On each carbon overlaps and all of the sp hybrids on both atoms are in the same plane. Compare to your ethene model from Part A and have your instructor check your model and initial here before proceeding: b. Using this ethene orbital model orientation and the two carbon atoms below, sketch: 1) In the plane of the page, the 2p orbitals used to form the pi bond in ethene; 2) all of the spa hybrid orbitals used by used by the carbon atoms to form sigma bonds; and 3) the overlap of the four hydrogen Is orbitals with the sp hybrid orbitals to show the C-H bonds. Put one label for each orbital showing its type. H H Note: Larger H atoms C C are in the foreground; smaller H H H atoms are in the background. c. In terms of the orbitals involved, Why do all of the atoms in ethene have to be in the same plane? d. To model all of the orbitals used by the carbons in ethyne, construct two of the following, one to represent each carbon atom: Use a six-hole, yellow atom. Attach two pink paddles in a linear arrangement to represent the two sp hybrids used by the carbon to form sigma bonds. Then put two sets of two (four) purple paddles 180 apart in the remaining four holes to represent the two 2p orbitals used to form two pi bonds. Hold the two models (they won't be connected) so that one sp hybrid on each carbon overlaps and all of the sp hybrids on both atoms are linear. Line up a 2p orbital on each carbon so that they are parallel to each other. Compare to your ethyne model from Part A and have your instructor check your model and initial here before proceeding: e. What is the total number of orbitals used to form all sigma bonds in ethyne? f. What is the total number of orbitals used to form all pi bonds in ethyne?