CHM1045 Lecture 6 Outline of Last LectureI. Formulas:II. Ionic CompoundsIII. Chemical NomenclatureIV. Need to Memorize:Outline of Today’s Lecture:I. Molecular compoundsi. Example 1ii. Example 2II. CompoundCurrent LectureMolecular 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 iodideNF3 nitrogen trifluorideSO2 sulfur dioxideN2Cl4 dinitrogen tetrachloride NO2 nitrogen dioxide $ N2O dinitrogen monoxide $Example 1.Name the following molecular compounds: (a) SiCl4(b) P4O10a. Silicon tetrachlorideb. Tetraphosphorous decoxideExample2:Write chemical formulas for the following molecular compounds: (a) carbon disulfide(b) disilicon hexabromidea. CS2b. Si2Br6CompoundIonic MolecularCation: Metal or NH4+ Binary Compounds of nonmetalsAnion: monoatomic or polyatomic 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 numeralsname 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
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