Molecular geometry lab

Lab 12 Molecular Geometry Exercises 1. Determine the total number of valence electrons for the following molecules or ions. (a) ClO2− (b) N2O (c) (NH4)2SO4 Supporting Materials Periodic Table Constants and Factors Supplemental Data Lab 12 Molecular Geometry Exercises 2. (a) Draw the Lewis structure for ethylamine (CH3CH2NH2). (Assign lone pairs where appropriate.) Help Marvin JS H C N + O - S F P Cl Br I (b) Determine the number of nonbonding valence electrons present in a molecule of ethylamine (CH3CH2NH2). There are nonbonding valence electron(s) within a molecule of ethylamine. They all belong to the nitrogen atom. Tutorial Supporting Materials Periodic Table Constants and Factors Supplemental Data Lab 12 Molecular Geometry Exercises 3. Draw Lewis structures for each of the following compounds. (Assign lone pairs and radical electrons where appropriate.) (a) iodoamine (NH2I) Help Marvin JS H C N + O - S F P Cl Br I (b) chloroethyne (C2HCl) Help Marvin JS Lab 12 Molecular Geometry Exercises H C N + O - S F P Cl Br I (c) ethanol (C2H5OH) Help Marvin JS Lab 12 Molecular Geometry Exercises H C N + O - S F P Cl Br I Tutorial Supporting Materials Periodic Table Constants and Factors Supplemental Data Lab 12 Molecular Geometry Exercises 4. Draw Lewis structures for each of the following compounds. (Assign lone pairs and radical electrons where appropriate. Omit any atomic charges.) (a) dichlorodifluoromethane (CCl2F2) Help Marvin JS H C N + O - S F P Cl Br I (b) nitrogen (N2) Help Marvin JS Lab 12 Molecular Geometry Exercises H C N + O - S F P Cl Br I (c) dimethyl sulfide (CH3SCH3) Help Marvin JS Lab 12 Molecular Geometry Exercises H C N + O - S F P Cl Br I Tutorial Supporting Materials Periodic Table Constants and Factors Supplemental Data 5. What is the hybridization of the central atom in NH4+? The central atom in the NH4+ ion is ??? orbitals. sp sp2 sp3 Tutorial Supporting Materials Periodic Table Constants and Factors Supplemental Data . This ??? atom has the following hybridized Lab 12 Molecular Geometry Exercises 6. Use valence bond theory to describe the number and types of hybrid bonding orbitals on the central atom of each of the following. (a) BBr4− type of hybridization: sp-hybridization sp2-hybridization sp3-hybridization sp3d-hybridization sp3d2-hybridization In BBr4−, boron has (b) hybrid orbital(s). IBr3 type of hybridization: sp-hybridization sp2-hybridization sp3-hybridization sp3d-hybridization sp3d2-hybridization In IBr3, iodine has (c) CS2 type of hybridization: sp-hybridization sp2-hybridization sp3-hybridization sp3d-hybridization sp3d2-hybridization hybrid orbital(s). Lab 12 Molecular Geometry Exercises In CS2, carbon has hybrid orbital(s). Tutorial 7. (a) Using the valence bond theory, specify the type of hybridization on the central atom in the BH3 molecule. sp-hybridization sp2-hybridization sp3-hybridization sp3d-hybridization (b) Draw orbital diagrams to show the distribution of the central atom's valence electrons before and after hybridization. (Complete each energy level from left to right. Enter __ for an unoccupied orbital, ↑_ for a singly occupied orbital, and ↑↓ for a doubly occupied orbital.) before hybridization ?? ?? ?? 2p ?? 2s after hybridization ?? 2p ?? ?? hybrid orbitals Tutorial ?? Lab 12 Molecular Geometry Exercises 8. Use the VSEPR model to determine the electron-domain geometries of carbon tetrachloride (CCl4), carbon diselenide (CSe2), and phosphine (PH3). Carbon tetrachloride (CCl4): linear trigonal planar tetrahedral trigonal bipyramidal octahedral Carbon diselenide (CSe2): linear trigonal planar tetrahedral trigonal bipyramidal octahedral Phosphine (PH3): linear trigonal planar tetrahedral trigonal bipyramidal octahedral Tutorial Lab 12 Molecular Geometry Exercises 9. Using the VSEPR model, identify the molecular geometry of nitrogen tribromide, NBr3, based on the number of electron domains.