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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 an inverse relationship: as atomic size increases, ionization energy decreases. This is due to larger atoms having their outer electrons farther from the nucleus, which makes it easier to remove these electrons with less energy required. (b) In the periodic table, Helium (He) has the largest ionization energy, and Francium (Fr) has the smallest ionization energy.

Step by step solution

01

Understanding Ionization Energy

Ionization energy is the amount of energy required to remove an electron from a neutral atom in the gas phase. It is usually expressed in electron volts (eV) or kilojoules per mole (kJ/mol). Ionization energy generally increases from left to right across a period and decreases from top to bottom within a group in the periodic table. This is because as atoms get smaller, their nuclear charge increases, making it more difficult to remove an electron due to increased attraction.
02

Relationship Between Atomic Size and Ionization Energy

In general, there is an inverse relationship between atomic size and ionization energy. As the atomic size increases, the ionization energy decreases. This is because larger atoms have their outer electrons farther away from the nucleus, and thus, the nucleus has less of a "hold" on them, making it easier to remove these electrons with less energy required.
03

Finding the Element with the Largest Ionization Energy

The element with the largest ionization energy is the one in the top right corner of the periodic table, excluding the noble gases. This is because elements in the top right have smaller atomic sizes and greater nuclear charges, making it more difficult to remove an electron. In this case, the element with the largest ionization energy is Helium (He).
04

Finding the Element with the Smallest Ionization Energy

The element with the smallest ionization energy is the one in the bottom left corner of the periodic table. This is because elements in the bottom left have larger atomic sizes and smaller nuclear charges, making it easier to remove an electron. In this case, the element with the smallest ionization energy is Francium (Fr). Therefore, the general relationship between the size of an atom and its first ionization energy is that as atomic size increases, ionization energy decreases. The element with the largest ionization energy in the periodic table is Helium (He), and the one with the smallest ionization energy is Francium (Fr).

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Most popular questions from this chapter

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) \(\mathrm{K}, \mathrm{Li}, \mathrm{Cs} ;\) (b) \(\mathrm{Pb}, \mathrm{Sn}, \mathrm{Si} ;\) (c) \(\mathrm{F}, \mathrm{O}, \mathrm{N}\)

Elements in group \(7 \mathrm{~A}\) in the periodic table are the halogens; elements in group \(6 \mathrm{~A}\) are called the chalcogens. (a) What is the most common oxidation state of the chalcogens compared to the halogens? Can you suggest an explanation for the difference? (b) For each of the following periodic properties, state whether the halogens or the chalcogens have larger values: atomic radii; ionic radii of the most common oxidation state; first ionization energy; second ionization energy.

Some metal oxides, such as \(\mathrm{Sc}_{2} \mathrm{O}_{3},\) do not react with pure water, but they do react when the solution becomes either acidic or basic. Do you expect \(\mathrm{Sc}_{2} \mathrm{O}_{3}\) to react when the solution becomes acidic or when it becomes basic? Write a balanced chemical equation to support your answer.

Write a balanced equation for the reaction that occurs in each of the following cases: (a) Chlorine reacts with water. (b) Barium metal is heated in an atmosphere of hydrogen gas. (c) Lithium reacts with sulfur. (d) Fluorine reacts with magnesium metal.

(a) How is the concept of effective nuclear charge used to simplify the numerous electron-electron repulsions in a manyelectron 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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