Chem(6.1) What are Transition Metals? 1. You need to respond to my questions and to at least four classmates substantially over three days in a manner that furthers the discussion. Some ideas for responses might be: 2. Go a step further and explain what specifically happens to transition metals that results in solutions that give off distinct colors. 3. Give an example of a specific transition metal solution, including the oxidation state of the transition metal, and the color of the solution, and the complex ion that the transition metal forms in that solution if applicable.

QUESTION

Chem(6.1)

What are Transition Metals?

1. You need to respond to my questions and to at least four classmates substantially over three days in a manner that furthers the discussion. Some ideas for responses might be:

2. Go a step further and explain what specifically happens to transition metals that results in solutions that give off distinct colors.

3. Give an example of a specific transition metal solution, including the oxidation state of the transition metal, and the color of the solution, and the complex ion that the transition metal forms in that solution if applicable.

Chem (6.2)

What are complex ions?

1. You need to respond to my questions and to at least four classmates substantially over three days in a manner that furthers the discussion. Some ideas for responses might be:

2. Go a step further and explain how complex ions are formed, and how to name a complex ion.

3. Give an example of a specific complex ion including EITHER it’s formula or its name. Ask your fellow classmates to give either the missing name or formula using the rules for naming complex ions to explain how the name or formula was determined.

ANSWER

Chem(6.1)

Transition metals are a group of elements that are located in the d-block of the periodic table. They are called transition metals because their electron configurations involve the filling of inner d orbitals. These elements exhibit several common properties, including the ability to form complex ions, multiple oxidation states, and the tendency to form colored compounds.

When transition metals form solutions that give off distinct colors, it is due to the presence of unpaired d electrons in their outermost energy levels. The absorption of light by these electrons causes the solution to appear colored (Why Do Cations of the Same Transition Metal With Different Charges Show Different Colors?, n.d.). The specific color observed depends on the arrangement and energy levels of the d electrons. Transition metals exhibit a wide range of colors, such as the vibrant blue of copper sulfate, the deep purple of potassium permanganate, and the yellow of iron(III) chloride solutions.

An example of a specific transition metal solution is copper sulfate (CuSO4). In this compound, copper is in the +2 oxidation state. When dissolved in water, copper sulfate forms a blue solution. The transition metal copper (Cu) in this case forms a complex ion with the sulfate (SO4) anion, resulting in the formation of [Cu(H2O)6]2+ complex. This complex ion is responsible for the blue color observed in the solution.

Overall, the distinct colors exhibited by transition metal solutions arise from the interactions between light and the unpaired d electrons in their outermost energy levels.

Chem(6.2)

Complex ions, also known as coordination complexes, are species that consist of a central metal ion or atom surrounded by one or more ligands. Ligands are typically molecules or ions that donate electron pairs to the central metal ion, forming coordinate covalent bonds (Complex Ions, n.d.). Complex ions play a significant role in many chemical reactions and have diverse applications in fields such as catalysis, medicine, and materials science.

Complex ions are formed through a process called coordination or ligand exchange. The central metal ion attracts ligands and forms coordinate bonds by accepting electron pairs from the ligands. The number of ligands that surround the central metal ion is determined by its coordination number, which depends on the size and charge of the metal ion as well as the size and charge of the ligands.

Naming complex ions follows a specific set of rules. The name of a complex ion consists of two parts: the name of the ligands followed by the name of the central metal ion (Libretexts, 2023). The ligands are named first, using specific prefixes to indicate the number of ligands and their identity. The name of the metal ion is modified based on its oxidation state using Roman numerals in parentheses. If the complex ion has a charge, it is indicated by a superscript after the name.

For example, consider the complex ion [Fe(CN)6]4-. In this case, the formula tells us that there are six cyanide ligands coordinated to the central metal ion, iron (Fe). The cyanide ligand is named with the prefix “cyano-.” The oxidation state of iron is +2, as indicated by the Roman numeral (II) in parentheses. The overall charge of the complex ion is 4-, represented by the superscript.

References

Complex Ions. (n.d.). https://www.chem.fsu.edu/chemlab/chm1046course/complexions.html 

Libretexts. (2023). Nomenclature of Coordination Complexes. Chemistry LibreTexts. https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Coordination_Chemistry/Structure_and_Nomenclature_of_Coordination_Compounds/Nomenclature_of_Coordination_Complexes 

Why do cations of the same transition metal with different charges show different colors? (n.d.). Quora. https://www.quora.com/Why-do-cations-of-the-same-transition-metal-with-different-charges-show-different-colors