VSEPR

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chapter 8

chapter 8

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21 Terms

1
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AB

Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 1 | Lone pairs: 0 | Bond angle: 180° | Example: H₂

<p>Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 1 | Lone pairs: 0 | Bond angle: 180° | Example: H₂</p>
2
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AB2

Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 2 | Lone pairs: 0 | Bond angle: 180° | Example: CO₂

<p>Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 2 | Lone pairs: 0 | Bond angle: 180° | Example: CO₂</p>
3
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ABE

Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 1 | Lone pairs: 1 | Bond angle: 180° | Example: CN⁻

<p>Molecular shape: Linear | Electron geometry: Linear | Bonded atoms: 1 | Lone pairs: 1 | Bond angle: 180° | Example: CN⁻</p>
4
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AB3

Molecular shape: Trigonal planar | Electron geometry: Trigonal planar | Bonded atoms: 3 | Lone pairs: 0 | Bond angle: 120° | Example: AlBr3

<p>Molecular shape: Trigonal planar | Electron geometry: Trigonal planar | Bonded atoms: 3 | Lone pairs: 0 | Bond angle: 120° | Example: AlBr3</p>
5
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AB2E

Molecular shape: Bent | Electron geometry: Trigonal planar | Bonded atoms: 2 | Lone pairs: 1 | Bond angle: 120° | Example: SnCl₂

<p>Molecular shape: Bent | Electron geometry: Trigonal planar | Bonded atoms: 2 | Lone pairs: 1 | Bond angle: 120° | Example: SnCl₂</p>
6
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ABE2

Molecular shape: linear | Electron geometry: Trigonal planar | Bonded atoms: 1| Lone pairs: 2 | Bond angle: 120° | Example: O₂

<p>Molecular shape: linear | Electron geometry: Trigonal planar | Bonded atoms: 1| Lone pairs: 2 | Bond angle: 120° | Example: O₂</p>
7
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AB4

Molecular shape: Tetrahedral | Electron geometry: Tetrahedral | Bonded atoms: 4 | Lone pairs: 0 | Bond angle: 109.5° | Example: SiCl4

<p>Molecular shape: Tetrahedral | Electron geometry: Tetrahedral | Bonded atoms: 4 | Lone pairs: 0 | Bond angle: 109.5° | Example: SiCl4</p>
8
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AB3E

Molecular shape: Trigonal pyramid | Electron geometry: Tetrahedral | Bonded atoms: 3 | Lone pairs: 1 | Bond angle: 109.5°| Example: PH₃

<p>Molecular shape: Trigonal pyramid | Electron geometry: Tetrahedral | Bonded atoms: 3 | Lone pairs: 1 | Bond angle: 109.5°| Example: PH₃</p>
9
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AB2E2

Molecular shape: Bent | Electron geometry: Tetrahedral | Bonded atoms: 2 | Lone pairs: 2 | Bond angle: 109.5° | Example: SeBr2

<p>Molecular shape: Bent | Electron geometry: Tetrahedral | Bonded atoms: 2 | Lone pairs: 2 | Bond angle: 109.5° | Example: SeBr2</p>
10
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ABE3

Molecular shape: linear | Electron geometry: Tetrahedral | Bonded atoms: 1 | Lone pairs: 3 | Bond angle: 109.5°| Example: Cl2

<p>Molecular shape: linear | Electron geometry: Tetrahedral | Bonded atoms: 1 | Lone pairs: 3 | Bond angle: 109.5°| Example: Cl2</p>
11
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AB5

Molecular shape: Trigonal bipyramidal | Electron geometry: Trigonal bipyramidal | Bonded atoms: 5 | Lone pairs: 0 | Bond angle: 90° and 120° | Example: AsF₅

<p>Molecular shape: Trigonal bipyramidal | Electron geometry: Trigonal bipyramidal | Bonded atoms: 5 | Lone pairs: 0 | Bond angle: 90° and 120° | Example: AsF₅</p>
12
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AB4E

Molecular shape: See-Saw | Electron geometry: Trigonal bipyramidal | Bonded atoms: 4 | Lone pairs: 1 | Bond angle: 90° and 120° | Example: SeH₄

<p>Molecular shape: See-Saw | Electron geometry: Trigonal bipyramidal | Bonded atoms: 4 | Lone pairs: 1 | Bond angle: 90° and 120° | Example: SeH₄</p>
13
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AB3E2

Molecular shape: T-shape | Electron geometry: Trigonal bipyramidal | Bonded atoms: 3 | Lone pairs: 2 | Bond angle: 90° and 120° | Example: ICl₃

<p>Molecular shape: T-shape | Electron geometry: Trigonal bipyramidal | Bonded atoms: 3 | Lone pairs: 2 | Bond angle: 90° and 120° | Example: ICl₃</p>
14
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AB2E3

Molecular shape: Linear | Electron geometry: Trigonal bipyramidal | Bonded atoms: 2 | Lone pairs: 3 | Bond angle: 180° | Example: BrF₂⁻

<p>Molecular shape: Linear | Electron geometry: Trigonal bipyramidal | Bonded atoms: 2 | Lone pairs: 3 | Bond angle: 180° | Example: BrF₂⁻</p>
15
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AB6

Molecular shape: Octahedral | Electron geometry: Octahedral | Bonded atoms: 6 | Lone pairs: 0 | Bond angle: 90° | Example: SeCl₆

<p>Molecular shape: Octahedral | Electron geometry: Octahedral | Bonded atoms: 6 | Lone pairs: 0 | Bond angle: 90° | Example: SeCl₆</p>
16
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AB5E

Molecular shape: Square pyramidal | Electron geometry: Octahedral | Bonded atoms: 5 | Lone pairs: 1 | Bond angle: 90° | Example: IF₅

<p>Molecular shape: Square pyramidal | Electron geometry: Octahedral | Bonded atoms: 5 | Lone pairs: 1 | Bond angle: 90° | Example: IF₅</p>
17
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AB4E2

Molecular shape: Square planar | Electron geometry: Octahedral | Bonded atoms: 4 | Lone pairs: 2 | Bond angle: 90° | Example: XeF₄

<p>Molecular shape: Square planar | Electron geometry: Octahedral | Bonded atoms: 4 | Lone pairs: 2 | Bond angle: 90° | Example: XeF₄</p>
18
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ABE, ABE₃, ABE₄, ABE₅

There are no stable ABE, ABE₃, ABE₄, or ABE₅ molecules.

19
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Bond representation

All bonds are represented as a line whether the bond is single, double, or triple.

20
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Bonding domains

Any atom bonded to the center atom counts as one domain, even if bonded by a double or triple bond.

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Domain count rule

The number of bonded atoms plus lone pairs always adds up to the total number of domains.