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Chapter 9: Problem 8

Name five metals and five nonmetals that are very likely to form ionic compounds. Write formulas for compounds that might result from the combination of these metals and nonmetals. Name these compounds.

Short Answer

Expert verified
Five metals are Sodium, Magnesium, Aluminum, Potassium, and Calcium. Five nonmetals are Fluorine, Oxygen, Nitrogen, Chlorine, and Sulfur. Ionic compounds formed are Sodium Fluoride (NaF), Magnesium Oxide (MgO), Aluminum Nitride (AlN), Potassium Chloride (KCl), and Calcium Sulfide (CaS).

Step by step solution

01

Naming five metals

First, choose five metals. For this exercise, Sodium (Na), Magnesium (Mg), Aluminium (Al), Potassium (K) and Calcium (Ca) will be selected.
02

Naming five nonmetals

Now, choose five nonmetals. For this exercise, Fluorine (F), Oxygen (O), Nitrogen (N), Chlorine (Cl), and Sulfur (S) will be selected.
03

Forming Ionic Bonds

Next step is to pair up the metals and nonmetals to form ionic compounds. For example: Sodium (Na) can combine with Fluorine (F) to form Sodium Fluoride (NaF). Similarly, Magnesium (Mg) combines with Oxygen (O) to form Magnesium Oxide (MgO), Aluminium (Al) combines with Nitrogen (N) to form Aluminium Nitride (AlN), Potassium (K) combines with Chlorine (Cl) to form Potassium Chloride (KCl), and Calcium (Ca) combines with Sulfur (S) to form Calcium Sulfide (CaS). Note that these are just examples and other compounds can be formed based on combining different elements.
04

Formulas of Ionic Compounds

Now, moving on to writing the formulas of these ionic compounds, it important to remember that ionic compounds are neutral, i.e., they have equal number of positive and negative charges. This is the reason why Magnesium Oxide is written as MgO and not MgO2, and Aluminium Nitride is written as AlN and not AlN3.
05

Naming the Compounds

Finally, the compounds formed are named. From our examples, Sodium and Fluorine combine to form Sodium Fluoride, Magnesium and Oxygen form Magnesium Oxide, Aluminium and Nitrogen form Aluminium Nitride, Potassium and Chlorine form Potassium Chloride, and Calcium and Sulfur form Calcium Sulfide.

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Most popular questions from this chapter

List these bonds in order of increasing ionic character: the lithium-to- fluorine bond in \(\mathrm{LiF},\) the potassium-to-oxygen bond in \(\mathrm{K}_{2} \mathrm{O},\) the nitrogen-tonitrogen bond in \(\mathrm{N}_{2}\), the sulfur-to-oxygen bond in \(\mathrm{SO}_{2}\), the chlorine-to-fluorine bond in \(\mathrm{ClF}_{3}\).

Using this information: $$ \begin{array}{rr} \mathrm{C}(s) \longrightarrow \mathrm{C}(g) & \Delta H_{\mathrm{rxn}}^{\circ}=716 \mathrm{~kJ} / \mathrm{mol} \\ 2 \mathrm{H}_{2}(g) \longrightarrow 4 \mathrm{H}(g) & \Delta H_{\mathrm{rxn}}^{\circ}=872.8 \mathrm{~kJ} / \mathrm{mol} \end{array} $$ and the fact that the average \(\mathrm{C}-\mathrm{H}\) bond enthalpy is \(414 \mathrm{~kJ} / \mathrm{mol}\), estimate the standard enthalpy of formation of methane \(\left(\mathrm{CH}_{4}\right)\).

Explain how ionization energy and electron affinity determine whether atoms of elements will combine to form ionic compounds.

What is a coordinate covalent bond? Is it different from a normal covalent bond?

Without referring to Figure 9.1 , write Lewis dot symbols for atoms of the following elements: (a) Be, (b) \(\mathrm{K},\) (c) \(\mathrm{Ca},\) (d) \(\mathrm{Ga},\) (e) \(\mathrm{O},\) (f) \(\mathrm{Br},(\mathrm{g}) \mathrm{N},(\mathrm{h}) \mathrm{I},\) (i) \(\mathrm{As}\), (j) F.
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