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Chapter 6

Chapter 6. Naming Compounds. Binary Ionic Compounds. These have only 2 elements and are ionic (1 metal and 1 nonmetal). Write the name of the cation (metal). Then write the name of the anion (nonmetal) but end it with the suffix –ide. Examples: sodium chloride (NaCl) Calcium oxide (CaO).

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Chapter 6

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  1. Chapter 6 Naming Compounds

  2. Binary Ionic Compounds • These have only 2 elements and are ionic (1 metal and 1 nonmetal). • Write the name of the cation (metal). • Then write the name of the anion (nonmetal) but end it with the suffix –ide. • Examples: • sodium chloride (NaCl) • Calcium oxide (CaO)

  3. Anions • Anion nonmetals form ions with negative charges. • Group number – 8 = charge • Examples: • nitrogen: 5-8=-3 • Oxygen: 6-8=-2 • Iodine: 7-8=-1

  4. Common Anions

  5. Cations • The alkali metals (group 1A), alkaline earth metals (group 2A), and aluminum form ions with a positive charge equal to their number of valence electrons (or group number). • Examples:

  6. Cations • The transition metals form cations differently. • They form more than 1 type of ion. • Use a Roman numeral next to the ion name to indicate its charge. • Examples: copper can be copper (I) with a +1 charge or copper (II) with a +2 charge

  7. Transition Metal Cations

  8. Ionic Compounds • The total (net) charge of an ionic compound must be 0 (zero). • The cation and anion charges must cancel each other out. • Example: • Copper (II) oxide– copper has a charge of +2 and oxygen has a charge of -2 • +2 cancels -2 to equal 0

  9. Which of these ionic compounds have a net charge of 0? • Titanium (II) sulfide • Copper (I) oxide • Lead (II) oxide • Lead (IV) nitride • Mercury (II) iodide

  10. Which of these ionic compounds have a net charge of 0? • **Titanium (II) sulfide +2-2=0 • Copper (I) oxide +1-2=-1 • **Lead (II) oxide +2-2=0 • Lead (IV) nitride +4-3=+1 • Mercury (II) iodide +2-1=+1

  11. Balancing Compounds • Copper (1) oxide • CuO • Does not balance to 0 • +1-2=-1 • But 2 atoms of copper (1) would make it equal 0 • Cu20 • +1+1-2=0

  12. Balancing Compounds • Mercury (II) iodide +2-1=+1 • HgI • Does not balance to 0, but… • HgI2 • +2-1-1=0

  13. Balancing Compounds • Lead (IV) nitride +4-3=+1 • PbN • Does not balance to 0, but… • Pb3N4 • +4+4+4-3-3-3-3=0 • +12-12=0

  14. Write a balanced formula for the following compounds. • Iron (II) bromide • Chromium (III) nitride • Lead (IV) oxide • Titanium (III) fluoride • Lead (IV) phosphide

  15. Write a balanced formula for the following compounds. • Iron (II) bromide FeBr2 • Chromium (III) nitride CrN • Lead (IV) oxide PbO2 • Titanium (III) fluoride TiF3 • Lead (IV) phosphide Pb3P4

  16. Polyatomic Ions • The atoms in polyatomic ions are joined by covalent bonds but have a net + or – charge. • The prefix poly- means many. • Polyatomic ions contain many ions. • Example: • Ammonium contains 1 nitrogen and 4 hydrogen atoms. • -3+1+1+1+1=-3+4=+1 (net charge)

  17. Polyatomic Ions

  18. Polyatomic Ions • I will give you polyatomic ion formulas on the test. • There is a chart in your book on page 173 to use on classwork and homework.

  19. Polyatomic Ions • Polyatomic ions can combine with metals to form compounds. • Put the polyatomic ion in parentheses when you write the formula. • Example: • Iron (III) hydroxide Fe(OH)3 • Iron has a +3 charge and hydroxide has a -1 charge. You must have 3 hydroxide ions to balance the iron and make the net charge 0.

  20. Write a balanced formula for the following. • Chromium (II) sulfate • Lead (IV) hydroxide • Mercury (II) acetate • Copper (I) sulfate • Titanium (IV) dichromate • See page 173 for the polyatomic ion formulas.

  21. Write a balanced formula for the following. • Chromium (II) sulfate Cr(SO4) • Lead (IV) hydroxide Pb(OH)4 • Mercury (II) acetate Hg(C2H3O2)2 • Copper (I) sulfate Cu2(SO4) • Titanium (IV) dichromate Ti(Cr2O7)2

  22. Naming Covalent Compounds • These are called molecules. • Name the most metallic element (the one that appears the furthest left on the periodic table) first. • If both elements are in the same group, name the one closest to the bottom first. • Add the suffix –ide to the second element. • Example: carbon dioxide

  23. Naming Covalent Compounds • Use the Greek prefixes to indicate how many of each atom are in the molecule.

  24. Naming Covalent Compounds • N2O4 • Dinitrogen tetraoxide • Di = 2 nitrogens • Tetra = 4 oxygens • Because nitrogen is a group left of oxygen name it first • Because oxygen is named second, change it to end in -ide

  25. Naming Covalent Compounds • NO2 • Mononitrogen dioxide • If there is only 1 of the first element, it is not necessary to use the mono- prefix. • Nitrogen dioxide

  26. Name the following molecular compounds. • NO2 • P2F4 • P2O5 • CO • N2S5

  27. Name the following molecular compounds. • NO2 nitrogen dioxide • P2F4 diphosphorus tetrafluoride • P2O5 diphosphorus pentaoxide • CO carbon monooxide • N2S5 dinitrogen pentasulfide

  28. Write the name of the molecular compound. • Nitrogen dioxide • Diphosphorus tetrafluoride • Carbon dioxide • Dihydrogen oxide • Dinitrogen tetraoxide

  29. Write the name of the molecular compound. • Nitrogen dioxide NO2 • Diphosphorus tetrafluoride P2F4 • Carbon dioxide CO2 • Dihydrogen oxide H2O • Dinitrogen tetraoxide N2O4

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