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Chapter 7: Problem 102

Which of the following is the expected product of the reaction of \(\mathrm{Mg}(s)\) and \(\mathrm{N}_{2}(g)\) under heat? (i) \(\mathrm{Mg}_{3} \mathrm{~N}(s)\) (ii) \(\mathrm{MgN}_{2}(s)\) (iii) \(\mathrm{Mg}_{3} \mathrm{~N}_{2}(s),\) (iv) \(\mathrm{Mg}(s)\) and \(\mathrm{N}_{2}(g)\) will not react with one another.

Short Answer

Expert verified
The expected product of the reaction of Mg(s) and N₂(g) under heat is \(Mg_3N_2(s)\).

Step by step solution

01

Identify the type of reaction

Magnesium (Mg) is a metal and Nitrogen (N₂) is a non-metal. When a metal reacts with a non-metal, they usually form an ionic compound. This means we need to look for an ionic compound in the given options. Step 2: Determine the charges of the ions
02

Determine the charges of the ions

Magnesium (Mg) has a valency of +2, as it has two electrons in the outer shell that it can lose. Nitrogen (N) has a valency of -3, as it has five electrons in the outer shell, requiring three more electrons to complete its octet. Now, we will use these charges to figure out the correct product. Step 3: Find the correct product
03

Find the correct product

In an ionic compound, the charges of its ions must balance. We are given four options for possible products: (i): \(Mg_3N(s)\): Charges: (+2) + (-3) = -1, which is not balanced. (ii): \(MgN_2(s)\): Charges: (+2) + 2*(-3) = -4, which is not balanced. (iii): \(Mg_3N_2(s)\): Charges: 3*(+2) + 2*(-3) = 0, which is balanced. (iv): \(Mg(s)\) and \(N_2(g)\) do not react: This is a possibility if none of the other options are correct. The only option that gives a charge balance is option (iii), which is therefore our answer. Answer: The expected product of the reaction of Mg(s) and N₂(g) under heat is \(Mg_3N_2(s)\).

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Most popular questions from this chapter

Write the electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Ti}^{2+},(\mathbf{b})\) (d) \(\mathrm{PO}^{2-}\), (f) \(\mathrm{V}^{3+}\) \(\mathrm{Br}^{-}\) (c) \(\mathrm{Mg}^{2+}\) (e) \(\mathrm{Pt}^{2+}\)

(a) Does metallic character increase, decrease, or remain unchanged as one goes from left to right across a row of the periodic table? (b) Does metallic character increase, decrease, or remain unchanged as one goes down a column of the periodic table? (c) Are the periodic trends in (a) and (b) the same as or different from those for first ionization energy?

Based on their positions in the periodic table, predict which atom of the following pairs will have the smaller first ionization energy: (a) $\mathrm{Br}, \mathrm{Kr} ; \mathbf{( b )} \mathrm{C}, \mathrm{Ca} ;(\mathbf{c}) \mathrm{Li}, \mathrm{Rb} ;\(; (d) \)\mathrm{Pb}, \mathrm{Si} ;$ (e) \(\mathrm{Al}, \mathrm{B}\).

It is possible to define metallic character as we do in this book and base it on the reactivity of the element and the ease with which it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements to determine how "metallic" the elements are. On the basis of conductivity, there is not much of a trend in the periodic table: Silver is the most conductive metal, and manganese the least. Look up the first ionization energies of silver and manganese; which of these two elements would you call more metallic based on the way we define it in this book?

Consider the stable elements through lead \((Z=82) .\) In how many instances are the atomic weights of the elements out of order relative to the atomic numbers of the elements?
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