1 7 Structural Formulas of Organic Molecules Constitution

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1. 7 Structural Formulas of Organic Molecules

1. 7 Structural Formulas of Organic Molecules

Constitution The order in which the atoms of a molecule are connected is called

Constitution The order in which the atoms of a molecule are connected is called its constitution or connectivity. The constitution of a molecule must be determined in order to write a Lewis structure.

Table 1. 4 How to Write Lewis Structures Step 1: The molecular formula and

Table 1. 4 How to Write Lewis Structures Step 1: The molecular formula and the connectivity are determined by experiment.

Table 1. 4 How to Write Lewis Structures Step 1: The molecular formula and

Table 1. 4 How to Write Lewis Structures Step 1: The molecular formula and the connectivity are determined by experiment. Example: Methyl nitrite has the molecular formula CH 3 NO 2. All hydrogens are bonded to carbon, and the order of atomic connections is CONO.

Table 1. 4 How to Write Lewis Structures Step 2: Count the number of

Table 1. 4 How to Write Lewis Structures Step 2: Count the number of valence electrons. For a neutral molecule this is equal to the number of valence electrons of the constituent atoms.

Table 1. 4 How to Write Lewis Structures Step 2: Count the number of

Table 1. 4 How to Write Lewis Structures Step 2: Count the number of valence electrons. For a neutral molecule this is equal to the number of valence electrons of the constituent atoms. Example (CH 3 NO 2): Each hydrogen contributes 1 valence electron. Each carbon contributes 4, nitrogen 5, and each oxygen 6 for a total of 24.

Table 1. 4 How to Write Lewis Structures Step 3: Connect the atoms by

Table 1. 4 How to Write Lewis Structures Step 3: Connect the atoms by a covalent bond represented by a dash.

Table 1. 4 How to Write Lewis Structures Step 3: Connect the atoms by

Table 1. 4 How to Write Lewis Structures Step 3: Connect the atoms by a covalent bond represented by a dash. Example: Methyl nitrite has the partial structure: H H C H O N O

Table 1. 4 How to Write Lewis Structures Step 4: Subtract the number of

Table 1. 4 How to Write Lewis Structures Step 4: Subtract the number of electrons in bonds from the total number of valence electrons. H H C H O N O

Table 1. 4 How to Write Lewis Structures Step 4: Subtract the number of

Table 1. 4 How to Write Lewis Structures Step 4: Subtract the number of electrons in bonds from the total number of valence electrons. Example: 24 valence electrons – 12 electrons in bonds. Therefore, 12 more electrons to assign.

Table 1. 4 How to Write Lewis Structures Step 5: Add electrons in pairs

Table 1. 4 How to Write Lewis Structures Step 5: Add electrons in pairs so that as many atoms as possible have 8 electrons. Start with the most electronegative atom.

Table 1. 4 How to Write Lewis Structures Step 5: Add electrons in pairs

Table 1. 4 How to Write Lewis Structures Step 5: Add electrons in pairs so that as many atoms as possible have 8 electrons. Start with the most electronegative atom. Example: The remaining 12 electrons in methyl nitrite are added as 6 pairs. H. . : H C O N O. . . H

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks an octet, use electron pairs on an adjacent atom to form a double or triple bond. Example: Nitrogen has only 6 electrons in the structure shown. H. . : H C O N O. . . H

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks an octet, use electron pairs on an adjacent atom to form a double or triple bond. Example: All the atoms have octets in this Lewis structure. H. . : H C O N O. . H

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example:

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example: None of the atoms possess a formal charge in this Lewis structure. H. . : H C O N O. . H

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example:

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example: This structure has formal charges; is less stable Lewis structure. H. . – + : H C O N O. . . H

Condensed structural formulas Lewis structures in which many (or all) covalent bonds and electron

Condensed structural formulas Lewis structures in which many (or all) covalent bonds and electron pairs are omitted. H H C C C H : O: H H H can be condensed to: CH 3 CHCH 3 or (CH 3)2 CHOH OH

Bond-line formulas CH 3 CH 2 CH 3 is shown as CH 3 CH

Bond-line formulas CH 3 CH 2 CH 3 is shown as CH 3 CH 2 CH 2 OH is shown as Omit atom symbols. Represent structure by showing bonds between carbons and atoms other than hydrogen. Atoms other than carbon and hydrogen are called heteroatoms. OH

Bond-line formulas H H 2 C Cl CH 2 is shown as H H

Bond-line formulas H H 2 C Cl CH 2 is shown as H H Omit atom symbols. Represent structure by showing bonds between carbons and atoms other than hydrogen. Atoms other than carbon and hydrogen are called heteroatoms.

