CHM1045 Lecture 6 Outline of Last Lecture I Formulas II Ionic Compounds III Chemical Nomenclature IV Need to Memorize Outline of Today s Lecture I Molecular compounds i Example 1 ii Example 2 II Compound Current Lecture Molecular compounds Nonmetals or nonmetals metalloids Common names H2O NH3 CH4 Element furthest to the left in a period and closest to the bottom of a group on periodic table is placed first in formula If more than one compound can be formed from the same elements use prefixes to indicate number of each kind of atom Last element name ends in ide HI hydrogen iodide NF3 nitrogen trifluoride SO2 sulfur dioxide N2Cl4 dinitrogen tetrachloride NO2 nitrogen dioxide N2O dinitrogen monoxide Example 1 Name the following molecular compounds a SiCl4 b P4O10 a Silicon tetrachloride b Tetraphosphorous decoxide Example2 Write chemical formulas for the following molecular compounds a carbon disulfide b disilicon hexabromide a CS2 b Si2Br6 Compound Ionic Cation Metal or NH4 Anion monoatomic or polyatomic Molecular Binary Compounds of nonmetals Cation has only 1 charge Cation has 1 charge Alkali metal cations Other metal cations Alkaline earth metals Naming Cations Use Prefixes for both elements Ag Al3 Cd2 Zn2 present prefix mono usually Omitted for the first element Add ide to the root of the 2nd element Naming Naming Name metal first Name metal 1st If Monoatomic anion add Specify change of metal cation with ide to the root of the element Roman numerals name If monoatomic anion add ide to the If polyatomic anion use name root if the element change Of anion If polyatomic anion use name of anion
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