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H. C=C H

H. C=C H

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Use bond energies to calculate the heat of reaction:

=kj

The image shows the structural formula of ethene (also known as ethylene), a simple hydrocarbon. In this structure: - There are two carbon atoms (C) in the center, connected by a double bond, which is depicted by a pair of parallel lines (=). - Each carbon atom is bonded to two hydrogen atoms (H), represented by single lines extending outwards. - The molecular arrangement is planar, showing that the double bond between the carbon atoms influences the geometry, maintaining a roughly 120-degree angle between the hydrogen atoms around each carbon. This structural diagram emphasizes the molecular geometry and bonding in ethene, highlighting the presence of the carbon-carbon double bond, which is characteristic of alkenes.
Transcribed Image Text:The image shows the structural formula of ethene (also known as ethylene), a simple hydrocarbon. In this structure: - There are two carbon atoms (C) in the center, connected by a double bond, which is depicted by a pair of parallel lines (=). - Each carbon atom is bonded to two hydrogen atoms (H), represented by single lines extending outwards. - The molecular arrangement is planar, showing that the double bond between the carbon atoms influences the geometry, maintaining a roughly 120-degree angle between the hydrogen atoms around each carbon. This structural diagram emphasizes the molecular geometry and bonding in ethene, highlighting the presence of the carbon-carbon double bond, which is characteristic of alkenes.
### Average Bond Energies | Bond | Energy (kJ/mol) | |-------|-----------------| | C—C | 347 | | C═C | 614 | | C—H | 413 | | C—Cl | 339 | | Cl—Cl | 243 | #### Explanation: The table lists the average bond energies for different types of bonds in kilojoules per mole (kJ/mol). - **C—C (Carbon-Carbon Single Bond)**: 347 kJ/mol - **C═C (Carbon-Carbon Double Bond)**: 614 kJ/mol - **C—H (Carbon-Hydrogen Single Bond)**: 413 kJ/mol - **C—Cl (Carbon-Chlorine Single Bond)**: 339 kJ/mol - **Cl—Cl (Chlorine-Chlorine Single Bond)**: 243 kJ/mol These values represent the average amount of energy required to break one mole of the respective bonds in a gaseous state. Higher energy values indicate stronger bonds. For example, the C═C bond has greater energy than the C—C bond, reflecting the increased strength of a double bond compared to a single bond.
Transcribed Image Text:### Average Bond Energies | Bond | Energy (kJ/mol) | |-------|-----------------| | C—C | 347 | | C═C | 614 | | C—H | 413 | | C—Cl | 339 | | Cl—Cl | 243 | #### Explanation: The table lists the average bond energies for different types of bonds in kilojoules per mole (kJ/mol). - **C—C (Carbon-Carbon Single Bond)**: 347 kJ/mol - **C═C (Carbon-Carbon Double Bond)**: 614 kJ/mol - **C—H (Carbon-Hydrogen Single Bond)**: 413 kJ/mol - **C—Cl (Carbon-Chlorine Single Bond)**: 339 kJ/mol - **Cl—Cl (Chlorine-Chlorine Single Bond)**: 243 kJ/mol These values represent the average amount of energy required to break one mole of the respective bonds in a gaseous state. Higher energy values indicate stronger bonds. For example, the C═C bond has greater energy than the C—C bond, reflecting the increased strength of a double bond compared to a single bond.
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