1. 8 Constitutional Isomers

1. 8 Constitutional Isomers

Constitutional isomers Isomers are different compounds that have the same molecular formula. Constitutional isomers

Constitutional isomers Isomers are different compounds that have the same molecular formula. Constitutional isomers are isomers that differ in the order in which the atoms are connected. An older term for constitutional isomers is “structural isomers. ”

A Historical Note NH 4 OCN Ammonium cyanate O H 2 NCNH 2 Urea

A Historical Note NH 4 OCN Ammonium cyanate O H 2 NCNH 2 Urea In 1823 Friedrich Wöhler discovered that when ammonium cyanate was dissolved in hot water, it was converted to urea. Ammonium cyanate and urea are constitutional isomers of CH 4 N 2 O. Ammonium cyanate is “inorganic. ” Urea is “organic. ” Wöhler is credited with an important early contribution that helped overturn theory of “vitalism. ”

Examples of constitutional isomers H H C H . . O: N+ – :

Examples of constitutional isomers H H C H . . O: N+ – : : O. . Nitromethane H H C . . O. . N. . O: H Methyl nitrite Both have the molecular formula CH 3 NO 2 but the atoms are connected in a different order.

1. 9 Resonance

1. 9 Resonance

Resonance two or more Lewis structures may be written for certain compounds (or ions)

Resonance two or more Lewis structures may be written for certain compounds (or ions)

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks an octet, use electron pairs on an adjacent atom to form a double or triple bond. Example: Nitrogen has only 6 electrons in the structure shown. H. . : H C O N O. . . H

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks

Table 1. 4 How to Write Lewis Structures Step 6: If an atom lacks an octet, use electron pairs on an adjacent atom to form a double or triple bond. Example: All the atoms have octets in this Lewis structure. H. . : H C O N O. . H

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example:

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example: None of the atoms possess a formal charge in this Lewis structure. H. . : H C O N O. . H

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example:

Table 1. 4 How to Write Lewis Structures Step 7: Calculate formal charges. Example: This structure has formal charges; is less stable Lewis structure. H. . – + : H C O N O. . . H

Resonance Structures of Methyl Nitrite same atomic positions differ in electron positions H H

Resonance Structures of Methyl Nitrite same atomic positions differ in electron positions H H C . . O. . N. . H more stable Lewis structure . . O: H H C + O. . N. . H less stable Lewis structure . . – : O. .

Resonance Structures of Methyl Nitrite same atomic positions H H C . . O.

Resonance Structures of Methyl Nitrite same atomic positions H H C . . O. . differ in electron positions H. . : N O H C. . H more stable Lewis structure + O. . N. . H less stable Lewis structure . . – : O. .

Why Write Resonance Structures? Electrons in molecules are often delocalized between two or more

Why Write Resonance Structures? Electrons in molecules are often delocalized between two or more atoms. Electrons in a single Lewis structure assigned to specific atoms-a single Lewis structure is insufficient to show electron delocalization. Composite of resonance forms more accurately depicts electron distribution.

Example Ozone (O 3) Lewis structure of ozone shows one double bond and one

Example Ozone (O 3) Lewis structure of ozone shows one double bond and one single bond • • • O • Expect: one short bond and one long bond Reality: bonds are of equal length (128 pm) + O • • • – O • • •

Example Ozone (O 3) Lewis structure of ozone shows one double bond and one

Example Ozone (O 3) Lewis structure of ozone shows one double bond and one single bond • • • O • + O • • • – O • • • Resonance: • • • O • + O • • • – O • • • – • • • O • • • + O • •

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