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Chapter 9: Problem 7

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

Short Answer

Expert verified
Ionization Energy and Electron Affinity play vital roles in the formation of ionic compounds. Atoms with low Ionization Energy tend to lose electrons and form positive ions, while atoms with high Electron Affinity tend to accept electrons and form negative ions. The electrostatic attraction between these oppositely charged ions forms an ionic bond, resulting in an ionic compound, as exemplified by the case of Sodium (Na) and Chlorine (Cl) forming Sodium Chloride (NaCl).

Step by step solution

01

Define Ionization Energy and Electron Affinity

Ionization Energy is the energy required for an atom to remove an electron from its outer shell. On the other hand, Electron Affinity is the energy released when an atom accepts an electron in its outer shell.
02

Explain the Role of Ionization Energy and Electron Affinity in Ionic Bond Formation

In the formation of ionic compounds, an atom with low ionization energy tends to lose electrons and form a positive ion (a cation). At the same time, an atom with high electron affinity tends to accept electrons and form a negative ion (an anion). When these two oppositely charged ions come close, they attract each other and form an ionic bond resulting in the creation of an ionic compound.
03

Illustrate with an Example

For instance, consider sodium (Na) and chlorine (Cl). Sodium has a low Ionization Energy so it loses an electron easily, and chlorine has high Electron Affinity, so it tends to accept an electron readily. Sodium losses an electron and becomes a Na+ ion and chlorine accepts an electron and becomes Cl- ion. The attraction between the two oppositely charged ions results in the formation of an ionic compound, sodium chloride (NaCl).

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Most popular questions from this chapter

A rule for drawing plausible Lewis structures is that the central atom is invariably less electronegative than the surrounding atoms. Explain why this is so.

For each of the following pairs of elements, state whether the binary compound they form is likely to be ionic or covalent. Write the empirical formula and name of the compound: (a) \(\mathrm{B}\) and \(\mathrm{F}\), (b) \(\mathrm{K}\) and \(\mathrm{Br}\).

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.

What is Lewis's contribution to our understanding of the covalent bond?

Summarize the essential features of the Lewis octet rule. The octet rule applies mainly to the second period elements. Explain.
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