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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

For each of the following pairs, which element will have the greater metallic character: (a) Li or Be, (b) Li or Na, (c) Sn or \(\mathrm{P}_{\text {, }}\) (d) \(\mathrm{Al}\) or \(\mathrm{B}\) ?

(a) During the period from about 1800 to about 1865 , the atomic weights of many elements were accurately measured. Why was this important to Mendeleev's formulation of the periodic table? (b) What property of the atom did Moseley associate with the wavelength of X-rays emitted from an element in his experiments? (c) Why are chemical and physical properties of the elements more closely related to atomic number than they are to atomic weight?

When magnesium metal is burned in air (Figure 3.5), two products are produced. One is magnesium oxide, \(\mathrm{MgO}\). The other is the product of the reaction of \(\mathrm{Mg}\) with molecular nitrogen, magnesium nitride. When water is added to magnesium nitride, it reacts to form magnesium oxide and ammonia gas. (a) Based on the charge of the nitride ion (Table 2.5), predict the formula of magnesium nitride. (b) Write a balanced equation for the reaction of magnesium nitride with water. What is the driving force for this reaction? (c) In an experiment a piece of magnesium ribbon is burned in air in a crucible. The mass of the mixture of \(\mathrm{MgO}\) and magnesium nitride after burning is \(0.470 \mathrm{~g}\). Water is added to the crucible, further reaction occurs, and the crucible is heated to dryness until the final product is \(0.486 \mathrm{~g}\) of \(\mathrm{MgO}\). What was the mass percentage of magnesium nitride in the mixture obtained after the initial burning? (d) Magnesium nitride can also be formed by reaction of the metal with ammonia at high temperature. Write a balanced equation for this reaction. If a \(6.3-\mathrm{g} \mathrm{Mg}\) ribbon reacts with \(2.57 \mathrm{~g} \mathrm{NH}_{3}(\mathrm{~g})\) and the reaction goes to \(\mathrm{com}\) pletion, which component is the limiting reactant? What mass of \(\mathrm{H}_{2}(\mathrm{~g})\) is formed in the reaction? (e) The standard enthalpy of formation of solid magnesium nitride is \(-461.08 \mathrm{~kJ} / \mathrm{mol}\). Calculate the standard enthalpy change for the reaction between magnesium metal and ammonia gas.

The distance between \(\mathrm{W}\) atoms in tungsten metal is \(2.74 \mathrm{~A}\). What is the atomic radius of a tungsten atom in this environment? (This radius is called the metallic radius)

(a) How is the concept of effective nuclear charge used to simplify the numerous electron-electron repulsions in ? many-electron atom? (b) Which experiences a greater effective nuclear charge in a Be atom, the 1 s electrons or the 2 s electrons? Explain.
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