The document provides information on naming and writing formulas for various types of chemical compounds including: 1. Ionic compounds formed from cations and anions are named by writing the metal first followed by the nonmetal with the appropriate ending (e.g. NaCl is sodium chloride). 2. Molecular compounds formed from nonmetals use prefixes to indicate the number of atoms and the second element takes the "-ide" ending (e.g. CO2 is carbon dioxide). 3. Acids are named by identifying if they contain one or two elements and whether they contain oxygen, and using appropriate endings like "-ic", "-ous", or specifying the anion (e.g. HCl is hydrochlor

1. Nomenclature PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion HC 2 H 3 O 2 Acetic Acid Chemistry 1: Chapter 9 Chemistry 1 Honors: Chapter 4 ICP: Chapter 20 SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

2. Common Names A lot of chemicals have common names as well as the proper IUPAC name. Chemicals that should always be named by common name and never named by the IUPAC method are: H 2 O water, not dihydrogen monoxide NH 3 ammonia, not nitrogen trihydride

3. COMPOUNDS FORMED FROM IONS Na + + Cl - --> NaCl CATION + ANION ---> COMPOUND A neutral compound requires equal number of + and - charges.

4. Charges on Monatomic Ions +1 +2 -3 -2 -1 0 Cd +2

5. IONIC COMPOUNDS ammonium chloride, NH 4 Cl NH 4 + Cl -

6. Some Ionic Compounds Mg 2+ + N -3 ----> Mg 3 N 2 magnesium nitride Sn 4+ + O 2- ----> SnO 2 Tin (IV) oxide calcium fluoride Ca 2+ + 2 F - ---> CaF 2

7. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions     – Na  +  F :  Na + : F :  NaF     sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

8. Monatomic Ions

9. Writing a Formula Write the formula for the ionic compound that will form between Ba 2+ and Cl  . Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba 2+ Cl  Cl  3. Write the number of ions needed as subscripts BaCl 2

10. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na + , S 2- a) NaS b) Na 2 S c) NaS 2 2. Al 3+ , Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+ , N 3- a) MgN b) Mg 2 N 3 c) Mg 3 N 2

11. Solution 1. Na + , S 2- b) Na 2 S 2. Al 3+ , Cl - a) AlCl 3 3. Mg 2+ , N 3- c) Mg 3 N 2

12. Naming Compounds 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl  = chlor ide CaCl 2 = calcium chlor ide Binary Ionic Compounds:

13. Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

14. Learning Check Complete the names of the following binary compounds: Na 3 N sodium ________________ KBr potassium ________________ Al 2 O 3 aluminum ________________ MgS _________________________

15. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu + , Cu 2+ Fe 2+ , Fe 3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

16. Names of Variable Ions These elements REQUIRE Roman Numerals because they can have more than one possible charge: Transition metals and the metals in groups 4A and 5A (except Ag, Zn, Cd, and Al) require a Roman Numeral. FeCl 3 (Fe 3+ ) iron (III) chloride CuCl (Cu + ) copper (I) chloride SnF 4 (Sn 4+ ) tin (IV) fluoride PbCl 2 (Pb 2+ ) lead (II) chloride Fe 2 S 3 (Fe 3+ ) iron (III) sulfide

17. Examples of Older Names of Cations formed from Transition Metals

18. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr 2 iron (_____) bromide CuCl copper (_____) chloride SnO 2 ___(_____ ) ______________ Fe 2 O 3 ________________________ Hg 2 S ________________________

19. CO 3 -2 is carbonate HCO 3 – is hydrogen carbonate H 2 PO 4 – is dihydrogen phosphate HSO 4 – is hydrogen sulfate Polyatomic Ions

20. Ternary Ionic Nomenclature Writing Formulas Write each ion, cation first. Don’t show charges in the final formula. Overall charge must equal zero . If charges cancel, just write symbols. If not, use subscripts to balance charges. Use parentheses to show more than one of a particular polyatomic ion . Use Roman numerals indicate the ion’s charge when needed (stock system)

21. Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4 -2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4 + and CO 3 –2 (NH 4 ) 2 CO 3

22. Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(II) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOH b) Fe 3 OH c) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

