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Chapter 7: Q13E (page 391)

Predict which of the following compounds are ionic and which are covalent, based on the location of their constituent atoms in the periodic table:

(a) \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO}}\) (b) \({\rm{MnO}}\) (c) \({\rm{NC}}{{\rm{l}}_{\rm{3}}}\) (d) \({\rm{CoB}}{{\rm{r}}_{\rm{2}}}\) (e) \({{\rm{K}}_{\rm{2}}}{\rm{S}}\) (f) \({\rm{CO}}\) (g) \({\rm{Ca}}{{\rm{F}}_{\rm{2}}}\) (h) \({\rm{HI}}\) (i) \({\rm{CaO}}\) (j) \({\rm{IBr}}\) (k) \({\rm{C}}{{\rm{O}}_{\rm{2}}}\) .

Short Answer

Expert verified

The ionic compounds are: \({\rm{MnO, CoB}}{{\rm{r}}_{\rm{2}}}{\rm{, }}{{\rm{K}}_{\rm{2}}}{\rm{S, Ca}}{{\rm{F}}_{\rm{2}}}\) and \({\rm{CaO}}\).

The covalent compounds are: \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO, NC}}{{\rm{l}}_{\rm{3}}}{\rm{, CO, HI, IBr}}\) and \({\rm{C}}{{\rm{O}}_{\rm{2}}}\).

Step by step solution

01

Define Chemical Bonding 

A chemical bond is a long-term attraction between atoms, ions, or molecules that allows chemical compounds to form.

02

Predicting that the ions are ionic or covalent?

Based on the location of the elements in the periodic table: If the elements in a compound are close to one another in the periodic table, the bond is more likely to be covalent, but if the elements are far apart, the bond is more likely to be ionic.

Now, based on the above reasoning, we may conclude that:

Ionic compounds include\({\rm{MnO, CoB}}{{\rm{r}}_{\rm{2}}}{\rm{, }}{{\rm{K}}_{\rm{2}}}{\rm{S, Ca}}{{\rm{F}}_{\rm{2}}}\), and\({\rm{CaO}}\), whereas covalent compounds include\({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO, NC}}{{\rm{l}}_{\rm{3}}}{\rm{, CO, HI, IBr}}\), and\({\rm{C}}{{\rm{O}}_{\rm{2}}}\).

Therefore, Ionic include \({\rm{MnO, CoB}}{{\rm{r}}_{\rm{2}}}{\rm{, }}{{\rm{K}}_{\rm{2}}}{\rm{S, Ca}}{{\rm{F}}_{\rm{2}}}\), and \({\rm{CaO}}\), as well as covalent compounds are \({\rm{C}}{{\rm{l}}_{\rm{2}}}{\rm{CO, NC}}{{\rm{l}}_{\rm{3}}}{\rm{, CO, HI, IBr}}\), and \({\rm{C}}{{\rm{O}}_{\rm{2}}}\).

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Most popular questions from this chapter

Use the simulation (http://openstaxcollege.org/l/16MolecPolarity) to perform the following exercises for a real molecule. You may need to rotate the molecules in three dimensions to see certain dipoles. (a) Sketch the bond dipoles and molecular dipole (if any) for O3. Explain your observations. (b) Look at the bond dipoles for NH3. Use these dipoles to predict whether N or H is more electronegative. (c) Predict whether there should be a molecular dipole for NH3 and, if so, in which direction it will point. Check the molecular dipole box to test your hypothesis.

From the labels of several commercial products, prepare a list of six ionic compounds in the products. For each compound, write the formula. (You may need to look up some formulas in a suitable reference.)

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(a) a large radius vs. a small radius for \({{\rm{M}}^{{\rm{ + 2}}}}\)

(b) a high ionization energy vs. a low ionization energy for \({\rm{M}}\)

(c) an increasing bond energy for the halogen

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(e) an increasing size of the anion formed by the halogen

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