
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Research the molecular orbitals formed by the overlap of d orbitals with s and p orbitals. Draw diagrams to show how the d atomic orbitals overlap with s and p orbitals to form sigma and pi molecular orbitals
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What type of molecular orbital would result from the in-phase combination of the two dxz atomic orbitals shown below? Assume the x-axis is the internuclear axis.
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Bromine forms a number of oxides of varying stability. (a) One oxide has 90.90% Br and 9.10% O. Assuming its empirical and molecular formulas are the same, draw a Lewis structure of the molecule and specify the hybridization of the central atom (O). (b) Another oxide is unstable BrO. Assuming the molecular orbital diagram in Figure 9. 16 applies to BrO, write its electron configuration (where Br uses 45 and 4p orbitals). What is the highest occupied molecular orbital (HOMO) for the molecule?
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If molecular orbitals are created by combining five atomic orbitals from atom A and five atomic orbitals from atom B combine, how many molecular orbitals will result?
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Describe the bonding in NO+, NO, and NO, using both the localized electron and molecular orbital models. Account for any discrepancies between the two models.
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Consider the bonding in nitrate ion, NO3. First draw resonance formulas of this ion. Now describe the bonding of this ion in terms of molecular orbitals. (Refer to the delocalized bonding of the ozone molecule described in the text.) Suppose each atom uses sp2 hybrid orbitals. How many molecular orbitals can you form from the 2p orbitals that remain on these atoms? How many of these orbitals will be occupied?
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Show how a dxz. atomic orbital and a pz, atomic orbital combine to form a bonding molecular orbital. Assume the x-axis is the internuclear axis. Is a or a molecular orbital formed? Explain.
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Consider the following molecular orbitals formed from the combination of two hydrogen 1s orbitals: a. Which is the bonding molecular orbital and which is the antibonding molecular orbital? Explain how you can tell by looking at their shapes. b. Which of the two molecular orbitals is lower in energy? Why is this true?
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True or false: Boron contains 2s22p1 valence electrons, so only one p orbital is needed to form molecular orbitals.
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1. Consider the bonding of two boron atoms using MO theory. How many bonds will form based on the filling of its molecular orbitals? 2.T/F p orbitals always interact to form Pi or Pi* orbitals.
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Draw diagrams to show how the d atomic orbitals overlap with s and p orbitals to form s and p molecular orbitals
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Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because __________.
the bond order can be shown to be equal to 1.
there are more electrons in the bonding orbitals than in the antibonding orbitals.
. all electrons in the MO electron configuration are paired.
the energy of the π2p MOs is higher than that of the σ2p MO
the bond enthalpy is very low
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Two p orbitals from one atom and two p orbitals from another atom are combined to form molecular orbitals for the joined atoms. How many MOs will result from this combination? Explain.
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