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Resonance a): C1 Resonance b): C1 C2 03 C4 C5 06 C2 03 C4 C5 06 Resonance c): C1 C2 03 C4 C5 06 Resonance d): C1 C2 03 C4 C5 06 When examining the Lewis structures of organic molecules, to determine the location a reaction will occur, a chemist must identify the sites of maximum and minimum electron density, which is often emphasized by showing the formal charge on the atoms. The ability to quickly recognize the presence or absence of formal charges on atoms is an important skill. You should be able to recognize bonding around the common elements in organic chemistry, and determine the formal charge on the atom based on the number of bonds. The key elements to recognize include carbon, nitrogen, phosphorous, oxygen, sulfur and the halides. For every one of these elements there is a pattern of bonds and lone pairs which will allow rapid determination of formal charge without going through the exercise shown below in determining the formal charge on the nitrogen atom in diethyl amine: H₂C CH₂ Formal charge N = # electrons surrounding N as an isolated atom - # electrons in lone pairs - 1/2 the number of electrons in bonds to nitrogen. Formal charge N = 5 - electrons in lone pair - 1/2 the 6 electrons in bonds to N = 0 One of the times you will see formal charges used most frequently is in the generation of resonance structures, as one of the ways that resonance structures change as pairs of electrons are moved is in variation in the formal charges of the atoms. Assigning formal charges to various resonance structures of a molecule is often a significant clue about where in the molecule the reaction will occur: Determine the formal charges on all of the atoms in the resonance structures shown below that bear charges of +1 and -1 by highlighting each atoms below, remembering to take into account all of the lone pair electrons: H₂C 3. 2C IU C ÖH H₁₂C a H₂C :0: C :0: OH H₂C d

Resonance a): C1 Resonance b): C1 C2 03 C4 C5 06 C2 03 C4 C5 06 Resonance c): C1 C2 03 C4 C5 06 Resonance d): C1 C2 03 C4 C5 06 When examining the Lewis structures of organic molecules, to determine the location a reaction will occur, a chemist must identify the sites of maximum and minimum electron density, which is often emphasized by showing the formal charge on the atoms. The ability to quickly recognize the presence or absence of formal charges on atoms is an important skill. You should be able to recognize bonding around the common elements in organic chemistry, and determine the formal charge on the atom based on the number of bonds. The key elements to recognize include carbon, nitrogen, phosphorous, oxygen, sulfur and the halides. For every one of these elements there is a pattern of bonds and lone pairs which will allow rapid determination of formal charge without going through the exercise shown below in determining the formal charge on the nitrogen atom in diethyl amine: H₂C CH₂ Formal charge N = # electrons surrounding N as an isolated atom - # electrons in lone pairs - 1/2 the number of electrons in bonds to nitrogen. Formal charge N = 5 - electrons in lone pair - 1/2 the 6 electrons in bonds to N = 0 One of the times you will see formal charges used most frequently is in the generation of resonance structures, as one of the ways that resonance structures change as pairs of electrons are moved is in variation in the formal charges of the atoms. Assigning formal charges to various resonance structures of a molecule is often a significant clue about where in the molecule the reaction will occur: Determine the formal charges on all of the atoms in the resonance structures shown below that bear charges of +1 and -1 by highlighting each atoms below, remembering to take into account all of the lone pair electrons: H₂C 3. 2C IU C ÖH H₁₂C a H₂C :0: C :0: OH H₂C d

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter3: Atomic Shells And Classical Models Of Chemical Bonding
Section: Chapter Questions
Problem 94AP: The molecular ion S3N3 has the cyclic structure All SN bonds are equivalent. (a) Give six...
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Resonance a): C1 Resonance b): C1 C2 03 C4 C5 06 C2 03 C4 C5 06 Resonance c): C1 C2 03 C4 C5 06 Resonance d): C1 C2 03 C4 C5 06 When examining the Lewis structures of organic molecules, to determine the location a reaction will occur, a chemist must identify the sites of maximum and minimum electron density, which is often emphasized by showing the formal charge on the atoms. The ability to quickly recognize the presence or absence of formal charges on atoms is an important skill. You should be able to recognize bonding around the common elements in organic chemistry, and determine the formal charge on the atom based on the number of bonds. The key elements to recognize include carbon, nitrogen, phosphorous, oxygen, sulfur and the halides. For every one of these elements there is a pattern of bonds and lone pairs which will allow rapid determination of formal charge without going through the exercise shown below in determining the formal charge on the nitrogen atom in diethyl amine: H₂C CH₂ Formal charge N = # electrons surrounding N as an isolated atom - # electrons in lone pairs - 1/2 the number of electrons in bonds to nitrogen. Formal charge N = 5 - electrons in lone pair - 1/2 the 6 electrons in bonds to N = 0 One of the times you will see formal charges used most frequently is in the generation of resonance structures, as one of the ways that resonance structures change as pairs of electrons are moved is in variation in the formal charges of the atoms. Assigning formal charges to various resonance structures of a molecule is often a significant clue about where in the molecule the reaction will occur: Determine the formal charges on all of the atoms in the resonance structures shown below that bear charges of +1 and -1 by highlighting each atoms below, remembering to take into account all of the lone pair electrons: H₂C 3. 2C IU C ÖH H₁₂C a H₂C :0: C :0: OH H₂C d
Transcribed Image Text:Resonance a): C1 Resonance b): C1 C2 03 C4 C5 06 C2 03 C4 C5 06 Resonance c): C1 C2 03 C4 C5 06 Resonance d): C1 C2 03 C4 C5 06 When examining the Lewis structures of organic molecules, to determine the location a reaction will occur, a chemist must identify the sites of maximum and minimum electron density, which is often emphasized by showing the formal charge on the atoms. The ability to quickly recognize the presence or absence of formal charges on atoms is an important skill. You should be able to recognize bonding around the common elements in organic chemistry, and determine the formal charge on the atom based on the number of bonds. The key elements to recognize include carbon, nitrogen, phosphorous, oxygen, sulfur and the halides. For every one of these elements there is a pattern of bonds and lone pairs which will allow rapid determination of formal charge without going through the exercise shown below in determining the formal charge on the nitrogen atom in diethyl amine: H₂C CH₂ Formal charge N = # electrons surrounding N as an isolated atom - # electrons in lone pairs - 1/2 the number of electrons in bonds to nitrogen. Formal charge N = 5 - electrons in lone pair - 1/2 the 6 electrons in bonds to N = 0 One of the times you will see formal charges used most frequently is in the generation of resonance structures, as one of the ways that resonance structures change as pairs of electrons are moved is in variation in the formal charges of the atoms. Assigning formal charges to various resonance structures of a molecule is often a significant clue about where in the molecule the reaction will occur: Determine the formal charges on all of the atoms in the resonance structures shown below that bear charges of +1 and -1 by highlighting each atoms below, remembering to take into account all of the lone pair electrons: H₂C 3. 2C IU C ÖH H₁₂C a H₂C :0: C :0: OH H₂C d
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