Metals and non-metals may be two different classes of elements, but they share some common chemical properties.
From oxidation to reactivity to their role in creating compounds or mixtures, both metals and non-metals have a wide range of characteristics that make them useful in various applications.
In this article, we will take an in-depth look at the chemical properties of metals and non-metals and explore the ways they are similar and different. Read on to learn more!
What are Chemical properties of metals?
The chemical properties of metals are determined by the number of valence electrons in the atom. Valence electrons are the outermost electrons in an atom and determine how the atom will react with other atoms. The more valence electrons an atom has, the more reactive it will be.
Metals generally have a low electronegativity, meaning they are willing to give up their valence electrons to other atoms. This makes them good conductors of electricity and heat. They are also malleable, meaning they can be pounded into thin sheets, and ductile, meaning they can be drawn into wires.
Non-metals generally have a high electronegativity, meaning they are not willing to give up their valence electrons to other atoms. This makes them poor conductors of electricity and heat. They are also brittle, meaning they break easily when pounded or drawn into wires.
Chemical properties of Transition metals
The electronic configuration of the d-block elements is such that they can readily lose or gain electrons to form cations or anions, respectively. As a result, these elements are known for their chemical reactivity.
Transition metals generally have high melting and boiling points and densities, as well as strong metallic bonds. They are also good conductors of electricity and heat.
The first-row transition metals (scandium through manganese) tend to be more reactive than the second-row transition metals (copper through zinc).
The increased reactivity is due to the fact that the 4s orbital is progressively filled before the 3d orbitals in the first row. Therefore, the 3d orbitals are relatively empty and more susceptible to electron transfer.
In addition, the smaller size of the first-row transition metals allows them to better donate electrons to achieve stability.
The lanthanides and actinides also exhibit similar trends in reactivity due to their filling of the f-orbitals.
The 4f orbitals are progressively filled before the 5d orbitals in the lanthanides, while the 5f orbitals are filled before the 6d orbitals in the actinides. Consequently, these elements are also known for their high chemical reactivity.
Chemical properties of Alkaline Earth metals
Alkaline Earth metals are a group of chemical elements in the periodic table with similar properties. They are all metals with a silvery-white appearance and high reactivity. All of the Alkaline Earth metals are found in nature, but only a few are used commercially.
The Alkaline Earth metals include: beryllium, magnesium, calcium, strontium, barium, and radium.
These elements all have similar properties due to their similar electron configurations. They are all highly reactive, meaning they readily form compounds with other elements.
The Alkaline Earth metals are also all silvery-white in color and have high densities.
Due to their high reactivity, Alkaline Earth metals are not found in pure form in nature. Instead, they are found as minerals or compounds.
For example, magnesium is found in the mineral dolomite (CaMg(CO3)2), and calcium is found in the mineral calcite (CaCO3).
Beryllium is found in the mineral beryl [(Be3Al2Si6O18)] , and strontium is found in the mineral strontianite (SrCO3).
While all of the Alkaline Earth metals are found in nature, only a few have commercial applications. Beryllium is used in aerospace and defense applications because of its low weight and high
What are the chemical properties of non-metals?
The chemical properties of non-metals can be divided into two groups: those that are similar to metals and those that are not.
The former group includes elements such as carbon and silicon, which form binary compounds with oxygen, hydrogen, and other non-metals. These compounds are similar to the corresponding metal oxides, hydrides, and halides.
The latter group comprises the remaining elements in the periodic table—the so-called chalcogens (oxygen and sulfur) and the halogens (fluorine, chlorine, bromine, iodine).
These elements show much greater variety in their chemical behavior than do metals.
The most important difference between metals and non-metals is in their bonding. Metals tend to form covalent or ionic bonds with other atoms, while non-metals tend to form only covalent bonds.
This difference is due to the fact that metals have a strong tendency to lose electrons, while non-metals have a strong tendency to gain them.
As a result, metal atoms are often found surrounded by a lattice of positive ions, while non-metal atoms are usually found bonded together in molecules.
Conclusion
In summary, metals and non-metals have distinct differences in their properties that can be observed at the chemical level.
Metals are generally malleable, ductile, shiny in appearance and good conductors of electricity and heat.
Non-metals tend to be brittle, dull in colour and poor conductors of electricity or heat.
Understanding the different chemical properties of these two types of elements helps us better understand the world around us.
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