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Ch.8 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.8 - Periodic Properties of the ElementsProblem 73d
Chapter 8, Problem 73d

Choose the element with the higher first ionization energy from each pair. d. P or Sn

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1
Step 1: Understand the concept of ionization energy. Ionization energy is the energy required to remove an electron from an atom or ion. The higher the ionization energy, the more difficult it is to remove an electron.
Step 2: Know that ionization energy generally increases from left to right across a period in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, which increases the positive charge and pulls the electrons closer to the nucleus, making them harder to remove.
Step 3: Also, ionization energy generally decreases from top to bottom within a group in the periodic table. This is because as you move down a group, the number of energy levels increases, which means the outermost electrons are further from the nucleus and easier to remove.
Step 4: Locate the elements P (Phosphorus) and Sn (Tin) on the periodic table. Phosphorus is in the 3rd period and group 15, while Tin is in the 5th period and group 14.
Step 5: Based on the trends in ionization energy and the positions of P and Sn on the periodic table, determine which element has the higher first ionization energy. Since P is to the right and above Sn on the periodic table, it should have a higher first ionization energy.

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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.
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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. Understanding these trends helps in comparing the ionization energies of different elements.
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Comparison of Elements

When comparing elements like phosphorus (P) and tin (Sn), it is essential to consider their positions in the periodic table. Phosphorus is located in Group 15 and Period 3, while tin is in Group 14 and Period 5. Due to its higher effective nuclear charge and smaller atomic radius, phosphorus is expected to have a higher first ionization energy than tin.
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Related Practice
Textbook Question

Choose the element with the higher first ionization energy from each pair. a. Br or Bi

Textbook Question

Choose the element with the higher first ionization energy from each pair. b. Na or Rb

Textbook Question

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

Textbook Question

Choose the element with the higher first ionization energy from each pair. a. P or I b. Si or Cl c. P or Sb d. Ga or Ge

Textbook Question

Arrange these elements in order of increasing first ionization energy: Si, F, In, N.