12. Molecular Shapes & Valence Bond Theory

MO Theory: Heteronuclear Diatomic Molecules

Molecular Orbital Theory and sp Orbital Mixing

MO Theory: Heteronuclear Diatomic Molecules Concept 1

Apply Molecular Orbital Theory to determine the MO orbital diagram for the CF+ ion.<img class="fr-dib"src="https://lightcat-files.s3.amazonaws.com/problem_images/00c854cd5aad45c0-1608581668415.jpg"style="width:300px;">

(σ2s)2(σ*2s)2(π2p)4

(σ2s)2(σ*2s)2(π2p)4(σ2p)2(π*2p)4

(σ2s)2(σ*2s)2(π2p)2(σ2p)2

(σ2s)2(σ*2s)2(π2p)2(σ2p)1(π*2p)2(σ*2p)1

Using a MO diagram, write the electron configuration for the BN molecule?&nbsp;<img class="fr-dib"src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/364031de"style="width:300px;">

Molecular Orbital Diagram for Nitric Oxide Heteronuclear molecule

MO Theory: Heteronuclear Diatomic Molecules Example 1

Molecular Orbital Diagrams of Heteronuclear Diatomics

Molecular Orbital Diagrams Heteronuclear Diatomic HF

MO Diagram #3 - CN-

Carbon monoxide is produced by incomplete combustion of 
fossil fuels. 
(a) Give the electron configuration for the valence molecular 
orbitals of CO. The orbitals have the same energy 
order as those of the N2 molecule.

Cyclooctatetraene dianion, C8H8 
2-, is an organic ion with the 
structure shown. Considering only the p bonds and not the 
s bonds, cyclooctatetraene dianion can be described by 
the following energy diagrams of its p molecular orbitals: 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/e1ec4a60b8ddb4b8-1670535636855.jpg" alt="" /> 
(c) Complete the MO energy diagram by assigning the appropriate 
numbers of p electrons to the various molecular 
orbitals, indicating the electrons using up/down arrows 1c T2.

a) Using only the valence atomic orbitals of a hydrogen
atom and a fluorine atom, and following the model of
Figure 9.46, how many MOs would you expect for the HF
molecule? <img src="https://lightcat-files.s3.amazonaws.com/problem_images/9ddfe888634cf451-1661275668435.jpg" alt="" />

The iodine bromide molecule, IBr, is an interhalogen compound.
Assume that the molecular orbitals of IBr are analogous to
the homonuclear diatomic molecule F2. (a) Which valence
atomic orbitals of I and of Br are used to construct the MOs of IBr?

Determine the electron configurations for CN+, CN, and 
CN-. (b) Which species, if any, has unpaired electrons?

Molecular Orbital Theory Heteronuclear Diatomic (Cyanide, CN-) Example

Introduction to Molecular Orbital Theory

Carbon monoxide, CO, is isoelectronic to N2. (d) Would you expect
the p2p MOs of CO to have equal atomic orbital contributions
from the C and O atoms? If not, which atom would
have the greater contribution?

The iodine bromide molecule, IBr, is an interhalogen compound. 
Assume that the molecular orbitals of IBr are analogous to 
the homonuclear diatomic molecule F2. (c) One of 
the valence MOs of IBr is sketched here. Why are the atomic 
orbital contributions to this MO different in size? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/1061864693109cf4-1664543480748.jpg" alt="" />

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1. Intro to General Chemistry

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[BOOK CHEM] Clutch Version

MO Theory: Homonuclear Diatomic Molecules

Homonuclear Diatomic Molecules are composed of 2 identical elements bonded together.

Equatorial and Axial Positions

Covalent compounds with 5 or 6&nbsp;electron groups have equatorial and axial positions for surrounding elements

Heteronuclear Diatomic Molecules are composed of 2 different elements bonded together.

Bond Angles

Bond Angles&nbsp;result from surrounding elements and lone pairs around the central element positioning themselves at an optimal distance.&nbsp;

Molecular Orbital Theory

Molecular Orbital Theory&nbsp;allows us to predict the distribution of electrons within a molecule.&nbsp;

MO Theory: Bond Order

Molecular Orbital Diagrams can be used to determine the bond order of a molecule.

Electron Geometry

The simplest system for geometrical shapes that focuses on the number of electron groups around the central atom.

Hybridization

How would an&nbsp;s orbital combine with a p orbital to form a covalent bond? The answer is through hybridization where a hybrid&nbsp;oribital is formed.&nbsp;

Molecular Geometry

True Shape of Molecules that takes into account differences&nbsp;in repulsion between lone pairs and surrounding elements.

Valence Shell Electron Pair Repulsion Theory

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