Question

Determine the highest possible oxidation state for each element. 26.2 a. V b. Re C. \(Pd\)

Short answer

The highest oxidation state of V is +5, Re is +7, and Pd is +4.

Step-by-step solution

Understanding oxidation states for Vanadium (V)

The highest oxidation state of an element is given by the number of valence electrons it can use for bonding. Vanadium (V) is in group 5 of the periodic table, which means it has 5 valence electrons and can reach an oxidation state of +5 by losing all its valence electrons.

Determining the highest oxidation state for Rhenium (Re)

Rhenium (Re) is in group 7 of the periodic table. Its highest oxidation state is typically +7, corresponding to the loss of all its valence electrons. However, Rhenium can achieve an oxidation state of +7 when it forms compounds like \( ReO_4^- \) or \( ReF_7 \).

Analyzing the case for Palladium (Pd)

Palladium (Pd) is in the 10th group of the periodic table. Group 10 elements typically have a maximum oxidation state equal to the number of electrons in the 'd' orbital, which is 10 electrons for palladium. However, in practice, palladium usually achieves its highest oxidation state of +4, as seen in compounds like \( PdO_2 \).

Key concepts

Vanadium Oxidation State

Vanadium (V) is an element that showcases how intriguing chemistry can be. Found in group 5 of the periodic table, it has 5 valence electrons, which are the electrons in the outermost shell of an atom that are available for bonding. These valence electrons are the key to understanding oxidation states, particularly how an element like vanadium can form compounds by either losing or sharing these electrons.

The highest oxidation state of vanadium is +5. This state occurs when vanadium loses all its valence electrons, forming a positively charged ion. Its range of oxidation states, from +2 to +5, allows vanadium to form diverse compounds, each with unique properties and uses. The vanadium (V) ion in particular shows how variable oxidation states can be, tying in directly with the versatile nature of this element in chemical reactions.

Rhenium Oxidation State

Rhenium (Re) sits in group 7 of the periodic table and inherently comes with 7 valence electrons. Its highest oxidation state is generally recognized as +7, which aligns with the total number of its valence electrons.

However, there's more to the story. Rhenium sometimes behaves in extraordinary ways, expanding beyond the expected norms. For instance, in certain compounds like perrhenates (\( ReO_4^- \)) and rhenium heptafluoride (\( ReF_7 \)), rhenium actually reaches this maximal oxidation state of +7. Such compounds are prime examples of rhenium's rich chemistry and are the reason why learning about valence electrons and how they contribute to oxidation states is essential in understanding the fascinating world of inorganic chemistry.

Palladium Oxidation State

Stepping further into the periodic table, we encounter palladium (Pd), which is part of the 10th group. With moving to this section of the periodic table, the nature of oxidation states becomes more nuanced. Palladium, with its 'd' electron configuration, theoretically could have up to 10 valence electrons playing a role in its oxidation states.

However, through empirical observation, the most common and highest oxidation state for palladium is +4. This state can be seen in compounds such as palladium(II) oxide (\( PdO_2 \)), which is often used as a catalyst. Understanding the practical versus theoretical oxidation states emphasizes that chemistry is both an exact science and one anchored in real-world experimentation.

Valence Electrons

The concept of valence electrons is central to predicting the chemical behavior of elements. Valence electrons are located in the outermost electron shell of an atom and play a pivotal role in determining how an element will react with others. They are the 'social' electrons, reaching out to form bonds with neighboring atoms.

Elements strive to achieve a full valence shell, leading to stable electron configurations often seen in noble gases. Whether by losing, gaining, or sharing these electrons, they determine the type of bond (ionic or covalent) that will form. Through this, one can understand trends in the periodic table and predict chemical reactions, leading to a better comprehension of both organic and inorganic chemistry.

Periodic Table

The periodic table is not only a chemist's roadmap, but it is also a treasure trove of information, outlining the properties of each element. Its arrangement allows us to grasp how elements relate to each other and how they will behave in chemical reactions. Each column, known as a group, contains elements with similar chemical properties and the same number of valence electrons. These shared characteristics give us insights into understanding elements' reactivity and the types of compounds they can form.

The periodic table informs us about trends in atomic size, electronegativity, ionization energy, and metallic character, which all hinge on the configuration of valence electrons. It's a dynamic tool that, when mastered, can reveal the secrets of chemical behavior and interactions, laying the foundation for all chemical knowledge.