1. Chemical Names and Formulas Overview Metals and Non-Metals Ions and Ionic Charges Types of Compounds Systematic Names -Writing Names and Formulas

2. Naming Compounds Tutorial  General Information General Information  Binary Ionic Compounds Binary Ionic Compounds  Ternary Ionic Compounds/Poly- atomic Ions Ternary Ionic Compounds/Poly- atomic Ions  Naming w/metals that have more than 1 charge (Transition Metals) Naming w/metals that have more than 1 charge (Transition Metals)  Molecular Compounds Molecular Compounds  Naming Acids Naming Acids

3. Metals and Nonmetals  Stairway Of Division on Periodic Table non-metals  C, P, Se, I, Rn and to the right semi-metals  B, Si, As, Ge, Sb, Te, Po, At All others are metals

4. Ions  Cations Positively Charged Atoms  i.e.Na +  Anions Negatively Charged Atoms  i.e.Cl -

5. IONIC CHARGES  Group I ->  Group II ->  Group III ->  Group IV -> 1+ 2+ 3+ 4+

6. IONIC CHARGES  Group V ->  Group VI ->  Group VII ->  Group VIII -> 3- 2- 1- Noble Gases

7. Ionic Compounds composed of positive and negative ions. usually formed from a metal and non-metal. these elements are not attached to one another.

8. TYPES OF COMPOUNDS  Ionic Compounds con’t Examples NaCl CaBr 2 KI

9. CHEMICAL FORMULAS shows the kind and numbers of atoms in the smallest representative unit of the substance.  i. e. NaCl

10. IONIC COMPOUNDS  A formula unit is the lowest whole number ratio of ions in an ionic compound.  i.e. Na 2 Cl 2 -> NaCl  There is no such thing as a molecule of NaCl!!!!!!!!!

11. NAMING COMPOUNDS  Your ability to name compounds and write formula’s hinges on your ability to recognize whether a compound is Ionic or Molecular.

12. BINARY IONIC COMPOUNDS  Binary means 2 elements  Ionic means a metal and a non- metal (or cation and anion) charges must balance so compound charge is neutral.

13. BINARY IONIC COMPOUNDS  Writing Formulas from Names 1st word = CATION 2nd word = ANION name with ide ending.

14. BINARY IONIC COMPOUNDS  NaBr  MgF 2  Sodium Bromide  Magnesiu m Fluoride

15. BINARY IONIC COMPOUNDS  Potassium Chloride  Aluminum Oxide notice ending of name is ide! K + Cl - -> KCl Al 2 3+ O 3 2- - > Al 2 O 3

16. Polyatomic Ions  Definitiontightly bound groups of atoms that behave as a unit and carry a charge.  Example SO 3 2-, NO 2 -, ClO 2 -

17. TERNARY IONIC COMPOUNDS  Ternary means 3 different elements  Usually contain Poly-atomic Ions  Ionic means cation and anion

18. TERNARY IONIC COMPOUNDS:Writing Formulas  Ca 2+ CO 3 2- -> CaCO 3  Calcium Carbonate

19. TERNARY IONIC COMPOUNDS: Naming  Calcium Nitrate  Ca(NO 3 ) 2

20. Naming with Transition Metals  First word = CATION  Second word = ANION You need to determine what charge is on the transition metal if more than one exists.

21. Naming Transition Metals  Copper (I) Oxide  Cu 2 O

22. Writing Formulas with Transition Metals  FeCl 3  FeCl 2  Iron (III) Chloride  Iron (II) Chloride

23. TYPES OF COMPOUNDS  Molecular Compounds composed of molecules in which elements share electrons. usually composed of 2 nonmetals. these elements are attached

24. MOLECULAR FORMULA  Definition shows the numbers and kinds of atoms present in a molecule of a compound.  i. e. CO

25. TYPES OF COMPOUNDS  Molecular Compounds con’t Examples CS 2 SiO 2 BF 3

26. BINARY MOLECULAR COMPOUNDS  Binary means 2 elements  Molecular means 2 non-metals  NO ionic charges are present

27. Naming Binary Molecular Compounds  Prefixes are used to show how many atoms are present in each molecule.  mono, di, tri,tetra, penta, hexa, hepta, octa, nona, deca

28. Writing Binary Molecular Compounds  CO 2 no mono prefix is used on first element  Carbon Dioxide Di means 2 oxygens!!

29. Naming Binary Molecular Compounds PCl 3 Phosphorous Trichloride  All binary compounds end in ide!!!

30. Naming with Acids  Anion Endings ide  Example HCl  Acid Name hydro-(stem)- ic acid  Hydrochloric Acid

31. Naming with Acids  Anion Ending ite  Example Hydrogen Sulfite  Acid Name (stem)-ous acid  Sulfurous Acid

32. Naming with Acids  Anion Ending ate  Example Hydrogen Sulfate  Acid Name (stem)-ic acid  Sulfuric Acid