1. 1 NOMENCLATURE NAMES AND FORMULAS OF CHEMICAL COMPOUNDS

2. 2 TYPES OF COMPOUNDS

3. 3 RECOGNIZING BONDS COVALENT BONDS BETWEEN TWO NONMETALS IONIC BONDS BETWEEN ONE METAL AND ONE NONMETAL REMINDER THAT METALS ARE LEFT OF STAIRSTEPS AND NONMETALS ARE RIGHT

4. 4 RECOGNIZING BOND EXAMPLES WHAT KIND OF BOND IS BETWEEN: –K AND Cl –S AND P –Ba AND O –Pb AND N

5. 5 BONDS AND COMPOUND TYPES COMPOUNDS FORMED FROM –IONICALLY BONDED ELEMENTS ARE CALLED IONIC COMPOUNDS –COVALENTLY BONDED ELEMENTS ARE CALLED MOLECULAR COMPOUNDS

6. 6 NAMES OF BINARY MOLECULAR COMPOUNDS PREFIXES INDICATE THE NUMBER OF ATOMS IN A COMPOUND DON’T USE PREFIX FOR FIRST ELEMENT IF THERE IS ONE ATOM SECOND ELEMENT ENDS IN “IDE”

7. 7 PREFIXES FOR MOLECULAR COMPOUNDS MONO DI TRI TETRA PENTA HEXA HEPTA OCTA NONA DECA

8. 8 EXAMPLE MOLECULAR NAMES CO 2 CARBON DIOXIDE CO CARBON MONOXIDE N 2 O 5 DINITROGEN PENTOXIDE As 3 N 6 TRIARSENIC HEXANITRIDE

9. 9 2ND ELEMENT SPELLING NITRIDEOXIDEFLUORIDE PHOSPHIDESULFIDECHLORIDE ARSENIDESELENIDEBROMIDE TELLURIDEIODIDE ASTATIDE

10. 10 MOLECULAR COMPOUND FORMULAS CHANGE PREFIX TO SUBSCRIPT DON’T WRITE A “1” SUBSCRIPT

11. 11 EXAMPLE MOLCULAR FORMULAS ARSENIC TRIFLUORIDE AsF 3 CARBON TETRAFLUORIDE CF 4 DIPHOSPHORUS HEXABROMIDE P 2 Br 6

12. 12 MOLECULES ATOMS OF TWO (OR MORE) DIFFERENT ELEMENTS COVALENTLY BONDED SIMPLEST UNIT OF COVALENTLY BONDED ATOMS

13. 13 MOLECULE EXAMPLES ARE THE FOLLOWING MOLECULES? –BaS –N2O–N2O –Br 2 –S8–S8

14. 14 IONS CATION - ATOM THAT HAS LOST 1 OR MORE ELECTRONS IS IS POSITIVE ANION - ATOM THAT HAS GAINED 1 OR MORE ELECTRONS AND IS NEGATIVE

15. 15 VALENCE NUMBER CHARGE ON AN ION AFTER IT HAS GAINED OR LOST ELECTRONS ALSO CALLED OXIDATION STATE SHOWN ON PERIODIC TABLE

16. 16 VALENCE NUMBERS

17. 17 MULTI-VALENCE METALS METALS IN SUNKEN SECTION OF PERIODIC TABLE CAN HAVE MORE THAN ONE CHARGE OR VALENCE NUMBER MUST LOOK THEM UP ON PT

18. 18 FORMULA UNIT SIMPLEST UNIT OF IONICALLY BONDED ATOMS LOWEST POSSIBLE SUBSCRIPTS MUST BE USED FOR IONIC COMPOUNDS TO HAVE CORRECT FORMULA UNIT

19. 19 IONIC COMPOUNDS FORMED FROM A CATION AND AN ANION TOTAL POSITIVE CHARGE = TOTAL NEGATIVE CHARGE

20. 20 FORMULAS OF BINARY IONIC COMPOUNDS CATIONS ARE ALWAYS WRITTEN 1 ST Na +1 Cl -1 Na 1 Cl 1 DON’T WRITE 1’S NaCl

21. 21 CRISSCROSS RULE CROSS VALENCE NUMBERS (IGNORE SIGNS) REDUCE TO LOWEST VALUES INSURES FORMULA UNITS ARE NEUTRAL (CHARGES CANCEL)

22. 22 EXAMPLES OF BINARY IONIC COMPOUNDS Mg Cl MgCl 2 Ca O Ca 2 O 2 WHICH REDUCES TO CaO Sn +4 S SnS 2

23. 23 NAMES OF BINARY IONIC COMPOUNDS WRITE NAME OF CATION FOLLOW WITH NAME OF THE ANION BUT CHANGE ENDING TO “IDE” NUMBER OF ATOMS DOES NOT AFFECT NAME OF AN IONIC COMPOUND! NO PREFIXES! SAME SPELLING AS MOLECULAR COMPOUNDS

24. 24 EXAMPLES OF NAMES NaCl SODIUM CHLORIDE MgCl 2 MAGNESIUM CHLORIDE CaO CALCIUM OXIDE

25. 25 NAMES OF IONIC CMPDS WITH MULTI-VALENCE CATIONS VALENCE NUMBER OF CATION BECOMES ROMAN NUMERAL WRITTEN IN PARENTHESES AFTER CATION NAME CALLED THE STOCK SYSTEM

