Advanced Placement (AP) Chemistry Practice Exam

The oxidation state of an element in a compound is determined by following established rules based on the type of element and the nature of its bonding within the compound. These rules include considerations such as the usual oxidation states of individual elements, the electronegativity differences between bonded atoms, and the overall charge of the compound.

For instance, oxidation states are assigned by considering the most common states of elements, such as hydrogen being +1, oxygen being -2, and alkali metals being +1 in compounds. Also, in ionic compounds, the sum of the oxidation states must equal the net charge of the compound, while in covalent compounds, the valence electrons can help establish a formal oxidation state based on bonding.

This systematic approach ensures accurate determination of oxidation states, which are crucial for predicting reactivity, understanding redox processes, and balancing chemical equations. The other choices do not provide a comprehensive or correct methodology for determining oxidation states; counting outer shell electrons alone does not encapsulate all factors involved, and the considerations of ionic radius and molecular mass do not contribute to oxidation state determination effectively.