Give the charge most likely to result from ionization of the following nonmetals. (b) Sulfur

Verified step by step guidance

1. Identify the group number of sulfur in the periodic table. Sulfur is in group 16.
2. Determine the number of valence electrons for sulfur. Elements in group 16 have 6 valence electrons.
3. Consider the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a full set of 8 valence electrons.
4. Calculate how many electrons sulfur needs to gain to achieve a full octet. Sulfur needs 2 more electrons to reach 8 valence electrons.
5. Conclude that sulfur will likely gain 2 electrons during ionization, resulting in a charge of -2.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion. For nonmetals like sulfur, this energy is relatively high due to their tendency to attract electrons. Understanding ionization energy helps predict how easily an atom can lose an electron and form a positive ion.

Common Oxidation States

Nonmetals often exhibit specific oxidation states based on their electron configurations. Sulfur, for instance, commonly has oxidation states of -2, +4, and +6. Recognizing these states is crucial for predicting the charge that sulfur will likely adopt when it ionizes.

Electron Affinity

Electron affinity refers to the energy change that occurs when an electron is added to a neutral atom. For sulfur, the addition of an electron typically results in a stable anion with a -2 charge, as it seeks to achieve a full outer electron shell. This concept is essential for understanding the behavior of sulfur in ionic compounds.