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scoundrel [369]
3 years ago
9

In the molecules below, areas that have a partial negative charge are pink and areas that have a partial positive charge are blu

e. The attractive force between these two molecules has most likely been produced by covalent bonds. dipole-dipole interactions. dipole-induced dipole interactions. London dispersion forces.

Chemistry
1 answer:
Kaylis [27]3 years ago
4 0

Answer:

Dipole-dipole interactions

Step-by-step explanation:

Each molecule consists of <em>two different elements</em>.

Thus, each molecule has permanent <em>bond dipoles</em>.

The dipoles do not cancel, so the attractive forces are dipole-dipole attractions.

"Covalent bonds" is <em>wrong,</em> because there are no bonds between the two molecules.

There are dipole-induced dipole and London dispersion forces, but they are much weaker than the dipole-dipole attractions.

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We know that the molar mass of C₈H₁₈ is 114.0g/mol. Then, using proportions:

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2mol \times\frac{1.306 \times 10^{3}kcal }{1mol} =2.612\times 10^{3}kcal

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