Metallic Character of Transition Elements

According to the modern periodic table, as an element moves from left to right across a period, the metallic character of the element decreases. This occurs as a result of the fact that as a period progresses from left to right, the number of electrons and protons in an atom increases, resulting in an increase in the nuclear force exerted on the electrons, making it more difficult to lose electrons. The metallic character increases as one moves down the group, and this is due to the fact that as one moves down the group, the atomic radius increases, making it easier for electrons to be lost.

For the most part, the transition elements exhibit the typical metallic properties such as lustre and malleability. They also have high tensile strength, as well as excellent thermal and electrical conductivity. Zn, Cd, Hg, and Mn are the only elements that do not exhibit metallic characteristics at normal temperatures; the rest of the elements exhibit one or more metallic characteristics at normal temperatures. The elements, with the exception of metals, are hard and have low volatility, with the exception of the metals, which are exceptional.

Explanation for metallic character : 

Due to their low ionisation energies and the presence of several vacant orbitals in their outermost shell, transition elements exhibit metallic characteristics. This property encourages the formation of metallic bonds in transition metals, which results in the transition metals exhibiting characteristic metallic properties. The hardness of these metals indicates the presence of covalent bonds in their structure. This occurs as a result of the presence of unpaired d-electrons in transition metals. The d-orbital, which contains the unpaired electrons, has the potential to overlap and form covalent bonds with other electrons. The number of covalent bonds formed by transition metals increases in direct proportion to the number of unpaired electrons present in the transition metals. The metal’s hardness and strength are both increased even further as a result of this.

The metals chromium (Cr), tungsten (W), and molybdenum (Mo) contain the greatest number of unpaired d-electrons of any other element. As a result, these transition metals have extremely high hardness. In contrast, we have the metals zinc (Zn), cadmium (Cd), and mercury (Hg), which are not particularly difficult to work with because they do not contain unpaired d-electron pairs. They are extremely hard and have metallic characteristics, which indicates that they are characterised by the presence of both metallic and covalent bonding at the same time in these elements.

We have discussed the metallic nature of transition elements as well as the reasons for this characteristic. Install BYJU’S the learning app and enjoy the journey of learning in a unique and simplified way. 

Ductility : 

Metals have a physical property known as ductility, which means that if we pull on the metal, it will stretch rather than break. In other words, the ductile properties of a material refer to the material’s ability to undergo significant plastic deformation under tensile stress before rupturing. Nickel, copper, steel, and other ductile materials are examples of such materials.

Brittleness is defined as the property of a metal that breaks without forming stretch when subjected to tensile stress. It is also referred to as a “sudden failure.” Glass, cast iron, and other brittle materials are examples.

Ductility is an important consideration in engineering and manufacturing because it determines whether a material is suitable for a particular manufacturing process and whether it has the ability to withstand mechanical overload.

Ductility of transition metals : 

Transition metals are excellent heat and electricity conductors, and they are also excellent conductors of light. Their malleability means that they can be formed into sheets, and their ductility means that they can be formed into wires, among other things. They all have high melting and boiling points, and they are all solids at room temperature, with the exception of mercury (Hg), which is a liquid at this temperature.

Melting point of transition metals:

The melting points of most transition metal elements (with the exception of Zn, Cd, and Hg) are in excess of 900°C. The melting and boiling points of these elements are significantly higher than those of s-block and p-block elements.

In their metallic crystal lattice, transition metals exhibit extremely high melting and boiling points due to the presence of extremely strong metallic bonds as well as covalent bonds, which results in extremely high melting and boiling temperatures.

Furthermore, transition metal elements are tightly packed and held together by the strong metallic bonds that exist between them.

Inter-atomic metallic bonds between atoms are formed in transition metals by electrons from the ns-sub shell as well as odd electrons from (n-1)d-sub shell, which are both electrons from the ns-sub shell.

Conclusion : 

According to the modern periodic table, as an element moves from left to right across a period, the metallic character of the element decreases.Transition metals are excellent heat and electricity conductors, and they are also excellent conductors of light.The melting points of most transition metal elements (with the exception of Zn, Cd, and Hg) are in excess of 900°C. The melting and boiling points of these elements are significantly higher than those of s-block and p-block elements.