Transition Metals - The Transition Metals (A-Level Chemistry)
The Transition Metals
Electronic Structure of Transition Metals and Their Ions
Defining Transition Metals
Transition metals are found in the “d-block” of the periodic table.
The definition of transition metals is they have an incomplete d sub- level in their atoms or ions. This means they can form one or more stable ions with a partially filled d sub-shells.
Examples of Transition Metals
• Scandium – Normally forms Sc³+ ion, in which the 4s² and 3d¹ electrons are lost. There are no electrons in the 3d subshell, so scandium is not a transition metal by definition.
• Zinc – Forms Zn²+ ions. The 4s² electrons are lost, leaving a full 3d subshell. As the 3d shell is not partially filled, zinc is also not a transition metal by definition.
Electronic Structure
Transition metals in period four range from titanium to copper.
The properties of transition metals are directly related to their electronic structure.
The 4s subshell and 3d subshells have very similar energies. The 4s subshell is at a lower energy than the 3d subshell, so the 4s subshell fills up first. There are two exceptions: chromium and copper:
• Chromium – Chromium atoms can promote a 4s electron to the 3d subshell. This results in a half-filled 4s and 3d subshell: (Ar)3d54s1
• Copper – Copper atoms can promote a 4s electron to the 3d subshell. This results in a fully filled 3-d shell: (Ar)3d10.
These electron arrangements are more stable than having fully filled 4s subshells.
Transition metals are a group of metallic elements in the middle of the periodic table that have partially filled d-orbitals.
Examples of Transition Metals include iron, copper, nickel, chromium, and gold.
Transition Metals have many unique properties, including high melting and boiling points, high density, and good conductivity.
Transition Metals have unique electron configurations that give them distinct chemical and physical properties. They also tend to form complex ions and compounds due to their ability to form multiple oxidation states.
An oxidation state is a measure of the degree of oxidation of an atom in a compound. It is represented by a positive or negative number, and it indicates the number of electrons an atom has gained or lost.
Transition Metals can form multiple oxidation states due to the presence of partially filled d-orbitals. These orbitals can be easily filled or emptied by gaining or losing electrons, allowing the metal to form ions with different oxidation states.
A complex ion is an ion made up of a central metal ion and one or more ligands. Ligands are molecules or ions that can donate electrons to the central metal ion, forming coordinate covalent bonds.
Complex ions often have vibrant colors and are more stable than simple ions. They also have unique magnetic properties and can form chelates with other ions.
Chelates are compounds formed when a central metal ion is bonded to a ligand through more than one coordination site. The resulting complex is more stable than the individual ions, and it can be used in applications such as medicine and environmental science.
Transition Metals have many important uses in industry, medicine, and technology. For example, iron is used in the production of steel, while copper is used in electrical wiring. Platinum is used in catalytic converters in automobiles, and gold is used in jewelry and as a currency.
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