VESPR

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VESPR. Valence Electron Shared Pair Repulsion Atoms and non bonding pairs of electrons surrounding a central bond in such a way as to get as far away as possible from each other. VESPR. Valence Electron Shared Pair Repulsion - PowerPoint PPT Presentation

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VESPR

• Valence Electron Shared Pair Repulsion

• Atoms and non bonding pairs of electrons surrounding a central bond in such a way as to get as far away as possible from each other.

VESPR

• Valence Electron Shared Pair Repulsion

• Atoms and non bonding pairs of electrons surrounding a central bond in such a way as to get as far away as possible from each other.

VESPR

• Valence Electron Shared Pair Repulsion

• Atoms and non bonding pairs of electrons surrounding a central bond in such a way as to get as far away as possible from each other.

VESPR

• Valence Electron Shared Pair Repulsion

• Atoms and non bonding pairs of electrons surrounding a central bond in such a way as to get as far away as possible from each other.

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom if possible• Determine bond angles and bond shapes associated

with the central atoms

VESPR Rules

• Determine the number of valence electrons.• Single bond atoms to the central atom• Each bond accounts for two electrons• Double or triple bonds to the central atom if possible• If possible make the outer atoms octets by surrounding

them with the appropriate number of electrons.• If there are additional valence electrons available place

them on the central atom if possible• Determine bond angles and bond shapes associated

with the central atoms

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

Bond Angles Bond Shapes

Atoms NBPE Bond Angle Bond Shape

1 to 1 0 NA Linear

2 to 1 0 180 Linear

3 to 1 0 120 Trigonal planar

4 to 1 0 109.5 Tetrahedral

2 to 1 2 <109.5 Bent

3 to 1 1 <109.5 Pyrimidal

5 to 1 0 90/120 Trigonal Bipryimidal

6 to 1 0 90 Octahedral

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

HF

• H = 1 valence electron

• F = 7 valence electron

• H – F

• Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

CO2

• C=4 valence electrons = 4• O= 2 (6) valence electrons = 12• O-C-O 16 electrons• O=C=O• O=C=O 16 electrons• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 2 to 1, 0 NBPE, 180o, Linear

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete octet• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete 0 Nonbonding Pairs Electrons

• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete • 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete• 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

BF3

• B= 3 valence electrons = 3• F= 3 (7) valence electrons = 21• F B F 24 electrons• F• No Double Bonds Possible• F B F 24 electrons• F

• 6 surrounding central atom, incomplete • 0 Nonbonding Pairs Electrons• 3 to 1, 0 NBPE, 120o, trigonal planar

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

CCl4• C= 4 valence electrons = 4• Cl= 4 (7) valence electrons = 28• Cl 32 electrons• Cl C Cl • Cl No Double Bonds Possible• • Cl• Cl C Cl 32 electrons• Cl

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

NH3

• N= 5 valence electrons = 5• H= 3 (1) valence electrons = 3• H N H 8 electrons• H• No Double Bonds Possible• H N H 8 electrons• H

• 8 surrounding central atom, octet• 1 Nonbonding Pairs Electrons• 3 to 1, 1 NBPE, <109.5o, pyrimidal

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

H2O

• O= 6 valence electrons = 6• H= 2 (1) valence electrons = 2• H O H 8 electrons• • No Double Bonds Possible• H O 8 electrons• H

• 8 surrounding central atom, octet• 2 Nonbonding Pairs Electrons• 2 to 1, 2 NBPE, <109.5o, bent

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 8 surrounding central atom, octet• 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 10 surrounding central atom, expanded 0 Nonbonding Pairs Electrons

• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 10 surrounding central atom, expanded • 0 Nonbonding Pairs Electrons• 4 to 1, 0 NBPE, 109.5o, tetrahedral

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 10 surrounding central atom, expanded • 0 Nonbonding Pairs Electrons• 5 to 1, 0 NBPE, 900/1200 , trigonal bipyrimidal

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 10 surrounding central atom, expanded • 0 Nonbonding Pairs Electrons• 5 to 1, 0 NBPE, 900/1200 , trigonal bipyrimidal

PF5

• P= 5 valence electrons = 5• F= 5 (7) valence electrons = 35• F F 40 electrons• C F • F F No Double Bonds Possible• F F C F 40 electrons F F

• 10 surrounding central atom, expanded • 0 Nonbonding Pairs Electrons• 5 to 1, 0 NBPE, 900/1200 , trigonal bipyrimidal

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 32 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 32 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 32 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 32 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 32 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

SCl6• S= 6 valence electrons = 6• Cl= 6 (7) valence electrons = 42• Cl Cl 48 electrons• Cl S Cl • Cl Cl No Double Bonds Possible• Cl• Cl • Cl S Cl 48 electrons• Cl• Cl

• 12 surrounding central atom, expanded octet• 0 Nonbonding Pairs Electrons• 6 to 1, 0 NBPE, 90o, octahedral

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 3 to 1

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 3 to 1 1 NBPE

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 3 to 1 1 NBPE <109.5

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 3 to 1 1 NBPE <109.5 pyrimidal

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 4 to 1 0 NBPE 109.5 tetrahedral

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 3 to 1 0 NBPE 120o trigonal planar

H2NCH2COOH

• Hydrogen (1)5 = 5 electrons• Nitrogen (5) 1 = 5 electrons• Oxygen (6) 2 = 12 electrons• Carbon (4) 2 =8 electrons• 30 electrons

• H H O• N C C O H• H H• 2 to 1 2 NBPE <109.5o bent

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