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Chapter 7: Problem 43

(a) What is the general relationship between the size of an atom and its first ionization energy? (b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

Short Answer

Expert verified
a) The general relationship between the size of an atom and its first ionization energy is that ionization energy decreases as the size of the atom increases because larger atoms have weaker attractive forces between their valence electrons and the nucleus. b) Helium (He) has the largest ionization energy, while francium (Fr) has the smallest ionization energy in the periodic table.

Step by step solution

01

Define Ionization Energy

First, let's define ionization energy. Ionization energy is the amount of energy required to remove a valence electron from an atom. It is usually measured in electron volts (eV) or kilojoules per mole (kJ/mol).
02

Understand Atomic Size and Ionization Energy Relationship

Now, we need to understand the relationship between the size of an atom and its first ionization energy. In general, ionization energy decreases as the size of the atom increases. This is because larger atoms have more electron shells, meaning their valence electrons are further away from the nucleus. As a result, the attractive force between the electrons and the nucleus is weaker, making it easier to remove the valence electrons from the atom.
03

Elements with Largest Ionization Energy

Elements in the top-right corner of the periodic table, with the smallest atomic radii and most positive effective nuclear charges, have the highest ionization energies. Therefore, helium (He) has the largest ionization energy in the periodic table.
04

Elements with Smallest Ionization Energy

Elements in the bottom-left corner of the periodic table, with the largest atomic radii and most negative effective nuclear charges, have the lowest ionization energies. Thus, francium (Fr) has the smallest ionization energy in the periodic table. In summary: a) The general relationship between the size of an atom and its first ionization energy is that larger atoms have lower ionization energies, while smaller atoms have higher ionization energies. b) Helium (He) has the largest ionization energy, while francium (Fr) has the smallest ionization energy in the periodic table.

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Most popular questions from this chapter

The experimental \(\mathrm{Bi}-\mathrm{I}\) bond length in bismuth triiodide, \(\mathrm{BiI}_{3}\), is \(2.81 \AA\). Based on this value and data in Figure \(7.7\), predict the atomic radius of \(B\) i.

Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like a nonmetal. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens. (b) Is the following statement true? "Hydrogen has the smallest bonding atomic radius of any element that forms chemical compounds." If not, correct it. If it is, explain in terms of electron configurations. (c) Explain why the ionization energy of hydrogen is closer to the values for the halogens than for the alkali metals.

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