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Chapter 7: Problem 8

An element X reacts with \(\mathrm{F}_{2}(g)\) to form the molecular product shown here. (a) Write a balanced equation for this reaction (do not worry about the phases for \(\mathrm{X}\) and the product). (b) Do you think that \(\mathrm{X}\) is a metal or nonmetal? [Section 7.6\(]\)

Short Answer

Expert verified
The molecular product formed when element X reacts with F2 gas is XF2. The balanced chemical equation for the reaction is: \(X + \mathrm{F_2} \rightarrow XF_2\). Since XF2 has covalent bonding, which typically forms between nonmetals, we can deduce that element X is likely a nonmetal.

Step by step solution

01

Identify the Molecular Product formed

Given the information in the question, we know that element X reacts with F2 gas to form the molecular product, represented by XF2. This is because each fluorine atom contributes one electron in a bond, and there should be two fluorine atoms to complete the bond with the element X.
02

Write a balanced chemical equation

Now that we know the molecular product, we can write a balanced chemical equation for the reaction. The unbalanced equation can be written as: \[X + \mathrm{F_2}\rightarrow XF_2\] To balance the equation, we need the same number of atoms of each element on both sides of the equation. The equation is already balanced as written, with one atom of element X, and two atoms of fluorine in both reactants and product: \[X + \mathrm{F_2}\rightarrow XF_2\]
03

Determine whether X is a metal or nonmetal

To determine whether the element X is a metal or a nonmetal, we can look at the type of bonding present in the molecular product XF2. In XF2, there is a sharing of electrons between X and the fluorine atoms, indicating a covalent bond. Covalent bonds typically form between nonmetals, so we can deduce that element X is likely a nonmetal.

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Most popular questions from this chapter

Discussing this chapter, a classmate says, "Since elements that form cations are metals and elements that form anions are nonmetals, elements that do not form ions are metalloids." Do you agree or disagree?

Which of the following chemical equations is connected to the definitions of (a) the first ionization energy of oxygen, (b) the second ionization energy of ox ygen, and (c) the electron affinity of oxygen? (i) \(\mathrm{O}(g)+\mathrm{e}^{-} \longrightarrow \mathrm{O}^{-}(g)\) (ii) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{+}(g)+\mathrm{e}^{-}\) (iii) \(\mathrm{O}(g)+2 \mathrm{e}^{-} \longrightarrow \mathrm{O}^{2-}(g)\) (iv) \(\mathrm{O}(g) \longrightarrow \mathrm{O}^{2+}(g)+2 \mathrm{e}^{-}\) $(\mathbf{v}) \mathrm{O}^{+}(g) \longrightarrow \mathrm{O}^{2+}(g)+\mathrm{e}^{-}$

Mercury in the environment can exist in oxidation states \(0,\) \(+1,\) and \(+2 .\) One major question in environmental chemistry research is how to best measure the oxidation state of mercury in natural systems; this is made more complicated by the fact that mercury can be reduced or oxidized on surfaces differently than it would be if it were free in solution. XPS, X-ray photoelectron spectroscopy, is a technique related to PES (see Exercise 7.111 ), but instead of using ultraviolet light to eject valence electrons, X rays are used to eject core electrons. The energies of the core electrons are different for different oxidation states of the element. In one set of experiments, researchers examined mercury contamination of minerals in water. They measured the XPS signals that corresponded to electrons ejected from mercury's 4 forbitals at \(105 \mathrm{eV}\), from an X-ray source that provided \(1253.6 \mathrm{eV}\) of energy $\left(1 \mathrm{ev}=1.602 \times 10^{-19} \mathrm{~J}\right)$ The oxygen on the mineral surface gave emitted electron energies at $531 \mathrm{eV}\(, corresponding to the \)1 s$ orbital of oxygen. Overall the researchers concluded that oxidation states were +2 for \(\mathrm{Hg}\) and -2 for O. (a) Calculate the wavelength of the \(\mathrm{X}\) rays used in this experiment. (b) Compare the energies of the \(4 f\) electrons in mercury and the \(1 s\) electrons in oxygen from these data to the first ionization energies of mercury and oxygen from the data in this chapter. (c) Write out the ground- state electron configurations for \(\mathrm{Hg}^{2+}\) and \(\mathrm{O}^{2-}\); which electrons are the valence electrons in each case?

Use electron configurations to explain the following observations: (a) The first ionization energy of phosphorus is greater than that of sulfur. (b) The electron affinity of nitrogen is lower (less negative) than those of both carbon and oxygen. (c) The second ionization energy of oxygen is greater than the first ionization energy of fluorine. (d) The third ionization energy of manganese is greater than those of both chromium and iron.

Moseley's experiments on \(\mathrm{X}\) rays emitted from atoms led to the concept of atomic numbers. (a) If arranged in order of increasing atomic mass, which element would come after chlorine? (b) Describe two ways in which the properties of this element differ from the other elements in group $8 \mathrm{~A}$.
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