The p-Block Elements

The p-block is located on the right side of the periodic table. The p-block elements are unified by the valence electrons and consist of six lobed shapes coming out of a central point at evenly spaced angles arranged in three-dimensional spaces.

This block contains variables of elements like metals, metalloids, and non-metals as well. Hence, the general properties will vary naturally to a great extent. The metals like Al, Ga, In, Tl, Sn, Pb, Bi have a shiny look, good conductor of electricity and heat, malleable, ductile, high melting and boiling points, and many more.

Similarly, non-metals like C, N, P, O, S, Se show characteristics opposite to metals like poor conductivity of heat and electricity, non-ductile, malleability, etc. And the metalloids B, Si, Ge, As, Sb, Te, Po will show up characteristics that mix up both the properties. Metalloids mix up with metals and non-metals to form p-type and n-type semiconductors, respectively.

Group 13 elements- The Boron Family

The members of this family constitute B, Al, Ga, In, and Tl. The general electronic configuration of this family is ns2np1. Down the group, the atomic radii increases, but the ionisation enthalpy increases due to an increase in its metallic characteristics.

Electro-negativity first decreases then increases. The physical properties of the boron family consist of low melting points and high electrical conductivity. Some elements can exist in a liquid state in very high temperatures, and the density increases down the group.

The chemical properties of this family include the oxidation state in two forms, i.e., +1 and+3 forms. They form electron deficit molecules. On reacting with air, the boron and aluminium form nitrides which are acidic in nature, and the elements present in the bottom of the periodic table form basic compounds.

All the elements react vigorously with halogen to form trihalides except TlI3. Some of the important products of boron are Borax, Orthoboric acid, Diborane, and Borohydrides.

Group 14 elements- The Carbon Family

The members of this family consist of C, Si, Ge, Sn, and Pb. The general electronic configuration is ns2np2. Down the group, atomic radii increase, and the ionisation effect increases due to the poor shielding effect of intervening d and f orbitals. The electro-negativity is more than in comparison to the boron family. The general physical properties are similar to that of the metalloids. 

The chemical properties like oxidation states vary from +4 to+2. It reacts with oxygen molecules to form monoxide and dioxides, and in the case of halogen, it forms tetrahalide covalent bonds. Carbon element exists in the allotropic form of diamond, graphite, and fluorescent ball. Some of the major compounds formed are carbon dioxide, silicon dioxide, silicones, zeolites, and silicates.

Group 15 elements- The Nitrogen Family

The members are N, P, As, Sb and Bi. They are collectively said to be pnicogens. The general electronic configuration is ns2np3. As we move down the group, ionisation potential and electro-negativity of elements decrease, whereas the metallic character and density increase.

The chemical properties like oxidation state are variable of -3, +3, and+5, and nitrogen exhibits +1, +2, +3, +4, and +5 only. The member of this family reacts with the halogen group to form trihalides and pentahalides, whereas, in the case of oxygen, it forms oxyacids.

Group 16 elements- The Oxygen Family

The oxygen family has its family members, namely O, S, Se, Te, and Po. This family is otherwise said to be chalcogens, which means the ore-forming elements due to its availability on a large scale in the earth’s crust in the form of oxides and sulphides.

Oxygen is the most abundant of all elements found among the others in this particular family. The general electronic configuration of this family is ns2np4. The physical properties of the elements of this group are their existence in the solid form, except to that of the oxygen.

The element possesses high ionisation enthalpy due to its small size due to increased effective nuclear force of attraction. As we go down the group, electro-negativity gradually decreases, whereas the melting point, boiling point, and density increase regularly.

The chemical properties that the elements of this group exhibit are one of the strongest electro-negativity abilities due to their small size and hydrogen bonding forming ability. They generally exhibit +2, +4, and +6 oxidation states due to the promotion of electrons to vacant d-orbitals. The thermal stability of hydrides of this group decreases down the group, whereas the acidic strength increases. They form oxoacids when they react with the hydrogen molecule. Some of the major oxygen compounds formed are ozone, sulphur dioxide, sulphuric acids, and many more.

Group 17 elements- The Halogen Group

This group in the periodic table consists of F, Cl, Br, I, and At. They are said to be halogens because they are found in seawater mostly. The general electronic configuration is ns2np5. The atomic radius is least among all other groups of the p-block due to increased charge but increases down the group due to an increase in the number of shells.

The ionisation potential decreases down the group due to an increase in the shielding effect. The most electronegative element in the periodic table is present in this group. They simply tend to gain an electron to complete its octet. Except for the fluorine atom, all other elements show +1 and-1 oxidation states. 

The general chemical properties exhibited by the members of the family is its reactivity that decreases down the group, whereas the reducing capacity increases due to a decrease in bond energy. Some of the important molecules formed of these elements that show wide ranges of properties are hydrochloric acid, hydrogen fluoride that shows hydrogen bonding, etc.

Group 18 elements- Zero group elements

This group has He, Ne, Ar, Kr, Xe, and Rn as its family members. These are the last group elements located at the right-most side of the periodic table with complete electronic configuration, i.e., ns2np8 except for that of helium.

As these elements do not take part in chemical reactions, they are said as zero group elements or otherwise said as inert elements. They are found in the earth’s atmosphere except for Rn, due to their inert nature. They are not harmful to living organisms.

The chemical properties of this group’s elements possess zero electro-negativity and maximum ionisation potential due to its complete electronic configuration. They are tasteless, odourless, and colourless.

Conclusion

Therefore, as the last electrons enter into the p-shell, they are referred to as p-block elements. All the elements show a variety of properties due to the presence of different types of elements, i.e., metals, non-metals, and metalloids. A difference in the inner core of their electronic configuration influences the physical as well as chemical properties greatly. While the group oxidation state is most stable for the lighter elements and lower state becomes progressively more stable than the heavier elements.