Inorganic Chemistry
5th Edition
ISBN: 9781292134147
Author: Housecroft, Catherine E.
Publisher: Pearson,
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Chapter 11, Problem 13P
Interpretation Introduction
To Construct: The approximate MO diagrams for [O2]- and [O2]2- and confirm that [O2]- is paramagnetic, while [O2]2- is diamagnetic.
Concept Introduction: A molecular orbital energy level diagram is a qualitative descriptive tool explaining
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Chapter 11 Solutions
Inorganic Chemistry
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- Explain how many unpaired electrons a tetrahedral d4 ion will have.arrow_forwardDraw the MO diagram for Trihydridoboron. Which orbital on boron is completely nonbonding? Explain why. Using character tables and their corresponding orbital shapes, draw the H3 group orbitals and how they bond/nonbond to boron.arrow_forwardWhat information do we need to predict the bond order and magnetism of CO+? Group of answer choices the total number of valence electrons the Lewis structure of CO+ the total number of protons the molecular orbitals for 2s and 2parrow_forward
- The photoelectron spectrum of CO has four major peaks with ionization energies of 14.5, 17.2, 20.1, and 38.3 eV. Assign these peaks of molecular orbitals of CO, and prepare a quantitative energy level correlation diagram for CO. The ionization energy of carbon atoms is 11.26 eV, and the ionization energy of oxygen atoms is 13.62 eV.arrow_forwardWhat information do we need to predict the bond order and magnetism of CO+? Group of answer choices the Lewis structure of CO+ the total number of protons the molecular orbitals for 2s and 2p the total number of valence electronsarrow_forwardComplete the MO diagram to determine if BN is paramagnetic or diamagnetic.arrow_forward
- Sketch the geometry of (a) tans-[Cu(Br)2(H2O)4] (b) [Zn(OH)2I22-](tetrahedral) (c) [Pt(NH3)42+](square planar) (d) cis-[Ni(H2O)2(C2O4]22- (e) [Au(CN)(NH3)]arrow_forwardSketch the geometry of (a) [Zn(NH3)2Cl2](tetrahedral) (b) cis-[Co(H2O)4Cl2]+ (c) tans-[Pt(NH3)2Br2]2+ (d) tans-[Ni(ox)2(OH)2]3- (e) [Au(CN)Br]+arrow_forwardUsing an MO energy-level diagram, would you expect F2 to have a lower or higher first ionization energy than atomic fluorine? Why?arrow_forward
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