How many pi bonds are formed when sp3 hybridizatio...

Question

How many pi bonds are formed when sp3 hybridization occurs in ethene, C2H4?

Jules Bruno · Accepted Answer

We’re being asked to determine thenumber of π bonds in C2H4. For this, we first need to draw the Lewis structure of C2H4. The steps in drawing Lewis structures are as follows:Step 1: Determine the central atom in this molecule.Step 2: Calculate the total number of valence electrons present.Step 3: Draw the Lewis structure for the molecule.[readmore]Step 1: Hydrogen cannot be the central atom which means Carbon is the central atom.Step 2: The total number of valence electrons present in C2H4 is:            Group            Valence ElectronsC         4A                   2 × 4 e– = 8 e–H         1A                   4 × 1 e– = 4 e–Total:  12 valence e–Step 3: The two carbons will be bonded to each other:Then we’ll add hydrogens to each carbon based on the formula (both carbons will have 2 Hs):To complete the structure, we need to make sure that each carbon forms 4 bonds. Both carbons both have 3 so it needs another bond to be tetravalent. The complete Lewis structure will appear as: Now that we have the Lewis structure, we can count the number of π bonds in the molecule. Sigma (σ) bonds are the single bonds in molecules. Also, recall that a double bond is composed of 1 σ bond and 1 π bond and a triple bond is composed of 1 σ bond and 2 π bonds. This means in the given molecule:There is one π bond in C2H4

Problem: How many pi bonds are formed when sp3 hybridization occurs in ethene, C2H4?

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Problem: How many pi bonds are formed when sp3 hybridization occurs in ethene, C2H4?

FREE Expert Solution

Problem Details

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