Naming Chemical Compounds

1. Naming Chemical Compounds

2. Class I Binary Compounds • Made from “Predictable” metals on the periodic table • Metal plus non-metal • Name from formula: • Always write the metal first • Add –ide to the end of the non-metal name • Formula from name: • Write symbol for metal first • Look up charges on metal and non-metal • Balance charges to zero between metal and non-metal with ratio of atoms using subscripts

3. Class II Binary Compounds • Made from “Un-predictable” metals on the periodic table (metals that are NOT Class I) • Metal plus non-metal • Name from formula: • Always write the metal first • Determine the charge on the metal from the charge on the non-metal and the ratio of atoms. • Use roman numerals to indicate metal charge • Add –ide to the end of the non-metal name • Formula from name: • Write the symbols for metal and non-metal – metal first • Determine the charge on the metal from the roman numeral • Balance charges to zero between metal and non-metal with ratio of atoms using subscripts

4. Class III Binary Compounds • Made from non-metals and non-metals • NO CHARGES – atoms share electrons • Use prefixes to indicate number of atoms in compound • Mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-. • Name from formula: • Names use prefixes to indicate the number of atoms of an element in a compound – DO NOT use mono- for first element. • Assign prefixes from subscripts in formula. • Add –ide to the end of the second non-metal name • Formula from name: • Non-metal element further to the left written first • Prefixes indicate number of atoms . Convert prefixes in names to subscripts in formula.

5. The Common Polyatomicsthe -ates • Phosphate PO43-Please -3 • Sulfate SO42- Send -2 • Carbonate CO32- Cake and -2 • Chlorate ClO31-Chocolate -1 • Acetate C2H3O2-1Angels -1 • Nitrate NO31- Now -1 Knowing these plus the rules covers 12 of the poly-atomics!

6. Polyatomic Naming Rules • Learn (memorize) Common Ions – Then: • Per- is one more oxygen • -ite = one less oxygen, same charge except for phosphorus • Hypo- -ite = two less oxygens same charge except for phosphorus

7. Phosphate • Phosphate PO43- • Phosphite PO32- • Hypophosphite PO2-1 One less oxygen – one less charge Two less oxygen – two less charge

8. Sulfate • Sulfate SO42- • Sulfite SO32- One less oxygen – same charge

9. Carbonate • Carbonate CO32- • Hydrogen Carbonate HCO32- (Bicarbonate)

10. Chlorate • Chlorate ClO3-1 • Chlorite ClO2-1 • Hypochlorite ClO-1 One and two less oxygens – same charge • Perchlorate ClO4-1 One more oxygen

11. Nitrate • Nitrate NO3-1 • Nitrite NO2-1 One less oxygen – same charge

12. Common Negative Charge Poly- atomic ions • Acetate C2H3O2-1 • Cyanide CN-1 • Hydroxide OH-1 • Permanganate MnO4-1 • Chromate CrO4-2 • Dichromate Cr2O7-2 Note All = -1

13. The Positively Charged Polyatomics • Ammonium NH4+1 • Hydronium H30+1 (aka H+)

14. Sulfite SO32-

15. Hydrogen Carbonate HCO31-

16. Phosphate PO43-

17. Nitrate NO31-

18. Perchlorate ClO4-1

19. Nitrite NO21-

20. Chlorite ClO21-

21. Naming Acids • Hydrogen can act like a metal = H+1 • Hydrogen as the first element in a compound indicates an acid. • Binary acids are named by adding hydro- to the beginning and –ic to the end • HCl = Hydro chlor ic Acid • Polyatomic acids are named by taking the common name ending in –ate and changing to –ic • H2SO4 = from sulfate/SO4-2 = sulfuric acid • Polyatomic compounds with one less oxygen are named by substituting –ous for –ite • HNO2 = from nitrite/NO2-1 = nitrous acid

22. Naming Bases • Bases contain the polyatomic anion hydroxide – OH-1

23. Common Ions plus Hydrogen • Dihydrogen Phosphate H2PO4-1 • Hydrogen Phosphate HPO4-2 • Hydrogen Sulfate HSO4-1 • Bisulfate • Hydrogen Carbonate HCO3-1 • Bicarbonate