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Chapter 7: Problem 65

Show how two \(\mathrm{CH}_{2} \mathrm{Cl}_{2}\) molecules in the liquid phase are oriented with respect to each other and explain why the molecules align this way.

Short Answer

Expert verified
In the liquid phase, two CH2Cl2 molecules with their polar tetrahedral structure orient themselves to maximize the attractive forces between the opposite charges, specifically aligning the negative Chlorines of one molecule with the positive Hydrogens of the neighboring molecule. This arrangement is due to the dipole-dipole interactions resulting from the polar covalent bonds, which create an uneven distribution of electron density and a net dipole moment in the molecules, thus stabilizing the liquid phase.

Step by step solution

01

The CH2Cl2 molecule consists of two Hydrogens (H), two Chlorines (Cl), and one central Carbon (C). The shape of this molecule is tetrahedral, with bond angles close to 109.5°. The molecule is polar because there are polar covalent bonds between the central Carbon atom and the Chlorine atoms, causing a partial negative charge on the Chlorine atoms and a partial positive charge on the Hydrogen atoms. #Step 2: Analyze the interactions between the polar CH2Cl2 molecules#

When two CH2Cl2 molecules are close to each other, their polar nature allows them to interact through dipole-dipole interactions. The negative ends (chlorines) of one molecule are attracted to the positive ends (hydrogens) of the other molecule, and vice versa. This interaction results in a more energetically favorable and stable alignment of the molecules. #Step 3: Describe the orientation of CH2Cl2 molecules in the liquid phase#
02

In the liquid phase, CH2Cl2 molecules orient themselves in such a way that there are attractive forces between the opposite charges. Specifically, the negative Chlorines from one molecule will align with the positive Hydrogens of the neighboring molecule. This arrangement maximizes the attractive forces and stabilizes the system, allowing the liquid phase to form and making it difficult for the molecules to break away from each other. #Step 4: Explain the reason for this orientation#

The alignment of CH2Cl2 molecules in the liquid phase is based on the attractive forces between positive and negative charges on the different CH2Cl2 molecules. This alignment minimizes the energy between the molecules and stabilizes the liquid phase. The reason for this orientation is that the polar covalent bonds create an uneven distribution of electron density, which causes a net dipole moment in the molecule that attracts other polar molecules to arrange accordingly.

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Most popular questions from this chapter

Eicosane, \(\mathrm{C}_{20} \mathrm{H}_{42}\), has a higher melting point and a higher boiling point than water, even though water has hydrogen bonds between molecules and eicosane does not. Explain how this can be.

Predict which compound in each pair will have the higher melting point, and explain why for each pair. (a) HI or KI (b) \(\mathrm{Na}_{2} \mathrm{O}\) or \(\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{CaF}_{2}\) or \(\mathrm{HF}\) (d) \(\mathrm{SiO}_{2}\) or \(\mathrm{CO}_{2}\)

Which of the following do you expect to be nonmolecular solids? (a) Sodium hydroxide, \(\mathrm{NaOH}\) (b) Solid ethanol, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (c) Iron, Fe (d) Solid silane, \(\mathrm{SiH}_{4}\)

Arrange in order of increasing boiling point: \(\mathrm{CO}_{2}, \mathrm{SO}_{2}, \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}, \mathrm{Al}\)

Why would either covalent bonds or London forces be inappropriate for attaching the two strands of DNA to each other?
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