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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

An unknown element is a nonmetal and has a valence electron configuration of \(n s^{2} n p^{4}\). a. How many valence electrons does this element have? b. What are some possible identities for this element? c. What is the formula of the compound this element would form with potassium? d. Would this element have a larger or smaller radius than barium? e. Would this element have a greater or smaller ionization energy than fluorine?

Give the maximum number of electrons in an atom that can have these quantum numbers: a. \(n=0, \ell=0, m_{\ell}=0\) b. \(n=2, \ell=1, m_{\ell}=-1, m_{s}=-\frac{1}{2}\) c. \(n=3, m_{s}=+\frac{1}{2}\) d. \(n=2, \ell=2\) e. \(n=1, \ell=0, m_{\ell}=0\)

It takes \(476 \mathrm{kJ}\) to remove 1 mole of electrons from the atoms at the surface of a solid metal. How much energy (in kJ) does it take to remove a single electron from an atom at the surface of this solid metal?

Which of elements \(1-36\) have two unpaired electrons in the ground state?

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically?
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