26. 26 NAMES W/ MULTI- VALENCE II REVERSE THE CRISS CROSS TO FIGURE OUT THE CATION VALENCE USE ANION TO DETERMINE IF REDUCING OCCURRED, IF SO UNREDUCE

27. 27 EXAMPLES OF STOCK SYSTEM NAMES Fe 2 O 3 IRON (III) OXIDE SnS TIN (IV) SULFIDE MnP 2 MANGANESE (VI) PHOSPHIDE

28. 28 POLYATOMIC IONS 2 OR MORE ATOMS COVALENTLY BONDED THAT ACT LIKE A SINGLE ION FORM IONIC BONDS USUALLY ANIONS

29. 29 EXAMPLE POLYATOMIC IONS NO 3 -1 IS NITRATE SO 4 -2 IS SULFATE CO 3 -2 IS CARBONATE PO 4 -3 IS PHOSPHATE SEE HANDOUT CHART FOR OTHERS

30. 30 FORMULAS FOR TERNARY IONIC COMPOUNDS USE PARENTHESES AROUND POLYATOMIC ION USE CRISS-CROSS RULE REDUCE OUTSIDE PARENTHESES – NOT INSIDE REMOVE PARENTHESES ONLY IF SUBSCRIPT OUTSIDE IS 1

31. 31 FORMULA EXAMPLES Na (NO 3 ) Na 1 (NO 3 ) 1 WHICH REDUCES TO NaNO 3 Ca (IO 3 ) Ca(IO 3 ) 2 Al (SO 4 ) Al 2 (SO 4 ) 3

32. 32 NAMES OF MOST TERNARY IONIC COMPOUNDS WRITE NAME OF CATION FOLLOW WITH NAME OF ANION (NO CHANGES TO POLYATOMIC NAME) NUMBER OF EACH DOES NOT AFFECT THE NAME NO PREFIXES!

33. 33 EXAMPLE OF NAMES NaNO 3 SODIUM NITRATE Na 2 SO 4 SODIUM SULFATE Ca(IO 3 ) 2 CALCIUM IODATE

34. 34 NAMES OF IONIC CMPDS W/ AMMONIUM CATION WRITE AMMONIUM FOLLOW WITH ANION IF ANION IS AN ELEMENT, CHANGE ENDING TO “IDE” IF ANION IS POLYATOMIC, MAKE NO CHANGES

35. 35 AMMONIUM EXAMPLES NH 4 OH AMMONIUM HYDROXIDE (NH 4 ) 2 CrO 4 AMMONIUM CHROMATE (NH 4 ) 3 N AMMONIUM NITRIDE

36. 36 MORE POLYATOMIC NAMING EXAMPLES Cu(HCO 3 ) 2 COPPER (II) BICARBONATE FeSO 3 IRON (II) SULFITE CrC 2 O 4 CHROMIUM (II) OXALATE

37. 37 AQUEOUS SOLUTIONS SOLUTION IN WHICH WATER IS THE SOLVENT IS CALLED AQUEOUS A SUBSCRIPT OF (aq) INDICATES AN AQUEOUS SOLUTION

38. 38 DISSOCIATION THE SEPARATION OF AN IONIC COMPOUND INTO IONS BY WATER (AS IT DISSOLVES)

39. 39 IONIC ACIDS CONTAIN HYDROGEN AS A CATION RELEASE HYDROGEN IONS AS THEY DISSOCIATE

40. 40 BINARY IONIC ACIDS NAMES BEGIN WITH HYDRO- AND END WITH –IC FORMULAS: CRISSCROSS VALENCE NUMBERS SUBSCRIPTS AND ADD (aq) AFTER ANION SUBSCRIPT

41. 41 EXAMPLE BINARY ACID NAMES HCl (aq) HYDROCHLORIC ACID HF (aq) HYDROFLUORIC ACID HI (aq) HYDROIODIC ACID

42. 42 EXAMPLE BINARY ACID FORMULAS HYDROSULFURIC ACID H 2 S (aq) HYDROBROMIC ACID HBr (aq)

43. 43 TERNARY IONIC ACID NAMES CONTAIN HYDROGEN AND A POLYATOMIC ANION NAMES DO NOT BEGIN WITH HYDRO- NAMES END IN –IC IF ANION ENDS IN –ATE OR –IDE NAMES END IN –OUS IF ANION ENDS IN –ITE

44. 44 EXAMPLE TERNARY ACID NAMES HNO 3 (aq) NITRIC ACID H 2 SO 4 (aq) SULFURIC ACID HNO 2 (aq) NITROUS ACID

45. 45 TERNARY ACID FORMULAS HYDROGEN MUST BE THE CATION DETERMINE ANION FROM ACID NAME FOLLOW RULES FOR IONIC COMPOUNDS WITH POLYATOMIC IONS ADD (aq) AFTER ANION SUBSCRIPT

46. 46 EXAMPLE TERNARY ACID FORMULAS CHROMIC ACID H 2 CrO 4(aq) SULFUROUS ACID H 2 SO 3(aq) PHOSPHORIC ACID H 3 PO 4(aq)