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Chemical Nomenclature: Naming Compounds in Antacids

Learn and practice the rules of nomenclature in chemistry for naming chemicals used in antacids. Understand the language of chemistry, including element symbols, chemical formulas, and chemical equations.

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Chemical Nomenclature: Naming Compounds in Antacids

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  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

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