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Chapter 2: Problem 30

London dispersion forces are caused by (A) temporary dipoles created by the position of electrons around the nuclei in a molecule (B) the three-dimensional intermolecular bonding present in all covalent substances (C) the uneven electron-to-proton ratio found on individual atoms of a molecule (D) the electronegativity differences between the different atoms in a molecule

Short Answer

Expert verified
The correct answer is (A) temporary dipoles created by the position of electrons around the nuclei in a molecule.

Step by step solution

01

Understand London Dispersion Forces

London Dispersion Forces are one of the three van der Waals forces. These are the weakest intermolecular attractions, and they occur between all types of molecules, both polar and non-polar. They are caused by temporary fluctuations in electron distribution around the atoms, which create short-lived positive and negative regions within the molecule.
02

Analyzing the Options

Looking at the options given, option A refers to temporary dipoles created by the position of electrons around the nuclei in a molecule, B refers to the three-dimensional intermolecular bonding present in all covalent substances, C refers to the uneven electron-to-proton ratio found on individual atoms of a molecule and finally, option D refers to the electronegativity differences between the different atoms in a molecule. It is important to match the right cause with our understanding of London dispersion forces.
03

Choosing the Correct Option

Based on the understanding of London Dispersion Forces, we know these forces are caused due to temporary dipoles created due to fluctuations in electron distribution around the nuclei. Therefore, option A, which states 'temporary dipoles created by the position of electrons around the nuclei in a molecule' is the correct answer.

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Most popular questions from this chapter

Which of the following is true for all bases? (A) All bases donate \(\mathrm{OH}^{-}\) ions into solution. (B) Only strong bases create solutions in which \(\mathrm{OH}^{-}\) ions are present. (C) Only strong bases are good conductors when dissolved in solution. (D) For weak bases, the concentration of the \(\mathrm{OH}^{-}\) ions exceeds the concentration of the base in the solution.

A solution contains a mixture of four different compound: \(\mathrm{KCl}(a q),\) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q), \mathrm{MgSO}_{4}(a q),\) and \(\mathrm{N}_{2} \mathrm{H}_{4}(a q) .\) Which of these compounds would be easiest to separate via distillation? (A) \(\mathrm{KCl}(a q)\) (B) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)\) (C) \(\mathrm{MgSO}_{4}(a q)\) (D) \(\mathrm{N}_{2} \mathrm{H}_{4}(a q)\)

$$\mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) \rightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)$$ Increasing the temperature of the above reaction will increase the rate of reaction. Which of the following is NOT a reason that increased temperature increases reaction rate? (A) The reactants will be more likely to overcome the activation energy. (B) The number of collisions between reactant molecules will increase. (C) A greater distribution of reactant molecules will have high velocities. (D) Alternate reaction pathways become available at higher temperatures.

A sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ As the reaction progresses at a constant temperature of 1000 K, how does the value for the Gibbs free energy constant for the reaction change? (A) It stays constant. (B) It increases exponentially. (C) It increases linearly. (D) It decreases exponentially.

$$\begin{array}{|c|c|c|}\hline & {\text { Initial pH }} & {\text { PH after NaOH }} \\ \hline \text { Acid 1 } & {3.0} & {3.5} \\ \hline \text { Acid 2 } & {3.0} & {5.0} \\ \hline\end{array}$$ Two different acids with identical pH are placed in separate beakers. Identical portions of NaOH are added to each beaker, and the resulting pH is indicated in the table above. What can be determined about the strength of each acid? (A) Acid 1 is a strong acid and acid 2 is a weak acid because acid 1 resists change in pH more effectively. (B) Acid 1 is a strong acid and acid 2 is a weak acid because the NaOH is more effective at neutralizing acid 2. (C) Acid 1 is a weak acid and acid 2 is a strong acid because the concentration of the weak acid must be significantly greater to have the same pH as the strong acid. (D) Acid 1 is a weak acid and acid 2 is a strong acid because the concentration of the hydrogen ions will be greater in acid 2 after the NaOH addition.
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