1 / 56

Section 2.2—Naming Chemicals

Section 2.2—Naming Chemicals. We need to be able to name the chemicals in the antacids!. The Language of Chemistry. Chemistry has a language all of its own. Chemistry. English. Element Symbols. Letters. Chemical Formulas. Words. Chemical Equations. Sentences.

keiran
Download Presentation

Section 2.2—Naming Chemicals

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Section 2.2—Naming Chemicals We need to be able to name the chemicals in the antacids!

  2. The Language of Chemistry Chemistry has a language all of its own Chemistry English Element Symbols Letters Chemical Formulas Words Chemical Equations Sentences Each element symbol starts with a capital letter

  3. Binary Ionic compounds

  4. Ionic Compound Definitions Ionic bond- bond formed by attraction between + and - ions Binary Ionic Compound- compound containing two elements—one metal and one non-metal + Cation - Anion

  5. Metals & Non-Metals Ionic Bonds are between metals & non-metals

  6. Identifying & Naming Binary Ionic • These compounds have: • 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

  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 Compounds

  16. Polyatomic Ionic Compound - Polyatomic Anion Definition Polyatomic Ion- more than one atom that together have a charge Polyatomic Ionic Compound- compound containing at least one polyatomic ion + Cation

  17. Common Polyatomic Ions The Appendix of your book (Page A-2) has the following chart

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

  19. Practice Identifying Polyatomic Ions NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3 Example: Identify and name the polyatomic ion in each compound

  20. Practice Identifying Polyatomic Ions NaNO3 NH4Cl Ca(OH)2 (NH4)3PO4 K2CO3 Nitrate Ammonium Hydroxide Ammonium & phosphate Carbonate Example: Identify and name the polyatomic ion in each compound

  21. Identifying & Naming Polyatomic Ionic • These compounds have: • More than 2 capital letters (non starting with H) • 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 just as it is • If the anion is a single non-metal element, write its name with the suffix “-ide”

  22. Example #4 NaNO3

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

  24. Example #5 K2SO4

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

  26. Example #6 Ca(OH)2

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

  28. Example #7 (NH4)2S

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

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

  31. 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

  32. Multivalent Metals

  33. Definition Multivalent Metal- metal that has more than one possibility for cationic charge The Appendix of your book (Page A-2) has the following chart

  34. Identifying & Naming Multivalent Metals • These compounds have: • One of the multi-valent metals in that chart • To name these compounds: • Write the name of the metal element (cation) • Write the name of the anion (element name with “-ide” or polyatomic ion name) • Determine the total negative charge • Total negative charge = total positive charge for all neutral compounds • Determine the charge on each metal atom • Write the charge in roman numerals in parenthesis after the metal’s name

  35. Common Ions Use the periodic table to determine charges on common elemental anions

  36. Example #8 CuCl

  37. Example #8 “Copper” Cation CuCl Anion “Chlorine” becomes “Chloride” Copper Chloride

  38. Example #8 “Copper” Cation Chloride has a –1 charge CuCl -1 charge * 1 ion = -1 A –1 charge needs a +1 charge Anion “Chlorine” becomes “Chloride” Therefore, copper must be +1 Copper Chloride (I)

  39. Example #9 Fe2(CO3)3

  40. Example #9 “Iron” Cation Fe2(CO3)3 Polyatomic Anion “Carbonate” Iron carbonate

  41. Example #9 “Iron” Cation Carbonate has a –2 charge Fe2(CO3)3 -2 charge * 3 ions = -6 A –6 charge needs a +6 charge and there are 2 iron ions Polyatomic Anion “Carbonate” Therefore, iron must be +3 Iron carbonate (III)

  42. Let’s Practice PbCl2 PbCl4 MnO Mn2O3 Example: Write the name for the following compounds

  43. Let’s Practice PbCl2 PbCl4 MnO Mn2O3 Lead (II) chloride Lead (IV) chloride Manganese (II) oxide Manganese (III) oxide Example: Write the name for the following compounds

  44. Binary Covalent Compounds

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

  46. 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 the prefix indicating the number of atoms (except don’t use “mono-”) • Write the name of the second element with the prefix indicating the number of atoms (including “mono-”) and the suffix “ide”

  47. Covalent Prefixes The Appendix of your book (Page A-2) has the following chart

  48. Example #10 P2O5

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

  50. Example #11 SiO2

More Related