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: Predict the shape, state the hybridization of the central atom, and give the ideal bond angle(s) and any expected deviations for IF4+.

Solution: Predict the shape, state the hybridization of the central atom, and give the ideal bond angle(s) and any expected deviations for IF4+.

Problem

Predict the shape, state the hybridization of the central atom, and give the ideal bond angle(s) and any expected deviations for IF4+.

Solution

In writing Lewis structures, we place the least electronegative element in the center because it can better share its electrons and form bonds than more electronegative elements.

Iodine (EN = 2.66) is less electronegative than fluorine (EN = 3.98) so iodine goes in the center of the Lewis structure. Since iodine belongs to Period 5, we can use an expanded octet to accommodate more F atoms in the molecule.

The Lewis structure for IF4+ is:

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