Learning of Metallic Character

The chemical properties related with the elements categorised as metals in periodic table are referred to as metallic character. The capacity of an element to lose the outermost valence electrons determines its metallic nature.

Metallic Character

Metallic character refers to a set of chemical traits which are linked with the metals. These chemical features are caused by the ease with which metals lose electrons and form cations (+vely charged ions).

Physical properties related to metallic character involve shiny appearance, metallic luster, high thermal conductivity, high density, and high electrical conductivity. 

The majority of metals are malleable and ductile, meaning they can be bent without breaking. Many metals are hard and dense.

Elements Having Metallic Character

Metals, that are all found on the periodic table’s left side, have a metallic property. Hydrogen, on the other hand, is non-metal under normal circumstances. Even though hydrogen behaves like a metal if it is a liquid or solid, it’s best to think of it as non-metallic for most applications.

Metallic elements are found in certain groups or columns of the periodic table, such as alkaline earth metals, alkali metals, transition metals (including actinides and lanthanide below the main body), and basic metals. Base metals, ferrous metals, heavy metals, noble metals, and precious metals are some of the other types of metals. Although the metalloids have certain metallic features, they also have non-metallic properties.

Trends in Periodic Table

Even for elements that are regarded highly metallic, metals have a wide range of values for these attributes. Mercury, for example, is a liquid rather than a solid at ambient temperature. Its electrical conductivity is also lower than that of other metals. Some noble metals are brittle as opposed to malleable. These metals are still lustrous and metallic-looking, and they also form cations.

Metallic Character Down the Group

As we go down the groups, the metallic character tends to increases. Because the ionisation energy reduces as you go down a group (and increases as you go up a group), metals lower in the group have a greater propensity to lose electrons, making them more reactive. Furthermore, when one moves down a group, the atomic radius grows, pushing the outside electrons further away from nucleus and making this electron least attracted to the nucleus.

Metallic Character and Alloys

Metallic character is usually used to define the pure elements, alloys can also have it. Bronze and most copper, magnesium, aluminium, and titanium alloys, for example, have a high amount of metallicity. Some metallic alloys are made entirely of metals, while the majority comprise metalloids and nonmetals while still retaining metal characteristics.

Metallic Character of Metals

The degree of reactivity of the metal is defined by its metallic character. Metals have low ionisation energies, which indicates that they lose electrons in chemical processes. Within a complex, metal atoms have a relatively low affinity for electrons. Their low electronegativities imply this.

Caesium, which isn’t really found in the nature as a free element, is the most reactive metal. It interacts violently with water and spontaneously ignites in the air.

In the alkali metal group, francium is below caesium. It is, however, so uncommon that most of its characteristics have never been observed.

Non-metallic Character

The ability of an element to receive electrons and create anions or negative ions is recognised as its non-metallic character.

Non-metals have a strong affinity for electrons within a compound and tend to gain electrons in the chemical processes. The most reactive non-metals are found in the periodic table’s upper right corner. Fluorine is the most reactive non-metal because noble gases constitute a distinct group due to their lack of reactivity. It does not exist in nature as a free element. Fluorine gas reacts violently with a wide range of other elements and compounds, making it the most hazardous substance ever discovered.

Conclusion

Metallic character depends on the capacity of an element to lose the outer valence electrons. Examples of properties which are related to metallic character involve metallic luster, thermal and electrical conductivity, ductility, hardness, and malleability. The most metallic element is Francium, which is followed by Cesium.

As we go down the groups, metallic character of an element increases.

The non-metallic character of an element is defined as its ability to accept electrons and produce anions or negative ions.