23. Naming Ternary Compounds Contains at least 3 elements There MUST be at least one polyatomic ion Examples: Na NO 3 Sodium nitrate K 2 SO 4 Potassium sulfate Al (HCO 3 ) 3 Aluminum bicarbonate or Aluminum hydrogen carbonate

24. Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2 . Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

25. Mixed Practice! Name the following: Na 2 O CaCO 3 PbS 2 Sn 3 N 2 Cu 3 PO 4 HgF 2

26. Mixed Up… The Other Way Write the formula: Copper (II) chlorate Calcium nitride Aluminum carbonate Potassium bromide Barium fluoride Cesium hydroxide

27. Naming Molecular Compounds CH 4 methane BCl 3 boron trichloride CO 2 Carbon dioxide All are formed from two or more nonmetals. Ionic compounds generally involve a metal and nonmetal (NaCl)

28. Molecular (Covalent) Nomenclature for two non metals Prefix System (binary compounds) 1. Less electronegative atom comes first. 2. Add prefixes to indicate # of atoms. Omit mono- prefix on the FIRST element. Mono- is OPTIONAL on the SECOND element (in this class, it’s NOT optional!). 3. Change the ending of the second element to -ide .

29. PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10 Molecular Nomenclature Prefixes

30. Molecular Nomenclature: Examples CCl 4 N 2 O SF 6 carbon tetrachloride dinitrogen monoxide sulfur hexafluoride

31. More Molecular Examples arsenic trichloride dinitrogen pentoxide tetraphosphorus decoxide AsCl 3 N 2 O 5 P 4 O 10

32. Learning Check Fill in the blanks to complete the following names of covalent compounds. CO carbon ______oxide CO 2 carbon _______________ PCl 3 phosphorus _______chloride CCl 4 carbon ________chloride N 2 O _____nitrogen _____oxide

33. Learning Check 1. P 2 O 5 a) phosphorus oxide b) phosphorus pentoxide c) diphosphorus pentoxide 2. Cl 2 O 7 a) dichlorine heptoxide b) dichlorine oxide c) chlorine heptoxide 3. Cl 2 a) chlorine b) dichlorine c) dichloride

34. Mixed Review Name the following compounds: 1. CaO a) calcium oxide b) calcium(I) oxide c) calcium (II) oxide 2. SnCl 4 a) tin tetrachloride b) tin(II) chloride c) tin(IV) chloride 3. N 2 O 3 a) nitrogen oxide b) dinitrogen trioxide c) nitrogen trioxide

35. Solution Name the following compounds: 1. CaO 2. SnCl 4 3. N 2 O 3 a) calcium oxide c) tin(IV) chloride b) Dinitrogen trioxide

36. Mixed Practice Dinitrogen monoxide Potassium sulfide Copper (II) nitrate Dichlorine heptoxide Chromium (III) sulfate Iron (III) sulfite Calcium oxide Barium carbonate Iodine monochloride

37. Mixed Practice BaI 2 P 4 S 3 Ca(OH) 2 FeCO 3 Na 2 Cr 2 O 7 I 2 O 5 Cu(ClO 4 ) 2 CS 2 B 2 Cl 4

38. Acid Nomenclature Acids Compounds that form H + in water. Formulas usually begin with ‘H’. Examples: HCl (aq) – hydrochloric acid HNO 3 – nitric acid H 2 SO 4 – sulfuric acid

39. Acid Nomenclature Review No Oxygen  w/Oxygen

40. Acid Nomenclature Flowchart

41. Acid Nomenclature HBr (aq) H 2 CO 3 H 2 SO 3 2 elements, - ide 3 elements, -ate 3 elements, -ite  hydro bromic acid  carbon ic acid  sulfur ous acid

42. Acid Nomenclature hydrofluoric acid sulfuric acid nitrous acid 2 elements 3 elements, -ic 3 elements, -ous  HF (aq)  H 2 SO 4  HNO 2  H + F-  H + SO 4 2-  H + NO 2 -

43. Name ‘Em! HI (aq) HCl H 2 SO 3 HNO 3 HIO 4

44. Write the Formula! Hydrobromic acid Nitrous acid Carbonic acid Phosphoric acid Hydrotelluric acid

45. Now it’s Study Time DONE