Complete the exercises below. Write the chemical formula for each of the following compounds, and indicate the oxidation state of the group 6A element in each: a. sulfur tetrachloride, b. selenium trioxide, c. sodium thiosulfate, d. hydrogen sulfide, e. sulfuric acid, f. sulfur dioxide, g. mercury telluride.

A chemical formula represents the composition of a compound, indicating the types and numbers of atoms present. For example, in sulfur tetrachloride (SCl4), the formula shows one sulfur atom bonded to four chlorine atoms. Understanding how to derive these formulas involves knowledge of valence electrons and bonding patterns.

The oxidation state, or oxidation number, of an element in a compound reflects its degree of oxidation or reduction. It is a useful concept for understanding electron transfer in reactions. For instance, in sulfuric acid (H2SO4), sulfur has an oxidation state of +6, indicating it has lost electrons compared to its elemental form.

Group 6A elements, also known as the chalcogens, include oxygen, sulfur, selenium, and tellurium. These elements typically exhibit a range of oxidation states, commonly -2, 0, +4, and +6, depending on their bonding environment. Recognizing the typical oxidation states of these elements is crucial for determining their behavior in various compounds.