1 / 18

Ch. 5 Ionic Bonding

Ch. 5 Ionic Bonding. Naming Section 3. Need to Know. Binary Ionic Compounds Binary – indicates that the compound is made up of just two elements. Rules for Naming Ions. Simple Cations Borrow names from names of elements Examples K + → potassium ion Zn 2+ → zinc ion.

ivie
Download Presentation

Ch. 5 Ionic Bonding

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. Ch. 5Ionic Bonding Naming Section 3

  2. Need to Know • BinaryIonic Compounds • Binary – indicates that the compound is made up of just two elements

  3. Rules for Naming Ions • Simple Cations • Borrow names from names of elements • Examples • K+ → potassium ion • Zn2+ → zinc ion

  4. Rules for Naming Ions • Elements that form two or more ions • Use Roman #’s • Examples • Cu+ → copper (I) ion • Cu2+ → copper (II) ion

  5. Rules for Naming Ions • Simple Anions • Formed from name of element, but it ends in –ide • Examples • Cl-→ chloride ion • O2-→ oxide ion • P3-→ phosphide ion

  6. Naming Binary Ionic Compounds • The cation is always named first • Examples • NaCl→ SodiumChloride • ZnS→ ZincSulfide • K2O→ PotassiumOxide • CuCl2→ Copper (II)Chloride

  7. Polyatomic Ions • poly – “many” • an ion made of two or more atoms • can be treated as a single ion  charge is not found on a single atom

  8. Polyatomic Ions • Endings • Contains oxygen • ends with –ite or –ate • -ite “less oxygen” • -ate  “more oxygen” • Examples • Nitrate – NO3- • Nitrite – NO2-

  9. Polyatomic Ions • Prefixes • mono – “one” • di – “two” • thio – “replace oxygen with sulfur” • Examples • monohydrogen phosphate HPO42- • dihydrogen phosphate H2PO42-

  10. Ch. 5Ionic Bonding Practice Section 5.3

  11. N3- Fe3+ Mg2+ Ca3N2 FeI3 Na2O AlCl3 SrO CuCl2 Al2S3 PracticeWrite the names for the following:

  12. PracticeWrite the formulas for the following: • Copper (II) oxide • Sodium fluoride • Zinc chloride • Aluminum sulfide • Potassium nitride

  13. Practice Write the formula for he following: Write the name for the following: Ca(NO3)2 CuSO4 CuNO3 Na2CO3 K2Cr2O7 • Aluminum nitrate • Ammonium phosphate • Ammonium acetate • Potassium permanganate

  14. Homework Section Review 5.3 #’s 5 - 8

More Related