Chemical Nomenclature: Naming Compounds in Antacids

1. Section 2.2—Naming Chemicals (We need to be able to name the chemicals in the antacids!) • Objectives • Explain and practice nomenclature rules • in naming chemicals

2. The Language of Chemistry Chemistry has a language all of its own. Chemistry English Element Symbols Letters Chemical Formulas Words Chemical Equations Sentences

3. Symbols & Formulas • Each element symbol starts with a capital letter. If the element symbol is more than one letter, ONLY the first one is capitalized. • Na not NA represents sodium. • CO is 2 elements; Co is one. • Subscripts (numbers written below the text line) tell how many atoms of each element are in the compound. • Na2SO4 contains . . . .

4. Ionic Compound Naming Binary Ionic Compounds Ionic bond- bond formed by attraction between + and – ions. (An ion is any charged particle.) Binary Ionic Compound- compound containing two elements - one metal and one non-metal - bonded through an ionic bond. + Cation - Anion

5. Ionic Bonds are between metals (on the LEFT) & non-metals (on the RIGHT).

6. Identifying & Naming Binary Ionic • To identify: look for • 2 elements (“binary”) • A metal & a non-metal (“ionic”) • To name these compounds: • Write the name of the metal (the cation) • Write the name of the non-metal (the anion) with the suffix “-ide” • The subscripts in the formula do not matter when naming this type of compound.

7. Example #1 NaCl

8. Example #1 “Sodium” Cation NaCl Anion “Chlorine” becomes “Chloride” Sodium Chloride

9. Example #2 CaBr2

10. Example #2 “Calcium” Cation CaBr2 Anion “Bromine” becomes “Bromide” Calcium Bromide

11. Example #3 K2O

12. Example #3 “Potassium” Cation K2O Anion “Oxygen” becomes “Oxide” Potassium Oxide

13. Let’s Practice CaF2 Na3P NaCl SrBr2 Example: Write the name for the following compounds

14. Let’s Practice CaF2 Na3P NaCl SrBr2 Calcium fluoride Sodium phosphide Sodium chloride Strontium bromide Example: Write the name for the following compounds

15. Polyatomic Ionic Compound - Polyatomic Anion Naming Polyatomic Ionic Compounds Polyatomic Ion- a group of atoms (i.e. MORE THAN 1 ATOM) that are bonded together and have an overall charge Polyatomic Ionic Compound- compound containing at least one polyatomic ion + Cation

16. Common Polyatomic Ions The Appendix of your textbook has a chart like this on pg. 432.

17. Help Identifying Polyatomic Ions • The only cation (front-half) polyatomic ion is “NH4+” • All other polyatomic ions are anions (back-half) • The subscript within the polyatomic ion is important (it must ALWAYS match exactly with the one on your ion list) • If there are parenthesis, the polyatomic ion is inside (ignore the number outside)

18. Practice Identifying Polyatomic Ions NaNO3 Al(NO3)3 NH4Cl (NH4)3PO4 Ca(OH)2 NaOH Example: Identify and name the polyatomic ion in each compound

19. Practice Identifying Polyatomic Ions NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 Nitrate Ammonium Hydroxide Ammonium & phosphate Example: Identify and name the polyatomic ion in each compound

20. Identifying & Naming Polyatomic Ionic • These compounds have: • More than 2 capital letters (none starting with H) • Usually contain at least 1 metal & 1 non-metal • To name these compounds: • Write the name of the cation (the metal element name or “Ammonium” for “NH4”) • If the anion is a polyatomic ion, write the polyatomic ion’s name (from the look-up sheet) • If the anion is a single non-metal element, write its name with the suffix “-ide”

21. Example #4 NaNO3

22. Example #4 “Sodium” Cation NaNO3 Polyatomic Anion “Nitrate” Sodium Nitrate

23. Example #5 K2SO4

24. Example #5 “Potassium” Cation K2SO4 Polyatomic Anion “sulfate” Potassium sulfate

25. Example #6 Ca(OH)2

26. Example #6 “Calcium” Cation Ca(OH)2 Polyatomic Anion “hydroxide” Calcium hydroxide

27. Example #7 (NH4)2S

28. Example #7 “Ammonium” Polyatomic Cation (NH4)2S Anion “sulfur” becomes “sulfide” Ammonium sulfide

29. Let’s Practice Ca(NO3)2 Na3PO4 NH4ClO K2CO3 Example: Write the name for the following compounds

30. Let’s Practice Ca(NO3)2 Na3PO4 NH4ClO K2CO3 Calcium nitrate Sodium phosphate Ammonium hypochlorite Potassium carbonate Example: Write the name for the following compounds

31. Covalent compound Binary Covalent Compounds Covalent bond atoms share electrons Binary Covalent Compound compound made from two non-metals that share electrons Non metal Non metal

32. Identifying & Naming Binary Covalent • These compounds have: • 2 elements (“binary”) • Both non-metals (“covalent”) • To name these compounds: • Write the name of the first element with a prefix indicating the number of atoms. One important exception: “Mono” is never used!! • Write the name of the second element with the prefix indicating the number of atoms (including “mono-”) and the suffix “ide”

33. The Appendix of your book (Page 433) has a prefix chart. P2O5

34. Example #10 2 = “di-” Phosphorus P2O5 Oxygen 5 = “penta-” Use “-ide” Diphosphorus pentaoxide

35. Example #11 SiO2

36. Example #11 Don’t use “mono-” on first element Silicon SiO2 Oxygen 2 = “di-” Use “-ide” Silicon dioxide

37. Let’s Practice CO2 N2O4 P4O10 CO Example: Write the name for the following compounds

38. Let’s Practice CO2 N2O4 P4O10 CO Carbon dioxide Dinitrogen tetraoxide Tetraphosphorus decaoxide Carbon monoxide Example: Write the name for the following compounds