Question

Which of the following metals have more than one oxidation state? (a) \(\mathrm{Zn}\) (b) \(\mathrm{Mn}\) (c) \(\mathrm{Sr}\) (d) \(\overline{\mathrm{Cu}}\)

Short answer

Manganese (Mn) and Copper (Cu) have more than one oxidation state.

Step-by-step solution

Determine the Oxidation States of Each Metal

First, we need to identify the common oxidation states of the metals provided, which are Zinc (Zn), Manganese (Mn), Strontium (Sr), and Copper (Cu). These oxidation states are usually found in a periodic table or a chemistry reference.

Analyze Each Metal

- **Zinc (Zn):** Typically has only one oxidation state, which is +2. - **Manganese (Mn):** Can have multiple oxidation states, including +2, +3, +4, +6, and +7. - **Strontium (Sr):** Typically shows one oxidation state, which is +2. - **Copper (Cu):** Commonly found in two oxidation states: +1 and +2.

Identify Metals with Multiple Oxidation States

From the analysis: - Zinc (Zn) has only +2. - Manganese (Mn) has multiple oxidation states. - Strontium (Sr) has only +2. - Copper (Cu) also has multiple oxidation states.

Conclude Which Metals Have Multiple Oxidation States

Based on the previous analysis, the metals with more than one oxidation state are Manganese (Mn) and Copper (Cu).

Key concepts

Transition Metals

Transition metals are a unique group of elements found in the middle of the periodic table. These metals, which include elements like manganese (Mn) and copper (Cu), are known for their ability to possess multiple oxidation states. This characteristic is due to the involvement of their d-electrons in chemical reactions.
To identify a transition metal, look for elements that have partially filled d orbital electrons. Their capability to switch oxidation states makes them highly versatile and valuable in many chemical processes.
For example, manganese can exhibit a remarkable range of oxidation states: +2, +3, +4, +6, and +7. Similarly, copper can transition between +1 and +2 oxidation states. These properties are exploited in various industrial applications, including catalysis and electronic materials.

Periodic Table

The periodic table is a comprehensive chart that organizes all known chemical elements in a systematic way based on their atomic number, electron configuration, and recurring chemical properties. It provides crucial information about each element and allows chemists to derive and predict various properties of the elements, such as oxidation states.
Transition metals occupy the central block of the periodic table, specifically in groups 3 to 12. They are notable for their wide range of oxidation states, often providing multiple options for chemical bonding and reactions.

• The position of an element in the periodic table can influence its chemical behavior, including its preferred oxidation states.
• The table helps to quickly identify trends across different element groups, like how the transition metals can change states to form ions with different charges.

Understanding the layout and the pattern of the periodic table can greatly enhance the grasp of an element's properties and their reactions.

Chemical Properties

The chemical properties of metals are determined by their ability to lose electrons and form positive ions (cations). This is especially true for transition metals, which can form ions in multiple oxidation states due to the involvement of their d electrons.
These properties significantly influence their roles in various chemical reactions and industrial processes. For instance, the ability of transition metals to change oxidation states allows them to act as catalysts in numerous biochemical and industrial reactions.

• Manganese, in its various oxidation states, participates in many oxidation-reduction reactions.
• Copper's variable oxidation states make it crucial in electrical wiring and coins, due to its conductivity and corrosion resistance.

Understanding these properties is essential for predicting how metals will behave in different chemical environments, which is vital for chemistry students studying the versatility and utility of metals in the periodic table.