CHAPTER 3 Ionic Bonding transfer of one or more electrons o Interaction between cations positive charge and anions negative charged o Cations lose electrons and anions gain electrons POLAR BOND o Occurs between metals non metals Covalent molecular Bonding sharing of electrons o Occur when two elements are close non metals with non metals right side table 3 Types of Compounds 1 Molecular covalent 2 Ionic polar a Type I metal forms only 1 type of ions b Type II metal forms more than 1 type of ion multiple charge states transition Ionic Compound Type I metal forms only 1 type of ion Includes groups 1 2 3 Zn Cd Al Ag lanthanides Group 1 has 1 charge because they lose 1 electrons group 2 has 2 charge etc Group 11 Ag ion 1 charge Group 12 Zn Cd ion 2 charge Lanthanides form 3 ions When naming these compounds you must include whether or not they are an ion Ex K is called Potassium Ion not just potassium Ca2 is Calcium Ion not calcium Sc3 is Scandium Ion it would be incorrect to call this scandium Na is Sodium 11protons electrons Na is sodium ion 11 protons 10 electrons Anions Negatively charged ions Group 17 1 charge Group 16 2 charge Group 15 3 charge Cl chloride S2 sulfide O2 oxide N3 nitride Ionic Compound Type II Metals with multiple charge states form more than 1 type cation Includes groups 4 11 transition metals NAMING IONIC COMPOUNDS 1 Cation written 1st anion written 2nd 2 add IDE to end of anion 3 Balance the charges 4 Identify charge with roman numeral after cation with multiple charge states transition NAMING MOLECULAR COVALENT COMPOUNDS 1 Cation written 1st anion written 2nd 2 add IDE to end of anion 3 Add Greek Prefix mono di tri tetra penta hexa hepta octa nona deca a Do not need to use prefix mono on the cation Ex NO Nitrogen monoxide NOT mononitrogen monoxide b If two vowels in a row drop the first vowel Ex N2O5 dinitrogen pentoxide NOT dinitrogen pentaoxide NAMING ACIDS 1 Can be H single atom ex HF hydrofluoric acid use Hydro 2 Can be H ion a b If an ion ends in ATE it becomes IC ex H2SO4 sulfuric acid If an ion ends in ITE it becomes OUS ex H2SO3 sulfurous acid Ionic Compounds Type I Examples KCl Potassium chloride NaCl Sodium chloride Na2S sodium sulfide Rb2S Rubidium sulfide Rb3PO4 Rubidium phosphate Mg CH3COO 2 magnesium acetate Mg3N2 magnesium nitride Al2O3 Aluminum oxide La2S3 Lanthanum sulfide La has 3 charge so you need 2 to balance S2 Ionic Compounds Type II Examples FeCl3 Iron III chloride chloride has 1 charge but there are 3 of them FeO Iron II oxide oxygen has 2 charge so you need 2 Fe s to balance Co3 PO4 2 Cobalt II phosphate MnO mangaenese II oxide FeCl2 Iron II chloride Cr2S3 Chromium III sulfide Ti3N4 Titanium IV nitride Covalent molecular Compounds Examples P2O5 diphosphorus pentoxide note it is not pentAoxide dropped the a N2O dinitrogen monoxide BI3 Boron triiodide PCl5 Phosphorus pentachloride CO2 carbon dioxide CO carbon monoxide CBr4 carbon tetrabromide N2O5 dinitrogen pentoxide
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