3.- Based on the molecular orbitals of hydrogen, and the hybridized orbitals of single, double and triple bonded-carbon, assign the type of interaction for the following bonds (HINT: all answers must be expressed in "orbitai-orbital" format, review the double and triple bond slides form your ppt). H. H- H--c-H H' CC--H Blue= Red= Green= Orange= Purple=

3.- Based on the molecular orbitals of hydrogen, and the hybridized orbitals of single, double and triple bonded-carbon, assign the type of interaction for the following bonds (HINT: all answers must be expressed in "orbitai-orbital" format, review the double and triple bond slides form your ppt). H. H- H--c-H H' CC--H Blue= Red= Green= Orange= Purple=

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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Give detailed Solution with explanation needed with Lewis structures..don't give Handwritten answer...
2p Atomic Orbitals 2p Molecular Orbitals X Recheck Next> (12 of 14) 6th attempt 2s 2p Atomic Orbitals Instructions: Fill molecular orbitals in the diagram by dragging either single electrons or pairs. Click on an occupied orbital to remove electrons. Determine the net number of sigma bonds, the net number of pi bonds, and the overall bond order for O₂. Use 0.5 to indicate a fractional bond order. a bonds 1 bonds o overall bond order 1.5 Fill All Clear Partially Correct A pair of electrons in a bonding molecular orbital count as +1 bond. A pair of electrons in an antibonding orbital count as -1 bond. The total number of bonds is equal to the sum of all bonding and antibonding interactions. A single electron in an orbital counts as either +0.5 or -0.5 bond.
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Solution please, asked two times before but getting wrong answer. Please need correct, otherwise will report.