Elements of p block

Elements of p block

Introduction

The elements of the p-block and the elements of the s-block are jointly called representative elements or main group elements. The electronic configuration of the extracellular space of these elements is ns2np1 -6, where n is the last shell. The s-nucleus of the last shell of the elements of this block already has two electrons and the p-subcell contains one to six electrons, while the first cell from the extracellular space contains 8 or 18 electrons (excluding He).

Their outermost electronic configuration changes from ns2, np1 to ns2, np6 in each period. Each period ends with an electronic configuration of ns2, np6, noble gas. In noble gases, all the orbits in the valence shell are filled with electrons. It is very difficult to change this permanent arrangement by removing or adding electrons. That is why the chemical reactivity of noble gases is very low. Before the family of noble gases, there are two chemically important classes of non-metals - halogen in the 17th class and chalcogen in the 16th class. Elements of these two classes have high negative electron gain enthalpy. These elements easily attain one or two electrons, respectively, and obtain a permanent noble gas electronic configuration.

Characteristics of elements of p - Block

Following are the characteristics of these elements of the periodic table.

Electronic configuration

These elements have 2 electrons in the s - subfamily of the extracellular space and 1 to 6 electrons in the p - epithelium such as -

B = 2,3     1s2, 2s2, 2p1

C = 2,4     1s2, 2s2, 2p2

N = 2,5     1s2, 2s2, 2p3

O = 2,6     1s2, 2s2, 2p4

F = 2,7     1s2, 2s2, 2p5

Ne = 2,8    1s2, 2s2, 2p6

Valency

Except for oxygen, fluorine, and inert gases, the sensitivity of all p-block elements to oxygen is equal to the number of electrons in their extracellular space. The valence of some p-block elements may be different in their different compounds, ie some elements in them also express variable valence. Such as - PCl3, PCl5, N2O, N2O3, N2O5 etc.

Atomic radius

The atomic radius of these elements is relatively small. The atomic radius of the elements of the shale class is often greater).

Ionization enthalpy

The ionisation enthalpy of these elements is of high quality. This is why most p-block elements do not form cations. (Ion enthalpy is highest for zero class elements).

Electron gain enthalpy

The electron gain enthalpy of these elements is high (the electron gain enthalpy of zero class elements is zero).

Electronegativity

The negative power of these elements is of relatively high quality (except for zero class elements).

Reactivity

Except for halogens, oxygen, sulfur and phosphorus, 'other p-block elements have low reactivity.

Non-metallic character

There are three types of p-block elements, metals (Al, Sn, Pb etc.), non-metals (N, P, 0 and halogen etc.) and submetals (Ge, As, Sb etc.). For this reason, they are called common elements. In the period, moving from left to right there is an increase in the atomic characteristics of the elements. And when you go from top to bottom in a class, metallic symptoms increase.

Nature of compounds

These elements mainly form covalent compounds, the oxides of non-metals are often acidic. The oxides of Al, Sn, As and Sb are amphoteric.