1 / 29

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).

keenan
Download Presentation

Chapter 6

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. 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

More Related