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Chapter 2: Problem 36

Most transition metals share a common oxidation state of \(+2 .\) Which of the following best explains why? (A) Transition metals all have a minimum of two unpaired electrons. (B) Transition metals have unstable configurations and are very reactive. (C) Transition metals tend to gain electrons when reacting with other elements. (D) Transition metals will lose their outermost s-block electrons when forming bonds.

Short Answer

Expert verified
The correct answer is (D) Transition metals will lose their outermost s-block electrons when forming bonds.

Step by step solution

01

Understand the electronic structure of transition metals

Transition metals are those elements that have incompletely filled d-orbital even after losing two electrons. The outermost electronic configuration is usually s2d1-9. When these metals form ions, the 4s electrons are lost first. Therefore, they have a common oxidation state of +2.
02

Analyze given options

Option (A) mentions about unpaired electrons. But, this is not necessarily correct for all transition elements. Option (B) suggests that transition metals have unstable configurations and are very reactive, which is a broad statement. Reactivity varies among transition metals. Option (C) suggests that transition metals gain electrons. However, metals generally lose electrons. Option (D) says that transition metals will lose their outermost s-block electrons when forming bonds. This is consistent with the typical behavior of transition metals.
03

Select the best answer

Since we know that transition metals typically lose their outermost s-block electrons when forming bonds, Option (D) offers the best explanation for the common oxidation state of +2 in transition metals.

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Most popular questions from this chapter

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecule would have the shortest bonds? (A) \(\mathrm{CO}_{2}\) (B) \(\mathrm{CO}_{3}^{2-}\) (C) \(\mathrm{NO}_{2}^{-}\) (D) \(\mathrm{NO}_{3}^{-}\)

Consider the Lewis structures for the following molecules: $$\begin{equation} \mathrm{CO}_{2}, \mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-}, \text {and } \mathrm{NO}_{3}^{-} \end{equation}$$ Which molecules are best represented by multiple resonance structures? (A) \(\mathrm{CO}_{2}\) and \(\mathrm{CO}_{3}^{2-}\) (B) \(\mathrm{NO}_{2}^{-}\) and \(\mathrm{NO}_{3}^{-}\) (C) \(\mathrm{CO}_{3}^{2-}\) and \(\mathrm{NO}_{3^{-}}^{-}\) (D) \(\mathrm{CO}_{3}^{2-}, \mathrm{NO}_{2}^{-},\) and \(\mathrm{NO}_{3}^{-}\)

\(14 \mathrm{H}^{+}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+3 \mathrm{Ni}(s) \rightarrow\) \(2 \mathrm{Cr}^{3+}(a q)+3 \mathrm{Ni}^{2+}(a q)+7 \mathrm{H}_{2} \mathrm{O}(l)\) In the above reaction, a piece of solid nickel is added to a solution of potassium dichromate. Which species is being oxidized and which is being reduced? \(\quad\) Oxidized \(\quad\) Reduced (A) \(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q) \quad \mathrm{Ni}(s)\) (B) \(\mathrm{Cr}^{3+}(a q) \quad \mathrm{Ni}^{2+}(a q)\) (C) \(\mathrm{Ni}(s) \quad \mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)\) (D) \(\mathrm{Ni}^{2+}(a q) \quad \mathrm{Cr}^{3+}(a q)\)

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 \(1000 \mathrm{K} :\) $$2 \mathrm{H}_{2} \mathrm{S}(g) \rightarrow 2 \mathrm{H}_{2}(g)+\mathrm{S}_{2}(g) \qquad K_{\mathrm{c}}=1.0 \times 10^{-6}$$ If, at a given point in the reaction, the value for the reaction quotient \(Q\) is determined to be \(2.5 \times 10^{-8},\) which of the following is occurring? (A) The concentration of the reactant is decreasing while the concentration of the products is increasing. (B) The concentration of the reactant is increasing while the concentration of the products is decreasing. (C) The system has passed the equilibrium point, and the concentration of all species involved in the reaction will remain constant. (D) The concentrations of all species involved are changing at the same rate.

$$\mathrm{NH}_{4}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) \rightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)$$ 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.
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