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: How would you expect the H - X - H bond angle to vary in the series H2O, H2S, H2Se ? (Hint: The size of an electron pair domain depends in part on the electronegativity of the central atom.)

Problem

How would you expect the H - X - H bond angle to vary in the series H2O, H2S, H2Se ? (Hint: The size of an electron pair domain depends in part on the electronegativity of the central atom.)

Solution

We have to explain how the H–X–H bond angle varies in the series H2O, H2S, H2Se.


Oxygen, sulfur and selenium all belong to the 6A group of the periodic table. We will follow these steps to solve this problem:

Step 1: Draw a generic Lewis structure for a group 6A element.

Step 2: Explain the trend of electronegativity for O, S and Se.

Step 3: Link bond angles to the drawn structure.

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