Ch.8 - Periodic Properties of the Elements

Tro - Chemistry: A Molecular Approach 4th Edition

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Tro 4th Edition

Ch.8 - Periodic Properties of the Elements

Problem 73c

Chapter 8, Problem 73c

Choose the element with the higher first ionization energy from each pair. c. As or At

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First, understand that ionization energy is the energy required to remove an electron from an atom in the gaseous state.

Ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.

Identify the position of arsenic (As) and astatine (At) in the periodic table. As is in group 15 and period 4, while At is in group 17 and period 6.

Since As is higher up in the periodic table compared to At, it is expected to have a higher first ionization energy because it is closer to the top of its group.

Conclude that arsenic (As) has a higher first ionization energy than astatine (At) due to its position in the periodic table.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionization Energy

Ionization energy is the energy required to remove an electron from a gaseous atom or ion. It is a key factor in determining an element's reactivity and is influenced by the atomic size and the effective nuclear charge. Generally, ionization energy increases across a period and decreases down a group in the periodic table.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For ionization energy, elements on the right side of the table tend to have higher ionization energies than those on the left, while elements higher up in a group have higher ionization energies than those lower down due to decreased electron shielding.

Comparison of Elements

When comparing elements like arsenic (As) and astatine (At), it is essential to consider their positions in the periodic table. Astatine is located below arsenic in Group 17, which typically results in a lower ionization energy due to increased atomic size and electron shielding. Understanding these positions helps predict which element will have a higher first ionization energy.

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