CHEMICAL NOMENCLATURE 1. FORMING BINARY COMPOUNDS (mono-valent elements only) a) Binary Compounds - composed of only two different elements. • • b) 2. Metallic element is always first. Non-metallic element is then placed second. Cross-Valence Rule Mm+ Nn- ÿ MnNm NAMING BINARY COMPOUNDS (mono-valent elements only) • Name the metallic element by its ‘elemental’ name. • Use the ending ‘-ide” on the non-metallic element’s name. Examples: FORMING BINARY COMPOUNDS NAMING BINARY COMPOUNDS Element Valence Compound Metal Non-Metallide Na +1 NaCl sodium chloride Cl -1 Ca +2 CaBr2 calcium bromide Br -1 Al +3 Al2O3 aluminum oxide O -2 Mg +2 (Mg2S2) magnesium sulfide reduce to lowest terms S -2 MgS Monovalent metals include: groups 1, 2, 13, and transition metal ions Ag+ and Zn2+ MEMORIZE THESE ELEMENTS WITH THEIR VALENCES Practice NAME FORMULA Na2O __________________________ KF __________________________ silver oxide _________________________ calcium chloride _____________________ AgCl __________________________ aluminum sulfide _____________________ BaO __________________________ Znl2 __________________________ sodium bromide ______________________ cadmium oxide ______________________ Al2S3 __________________________ Ca3N2 __________________________ CdBr2 __________________________ MgCl2 __________________________ Cs2S __________________________ Ag3P __________________________ beryllium fluoride _____________________ potassium oxide ______________________ silver iodide _________________________ barium fluoride _______________________ magnesium hydride ___________________ zinc sulfide __________________________ 3. NAMING BINARY COMPOUNDS (Multi-valent elements) Multi-valent elements: Bismuth Bi 3+ 5+ Iron Fe 2+ 3+ Antimony Sb 3+ 5+ Nickel Ni 2+ 3+ Mercury Hg 1+ 2+ Chromium Cr 2+ 3+ Copper Cu 1+ 2+ Cobalt Co 2+ 3+ Lead Pb 2+ 4+ Gold Au 1+ 3+ Tin Sn 2+ 4+ Manganese Mn 2+ 4+ MEMORIZE THESE ELEMENTS WITH THEIR VALENCES Naming Methods for Compounds with Multivalent Elements • Roman Numeral Method A Roman numeral, in parenthesis, immediately following the name of the multi-valent element, indicates the valence of that element in the compound. nickel(lll) oxide Ni 3+ O 2- Ni2O 3 NiO Ni 2+ O 2- nickel(II) oxide Sn 4+ S 2- tin(IV) sulfide (Sn2S4) SnS2 Sn 2+ Cl - SnCl2 tin(ll) chloride • “-ous” and “-ic” Method “-ous” ending indicates the element is in a lower valence form. “-ic” ending indicates the element is in a higher valence form. stannic sulfide Sn 4+ S 2- stannous sulfide Sn 2+ S 2- Note ferrous ferric (Sn2S4) SnS2 SnS MEMORIZE THESE NAMES AND CHARGES (Fe2+) (Fe3+) stannous (Sn2+) stannic (Sn4+) mercurous (Hg+) mercuric (Hg2+) aurous auric • Prefix Method Prefixes: (Au+) (Au3+) plumbous plumbic (Pb2+) (Pb4+) cuprous cupric (Cu+) (Cu2+) stibnous stibnic (Sb3+) (Sb5+) manganous (Mn2+) manganic (Mn4+) Use for molecular compounds only. 1, mono-; 2, di-; 3, tri-; 4, tetra-; 5, penta-; 6, hexa-; 7, hepta-; 8, octa-; 9, nono-; 10, deca-; A prefix, preceding each atom of a compound indicates the number of atoms of THAT element in the compound. phosphorus trioxide phosphorus pentoxide P3+ O 2P5+ O 2- P2 O 3 P2 O 5 No need to use mono for the first element (lower electronegativity). • CO is carbon monoxide • SO3 is sulfur trioxide Exercise Naming Binary Compounds (Multi-valent elements) Write the formula for each. Formula Formula _________________ gold(III) iodide _________________ stannous bromide _________________ stannic sulfide _________________ tin(II) chloride _________________ stibnous oxide _________________ iron(III) bromide _________________ stibnic chloride _________________ ferric iodide _________________ mercury(II) oxide _________________ nitrogen dioxide _________________ mercurous fluoride _________________ carbon disulfide _________________ lead(IV) oxide _________________ dinitrogen pentoxide _________________ plumbic nitride _________________ carbon tetrachloride Name the following molecular compounds N2O5 ____________________________________________ NO _____________________________________________ PF5 _____________________________________________ IF7 _____________________________________________ SO2 _____________________________________________ SO3 _____________________________________________ CO _____________________________________________ CO2 _____________________________________________ SF6 _____________________________________________ SiF4 _____________________________________________ BCl3 _____________________________________________ ClO2 _____________________________________________ P2 S 5 ___________________________________________ Exercise Naming Binary Compounds (Multi-valent elements) Name the compounds using the Stock method and the “ous”/ “ic” system where possible. Formula Stock method Cu2S CuS HgBr HgBr2 Fe2O3 FeO SnF2 SnF4 MnO2 MnO AuCl Sb2P5 CrP AuBr3 CoO Co2O3 NiO Ni2O3 NiP CuF2 SnO2 Hg2S PbCl2 PbCl4 Sb2S5 Sb2S3 Asl3 4. ACID FORMING BINARY COMPOUNDS “-ous”/ “-ic” system Note the name change of these gases when they are dissolved in water (aqueous solution). Acids are molecular compounds that release hydrogen ions when they are dissolved in water in a process called ionization. Br -(aq) the ionization of hydrogen bromide NAME OF THE GAS FORMULA NAME OF THE ACID IN AQUEOUS SOLUTION hydrogen fluoride HF(g) hydrofluoric acid HF(aq) hydrogen chloride HCl(g) hydrochloric acid HCl(aq) hydrogen bromide HBr(g) hydrobromic acid HBr(aq) hydrogen iodide HI(g) hydriodic acid HI(aq) hydrogen sulfide H2S(g) hydrosulfuric acid H2S(aq) e.g. 5. HBr (g) º H + (aq) + FORMULA THE OXYACIDS “ic” ACID NAME FORMULA OXYANION FORMULA NAME chloric acid HClO3 ClO3 - chlorate nitric acid HNO3 NO3 - nitrate carbonic acid H2CO3 CO3 2- carbonate sulfuric acid H2SO4 SO4 2- sulfate phosphoric acid H3PO4 PO4 3- phosphate e.g. H2SO4 (l) º 2H + (aq) + SO4 2- (aq) the ionization of sulfuric acid A oxyanion is a group of atoms that acts as a unit. The charge of this ion need not be memorized because it is equal to the NUMBER OF HYDROGEN ATOMS with which it was combined in the acid. NOTE: The elements fluorine, chlorine, bromine and iodine behave in a similar manner. We can then easily add the following oxy-acids. “ic” ACID NAME FORMULA OXYANION FORMULA NAME fluoric acid HFO3 FO3 - fluorate bromic acid HBrO3 BrO3 - bromate iodic acid HIO3 IO3 - iodate MEMORIZE ALL OF THE “ic” OXYACIDS 6. NAMING OF OXYACID SALTS (mono- and multi-valent metals and an oxyanion) sodium sulfate Na+ SO4 2- Na2SO4 Ba3(PO4)2 Ba 2+ PO4 3- barium phosphate copper(II) carbonate Cu 2+ CO3 2- Cu2(CO3)2 Sn(NO3)2 Sn 2+ NO3 - tin(II) nitrate Exercise: Na2SO4 CuCO3 Name the compounds using the stock system if necessary, provide the formula for the compound. FORMULA NAME NAME AI(NO3)3 mercuric nitrate CaCO3 manganese(IV) chlorate Cu(ClO3)2 magnesium sulfate Sb2(SO4)5 lead(II) phosphate FePO4 potassium carbonate 7. FORMULA DERIVATIVES OF THE OXY-ACIDS All of these acids have different combinations with oxygen. For example: perchloric acid HCIO4 chloric acid HCIO3 chlorous acid HCIO2 hypochlorous acid HCIO The prefix and suffix indicate the number of oxygen atoms in the formula relative to “ic” acid. • NAMING OF DERIVATIVE RADICALS Acid Prefix and Suffix per Oxyanion Prefix and Suffix ____ - ic per ____ - ate ____ - ic ____ - ate ____ - ous ____ - ite hypo ____ - ous hypo ____ - ite Examples H2SO4 is sulfuric acid, H2SO5 is persulfuric acid, H2SO3 is sulfurous acid H2SO2 is hyposulfurous acid SO4 2- is sulfate SO5 2- is persulfate SO3 2- is sulfite SO2 2- is hyposulfite NOTE: the number of H atoms does not change in the compounds in these series. Exercise: Complete the following table. PARENT “ic” ACID ACID FORMULA sulfurous H2SO3 FORMULA of OXYANION NAME of OXYANION sulfite NO4 - HNO4 H3PO5 perphosphate hypobromous CO2 2nitrite HIO2 phosphorous CIO hyposulfite • NAMING OF OXY-ACID DERIVATIVE SALTS potassium perbromate K + BrO4 - KBrO4 Ca3(PO2)2 Ca 2+ PO2 3- calcium