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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
The ionization energy and electron affinity determine the formation of ionic compounds by controlling the exchange of electrons. A compound will form if it results in an overall lower energy state for both of the atoms involved. This manifests in atoms tending to full or empty their outer energy levels.

Step by step solution

01

Defining Ionization Energy

The first step is to understand ionization energy. It is defined as the amount of energy required to remove an electron from a gaseous atom or ion. The energy required increases with the number of electrons already removed because the remaining electrons are held more tightly by the positive charge of the nucleus.
02

Understanding Electron Affinity

Electron affinity, on the other hand, is the amount of energy released when an electron is added to a neutral atom to form a negative ion. When an atom's outer energy level is far from being full, they generally have strong affinities for electrons.
03

Combination of Atoms Forming Ionic Compounds

Ionic compounds are formed when one atom gives up one or more electrons to another atom, which contradicts the high ionization energies and low electron affinities. This is possible because atoms will usually do what is easiest to achieve full outer energy levels. If an atom's outer energy level is almost full, they will tend to gain electrons (low ionization energy, high electron affinity), while if the outer energy level is almost empty, they will give electrons up (high ionization energy, high electron affinity). This creates a balance that leads to ionic compounds.

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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. Why does this rule not apply to compounds like \(\mathrm{H}_{2} \mathrm{O}\) and \(\mathrm{NH}_{3} ?\)

Draw three resonance structures for the chlorate ion, \(\mathrm{ClO}_{3}^{-}\). Show formal charges.

Explain the concept of formal charge.

Explain why the bond enthalpy of a molecule is usually defined in terms of a gas-phase reaction. Why are bond-breaking processes always endothermic and bond-forming processes always exothermic?

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 \(\mathrm{Br}\)
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