The right side of the periodic table has the p-block elements and ranges from number 13 to number 18. The outermost electronics of the block are in the p orbital consisting of six elements named boron, carbon, nitrogen, oxygen, fluorine, helium. However, helium belongs to the s-block elements despite being a part of group 18. There are different electronic configurations of the elements, and the elements also have different physical properties and chemical properties. The sum of the s- and p-electrons shows the maximum oxidation state. All three types of elements are present in the p-block, metals, metalloids and nonmetals. On moving in the lower direction of the group, the atomic radii increases. All the elements of the group have a family of their own. 

1. The general characteristics of the p-block elements

• Electronic Configuration – The electronic configuration refers to the distribution of electrons of a particular atom in the atomic orbits. The electronic configuration of the valence shell of the p-block elements is ns2np1-6. However, each group in the p-block has a different configuration. 

• Chemical Behavior – The p-block elements of the periodic table are exceptional. This is because p-block is the only one where along with metals, both metalloids and nonmetals are present, unlike the other blocks. As we move downwards in the inner core, we observe that the non-metallic character of all the groups keeps on decreasing. 

• Anomalous behavior of Boron – The first element of each group shows properties different from all the other elements of the group. This is also true in the case of p-block elements. The first element, boron, shows anomalous behavior. Boron is the lightest element, having a very high boiling and melting point. It is non-metallic and a bad conductor of electricity. The covalency of boron limits to 4, and the d-orbitals are absent.

• Oxidation state – to find out the maximum oxidation state, the sum of ns and np electrons has to be obtained. This results in a total number of valence electrons. Some elements of the p-block have a limited number of oxidations, while others have a lot. On moving towards the right, the number increases. 

• Inert Pair Effect – This effect refers to the phenomenon of the pairing of the remaining electrons in the valence shell. The inner orbital is unable to shield the electrons. The valence s- electrons of the heavier elements in the p-block, are reluctant to participate in the bond formation. This is known as the inert pair effect. Hence the valence s- electrons are more susceptible to exposure of nucleus. As a result, the oxidation state decreases on moving downwards. 

• Ionization – when we move from left to right in the period, the ionization energy begins to increase because of the different orbitals that are at times full and at times half filled. 

• Additional properties of p-block elements – The elements react and form acidic oxides. The phenomenon of allotropy can be found in elements like carbon, silicon, sulfur, boron, tin, phosphorus and more. The catenation property is found in elements like nitrogen, germanium, oxygen, carbon, silicon and more. 

2. Properties of p-block elements 

3. P-block elements periodic table 

Present on the right-hand side of the periodic table, it consists of six columns in total. It begins with the number 13 and ends at the number 18. Helium, present at the top, is not included. All in all, 35 elements are present in the periodic table of p-block elements. Boron, Carbon, Nitrogen, Aluminum, Silicon, Tin, Gallium, and Bromine are some examples.

4. Compounds of p-block elements 

• Ozone- An allotrope of oxygen, ozone is a gas found in the earth’s atmosphere. When oxygen reacts with the sun’s ultraviolet rays, ozone is formed. It protects the earth from the harmful rays of the sun. 

• Ammonia – A compound made from hydrogen and nitrogen, ammonia forms when animals’ bodies decay. It is also present in soil and is important for life. 

• Sulphuric acid – It is a liquid that is colorless and corrosive. It releases heat when mixed with water. 

• Phosphine – is formed when phosphorus is heated in potassium carbonate solution and is an important part of the biochemical cycle of phosphorus. 

5. Uses of p-block elements 

The properties of p-block elements are such that these elements in their various forms become extremely useful. Some of the uses are listed below – 

• Borax is used as a cleaning agent to harden the steel in aircrafts and bulletproof vests.

• Aluminum can be used for making utensils, foils, cables etc.

• Silicon, gallium and arsenic can be used as semiconductors.

• Iodine is used to produce iodine tinctures in labs.

• Chlorine acts as a disinfectant and is used in swimming pools.

CONCLUSION

The p-block elements range from group 13 to group 18, and their valence electron falls in the p-orbital. The electronic configuration differs in the inner core. It is a unique period because there are metals, nonmetals and metalloids present in this element. The non-metallic character increases on moving downwards, and the first element of the period, which is boron, is anomalous in nature due to its high boiling and melting points. The elements show the inert pair effect and for acidic oxides on reaction. Ozone, ammonia, and sulphuric acid are some of the compounds. The elements in this period can be used for a variety of things. They act as cleaning agents, are used for making vessels, as disinfectants.