a) Which orbital is HOMO (Highest occupied)? b) Which orbital is LUMO (lowest unoccupied)? What do those MO look like? c) Paramagentic or diamagnetic d) What is the bond order - Will adding electrons increase or decrease the bond order? 2) Complete the MO for CO2+ 111 2p 2s TC O 11 T 1V 74 1114 2p 16 2s ned no

a) Which orbital is HOMO (Highest occupied)? b) Which orbital is LUMO (lowest unoccupied)? What do those MO look like? c) Paramagentic or diamagnetic d) What is the bond order - Will adding electrons increase or decrease the bond order? 2) Complete the MO for CO2+ 111 2p 2s TC O 11 T 1V 74 1114 2p 16 2s ned no

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter6: Quantum Mechanics And Molecular Structure

Section: Chapter Questions

Problem 17P

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Why do we hybtidize atomic orbitals to explain the bonding in covalent compounds? What type of bonds form from hybrid orbitals: sigma or pi? Explain.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) LiBe+ (b) CO+ (c) CN (d) OF Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
The molecular orbital diagram of NO shown in Figure 10.47 also applies to the following species. Write the molecular orbital electron configuration of each, indicating the bond order and the number of unpaired electrons. (a) CN (b) CO (c) BeB (d) BC+ Figure 10.47 Molecular orbital diagram for nitric oxide (NO). The molecular orbital diagram for NO predicts a bond order of 2.5 and predicts that the molecule is paramagnetic with one unpaired electron. These predictions are verified by experimental measurements.
Use MO diagrams and the bond orders you obtain from them to answer each of the following questions. (a) Is Be,* diamagnetic or paramagnetic? paramagnetic O diamagnetic (b) Is Bez+ stable? O unstable O stable (c) What is the outer (valence) electron configuration of 02? O (0 2,)?(0*25)?(0 2,)?(T 2p)²(T 2p)²(T*2,)²(T p)?(0*2p) O (0 2)?(0*29)?(02p)²(T 20)?(T 20)?(T*2p)?(T*2,)*(0*2p) O (0 25)'(0*25)?(o 2,)?(T 20)²(T 20)²(T*2p)²(T*2p)?(0*2») O (0 23)°(0*23)²(O 2p)?(T 20)?(T 20)²(T*2,)²(T 20)(0*20) O (0 25)?(0*25)²(O 2p)²(T 2p)²(T 2p)²(T*2p)²(0*2p)²(O 2p)
Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. diamagnetic or paramagnetic? molecule stable? bond order 믐 O yes diamagnetic H, ? no paramagnetic yes diamagnetic He, no paramagnetic yes O diamagnetic no paramagnetic
s Using the molecular orbital model, identify the correct (valence) electron configurations for the following diatomic species. O CN O N2 O CN OCN+ 02 A. (025)?(02s*)?(n2p)* B. (025)?(025*)?(02p)?(n2p)*(n2p*)3 c. (025) (02s*)?(n2p)*(02p)²(n2p*)! D. (025)?(02s*)?(n2p)*(02p)! E. (025)?(025*)?(n2p)*(02p)? F. (02s)2(02s*)?(02p)?(n2p)*(n2p*)? G. (025)?(02s*)?(02p)²(n2p)ª(n2p*)* 1 ar ec
4. How many unpaired electrons doe the cation B have? What's the bond order of the diatomic cation Bz*? Is B2* a stable species? Is it paramagnetic or diamagnetic? 5. What is the bonder order of Liz? Is it a stable diatomic molecule? Is it paramagnetic or diamagnetic?
a) Complete the molecular orbital electron energy level diagram for N, 2-. 2px. Py. Pz 2s a) What is the bond order in N,2? b) Which orbital is the HOMO? What is the other name for the HOMO in this case? c) Which orbital is the LUMO? d) Is N, paramagnetic or diamagnetic? Explain. e) What is the bond order for N,? Which species is more stable N, or N,? Explain.
Molecular Orbital Diagrams and Bond Order The blank molecular orbital diagram shown here (Figure 1) applies to the valence of diatomic lithium, beryllium, boron, carbon, or nitrogen. Bonding orbitals are marked with or π and antibonding orbitals with o* or *. Figure 2p CV 2p 1 of 1 What is the bond order of C₂? Express the bond order numerically. ▾ View Available Hint(s) ▶ ▶ Hint 2. Determine the number of valence electrons in C₂ ▸ Hint 3. Determine the number of bonding electrons Hint 4. Determine the number of antibonding electrons ▶ Hint 1. How to approach the problem 2 VE ΑΣΦ ↑ Submit B ? Previous Answers Request Answer * Incorrect; Try Again; 3 attempts remaining Check that you have filled the diagram correctly. Then double-check the numbers of bonding and antibonding electrons. You may want to review Hint 2. Determine the number of valence electrons in C₂_ Review | Ca
Use moiecuiar orbitai theory to determine the bond order of the F2* ion and if it is paramagnetic or diamagnetic. (The correct molecular orbital diagram for this ion is shown below.) Atomic orbitals Molecular orbitals Atomic orbitals 2p 2p 2s 2s O,, F2. Nez O 1.5 and paramagnetic 0.5 and paramagentic O 1 and diamagmetic O 1.5 and diamagnetic
What is the bond order of CO+? [(# bonding electrons - #anti-bonding electrons)/2]
Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: • Decide whether each molecule is stable or not. • Decide whether each molecule would be diamagnetic or paramagnetic. • Calculate each molecule's bond order. diamagnetic or paramagnetic? 믐 molecule stable? bond order yes O diamagnetic A N2 X. O no paramagnetic yes diamagnetic F paramagnetic yes O'diamagnetic Be, O no paramagnetic O O O