Questions and Answers
What does VSEPR stand for?
Valence Shell Electron Pair Repulsion Theory
What is VSEPR Theory?
The shape of a molecule is determined by the repulsion of electron pairs.
Steps for using VSEPR Theory include drawing a Lewis dot diagram, predicting the geometry around the central atom, and naming the molecular shape.
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You can also predict _______ _______ and _____________ ________ by using VSEPR Theory.
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What is the definition of 'domain' in VSEPR Theory?
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What does 'lone pair' mean in the context of VSEPR Theory?
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What is the definition of a 'bonding pair'?
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What is the molecular geometry of a linear arrangement?
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What defines a trigonal planar shape?
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Which of the following describes a bent molecular shape?
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What is the bond angle in a tetrahedral molecular shape?
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Describe the trigonal pyramidal shape.
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What does the term 'trigonal bipyramidal' refer to?
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What is the characteristic of an octahedral molecular shape?
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Study Notes
VSEPR Theory Overview
- VSEPR stands for Valence Shell Electron Pair Repulsion Theory, which predicts molecular shapes based on electron pair interactions.
- The geometry of a molecule is influenced by the repulsion between electron pairs surrounding the central atom.
Steps to Utilize VSEPR Theory
- Begin by drawing a Lewis dot diagram to visualize electron distribution.
- Predict the molecular geometry around the central atom based on the arrangement of electron pairs.
- Identify and name the molecular shape derived from this arrangement.
Predicting Molecular Properties
- VSEPR Theory can also indicate bond angles and the overall polarity of the molecule.
Important Definitions
- Domain: Refers to any electron pair, including both bonding pairs and non-bonding (lone pairs).
- Lone Pair: An unshared, non-bonding pair of electrons.
- Bonding Pair: A shared pair of electrons involved in chemical bonds.
Molecular Shapes and Their Properties
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Linear:
- Comprises 2 domains (both bonding pairs).
- Bond angle is 180 degrees, as pairs repel from each other directly opposite.
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Trigonal Planar:
- Contains 3 domains (all bonding pairs).
- Bond angle of 120 degrees, where pairs repel equally in a plane.
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Bent:
- Has 3 domains (2 bonding pairs and 1 lone pair).
- Bonding pairs are pushed apart by the lone pair, creating a bent shape.
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Bent/V-shaped:
- Features 4 domains (2 bonding pairs and 2 lone pairs).
- Bond angle is compressed due to lone pairs forcing bonding pairs closer together.
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Tetrahedral:
- Consists of 4 domains (all bonding pairs).
- Each pair has a bond angle of 109.5 degrees due to equal repulsion.
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Trigonal Pyramidal:
- Contains 4 domains (3 bonding pairs and 1 lone pair).
- The lone pair pushes the bonds downward, affecting angles.
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Trigonal Bipyramidal:
- Comprises 5 bonding pairs.
- Three pairs are positioned in a plane at 120 degrees, and the other two pairs are in axial positions at 180 and 90 degrees relative to the plane.
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Octahedral:
- Features 6 bonding pairs.
- Equal repulsion among pairs results in bond angles of 90 degrees among all pairs.
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Description
This quiz focuses on the Valence Shell Electron Pair Repulsion (VSEPR) Theory, which explains how the shape of molecules is influenced by the repulsion between electron pairs. Utilize these flashcards to familiarize yourself with key terms and concepts related to molecular geometry and predictions. Perfect for chemistry students looking to enhance their understanding of molecular shapes.