hypophosphite ferric sulfite Fe 3+ SO3 2- Fe2(SO3)3 Pb(CO3)2 Pb 4+ CO32- lead(IV) carbonate antimony(III) hypochlorite Sb3+ ClO - Sb(ClO)3 Exercise7 Naming Oxy-Acid Derivative Salts (with mono-valent elements) NAME FORMULA KlO2 magnesium hypocarbonite Al(NO3)3 barium persulfate Si(ClO4)4 silver perchlorate Zn3(PO3)2 calcium hypoiodite Na2CO potassium nitrite MgSO3 aluminum phosphate Ba(NO4)2 silicon percarbonate Exercise Naming Oxy-Acid Derivative Salts (with multi-valent elements) NAME FORMULA Cu(ClO3)2 stibnic carbonate Pb3(PO3)2 manganese(II) iodite Sb2(SO3)5 mercury dinitrite Hg(ClO)2 ferric persulfate Fe(BrO3)3 lead(IV) sulfite Mn(lO4)2 cuprous hyponitrite Sn3(PO5)4 arsenic(III) bromite PbCO4 iron(II) hypocarbonite Sb(NO3)3 stannous sulfite HgSO2 copper(II) perchlorate CulO manganic nitrate 8. OXYACID, ACID SALTS A bibasic acid (one that contains 2 H atoms), like H2SO4 or H2CO3 , or a tribasic acid (one that contains 3 H atoms) like H3PO4 may form an anion by losing one or more hydrogen ions (H+). H2SO4 º e.g. H+ + HSO4 - ACID NORMAL OXYANION ACID ANION NAME H2SO4 SO4 2- HSO4 - hydrogen sulfate H2CO3 CO3 2- HCO3 - hydrogen carbonate H3PO4 PO4 3- H2PO4 - dihydrogen phosphate H3PO4 PO4 3- HPO4 2- monohydrogen phosphate note: All of the derivatives of these oxyacids of C, S, P can form acid anions e.g., H3PO5 can form HPO5 2- and HPO5 • NAMING ACID SALTS The most important of these is sodium hydrogen carbonate, (sometimes called sodium bicarbonate or baking soda). NaHCO3 Na + Ca(H2PO4)2 Ca2+ H2PO4 - calcium dihydrogen phosphate Fe2(HPO3)3 Fe3+ HPO3 2- iron(III) monohydrogen phosphite lead(II) hydrogen sulfite Pb(HSO3)2 Pb 2+ HSO3 - sodium hydrogen carbonate HCO3 - other examples Exercise: Zn(HSO3)2 iron(II) hydrogen carbonite Mg(H2PO3)2 arsenic(V) hydrogen sulfate Ni(HCO2)2 stannous monohydrogen phoshphite HgHPO5 barium dihydrogen phosphate Mn(HSO5)4 auric hydrogen carbonite THE DIATOMIC ELEMENTS H O F Br I N Cl These elements exist as molecules of two atoms covalently bonded. hydrogen H2 iodine I2 fluorine F2 chlorine Cl2 bromine Br2 nitrogen N2 oxygen O2 Memorize these elements. 9. HYDRATES: Many ionic compounds form crystal structures which include a definite, chemically combined, number of water molecules. These water molecules are referred to as WATERS OF HYDRATION. Name these compounds as usual and include a prefix + hydrate. copper (II) sulfate pentahydrate CuSO4•5H2O BaCl2•2H2O barium chloride dihydrate sodium carbonate decahydrate Na2CO3•10H2O 10. SOME SPECIAL POLYATOMIC IONS: H+ H3O + OH NH4 + C2H3O2 MnO4 - hydrogen ion hydronium ion hydoxide ion ammonium ion acetate ion permanganate ion 11. SOME EXCEPTIONS: • peroxides H2O2 Na2O2 Compounds which have one more oxygen atom than the expected number. hydrogen peroxide sodium peroxide note: do not cancel to HO or NaO • water H2O, • organic compounds ammonia NH3, methane CH4 Memorize these These compounds will be introduced at a later date. Provide the correct formula and state where indicated. Nam e Chem ical Form ula Nam e alum inum carbonate m ercury(I) nitrite arsenic(V) peiodate copper(I) sulfide calcium dihydrogen phosphite ferric persulfate Chem ical Form ula m anganic iodate m ercuric brom ide hydrogen sulfide zinc nitrite water acetate ion potassium peroxide plum bous oxide hydronium ion iodine am m onium chloride barium sulfide antim ony(V) hydrogen sulfite silver hydrogen carbonate nitrogen cobalt(II) perm anganate hydroiodic acid arsenic(II) fluoride barium hydroxide potassium iodite calcium chloride stannous dihydrogen hypophosphite am m onia calcium hydride Provide the proper IUPAC nam e for each of the following com pounds. Use the Stock m ethod where necessary. Chem ical Form ula Nam e Chem ical Form ula SnO 2 H 2O 2 P 2S 5 FePO 3 F2 As 2(SO 5) 3 Hg 3N Al(H 2PO 4) 3 Ca(OH) 2 AgC 2H 3O 2 Na 2SO 4•7H 2O Cl2O Mn(BrO 4) 2 H 2S (g) HCl Hg(NO 3) 2 (aq) Sn(IO 2) 4 SF 6 K 2HPO 5 KMnO 4 Ca(HCO 2) 2 NH 4IO 3 H 2CO 2 BaCl2•2H 2O Nam e
