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Chapter 2: Problem 56

Atoms of four elements are examined: carbon, nitrogen, neon, and sulfur. Atoms of which element are most likely to form a structure with the formula \(\mathrm{XF}_{6}\) (where \(\mathrm{X}\) is one of the four atoms)? (A) Carbon (B) Nitrogen (C) Neon (D) Sulfur

Short Answer

Expert verified
Option (D) Sulfur is the correct answer as it is the only element among the given choices that has 6 electrons to share in its outer shell.

Step by step solution

01

Understand the Chemical Formula

In the formula XF6, X represents one of the given elements and F represents fluorine. The subscript 6 indicates that there are 6 atoms of fluorine. This implies that element X must be able to form 6 bonds with fluorine.
02

Observe the Electronic Configuration and Oxidation State

To form 6 bonds, an element must have 6 electrons available in its outer shell for bonding (either to give away, share, or accept). This typically corresponds to a +6 oxidation state. Among the given elements, sulfur (16th element in the periodic table) has 6 electrons in its outer shell (2-8-6 configuration). Thus, sulfur can form 6 bonds.
03

Confirm the Element

Carbon and nitrogen do not have 6 electrons in their outer shells for sharing. Neon is a noble gas with a full outer electronic shell, hence it is unlikely to form any compounds. Therefore, sulfur is the most probable element to form a compound with the given formula XF6.

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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 sample of \(\mathrm{H}_{2} \mathrm{S}\) gas is placed in an evacuated, sealed container and heated until the following decomposition reaction occurs at \(1000 \mathrm{K} :\) \(2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}\) (A) \(K_{\mathrm{c}}=\frac{\left[\mathrm{H}_{2}\right]^{2}\left[\mathrm{S}_{2}\right]}{\left[\mathrm{H}_{2} \mathrm{S}\right]^{2}}\) (B) \(K_{\mathrm{c}}=\frac{\left[\mathrm{H}_{2} \mathrm{S}\right]^{2}}{\left[\mathrm{H}_{2}\right]^{2}\left[\mathrm{S}_{2}\right]}\) (C) \(K_{\mathrm{c}}=\frac{2\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}{2\left[\mathrm{H}_{2} \mathrm{S}\right]}\) (D) \(K_{\mathrm{c}}=\frac{2\left[\mathrm{H}_{2} \mathrm{S}\right]}{2\left[\mathrm{H}_{2}\right]\left[\mathrm{S}_{2}\right]}\)

$$\begin{array}{|c|c|c|}\hline & {\text { Initial pH }} & {\text { PH after NaOH }} \\ \hline \text { Acid 1 } & {3.0} & {3.5} \\ \hline \text { Acid 2 } & {3.0} & {5.0} \\ \hline\end{array}$$ 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.

A sample of solid \(\mathrm{MgCl}_{2}\) would be most soluble in which of the following solutions? (A) \(\operatorname{LiOH}(a q)\) (B) \(\operatorname{CBr}_{4}(a q)\) (C) \(\operatorname{Mg}\left(\mathrm{NO}_{3}\right)_{2}(a q)\) (D) \(\mathrm{AlCl}_{3}(a q)\)

The average mass, in grams, of one mole of carbon atoms is equal to (A) the average mass of a single carbon atom, measured in amus (B) the ratio of the number of carbon atoms to the mass of a single carbon atom (C) the number of carbon atoms in one amu of carbon (D) the mass, in grams, of the most abundant isotope of carbon
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