11.50_CP - Chemistry: Molecular Nature Of Matter And Change

Question

The hydrocarbon allene, ${\mathbf{H}}_{\mathbf{2}}\mathbf{C}\mathbf{=}\mathbf{C}\mathbf{=}{\mathbf{CH}}_{\mathbf{2}}$ , is obtained indirectly from petroleum and used as a precursor for several types of plastics. What is the hybridization of each C atom in allene? Draw a bonding picture for allene with lines for sigma bonds, and show the arrangement of the pi bonds. Be sure to represent the geometry of the molecule in three dimensions.

Step-by-Step Solution

Answer

The hybridization of all ene is sp² hybridized having geometry Trigonal planar. The molecule has 3 sigma bond and 1 pi-bond.

Step 1: Bonding

 Bonding may be defined as the force of attraction between two or more atoms to form a compound. The molecule can have the same atom and a different atom.

 

Hybridization may be defined as the mixing of the atomic orbital to form a hybrid orbital before bonding with another atomic orbital having similar atomic orbital.

Step 2: VSPER Theory

The molecule is always bonded in geometry in a three-dimensional structure using the hybrid orbital by the atoms. Due to the difference in the hybridization of the molecule the geometry of the molecule changes. 

 

Allen hydrocarbons, H2C = C = CH2, are indirectly obtainedfrom petroleum and act as precursors for various types of plastics. The hybridization of allene is sp² hybridized having geometry Trigonal planar. The molecule has 3 sigma bond and 1 pi-bond. There is a side-ways-overlapping in the molecule, the double bond comes simultaneously in the molecule of allene. It is only possible by the direction of the p-orbital between the molecules which is different for both sides of the C-atom at a 90^o angle.