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Chapter 10: Problem 76

Sketch the propene molecule, \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\). Indicate the bond angles in this molecule. What is the maximum number of atoms that can be in the same plane?

Short Answer

Expert verified
The propene molecule forms a planar structure due to the double bond. In propene, bond angles around the central carbon are \(120^{\circ}\) and \(180^{\circ}\). The maximum number of atoms that can exist in the same plane, in this molecule, is all 9 atoms, which include, 3 Carbon atoms and 6 Hydrogen atoms.

Step by step solution

01

Draw the Structural Formula

A structural formula is used to indicate the arrangement of atoms in molecules. For propene (\(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\)), the structure emerges as a carbon atom with three Hydrogen atoms (CH3) linked to a Carbon atom that has one hydrogen (CH) which is in turn linked to a Carbon atom with two Hydrogen atoms (CH2). The link between the second and third Carbon atom is a double bond. This is due to the fact that propene is an alkene - characterized by a double bond.
02

Determine the Bond Angles

The geometry of a molecule can be figured out using the VSEPR theory (Valence Shell Electron Pair Repulsion) which states that electron pairs around a central atom orient themselves as far apart as possible to minimize repulsion. The bond angles are determined accordingly. In the molecule of propene, there are three sigma bonds and one pi bond. These pi bonds restrict the rotation and create a planar configuration. The two CH3 and CH parts form a bond angle of \(120^{\circ}\) around the center carbon atom because of the sp2 hybridization, while the CH and CH2 form a bond angle of \(180^{\circ}\), being parts of the same double bond.
03

Determine Maximum Number of Atoms in the Same Plane

The amount of atoms that can exist in the same plane is ascertained by the geometry of the molecule. In propene, all atoms are in the same plane due to the presence of the double bond which forms a planar configuration. Hence, in Propene, 9 atoms (3 Carbons and 6 Hydrogens) can exist in the same plane.

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Most popular questions from this chapter

The greatest bond length is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Br}_{2} ;\) (d) BrCl.

Predict the shapes of the following molecules, and then predict which would have resultant dipolemoments: (a) \(\mathrm{SO}_{2} ;\) (b) \(\mathrm{NH}_{3} ;\) (c) \(\mathrm{H}_{2} \mathrm{S} ;\) (d) \(\mathrm{C}_{2} \mathrm{H}_{4} ;\) (e) \(\mathrm{SF}_{6}\); (f) \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\).

In certain polar solvents, \(\mathrm{PCl}_{5}\) undergoes an ionization reaction in which a \(\mathrm{Cl}^{-}\) ion leaves one \(\mathrm{PCl}_{5}\) molecule and attaches itself to another. The products of the ionization are \(\mathrm{PCl}_{4}^{+}\) and \(\mathrm{PCl}_{6}^{-}\). Draw a sketch showing the changes in geometric shapes that occur in this ionization (that is, give the shapes of \(\mathrm{PCl}_{5}\), \(\mathrm{PCl}_{4}^{+},\) and \(\mathrm{PCl}_{6}^{-}\) ). $$2 \mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{4}^{+}+\mathrm{PCl}_{6}^{-}$$

Which of the following species requires a resonance hybrid for its Lewis structure: (a) \(\mathrm{CO}_{2},\) (b) \(\mathrm{OCl}^{-}\) (c) \(\mathrm{CO}_{3}^{2-},\) or \((\mathrm{d}) \mathrm{OH}^{-} ?\) Explain.

Explain the important distinctions between (a) ionic and covalent bonds; (b) lone-pair and bond-pair electrons; (c) molecular geometry and electron-group geometry; (d) bond dipole and resultant dipole moment; (e) polar molecule and nonpolar molecule.
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