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Home , Chemical nomenclature, Sodium selenide

Rules of Nomenclature for Binary Compounds

There are three types of binary compounds: Type I. A of fixed charge and a ; Type II. A metal of variable charge and a nonmetal; and Type III. Two of ‘variable charge’ tend to be transition elements with some exceptions; metals of fixed charge tend to be the alkali metals and the alkaline earths, along with zinc, cadmium and silver. Nonmetals are those compounds to the right of the bold zig-zag line (see attached) The rules for naming binary compounds are then as follows: • Rule 1. When writing a formula or naming a compound: a). For Type I and Type II compounds, first list the metal then the nonmetal; b) For Type III compounds always list the electropositive species first (the element furthest left in the periodic table) and then the electronegative species. Type III species tend to be exclusively covalently bound compounds. NOTE: It becomes very important that you KNOW YOUR AND THEIR CHARGES (especially the anions, since any given element anion does not have varying charges)!!!

• Rule 2. All compound must be neutral UNLESS indicated otherwise. • Rule 3. When naming binary compounds: a). For compounds of Type I and Type II, always use the FULL name of the metal and add the suffix -ide to the root name of the nonmetal (i.e. Metal Nonmetide); b). Type II compounds are handled the same as Type I except the charge on the metal is indicated by using a roman numeral in parentheses immediately following the metal (i.e. copper(I) ); c). Compounds of Type III use a prefix to indicate the number of atoms present; HOWEVER the prefix mono- is never used to name the first element!

To illustrate 3a, take for example Na2Se. This is a Type I compound. The metal is (we use its full name) and the nonmetal comes from ; the root of this is selen-; we add -ide to this and we get , so this compound is . For you own information, here is some other generally useful information: Roman Numerals I = 1; II = 2; III = 3; IV = 4; V = 5; VI = 6; VII = 7. Prefixes: mono = 1; di = 2; tri = 3; tetra = 4; penta = 5; hexa = 6; hepta = 7; octa = 8. Greek letters: = alpha; = beta; or = delta; = gamma = epsilon; = sigma; = pi; = nu Periodic Table of the Elements 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 IA VIIIA 1 2 H He 1.008 IIA IIIA IVA VA VIA VIIA 4.002 3 4 5 6 7 8 9 10 Li Be B C N O F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 13 14 15 16 17 18 Na Mg Al Si P S Cl Ar 22.99 24.30 IIIB IVB VB VIB VIIB VIII VIII VIII IB IIB 26.98 28.09 30.97 32.06 35.45 39.95 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.90 50.94 52.00 54.94 55.85 58.93 58.70 63.55 65.38 69.72 72.59 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 (99) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.9 137.3 138.9 178.5 180.9 183.9 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) (222) 87 88 89 104 105 106 107 108 109 110 Fr Ra Ac Rf Db Sg Bh Hs Mt ?? (223) 226.0 227.0 (261) (262) (263) (262) (265) (266) (269)

58 59 60 61 62 63 64 65 66 67 68 69 70 71 series Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 140.1 140.9 144.2 (147) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 series 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (260)

TYPE TYPE TYPE I II III Common Cationsc Ionic Charge +1 Ionic Charge +2 Ionic Charge +3 Alkali Metals ( 1A) Alkaline Earths (Group 2A) Group 3A

Li+ Lithium Be+2 Beryllium Al+3 Aluminum Na+ Sodium Mg+2 Magnesium Ga+3 Gallium K+ Potassium Ca+2 Calcium Transition Elements Rb+ Rubidium Sr+2 Strontium + +2 Cs Cesium Ba Barium Cr-+3 Chromium(III) +3 Transition Elements Transition Elements Mn Manganese(III) Fe+3 (III) Cu+ Copper(I) Cr+2 Chromium(II) Co+3 Cobalt(III) Ag+ Silver Mn+2 Manganese(II) Fe+2 Iron(II) Polyatomic Ions Co+2 Cobalt(II) +2 + Ni Nickel NH4 Cu+2 Copper(II) Others Zn+2 Zinc Cd+2 Cadmium H+ +2 Hg2 Mercury(I)b + a H3O Hg+2 Mercury(II)

Others

Sn+2 Tin(II) Pb+2 (II) a: this is the species that actually exists when H+ is present in ; b: mercury(I) ions always occur bound toegether to form Hg2+2 ions; c: Not included in the table are two common +4 ions: Pb+4 = Lead(IV) and Sn+4 = Tin(IV) Common Anions

Ionic Charge -1 Ionic Charge -2 Ionic Charge -3

Halogens (Group 7A) Oxyanions Group 6A Group 5A

- - -2 -3 F ClO4 O Oxide N Nitride - - -2 -3 Cl Chloride ClO3 S P Phosphide - - Br ClO2 - Oxyanions Oxyanion I Iodide ClO- BrO - Bromate -2 -3 Anions 3 CO3 PO4 - -2 BrO2 Bromite SO4 - a - -2 HCO3 Hydrogen carbonate BrO SO3 Sulfite - IO - -2 HS 4 C2O4 - IO - Iodate -2 HSO4 Hydrogen sulfate 3 CrO4 Chromate - NO - -2 HSO3 Hydrogen sulfite 3 Cr2O7 Dichromate - - H2PO4 NO2 OH- Acid Anion Other Anions - C2H3O2 -2 - HPO4 Hydrogen Phosphate SCN- MnO4 CN- Diatomic Elemental - H -2 O2 Peroxide a: Commonly referred to as Practice

A. Give the names or formulas of the following compounds:

2 Lead(II) nitrate 1 NaCl

3 BaCrO4 4 Ammonium hydroxide

5 ZnSO4 6 Cobalt(II) oxide

7 Al2O3 8 Copper(II) sulfate

9 NH4NO2 10 Iron(III) chloride

11 Zn3(PO4)2 12 Copper(I) sulfide

13 CaS 14 Cadmium hypochlorite

15 CO2 16

17 H2O2 18 Nickel(II) phosphate

19 Ni(MnO4)2 20 Sodium oxalate

21 Co3(AsO4)2 22 Zinc nitrite

23 KCN 24

25 H2SO3 26 Sodium

27 SnS2 28

29 HgC2O4 30 Bismuth(III) arsenate

31 Pb(HCO3)2 32 Cobalt(II) chloride