10. When you were learning about counting electron groups, you may have been a bit confused with how tocount double or triple bonds and why we only counted them as a group of electrons. In valence bond hieorysingle bonds are described differently than double bonds. The orbital overlap is different.Sigma (6) bonds are formed when orbitals overlap along the internuclear axis (these are the examples ofsingle bonds we practiced above). Pi (T) bonds are formed when singly occupied p orbitals overlap aboveand below the internuclear axis. Double bonds contain one o bond and one ↑ bond. Triple bonds containone o bond and two t bonds.Try sketching the valence bond orbitals for ethene (CH,CH2) and ethyne (CHCH) to practice with doubleand triple bonds. Use the steps listed in #8 and consult your group, a TA, or your book if you get stuck.

Answered: Image /qna-images/answer/2cf7e93e-72c6-4567-a6c1-b59d73600d3f.jpg

Try sketching the valence bond orbitals for ethene (CH,CH2) and ethyne (CHCH) to practice with double and triple bonds. Use the steps listed in #8 and consult your group, a TA, or your book if you get stuck.

Try sketching the valence bond orbitals for ethene (CH,CH2) and ethyne (CHCH) to practice with double and triple bonds. Use the steps listed in #8 and consult your group, a TA, or your book if you get stuck.

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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