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Naming Ionic Compounds

Naming Ionic Compounds. Chemistry Dr. May. 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. Electronegativity.

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Naming Ionic Compounds

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  1. Naming Ionic Compounds Chemistry Dr. May

  2. 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+1and Cl1 thus NaCl

  3. 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)

  4. 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

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

  6. KCl  Na2O  CaS  MgBr2  ZnCl2  Ag2S  Al2O3  CaC2  K3N  Potassium chloride Sodium oxide Calcium sulfide Magnesium bromide Zinc chloride Silver sulfide Aluminum oxide Calcium carbide Potassium nitride Name – ide Compounds

  7. SO4 –2 – CO3 –2 – NO3 –1 – PO4 –3 – Sulfate Carbonate Nitrate Phosphate The – ates Of Compound Names

  8. KNO3  CaCO3  AlPO4  MgSO4  Ca(NO3)2  K3PO4  Al2(SO4)3  Mg3(PO4)2  Potassium nitrate Calcium carbonate Aluminum phosphate Magnesium sulfate Calcium nitrate Potassium phosphate Aluminum sulfate Magnesium phosphate Name –ate Compounds

  9. OH1  NH4+1  CN1  HCO31  HSO41  Hydroxide Ammonium Cyanide Bicarbonate Bisulfate Some Other Polyatomics

  10. KOH  Al(OH)3  NH4Cl  (NH4)2SO4 KCN  HCN  NaHCO3 KHSO4 Potassium hydroxide Aluminum hydroxide Ammonium chloride Ammonium sulfate Potassium cyanide Hydrogen cyanide Sodium bicarbonate Potassium bisulfate Name Some Other Polyatomics

  11. Naming Covalent Compounds Chemistry Dr. May

  12. 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 SO2 SO3 SO4 CO CO2

  13. Naming Guidelines – PBr5 • 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) • PBr5 is phosphorus pentabromide

  14. One is Two is Three is Four is Five is Six is Seven is Eight is Nine is Ten is Mono- Di- Tri- Tetra- Penta- Hexa- Hepta- Octa- Nona- Deca- Possible Prefixes

  15. CO CO2 SO2 SO4 SF6 NI3 P2O5 CCl4 Carbon monoxide Carbon dioxide Sulfur dioxide Sulfur tetraoxide Sulfur hexafluoride Nitrogen triiodide Diphosphorus pentoxide Carbon tetrachloride Name Covalent Compounds

  16. MgCl2 NF3 Ca(OH)2 CCl4 K2SO4 SO3  Al2S3  CoO  Magnesium chloride Nitrogen trifluoride Calcium hydroxide Carbon tetrachloride Potassium sulfate Sulfur trioxide Aluminum sulfide Cobalt oxide Name Everything

  17. 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

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