1. Chapter 5 Molecules & Compounds Chemistry 100

2. Elements & Compounds

3. 1.Ionic compounds (a metal and a nonmetal) 2. Covalent compounds (two nonmetals) (Molecular Compounds) Binary Compounds

4. 1.Ionic compounds (a metal and a nonmetal) Binary Compounds

5. Metals: lose 1, 2 or 3 e - Cation (Y + ) Nonmetals: gain 1, 2 or 3 e - Anion (X - ) Ions Cation (Y + ): Na + Li + Ca 2+ Al 3+ Anion (X - ): Cl - F - O 2- Number of protons and neutrons in the nucleus remains unchanged.

6. Transition elements 1A2A 3A 4A5A6A7A 8A

7. Ionic bonds Metal-Nonmetal Anion Cation Opposite charges attract each other. Na  Na + + e - Cl + e -  Cl -

8. Sodium (Na) NaCl Chlorine (Cl)

9. Type I Monatomic Cations Metal has only one type of cation (main group elements) International Union of Pure and Applied Chemistry (IUPAC) systematic names Name of the metal + “ion” H + Hydrogen ion Li + Lithium ion Ca 2+ Calcium ion Al 3+ Aluminum ion

10. Type II Monatomic Cations Metal has two (or more) type of cations (transition elements) IUPAC or Systematic names 1 = I 2 = II 3 = III 4 = IV 5 = V 6 = VI Memorize!!!

11. Common name (old name) Name of the metal + “-ous”smaller charge “-ic”larger charge Cu 1+ Copper(I) ionCuprous ion Cu 2+ Copper(II) ionCupric ion Fe 2+ Iron(II) ion Ferrous ion Fe 3+ Iron(III) ion Ferric ion Pb 2+ Lead(II) ion Plumbous ion Pb 4+ Lead(IV) ion Plumbic ion Sn 2+ Tin(II) ionStannous ion Sn 4+ Tin(IV) ionStannic ion Type II Monatomic Cations

12. Naming Monatomic Anions Stem part of name + “-ide ion” AnionStem nameAnion name F-F- fluorFluoride ion Cl - chlorChloride ion Br - bromBromide ion I-I- iodIodide ion O 2- oxOxide ion S 2- sulfSulfide ion P 3- phosphPhosphide ion N 3- nitrNitride ion Memorize!!!

13. matter are neutral (uncharged): total number of positive charges = total number of negative charges Na + Cl - NaCl Ca 2+ Cl - CaCl 2 Al 3+ S 2- Al 2 S 3 Ba 2+ O 2- Ba 2 O 2 BaO Molecule of NaCl Formula of NaCl

14. Naming Binary Ionic compounds NaClSodium chloride CaOCalcium oxide Cu 2 OCopper(I) oxideCuprous oxide CuOCopper(II) oxideCupric oxide CsBr Cesium bromide MgSMagnesium sulfide FeCl 2 Iron(II) chloride Ferrous chloride FeCl 3 Iron(III) chloride Ferric chloride Name of metal cation Base name of anion + -ide

15. 1.Ionic compounds (a metal and a nonmetal) 2. Covalent compounds (two nonmetals) (Molecular Compounds) Binary Compounds

16. 2. Covalent compounds (two nonmetals) Binary Compounds

17. Naming Binary Covalent compounds (type III) Mono – Di – Tri – Tetra– Penta – Hexa – Hepta – Octa – Nona – Deca 1.Don’t use “mono” for the 1 st element. 2.Drop the “a” when followed by a vowel. 1 2 3 4 5 6 7 8 9 10 Rules: Prefix Name of 1 st Element Prefix Name of 2 nd Element + -ide

18. PCl 5 Phosphorous pentachloride SF 6 Sulfur hexafluoride Naming Binary Covalent compounds (type III) NO 2 Nitrogen dioxide N 2 O 4 Dinitrogen tetroxide CCl 4 Carbon tetrachloride S 2 O 3 Disulfur trioxide

19. Binary Compounds Metal present? Yes Does the metal form more than one cation? Yes No Yes No Type I Use the element name for the cation Type II Find the charge of the cation Use a Roman number after the element name. Type III Use prefixes

20. Naming Polyatomic Ionic Compounds They contain more than two elements.

21. Naming Polyatomic Ions Cation Memorize!!!

22. Oxyanions Polyatomic anions with different numbers of oxygen atoms. NO 2 - Nitrite NO 3 - Nitrate SO 3 2- Sulfite SO 4 2- Sulfate HSO 3 - Hydrogen Sulfite (bisulfite) HSO 4 - Hydrogen sulfate (bisulfate) PO 3 3- Phosphite PO 4 3- Phosphate HPO 4 2- Hydrogen phosphate H 2 PO 4 - Dihydrogen phosphate Smaller number of oxygen atoms ends with –ite. Larger number of oxygen atoms ends with –ate. When we have two oxyanions in a series:

23. Oxyanions When we have more than two oxyanions in a series: (Fewest oxygen atoms) Prefix hypo- (Most oxygen atoms) Prefix per- ClO - hypochlorite ClO 2 - chlorite ClO 3 - chlorate ClO 4 - perchlorate

24. matter are neutral (uncharged): total number of positive charges = total number of negative charges Na + NO 3 - NaNO 3 Ca 2+ CO 3 2- Ca 2 (CO 3 ) 2 CaCO 3 Al 3+ SO 4 2- Al 2 (SO 4 ) 3 Mg 2+ NO 2 - Mg(NO 2 ) 2

25. Naming Polyatomic Ionic compounds NaNO 3 CaCO 3 Al 2 (SO 4 ) 3 Mg(NO 2 ) 2 Sodium nitrate Calcium carbonate Aluminum sulfate Magnesium nitrite Name of metal cationName of polyatomic ion

26. Naming Polyatomic Ionic compounds FeCO 3 Fe 2 (CO 3 ) 3 Iron(II) carbonate Iron(III) carbonate Name of metal cation Name of polyatomic ion Charge of cation in Roman numerals ( )

27. Naming acids Acids: sour They produce H + (proton) in water.

28. Naming binary acids Hydro -ide ion -ic acid Anion : + HFF - : flouride ionHydroflouric acid HClCl - : chloride ionHydrochloric acid H2SH2SS 2- : sulfuride ionHydrosulfuric acid

29. Naming Polyatomic Acids Anion: -ite ion -ous acid -ate ion -ic acid HNO 3 NO 3 - :Nitrate ionNitric acid HNO 2 NO 2 - :Nitrite ionNitrous acid H 2 CO 3 CO 3 2- :Carbonate ionCarbonic acid H 2 SO 3 SO 3 2- :Sulfurite ionSulfurous acid