1 / 17

Chapter 6 Notes Part II

Chapter 6 Notes Part II. Naming Ionic Compounds. Naming Ionic C ompounds. For naming an ionic compound, 1) Name the metal. 2) Write the name of the non-metal, and change the end to –ide. Naming Ionic C ompounds. Example: NaBr Sodium bromide Example: CaF 2 Calcium fluoride.

kiersten-nels
Download Presentation

Chapter 6 Notes Part II

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 NotesPart II Naming Ionic Compounds

  2. Naming Ionic Compounds For naming an ionic compound, 1) Name the metal. 2) Write the name of the non-metal, and change the end to –ide.

  3. Naming Ionic Compounds • Example: NaBr • Sodium bromide • Example: CaF2 • Calcium fluoride

  4. Polyatomic Ions • Polyatomic ion – a charged covalently bonded group of atoms • Example: Sulfate SO4-2

  5. Naming Ionic Compounds If there is a polyatomic anion, then you do not change the ending: Ex) Na2SO4 – Sodium sulfate

  6. Name these: Na2O MgCl2 Na2CO3

  7. Name these: Na2O – sodium oxide MgCl2 – magnesium chloride Na2CO3 – sodium carbonate

  8. Naming Ionic Compounds 3) If a positive ion (a metal) can have more than one oxidation number, you have to designate its charge in the name!

  9. Naming Ionic Compounds We do this by putting the charge as a roman numeral in parenthesis between the positive and negative ion.

  10. Naming Ionic Compounds Why do we need to do that? Name: Fe2O3 andFeO These both exist in nature, so we have to show which one we mean.

  11. Naming Ionic Compounds Use the reverse of the criss cross to figure out the charge of the positive ion. • Fe2O3 is Iron III Oxide • FeO is Iron II Oxide

  12. Naming Ionic Compounds Metals that don’t need parentheses: Group I, II and IIIA Zn, Cd (always +2) Ag (always +1)

  13. Naming Ionic Compounds Which means transition, inner transition and other metals do need parentheses!

  14. Naming Ionic Compounds 1. Name the positive ion. 2. Does it need a roman numeral? If so, reverse criss cross, if not, ignore.

  15. Naming Ionic Compounds • Name the negative ion and: • If a nonmetal end in -ide; if a polyatomic ion, end normally.

  16. Name these: Na2S CuCl2 K2SO4 Pb(NO3)3

  17. Name these: Na2S – sodium sulfide CuCl2 – copper chloride K2SO4 – potassium sulfate Pb(NO3)3 – lead nitrate

More Related