1 / 28

Bell Work

Bell Work. Draw the electron dot structure for each of the following: MgF 2 C 2 H 4 O 2. Physical Science – Lecture 42. Naming Compounds. NAMING COMPOUNDS. Just like differing electron dot structures, covalent bonds have a different naming system than ionic bonding:. Ionic Compounds.

jera
Download Presentation

Bell Work

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. Bell Work • Draw the electron dot structure for each of the following: • MgF2 • C2H4O2

  2. Physical Science – Lecture 42 Naming Compounds

  3. NAMING COMPOUNDS • Just like differing electron dot structures, covalent bonds have a different naming system than ionic bonding:

  4. Ionic Compounds • Formed from a non-metal and a metal or a cation and an anion. • To create a compound, the charge of the cation and anion must cancel. • The numbers of each will be written as subscripts.

  5. Example – Magnesium Sulfide

  6. Special Considerations • When an ion is made of more than 1 capital letter and more than 1 of the ion is needed in a chemical formula, the entire ion must be put into parenthesis and the subscript is written outside the parenthesis.

  7. Example – Calcium Nitrate

  8. Practice - Ammonia Nitride

  9. Covalent Compounds • Formed from two non-metals. • Prefixes of mono, di, tri, and tetra are translated into numbers of each element.

  10. When Covalently Bonded • When two or more of one element are part of a covalently bonding compound, a prefix is needed to determine how many of each is present since there are no charges for covalently bonded atoms.

  11. Prefixes • Mono – one • Di – two • Tri – Three • Tetra – Four • Penta – Five • Deca - Ten

  12. Proper Endings • When non-metals form compounds, the ending of their name changes to –ide when they are the last element in the compound. • Oxygen = oxide • Nitrogen = nitride • Chlorine = Chloride

  13. Examples • “dioxide” – two oxygens • “trioxide” – three oxygens

  14. Example • Carbon disulfide

  15. Example • Nitrogen monoxide

  16. Example • Dinitrogen oxide

  17. Example - Sulfur dioxide

  18. Example - Carbon monoxide

  19. Practice • Sodium Sulfate

  20. Practice • Nitrogen monoxide

  21. Practice • Lithium hydroxide

  22. Practice • Potassium Phosphate

  23. Practice • Calcium Phosphate

  24. Practice • Aluminum Sulfate

  25. Practice • Beryllium Oxide

  26. Example • Sodium Oxide

  27. Practice • Carbon Tetra-Chloride

  28. Practice • Sulfur tri-oxide

More Related