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Chapter 8: Problem 18

Which ionic compound is expected to form from combining the following pairs of elements? (a) barium and fluorine, (b) cesium and chlorine, (c) lithium and nitrogen, (d) aluminum and oxygen.

Short Answer

Expert verified
The ionic compounds formed from the given pairs of elements are: (a) \(BaF_2\), (b) \(CsCl\), (c) \(Li_3N\), and (d) \(Al_2O_3\).

Step by step solution

01

(a) Barium and Fluorine

Step 1: Identify charges of ions - Barium (Ba) is in group 2 of the periodic table, so it forms a \(+2\) ion: \(Ba^{2+}\). - Fluorine (F) is in group 17 (group 7 in terms of valence electrons), so it forms a \(-1\) ion: \(F^-\). Step 2: Combine ions to form a neutral compound - As the charge of Ba is \(+2\) and the charge of F is \(-1\), we need to combine them in a way that results in a neutral compound, i.e., 1 Ba ion and 2 F ions: \(BaF_2\).
02

(b) Cesium and Chlorine

Step 1: Identify charges of ions - Cesium (Cs) is in group 1 of the periodic table, so it forms a \(+1\) ion: \(Cs^+\). - Chlorine (Cl) is in group 17 (group 7 in terms of valence electrons), so it forms a \(-1\) ion: \(Cl^-\). Step 2: Combine ions to form a neutral compound - As the charge of Cs is \(+1\) and the charge of Cl is \(-1\), we need to combine them in a way that results in a neutral compound, i.e., 1 Cs ion and 1 Cl ion: \(CsCl\).
03

(c) Lithium and Nitrogen

Step 1: Identify charges of ions - Lithium (Li) is in group 1 of the periodic table, so it forms a \(+1\) ion: \(Li^+\). - Nitrogen (N) is in group 15 (group 5 in terms of valence electrons), so it forms a \(-3\) ion: \(N^{3-}\). Step 2: Combine ions to form a neutral compound - As the charge of Li is \(+1\) and the charge of N is \(-3\), we need to combine them in a way that results in a neutral compound, i.e., 3 Li ions and 1 N ion: \(Li_3N\).
04

(d) Aluminum and Oxygen

Step 1: Identify charges of ions - Aluminum (Al) is in group 13 (group 3 in terms of valence electrons), so it forms a \(+3\) ion: \(Al^{3+}\). - Oxygen (O) is in group 16 (group 6 in terms of valence electrons), so it forms a \(-2\) ion: \(O^{2-}\). Step 2: Combine ions to form a neutral compound - As the charge of Al is \(+3\) and the charge of O is \(-2\), we need to combine them in a way that results in a neutral compound, i.e., 2 Al ions and 3 O ions: \(Al_2O_3\).

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Most popular questions from this chapter

Ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl},\) is a very soluble salt in water. (a) Draw the Lewis structures of the ammonium and chloride ions. (b) Is there an \(\mathrm{N}-\) Cl bond in solid ammonium chloride? (c) If you dissolve 14 gof ammonium chloride in 500.0 \(\mathrm{mL}\) of water, what is the molar concentration of the solution? (d) How many grams of silver nitrate do you need to add to the solution in part (c) to precipitate all of the chloride as silver chloride?

Energy is required to remove two electrons from Ca to form \(\mathrm{Ca}^{2+},\) and energy is required to add two electrons to \(\mathrm{O}\) to form \(\mathrm{O}^{2-} .\) Yet \(\mathrm{CaO}\) is stable relative to the free elements. Which statement is the best explanation? (a) The lattice energy of CaO is large enough to overcome these processes. (b) CaO is a covalent compound, and these processes are irrelevant. (c) CaO has a higher molar mass than either Ca or O. (d) The enthalpy of formation of CaO is small. (e) CaO is stable to atmospheric conditions.

Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Na, \(\mathrm{Mg}, \mathrm{K}, \mathrm{Ca} ;(\mathbf{b}) \mathrm{P}, \mathrm{S},\) As, \(\mathrm{Se} ;(\mathbf{c}) \mathrm{Be}, \mathrm{B}, \mathrm{C}, \mathrm{Si} ;(\mathbf{d}) \mathrm{Zn}, \mathrm{Ge}, \mathrm{Ga}, \mathrm{Gs}\)

Write electron configurations for the following ions, and determine which have noble-gas configurations: (a) \(\mathrm{Cd}^{2+}\) , \((\mathbf{b}) \mathrm{P}^{3-},(\mathbf{c}) \mathrm{Zr}^{4+},(\mathbf{d}) \mathrm{Ru}^{3+},(\mathbf{e}) \mathrm{As}^{3-},(\mathbf{f}) \mathrm{Ag}^{+}\)

The Ti \(\mathrm{Ti}^{2+}\) ion is isoelectronic with the Ca atom. (a) Write the electron configurations of \(\mathrm{Ti}^{2+}\) and (b) Calculate the number of unpaired electrons for Ca and for \(\mathrm{Ti}^{2+} .\) (c) What charge would Ti have to be isoelectronic with \(\mathrm{Ca}^{2}+?\)
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