. LiMnO4 217. Fe(NO2)3 257. nickel(II) fluoride 316. Al(C2H3O2)3178. Fe2(HPO4)3 218. Sn3(PO4)2 258. potassium cyanide 317. KAl(SO4)2179. Na2CO3 219. H2O2 259. manganese dioxide 318. Al(MnO4)3180. Mg(HCO3)2 220. Be(OH)2 260. osmium tetrachloride 319. (NH4)3PO4

181. Sn3(PO4)4 221. Sr(HCO3)2 261. rubidium carbonate 320. CoSO4 . 6 H2O

182. HNO3 222. Sr(OH)2 262. trisulfur dinitride 321. MgCl2 . 6 H2O

183. ZnCl2 223. P4S10 263. nitrogen trichloride 322. CuSO4 . 5 H2O184. NaH2PO4 224. Hg2O2 264. vanadium(V) oxide 323. NaHS . H2O185. Hg2Cl2 225. Hg2(OH)2 265. selenium tetrafluoride 324. MgSO4 . 9 H2O186. Fe(NO2)2 226. NH4F 266. stannous hypochlorite 325. NaH2PO4 . 9 H2O187. CuNH4PO4 227. XeF6 267. tellurium hexafluoride 326. Na2CrO4 . 4 H2O188. NaMgPO4 228. K2Cr2O7 268. lanthanum(III) phosphate 327. Pb(CH3COO)2 . 3 H2O189. Sn(HCO3)4 229. NH4OH 269. sodium hydrogen sulfate monohydrate190. NaMnO4 230. (NH4)3PO4 270. chromium(III) hydrogen phosphate

Write correct formulas of the compounds formed when the positive ions in the vertical column combine with the negative ions listed across the top row. The first two are done for you.

nitrate sulfate carbonate phosphate hydroxide chromate

sodium NaNO3 Na2SO4

silver

ammonium

mercury(I)

zinc

calcium

magnesium

copper(I)

lead(II)

aluminum

manganese(III)

cobalt(III)

cupric

ferric

plumbous

potassium

barium

hydrogencarbonate dichromate acetate sulfide chloride sulfite

sodium NaHCO3 Na2Cr2O7

silver

ammonium

mercury(II)

tin(II)

calcium

magnesium

copper(II)

lead(II)

aluminum

manganese(III)

cobalt(III)

cuprous

ferrous

plumbic

potassium

barium

Chemical Nomenclature Problem Set

Chemical Nomenclature Problem Set

This problem set was developed by S.E. Van Bramer for Chemistry 145 at Widener University.

1. Technetium (Tc) was the first synthetically produced element. Technetium (the word comes from the Greek word for artificial) was first produced by Perries and Serge in 1937 in Berkely, California, by bombarding a molybedenum plate with 2H nuclei. Elemental technetium is produced from ammonium pertechnetate. How many protons, neutrons, and electrons are in the nuclei of 98Tc and 99Tc? What is the formula of ammonium pertechnenate?

2. How many protons, neutrons, and electrons are present in each of the following atoms or ions? a. 24Mg b. 24Mg2+ c. 59Co2+ d. 59Co3+ e. 59Co f. 79Se g. 79Se2- h. 63Ni i. 59Ni2+

3. The formulas and common names for several substances are given below. Give the systematic names for thses substances.

Common Name Chemical Formula

a. Sugar of lead Pb(C2H3O2)2

b. Blue vitrol CuSO4

c. Epsom salts MgSO4

d. Milk of magnesia Mg(OH)2

e. Gypsum CaSO4

http://science.widener.edu/svb/pset/nomen_a.html (1 of 3)14/09/2006 12.33.57

Chemical Nomenclature Problem Set

f. Laughing gas N2O

4. Write the formula for each of the following compounds:

a. Sulfur difluoride b. Sulfur hexafluoride c. Sodium dihydrogen phosphate d. Lithium nitride e. Chromium (III) carbonate f. Tin (II) fluoride g. Ammonium acetate h. Ammonium hydrogen sulfate i. Cobalt (III) nitrate j. Mercury (I) chloride k. Potassium chlorate l. Sodium hydride

5. Name each of the following compounds. Where appropriate give both common and systematic names.

a. NaCl b. RbBr c. CsF d. AlI3

e. HI f. NO g. NF3

h. N2F4

i. N2Cl2

j. SiF4

k. H2Se

l. HNO3

m. HNO2

n. H3PO4

o. H3PO3

p. NaHSO4

http://science.widener.edu/svb/pset/nomen_a.html (2 of 3)14/09/2006 12.33.57

Chemical Nomenclature Problem Set

q. Ca(HSO3)2

r. Ru(NO3)3

s. V2O5

6. On the blank periodic table attached fill out as much as possible. Including:

a. Symbols for elements b. Charge for ions c. Names of groups (ie: halogens and noble gases, etc.) d. What else?

/svb/pset/nom_a_an.html

Please send comments or suggestions to svanbram@science.widener.edu

Scott Van Bramer Department of Chemistry Widener University Chester, PA 19013

© copyright 1996, S.E. Van Bramer This page has been accessed 42723 times since 1/5 /96 .

Last Updated: Saturday, May 18, 1996

http://science.widener.edu/svb/pset/nomen_a.html (3 of 3)14/09/2006 12.33.57

Nomenclature and Formula Practice Sheet Chemistry 115

Write formulas for each of the following:

barium chloride ________________________

copper (II) hydroxide ____________________

hypochlorous acid _______________________

tin (IV) oxide ___________________________

sodium acetate __________________________

lead (II) sulfate __________________________

ammonium carbonate _____________________

silver nitrate ____________________________

calcium chlorate _________________________

magnesium phosphate ____________________

hydrofluoric acid ________________________

aluminum sulfate ________________________

potassium nitrite _________________________

iron (III) sulfide _________________________

lithium sulfite ___________________________

sodium permanganate ____________________

potassium cyanide _______________________

sodium bicarbonate ______________________

mercury (II) bromide _____________________

periodic acid ____________________________

nitrogen triiodide_________________________

potassium dichromate_____________________

sulfur hexafluoride _______________________

manganese(IV) oxide _____________________

calcium iodate___________________________

Give unambiguous names for the following:

CuSO4 ________________________________

HgBr2 _________________________________

PbO2 __________________________________

HBrO__________________________________

NH4Cl _________________________________

KHSO4 ________________________________

KClO3 _________________________________

MgCO3 ________________________________

Ca(HCO3)2 _____________________________

Na2CrO4 _______________________________

Bi(OH)3 _______________________________

H2C2O4 ________________________________

LiH2PO4 _______________________________

Na2HPO4 _______________________________

KMnO4 ________________________________

CaF2 __________________________________

BaO2 __________________________________

SnCl2 _________________________________

FeO ___________________________________

LiClO4 ________________________________

NiO2 __________________________________

Hg2Cl2 _________________________________

ZnS ___________________________________

SF4 ___________________________________

Co(C2H3O2)2 ____________________________