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Chapter 2: Problem 133

Complete and balance the equations for the following reactions. a. \(\mathrm{Li}(s)+\mathrm{N}_{2}(g) \rightarrow\) b. \(\mathrm{Rb}(s)+\mathrm{S}(s) \rightarrow\)

Short Answer

Expert verified
The short answers are: a. \( 6\mathrm{Li}(s) + \mathrm{N}_{2}(g) \rightarrow 2\mathrm{Li}_{3}\mathrm{N}(s) \) b. \( 2\mathrm{Rb}(s) + \mathrm{S}(s) \rightarrow \mathrm{Rb}_{2}\mathrm{S}(s) \)

Step by step solution

01

Identify the product

For the first reaction, Li (lithium) reacts with N (nitrogen) to form lithium nitride (Li3N), an ionic compound, where lithium has a charge of +1 and nitrogen a charge of -3. So the chemical equation becomes: \[ \mathrm{Li}(s) + \mathrm{N}_{2}(g) \rightarrow \mathrm{Li}_{3}\mathrm{N}(s) \]
02

Balance the equation

To balance the equation, we need to ensure there are the same number of Lithium and Nitrogen atoms on both sides. To do so, we can add coefficients in front of the elements and compounds. The balanced equation becomes: \[ 6\mathrm{Li}(s) + \mathrm{N}_{2}(g) \rightarrow 2\mathrm{Li}_{3}\mathrm{N}(s) \] b.
03

Identify the product

For the second reaction, Rb (rubidium) reacts with S (sulfur) to form rubidium sulfide (Rb2S), an ionic compound, where rubidium has a charge of +1 and sulfur a charge of -2. So the chemical equation becomes: \[ \mathrm{Rb}(s) + \mathrm{S}(s) \rightarrow \mathrm{Rb}_{2}\mathrm{S}(s) \]
04

Balance the equation

To balance the equation, we need to ensure there are the same number of Rubidium and Sulfur atoms on both sides of the equation. To do so, we can add coefficients in front of the elements and compounds. The balanced equation becomes: \[ 2\mathrm{Rb}(s) + \mathrm{S}(s) \rightarrow \mathrm{Rb}_{2}\mathrm{S}(s) \]

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Most popular questions from this chapter

The elements \(\mathrm{Cu}, \mathrm{O}, \mathrm{La}, \mathrm{Y}, \mathrm{Ba}, \mathrm{Tl},\) and \(\mathrm{Bi}\) are all found in high-temperature ceramic superconductors. Write the expected electron configuration for these atoms.

How many orbitals in an atom can have the designation \(5 p,\) \(3 d_{z}, 4 d, n=5, n=4 ?\)

Which of the following sets of quantum numbers are not allowed? For each incorrect set, state why it is incorrect. a. \(n=3, \ell=3, m_{\ell}=0, m_{s}=-\frac{1}{2}\) b. \(n=4, \ell=3, m_{\ell}=2, m_{s}=-\frac{1}{2}\) c. \(n=4, \ell=1, m_{\ell}=1, m_{s}=+\frac{1}{2}\) d. \(n=2, \ell=1, m_{\ell}=-1, m_{s}=-1\) e. \(n=5, \ell=-4, m_{\ell}=2, m_{s}=+\frac{1}{2}\) f. \(n=3, \ell=1, m_{\ell}=2, m_{s}=-\frac{1}{2}\)

How many electrons in an atom can have the designation \(1 p\) \(6 d_{x^{2}-y^{2}}, 4 f, 7 p_{y}, 2 s, n=3 ?\)

A certain oxygen atom has the electron configuration \(1 s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2} .\) How many unpaired electrons are present? Is this an excited state of oxygen? In going from this state to the ground state, would energy be released or absorbed?
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