Part I. Hydrides and Periodicity 1. Determine the formulas of the hydrides of the following atoms: C, N, O, F, Si, P, S, Cl 2. Write these formulas in the appropriate place in Table 1 of your lab report. 3. Complete Table 1 by determining the number of valence electrons and Lewis Structures of the hydride compounds. 4. Determine the electron pair and molecular geometries of these compounds. Record your findings in Table 2 of your lab report. Part II. Fluorinated Compounds 5. Determine the electron pair and molecular geometries of the fluorinated compounds shown in Table 3. Record your findings in Table 3. Part III. Hydrocarbons 6. Draw a Lewis structure of methane, CH4. 7. Draw the Lewis structures of ethane, C2H6 and propane, C3H8. 8. Draw Lewis structures of butane, C4H10. 9. Enter the appropriate information in Table 4, and answer the appropriate questions in the laboratory report. 1 Part I: Hydrides and Periodicity Table 1: Lewis Structures of Hydrides Central Atom Formula Of Hydride Total # of Valence Electrons C CH4 8 N NH3 8 O H2O 8 F HF 8 Si SiH4 8 P PH3 5 S H2S 8 Cl HCl 8 2 Lewis Structure Part II, Table 2: Molecular Geometries Central Formula of # of Bonded # of Lone Electron Electron Pair Atom Hydride Electron Pairs Pairs Geometry C N O F Si P S Cl 3 Molecular Shape Bond Angle(s) Part II. Fluorinated Compounds Table 3: Fluorinated compounds Molecule Total # of E. Pairs # Of Bonding around Central Electron Pairs # of Lone Pairs Atom PF5 SF4 CIF3 SF6 BrF5 XeF4 NF3 4 Electron Pair Molecular Bond Geometry Geometry Angle(s) Part III: Hydrocarbons Table 4: Hydrocarbons NAME FORMULA Methane CH4 Ethane C2H6 Propane C3H8 Butane (structure 1) C4H10 Butane (structure 2) C4H10 5 LEWIS STRUCTURE 
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