Ch.10 - Molecular Shapes & Valence Bond TheoryWorksheetSee 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

Solution: Use the molecular orbital diagram shown to determine which of the following is most stable.A) N22+ B) B2C) B22+D) C22-E) C22+ 

Solution: Use the molecular orbital diagram shown to determine which of the following is most stable.A) N22+ B) B2C) B22+D) C22-E) C22+ 

Problem

Use the molecular orbital diagram shown to determine which of the following is most stable.

A) N22+ 

B) B2

C) B22+

D) C22-

E) C22+

 

Solution

We’re being asked which species is the most stable. For this, we need to determine the bond order for each species. The bond order tells us the stability of a bonda higher bond order means the bond is more stable.


Step 1: Calculate the total number of valence electrons present.

Step 2: Draw the molecular orbital diagram.

Step 3: Calculate the bond order of the molecule/ion. Recall that the formula for bond order is:



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