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Updated Mar 28, 2026

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Fun with VSEPR Theory: Molecule Shapes & Bond Angles Explained!

aurumm

@aurxm

VSEPR theory explains molecular shapes based on electron pair repulsions.... Show more

Shapes of molecules.
VSEPR-Valance shell electron pair repulsion.
• Each pair of electrons around on atom will repel each other
• Thee pairs

Shapes of Molecules and VSEPR Theory

The Valence Shell Electron Pair Repulsion (VSEPR) theory explains how molecules adopt different shapes based on the arrangement of electron pairs around the central atom. This theory is fundamental in understanding molecular geometry and bond angles.

Definition: VSEPR stands for Valence Shell Electron Pair Repulsion, a theory that predicts molecular shapes based on the repulsion between electron pairs.

The key principles of VSEPR theory are:

Electron pairs around an atom repel each other.
These pairs position themselves as far apart as possible to minimize repulsion and achieve the most stable arrangement.
Lone pairs of electrons exert stronger repulsion than bonding pairs.

Highlight: Lone pairs have a significant impact on molecular geometry, often leading to decreased bond angles due to increased repulsion.

The document outlines several molecular shapes predicted by VSEPR theory:

Linear: 2 electron pairs, 180° bond angle (e.g., BeCl₂)
Trigonal Planar: 3 electron pairs, 120° bond angle (e.g., BF₃)
Tetrahedral: 4 electron pairs, 109.5° bond angle (e.g., CH₄)
Trigonal Bipyramidal: 5 electron pairs, 90° and 120° bond angles (e.g., PCl₅)
Octahedral: 6 electron pairs, 90° bond angles (e.g., SF₆)

Example: In a water molecule (H₂O), the presence of two lone pairs on the oxygen atom causes the H-O-H bond angle to decrease from the ideal tetrahedral angle of 109.5° to approximately 104.5°.

The document also discusses variations of these basic shapes:

Bent: Based on tetrahedral geometry with 2 bonding pairs and 2 lone pairs (e.g., H₂O)
Pyramidal: Based on tetrahedral geometry with 3 bonding pairs and 1 lone pair (e.g., NH₃)
Square Planar: Based on octahedral geometry with 4 bonding pairs and 2 lone pairs
Distorted Square Pyramidal: Based on octahedral geometry with 5 bonding pairs and 1 lone pair

Vocabulary: Bond angle - the angle formed between two adjacent bonds in a molecule.

Understanding these shapes and the principles behind them is crucial for predicting molecular properties and reactivity in chemistry. The VSEPR theory chart provided in the document serves as a valuable reference for students studying molecular geometry.

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Updated Mar 28, 2026

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1 page

Fun with VSEPR Theory: Molecule Shapes & Bond Angles Explained!

aurumm

@aurxm

VSEPR theory explains molecular shapes based on electron pair repulsions. Key concepts include:

Electron pairs repel each other, positioning themselves to minimize repulsion
Lone pairs exert stronger repulsion than bonding pairs
Molecular geometry is determined by the number and arrangement... Show more

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Shapes of Molecules and VSEPR Theory

Definition: VSEPR stands for Valence Shell Electron Pair Repulsion, a theory that predicts molecular shapes based on the repulsion between electron pairs.

The key principles of VSEPR theory are:

Electron pairs around an atom repel each other.
These pairs position themselves as far apart as possible to minimize repulsion and achieve the most stable arrangement.
Lone pairs of electrons exert stronger repulsion than bonding pairs.

Highlight: Lone pairs have a significant impact on molecular geometry, often leading to decreased bond angles due to increased repulsion.

The document outlines several molecular shapes predicted by VSEPR theory:

Linear: 2 electron pairs, 180° bond angle (e.g., BeCl₂)
Trigonal Planar: 3 electron pairs, 120° bond angle (e.g., BF₃)
Tetrahedral: 4 electron pairs, 109.5° bond angle (e.g., CH₄)
Trigonal Bipyramidal: 5 electron pairs, 90° and 120° bond angles (e.g., PCl₅)
Octahedral: 6 electron pairs, 90° bond angles (e.g., SF₆)

Example: In a water molecule (H₂O), the presence of two lone pairs on the oxygen atom causes the H-O-H bond angle to decrease from the ideal tetrahedral angle of 109.5° to approximately 104.5°.

The document also discusses variations of these basic shapes:

Bent: Based on tetrahedral geometry with 2 bonding pairs and 2 lone pairs (e.g., H₂O)
Pyramidal: Based on tetrahedral geometry with 3 bonding pairs and 1 lone pair (e.g., NH₃)
Square Planar: Based on octahedral geometry with 4 bonding pairs and 2 lone pairs
Distorted Square Pyramidal: Based on octahedral geometry with 5 bonding pairs and 1 lone pair

Vocabulary: Bond angle - the angle formed between two adjacent bonds in a molecule.