Determine the oxidation number of sulfur in each of the following substances: (e) Locate sulfur in the periodic table in Exercise 4.47; what region is it in?

Verified step by step guidance

1. Identify the oxidation states of other atoms in the compounds mentioned in Exercise 4.47. Common oxidation states for elements like oxygen and hydrogen are -2 and +1, respectively.
2. Apply the rule that the sum of the oxidation numbers in a neutral compound must equal zero. For polyatomic ions, the sum of the oxidation numbers must equal the charge of the ion.
3. For each compound, set up an equation where the sum of the oxidation numbers multiplied by their respective subscripts equals zero (or the charge of the ion). Include the known oxidation states and solve for the oxidation number of sulfur.
4. To locate sulfur in the periodic table, find it by its symbol 'S'. Note its group and period to determine the region it belongs to in the periodic table.
5. Identify the region (e.g., nonmetals, chalcogens) where sulfur is located and describe its general properties based on its position in the periodic table.

Key Concepts

Oxidation Number

The oxidation number, or oxidation state, is a value assigned to an element in a compound that reflects its degree of oxidation or reduction. It indicates the number of electrons an atom gains, loses, or shares when forming chemical bonds. Understanding how to assign oxidation numbers is crucial for identifying redox reactions and balancing chemical equations.

Periodic Table Groups

The periodic table is organized into groups and periods, with elements in the same group sharing similar chemical properties. Sulfur is located in Group 16, also known as the chalcogens, which includes oxygen and selenium. This group is characterized by elements that typically have six valence electrons, influencing their reactivity and bonding behavior.

Chemical Bonding and Valence Electrons

Chemical bonding involves the interaction between atoms to form molecules, primarily through the sharing or transfer of valence electrons. The number of valence electrons determines how an element will bond with others. For sulfur, having six valence electrons allows it to form various compounds, influencing its oxidation states in different chemical environments.