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Chapter 8: Problem 17

Predict the chemical formula of the ionic compound formed between the following pairs of elements: (a) Al and Cl, (b) \(\mathrm{Mg}\) and \(\mathrm{O},(\mathbf{c}) \mathrm{Zn}\) and \(\mathrm{Cl}\), (d) \(\mathrm{Li}\) and \(\mathrm{O}\).

Short Answer

Expert verified
The chemical formulas for the ionic compounds between the given pairs of elements are: (a) \(AlCl_3\), (b) \(MgO\), (c) \(ZnCl_2\), and (d) \(Li_2O\).

Step by step solution

01

(a) Al and Cl

First, we need to find the valencies of Al and Cl. Aluminium (Al) belongs to group 13 in the periodic table, which means it has 3 valence electrons. It tends to lose these 3 electrons to obtain a stable electron configuration, and forms an Al^3+ ion. Chlorine (Cl) belongs to group 17 in the periodic table, which means it has 7 valence electrons. It tends to gain 1 electron to obtain a stable electron configuration, and forms a Cl^- ion. Now, to write the chemical formula, we need to balance the charges by having 3 Cl^- ions for each Al^3+ ion. The chemical formula for the ionic compound between Al and Cl is: \(AlCl_3\)
02

(b) Mg and O

First, we need to find the valencies of Mg and O. Magnesium (Mg) belongs to group 2 in the periodic table, which means it has 2 valence electrons. It tends to lose these 2 electrons to obtain a stable electron configuration, and forms an Mg^2+ ion. Oxygen (O) belongs to group 16 in the periodic table, which means it has 6 valence electrons. It tends to gain 2 electrons to obtain a stable electron configuration, and forms an O^2- ion. Now, to write the chemical formula, we need to balance the charges by having 1 Mg^2+ ion for each O^2- ion. The chemical formula for the ionic compound between Mg and O is: \(MgO\)
03

(c) Zn and Cl

First, we need to find the valencies of Zn and Cl. Zinc (Zn) has a unique property where it forms a stable Zn^2+ ion. Chlorine (Cl) belongs to group 17 in the periodic table, which means it has 7 valence electrons. It tends to gain 1 electron to obtain a stable electron configuration, and forms a Cl^- ion. Now, to write the chemical formula, we need to balance the charges by having 2 Cl^- ions for each Zn^2+ ion. The chemical formula for the ionic compound between Zn and Cl is: \(ZnCl_2\)
04

(d) Li and O

First, we need to find the valencies of Li and O. Lithium (Li) belongs to group 1 in the periodic table, which means it has 1 valence electron. It tends to lose this electron to obtain a stable electron configuration, and forms an Li^+ ion. Oxygen (O) belongs to group 16 in the periodic table, which means it has 6 valence electrons. It tends to gain 2 electrons to obtain a stable electron configuration, and forms an O^2- ion. Now, to write the chemical formula, we need to balance the charges by having 2 Li^+ ions for each O^2- ion. The chemical formula for the ionic compound between Li and O is: \(Li_2O\)

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Most popular questions from this chapter

A new compound is made that has a \(\mathrm{C}-\mathrm{O}\) bond length of $120 \mathrm{pm}$. Is this bond likely to be a single, double, or triple C-O bond?

Acetylene \(\left(\mathrm{C}_{2} \mathrm{H}_{2}\right)\) and nitrogen \(\left(\mathrm{N}_{2}\right)\) both contain a triple bond, but they differ greatly in their chemical properties. (a) Write the Lewis structures for the two substances. (b) By referring to Appendix C, look up the enthalpies of formation of acetylene and nitrogen. Which compound is more stable? (c) Write balanced chemical equations for the complete oxidation of \(\mathrm{N}_{2}\) to form \(\mathrm{N}_{2} \mathrm{O}_{5}(g)\) and of acetylene to form \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O (g) .\) (d) Calculate the enthalpy of oxidation per mole for \(\mathrm{N}_{2}\) and for $\mathrm{C}_{2} \mathrm{H}_{2}\( (the enthalpy of formation of \)\mathrm{N}_{2} \mathrm{O}_{5}(g)\( is \)11.30 \mathrm{~kJ} / \mathrm{mol}\( ). \)(\mathbf{e})$ Both \(\mathrm{N}_{2}\) and \(\mathrm{C}_{2} \mathrm{H}_{2}\) possess triple bonds with quite high bond enthalpies (Table 8.3). Calculate the enthalpy of hydrogenation per mole for both compounds: acetylene plus \(\mathrm{H}_{2}\) to make methane, \(\mathrm{CH}_{4}\); nitrogen plus \(\mathrm{H}_{2}\) to make ammonia, \(\mathrm{NH}_{3}\).

(a) Draw the best Lewis structure(s) for the nitrite ion, \(\mathrm{NO}_{2}^{-}\). (b) With what allotrope of oxygen is it isoelectronic? (c) What would you predict for the lengths of the bonds in \(\mathrm{NO}_{2}^{-}\) relative to \(\mathrm{N}-\mathrm{O}\) single bonds and double bonds?

(a) True or false: The hydrogen atom is most stable when it has a full octet of electrons. (b) How many electrons must a sulfur atom gain to achieve an octet in its valence shell? (c) If an atom has the electron configuration $1 s^{2} 2 s^{2} 2 p^{3},$ how many electrons must it gain to achieve an octet?

(a) Using Lewis symbols, make a sketch of the reaction between potassium and bromine atoms to give the ionic substance KBr. (b) How many electrons are transferred? (c) Which atom loses electrons in the reaction?
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