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VSEPR Theory Flashcards
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VSEPR Theory Flashcards

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Questions and Answers

What does the acronym VSEPR stand for?

Valence-shell electron-pair repulsion theory

What is the VSEPR Model used for?

To explain the 3-dimensional shape of molecules

What does VSEPR Theory state about molecular shapes?

The repulsion between electron pairs causes molecular shapes to adjust so that the valence-electron pairs stay as far away as possible.

What is an unshared pair?

<p>Strongly repels the bonding pairs, pushing them together.</p> Signup and view all the answers

Describe a linear pair in terms of molecular geometry.

<p>Drawn in a straight line, angle 180, one central, 2 peripheral electrons.</p> Signup and view all the answers

What is a Trigonal Planar arrangement?

<p>One central and 3 peripheral atoms on a plane, angle 120.</p> Signup and view all the answers

What characterizes a Tetrahedral arrangement?

<p>One central and 4 peripheral atoms, angle 109.5.</p> Signup and view all the answers

What happens in a Tetrahedral arrangement with 1 pair of unshared electrons?

<p>One central, 4 peripheral, 1 pair unshared electrons; forms trigonal pyramidal with angle 107.</p> Signup and view all the answers

How does a Tetrahedral arrangement with 2 pairs of unshared electrons differ?

<p>One central, 4 peripheral, 2 pairs unshared electrons; known as a bent angle 104.5.</p> Signup and view all the answers

What defines a Trigonal Bipyramidal arrangement?

<p>One central, 5 peripheral; angles are 120 on the plane &amp; 90 vertical.</p> Signup and view all the answers

Study Notes

VSEPR Theory Overview

  • VSEPR stands for valence-shell electron-pair repulsion theory.
  • The theory describes how the arrangement of electron pairs around a central atom determines the shape of a molecule.

VSEPR Model

  • The model provides a framework for predicting the three-dimensional structure of molecules based on electron pair repulsion.

Molecular Shape Determination

  • VSEPR theory emphasizes that electron pairs (bonding and lone pairs) repel each other, leading to the arrangement that maximizes their distance from each other.

Unshared Pairs

  • Unshared (lone) electron pairs exert stronger repulsion than bonded pairs, influencing molecular geometry significantly by pushing bonding pairs closer together.

Linear Geometry

  • A linear molecular shape consists of a central atom with two peripheral atoms, forming a straight line with a bond angle of 180 degrees.

Trigonal Planar Geometry

  • In a trigonal planar arrangement, one central atom is bonded to three peripheral atoms, arranged in a plane with a bond angle of 120 degrees.

Tetrahedral Geometry

  • A tetrahedral shape features one central atom bonded to four peripheral atoms, with a bond angle of 109.5 degrees.

Trigonal Pyramidal Geometry

  • A trigonal pyramidal shape occurs when one of the four pairs of electrons in a tetrahedral arrangement is a lone pair. This causes the angle between the peripheral atoms to be about 107 degrees.

Bent Geometry

  • In cases with two lone pairs, the shape becomes bent with a bond angle of approximately 104.5 degrees, derived from a tetrahedral structure.

Trigonal Bipyramidal Geometry

  • A trigonal bipyramidal arrangement consists of a central atom bonded to five peripheral atoms, with bond angles of 120 degrees in the equatorial plane and 90 degrees in the axial positions.

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Test your understanding of VSEPR theory with these flashcards. Each card provides key definitions and concepts related to valence-shell electron-pair repulsion theory and molecular shapes. Perfect for students studying chemistry!

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