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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
