Question

NAME SECTION DATE REPORT FOR EXPERIMENT 17 INSTRUCTOR Lewis Structures and Molecular Models For each of the following molecules or polyatomic ions, fill out columns A through G using the instructions provided in the procedure see- tion. These instructions are summarized briefly below. A. Calculate the total number of valence electrons in each formula B. Draw a Lewis structure for the molecule or ion which satisfies the rules provided in the procedure C. Build a model of the molecule and have it checked by the instructor D. Use your model to determine the molecular geometry for this molecule (don't try to guess the geometry without the model tetra- hedral, trigonal pyramidal, trigonal planar, bent, linear E. Determine the bond angle between the central atom and the atoms bonded to it. If there are only two atoms in the structure write "no central atom" in the space provided E Use the electronegativity table to determine the electronegativity of the bonded atoms. If the bonds are polar, indicate this with a modified arrow pointing to the more electronegative element. If the bonds are nonpolar, indicate this with a short line . If there are two or more different atoms bonded to the central atom, include each bond. G. Use your model and your knowledge of the bond polarity to determine if the molecule as a whole is nonpolar or a dipole. If it is polar, write dipole in G If it is not, write nonpolar - 155 D Molecule or Polyatomie Ion No. of Valence Electrons Lewis Structure Molecular Geometry Bond Angles Molecular Dipole Bond Polarity c-4 H - |x 4 CH, | H | C tetraedral - -H Nonpolar cs: S-c-s: s-6x2 linear 180 c-s Nonpolar

Answer 1