Understanding Molecular Shapes and VSEPR Theory

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21 Terms

1
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What do Lewis structures represent?

Lewis structures show the structure of molecules in two dimensions (flat).

2
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What is the actual shape of molecules in three dimensions?

Molecules take on a tetrahedral shape in three dimensions.

3
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What theory explains why molecules have three-dimensional shapes?

Valence Shell Electron Pair Repulsion (VSEPR) theory.

4
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What is the principle behind VSEPR theory?

Electron pairs repel one another, causing molecules to adjust their shapes to maximize distance between valence electron pairs.

5
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What types of electron pairs are considered in VSEPR theory?

Both bonding pairs (used in bonds) and non-bonding pairs (lone pairs not used in bonding) are considered.

6
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How do you determine the shape of a molecule using VSEPR theory?

Draw the electron dot or structural formula, count bonding and non-bonding pairs around the central atom, and apply the predicted geometry.

7
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What is the bond angle in a linear molecular shape?

180°.

8
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Give an example of a linear molecule.

Carbon dioxide (CO2) is an example of a linear molecule.

<p>Carbon dioxide (CO2) is an example of a linear molecule.</p>
9
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What is the bond angle in a bent molecular shape?

Approximately 104.4°.

10
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Give an example of a bent molecule.

Water (H2O) is an example of a bent molecule.

<p>Water (H2O) is an example of a bent molecule.</p>
11
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What is the bond angle in a tetrahedral molecular shape?

Approximately 109.5°.

12
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Give an example of a tetrahedral molecule.

Methane (CH4) is an example of a tetrahedral molecule.

<p>Methane (CH4) is an example of a tetrahedral molecule.</p>
13
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What is the bond angle in a pyramidal molecular shape?

Approximately 107.3°.

14
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Give an example of a pyramidal molecule.

Ammonia (NH3) is an example of a pyramidal molecule.

<p>Ammonia (NH3) is an example of a pyramidal molecule.</p>
15
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What is the bond angle in a trigonal planar molecular shape?

Approximately 120°.

16
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Give an example of a trigonal planar molecule.

Nitrate (NO3) is an example of a trigonal planar molecule.

<p>Nitrate (NO3) is an example of a trigonal planar molecule.</p>
17
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What does VSEPR theory assume about electron pairs?

VSEPR theory assumes that electron pairs will be spaced out as far apart as possible due to repulsion.

18
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What is a bonding pair of electrons?

A bonding pair of electrons is an electron pair used in a bond.

19
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What is a non-bonding pair of electrons?

A non-bonding pair of electrons is a lone pair of electrons not used in bonding.

20
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How are multiple bonds counted in VSEPR theory?

Multiple bonds (double, triple) count as one 'location' or 'region' for electron pairs.

21
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What is the significance of electron pair repulsion in molecular geometry?

Electron pair repulsion influences the shape of the molecule, leading to specific geometries.