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: Compared to the H−H bond in H 2, the H−H bond in H 2− is expected to be which of the following?a. longer and strongerb. longer and weakerc. shorter and weakerd. shorter and strongere. the same length


Compared to the H−H bond in H 2, the H−H bond in H 2 is expected to be which of the following?

a. longer and stronger

b. longer and weaker

c. shorter and weaker

d. shorter and stronger

e. the same length and strength


We’re being asked to compare the H–H bond in H2 and in H2. For this, we need to determine the bond order for each species. The bond order tells us the strength and length of a bonda higher bond order means the bond is stronger and shorter.

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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