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Chapter 7: Problem 129

The electron affinity for sulfur is more exothermic than that for oxygen. How do you account for this?

Short Answer

Expert verified
The more exothermic electron affinity in sulfur compared to oxygen can be attributed to two factors: the shielding effect of inner electrons and the larger size of the 3p orbitals in sulfur. Due to these factors, sulfur experiences weaker electrostatic attractions, making it easier to add an electron to its outermost shell and releasing more energy than oxygen during the process.

Step by step solution

01

Define Electron Affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gaseous state, forming a negative ion. A more negative, or more exothermic, electron affinity indicates that the atom releases more energy when gaining an electron.
02

Compare Electron Configurations

Let's look at the electron configurations for oxygen and sulfur. Oxygen (atomic number 8): 1s虏 2s虏 鈧俻鈦� Sulfur (atomic number 16): 1s虏 2s虏 鈧俻鈦� 3s虏 鈧僷鈦� Oxygen is in Period 2 and Group 16, whereas sulfur is in Period 3 and Group 16 in the periodic table. Both elements have the same outermost p orbitals, which are 2p orbitals for oxygen and 3p orbitals for sulfur.
03

Explain Shielding Effect

As we move down a group (from Period 2 to Period 3 in this case), the atomic number increases and additional electron orbitals are added. These inner shells are filled with electrons which "shield" or protect the outer electrons from the attraction of the nucleus. This shielding effect makes it easier for an electron to be added to the outermost shell as the repulsion from the inner electrons can counteract the electrostatic attraction from the nucleus.
04

Understand Orbital Size

In the case of oxygen and sulfur, the 3p orbitals in sulfur are larger than the 2p orbitals in oxygen. This means that electrons in the 3p orbitals are farther away from the nucleus, and the electrostatic attraction is weaker. As a result, it is easier to add an electron to the sulfur atom than the oxygen atom.
05

Combine the reasons

The shielding effect of the inner electrons and the larger size of the 3p orbitals in sulfur make it easier to add an electron to the atom. Consequently, sulfur has a more exothermic electron affinity than oxygen. This is because more energy is released when an electron is added to sulfur's 3p orbitals than when an electron is added to oxygen's 2p orbitals due to weaker electrostatic attractions in sulfur.

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Most popular questions from this chapter

A certain oxygen atom has the electron configuration 1\(s^{2} 2 s^{2} 2 p_{x}^{2} 2 p_{y}^{2} .\) How many unpaired electrons are present? Is this an excited state of oxygen? In going from this state to the ground state, would energy be released or absorbed?

Account for the fact that the line that separates the metals from the nonmetals on the periodic table is diagonal downward to the right instead of horizontal or vertical.

The Bohr model only works for one electron species. Why do we discuss it in this text (what鈥檚 good about it)?

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically? c. What will be the formula of the neutral binary compounds it forms with sodium, magnesium, carbon, and oxygen? d. What oxyanions would you expect Uus to form?

Which has the larger second ionization energy, lithium or beryllium? Why?
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