Ch.10 - Molecular Shapes & Valence Bond TheorySee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Molecular Orbital Diagrams

molecular orbital diagram explains chemical bonds within molecules based on the union of atomic orbials. 

Concept #1: A heteronuclear diatomic molecule is composed of two different elements covalently bonded together.

Concept #2: There are some key similarities and differences when comparing heteronuclear and homonuclear diatomic molecules. 

Example #1: Using your knowledge of molecular orbital diagrams, determine the bond order of the NO- ion. 

Additional Problems
Which of the following mixtures of atomic orbitals best describes the σ bonding orbitals in HeH+?   a. s + s b. s – s c. pz + pz d. px – pz e. px + py
Use the molecular orbital energy diagram below for the next three questions. How many unpaired electrons are in O 2+? a. 0       b. 1       c. 2       d. 3     What is the bond order of OF? a. 0       b. ½       c. 1       d. 1 ½       e. 2     Which of the following is not paramagnetic? a. O 2+       b. OF       c. NO       d. OF –       e. CO+
Utilize the molecular orbital diagram below to answer the following questions.   How many electrons are present in antibonding molecular orbitals?  (a) 2     (b) 4     (c) 6     (d) 8     (e) 10   What is the bond order for the molecule? (a) 3     (b) 2.5     (c) 2     (d) 1.5     (e) 1   What is the most likely formula for the molecule represented in the molecular orbital diagram? (a) O22−     (b) ONe     (c) ONe +     (d) OF     (e) OF +    
Use the molecular orbital diagram to figure out the electronic configuration for CN. Which of the following statements is correct? a) CN is diamagnetic. b) CN− is paramagnetic. c) If an electron is removed to give CN+, the bond order increases. d) The π*2p orbital is the highest energy orbital containing an electron in CN e) If an electron is added to give CN−, the bond length decreases.  
Complete this molecular orbital diagram for CN– then determine the bond order. Note that the 1s orbital is not shown in this problem.
Which of the following is false?a. KCl is a heteronuclear diatomic moleculeb. H2S is called hydrogen sulfide as a molecule and called hydrosulfuric acid as an acidc. HCl is called hydrogen chloride as a molecule and called hydrochloric acid as an acidd. H2 is a homonuclear diatomic molecule but is not a compounde. NO2 is called nitrogen dioxide and N2O is called dinitrogen monoxidef. H2O is a heteronuclear polyatomic molecule and also a compoundg. HCl is a heteronuclear diatomic molecule and also a compound
The nitric oxide molecule, NO, readily loses one electron to form the NO + ion. Why is this consistent with the electronic structure of NO?
Complete this molecular orbital diagram for CN– then determine the bond order. Note that the 1s orbital is not shown in this problem.
Is CO paramagnetic or diamagnetic?
If CO gained one election, becoming CO -, would the bond become weaker or stronger?