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Date Created: 04/19/14
Chemistry 162 Midterm 1 Study Guide Ch 13 Material Define electronegativity Describe the electronegativity trend in the periodic table Define ionic bond covalent bond and polar covalent bond and give an example of each Does CO2 have a dipole moment If so in what direction Draw the LDS partial charges and electronegativity arrows Does H20 have a dipole moment If so in what direction Again draw the LDS Define lattice energy Calculate delta H or reaction for the following reaction CH3C00H 8 9 CH4 8 C02 8 8 Draw the Lewis Dot Structures for each of the following molecules a CO b OH c HZCO d N02 9 What are structural isomers What is used to determine their most likely structures 10 Draw the resonance structures if any of a nitrate ion If there are resonance structures what is the most likely bond length 11 Determine the formal charge for each atom in the CO2 molecule for each of the resonance structures Which resonance structure is the most correct 12 Exceptions to the octet rule a Name some atoms that can participate in valence shell expansion b Name some atoms that can participate in sub octet systems c Name some radicals have an odd number of electrons 13 Name the electron pair geometry for each notation AXZE AX5 AX4 AXZE3 AX3E AX3E2 AX5 AX2 3quot quot 53399 14 How many electron groups are present on the central atom of each of these molecules a BF3 b HZCO C NH3 15 What are the electron pair and molecular geometries for S02 Ch 14 Material 1 Draw the Molecular Orbital MO diagram for the following homonuclear molecules a F2quot b Negquot c Begquot d Li e N2 f B22quot 2 For the homonuclear molecules above a f label whether they are paramagnetic or diamagnetic 3 For the homonuclear molecules above a f calculate the bond order and decide whether each one would be stable or not 4 What is the relative relationship between bond order bond length and bond strength 5 Consider the following data for these homonuclear diatomic species H2 Hf F2 Ff Bond energy 522 642 785 710 kJmo Bond length 121 115 110 117 pm of valence 2 1 14 13 electrons Removing an electron from H2 causes an increase in the bond energy of the resulting ion whereas removing an electron from F2 causes a decrease in the resulting ion Explain these differences by using MO diagrams 6 Respond to the following statements with either True or False If False explain why a Electrons are shared equally by heteronuclear bonds b The purpose of hybridization in molecules is to maximize electron repulsion j c Atoms in a molecule adjust their orbitals through hybridization in order for the molecule to have a structure with minimum energy j The hybridization for a molecule with the notation AX5 would be sp6d j There are 4 hybridized orbitals in a molecule with the configuration of sp3 Sigma bonding only occurs in central atoms with single bonds j The bond order value differs depends on which MO diagram is used the one for B C N or the one for O F j h The type of magnetism is affected by which MO diagram is used the one for B C N or for O F quot 7 What are some of the major limitations to using the Localized Electron LE model 8 What type of bonding would result from each of these two orbital interactions 9 What is this type of mixing called Draw the result of the mixture for each the shaded regions are negatively charged and the white regions are positively charged 88 88 10 How many sigma andor pi bonds are present in the highlighted atom in the molecules below 8 Label the sigma and pi bonds if any in this molecular bonding structure and explain the difference between the two bonding types
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