2. Naming Ionic Compounds Chemistry Dr. May

3. Ionic Compounds  Formed when electrons are transferred from the less electronegative atom (Na) to the more electronegative atom (Cl). Na    e -1    Cl to give Na +1 and Cl  1 thus NaCl

4. Electronegativity  Tendency for atoms to attract electrons  Metals have low electronegativity  Metals lose electrons to form ions (Na +1 )  Non-metals have high electronegativity  Non-metals gain electrons to form ions (Cl  1 )

5. Ionic Compounds (NaCl)  Formed between metals and non-metals  Use element name of the metal (sodium)  Add –ide to root name of non-metal (chloride)  We have: sodium chloride

6. The –ides Of Compound Names  Fluorine   Chlorine   Bromine   Iodine   Oxygen   Sulfur   Carbon   Nitrogen   Phosphorus  Fluoride Chloride Bromide Iodide Oxide Sulfide Carbide Nitride Phosphide

7. Name – ide Compounds  KCl   Na 2 O   CaS   MgBr 2   ZnCl 2   Ag 2 S   Al 2 O 3   CaC 2   K 3 N  Potassium chloride Sodium oxide Calcium sulfide Magnesium bromide Zinc chloride Silver sulfide Aluminum oxide Calcium carbide Potassium nitride

8. The – ates Of Compound Names  SO 4 –2 –  CO 3 –2 –  NO 3 –1 –  PO 4 –3 – Sulfate Carbonate Nitrate Phosphate

9. Name –ate Compounds  KNO 3   CaCO 3   AlPO 4   MgSO 4   Ca(NO 3 ) 2   K 3 PO 4   Al 2 (SO 4 ) 3   Mg 3 (PO 4 ) 2  Potassium nitrate Calcium carbonate Aluminum phosphate Magnesium sulfate Calcium nitrate Potassium phosphate Aluminum sulfate Magnesium phosphate

10. Some Other Polyatomics  OH  1   NH 4 +1   CN  1   HCO 3  1   HSO 4  1  Hydroxide Ammonium Cyanide Bicarbonate Bisulfate

11. Name Some Other Polyatomics  KOH   Al(OH) 3   NH 4 Cl   (NH 4 ) 2 SO 4   KCN   HCN   NaHCO 3   KHSO 4  Potassium hydroxide Aluminum hydroxide Ammonium chloride Ammonium sulfate Potassium cyanide Hydrogen cyanide Sodium bicarbonate Potassium bisulfate

12. Naming Covalent Compounds Chemistry Dr. May

13. Covalent Compounds  Formed when electrons are shared between two atoms having similar electronegativities  Formed between two non-metals such as sulfur (S) and oxygen (O) or carbon (C) and oxygen. SO SO 2 SO 3 SO 4 CO CO 2

14. Naming Guidelines – PBr 5  Less electronegative element comes first  Name of element (phosphorus)  Prefix needed if more than one atom  More electronegative element comes next  Prefix needed, even if 1 (mono)  Root name plus –ide (pentabromide)  PBr 5 is phosphorus pentabromide

15. Possible Prefixes  Oneis  Twois  Threeis  Fouris  Fiveis  Sixis  Sevenis  Eightis  Nineis  Tenis Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- Octa- Nona- Deca-

16. Name Covalent Compounds  CO  CO 2  SO 2  SO 4  SF 6  NI 3  P 2 O 5  CCl 4 Carbon monoxide Carbon dioxide Sulfur dioxide Sulfur tetraoxide Sulfur hexafluoride Nitrogen triiodide Diphosphorus pentoxide Carbon tetrachloride

17. Name Everything  MgCl 2   NF 3   Ca(OH) 2   CCl 4   K 2 SO 4   SO 3   Al 2 S 3   CoO  Magnesium chloride Nitrogen trifluoride Calcium hydroxide Carbon tetrachloride Potassium sulfate Sulfur trioxide Aluminum sulfide Cobalt oxide

18. The End  This presentation was created for the benefit of our students by the Science Department at Howard High School of Technology  Please send suggestions and comments to rmay@nccvt.k12.de.us