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Chapter 7: Q12E (page 390)

What information can you use to predict whether a bond between two atoms is covalent or ionic?

Short Answer

Expert verified

Based on element positions: 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 will be ionic.

If the difference in electronegativity of the elements involved is less than \({\rm{0}}{\rm{.4}}\), the bond is covalent; if it is between \({\rm{0}}{\rm{.4}}\) and \({\rm{0}}{\rm{.8}}\), the bond is polar covalent; and if it is greater than \({\rm{0}}{\rm{.8}}\), the link is ionic.

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

Explanation

Predict if a covalent or ionic link exists between two atoms: -

  1. On the basis of element positions: 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 will be ionic.
  2. If the difference between the electronegativity of the elements involved is \({\rm{ < 0}}{\rm{.4}}\), the bond is covalent; if the difference is between \({\rm{0}}{\rm{.4}}\) and \({\rm{0}}{\rm{.8}}\), the bond is polar covalent; and if the difference is \({\rm{ > 0}}{\rm{.8}}\), the link is ionic.

Therefore, based on element positions if the elements in a compound are near together in the periodic table, the bond is more likely to be covalent, whereas if the elements are far apart, the bond is more likely to be ionic.

If the electronegativity of the element involved differs by \({\rm{ < 0}}{\rm{.4}}\), the bond is covalent; if the difference is between \({\rm{0}}{\rm{.4}}\) and \({\rm{0}}{\rm{.8}}\), the bond is polar covalent; and if the difference is greater than \({\rm{0}}{\rm{.8}}\), the link is ionic.

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Most popular questions from this chapter

Question: Complete the following Lewis structure by adding bonds (not atoms), and then indicate the longest bond:

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.

The reaction of a metal, \({\rm{M}}\), with a halogen, \({{\rm{X}}_{\rm{2}}}\), proceeds by an exothermic reaction as indicated by this equation: \({\rm{M(s) + }}{{\rm{X}}_{\rm{2}}}{\rm{(g)}} \to {\rm{M}}{{\rm{X}}_{\rm{2}}}{\rm{(s)}}\). For each of the following, indicate which option will make the reaction more exothermic. Explain your answers.

(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

(d) a decreasing electron affinity for the halogen

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

Question: When a molecule can form two different structures, the structure with the stronger bonds is usually the more stable form. Use bond energies to predict the correct structure of the hydroxylamine molecule:

Question: Using the bond energies in Table \({\rm{7}}{\rm{.2}}\), determine the approximate enthalpy change for each of the following reactions:

(a) \({{\rm{H}}_{\rm{2}}}{\rm{(g) + B}}{{\rm{r}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2HBr(g)}}\)

(b) \({\rm{C}}{{\rm{H}}_{\rm{4}}}{\rm{(g) + }}{{\rm{I}}_{\rm{2}}}{\rm{(g)}} \to {\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{I(g) + HI(g)}}\)

(c) \({{\rm{C}}_{\rm{2}}}{{\rm{H}}_4}{\rm{(g) + 3}}{{\rm{O}}_{\rm{2}}}{\rm{(g)}} \to {\rm{2C}}{{\rm{O}}_{\rm{2}}}{\rm{(g) + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O(g)}}\)
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