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  Periodic Table and Its Properties Homework Help - K-12 Grade Level, College Level Chemistry

Introduction of Periodic table

A periodic table is a tabular display of the chemical elements that are organized on the basis of their, electron configurations, atomic numbers, and recurring chemical properties. Elements are presented in the order of increasing atomic number. Standard form of the table comprises an 18 × 7 grid or main body of elements, positioned above smaller double row of elements. Table can also be deconstructed into four rectangular blocks: the f-block to the south, the d-block in the centre, the s-block to the left, and the p-block on the right. Most of the columns and rows of the table have specific names: main body columns are called groups (such as the halogens or the noble gases); horizontal rows are called periods. Using periodic trends, the periodic table can help predict the properties of various elements and the relationships between properties. As result it provides a useful framework for analyzing chemical behaviour and is widely used in chemistry and other sciences.

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Periodic Properties

The properties of the elements exhibit trends. These trends can be predicted by using the periodic table and can be explained and understood by analyzing the electron configurations of the elements. Elements tend to lose or gain valence electrons to achieve stable octet formation. Stable octets are seen in inert gases or noble gases of Group VIII of the periodic table. There are two other main trends. 1st, electrons are added one at a time moving from left to right across a period. As it happen, electrons of the outermost shell experience increasingly strong nuclear attraction. Thus, the electrons become closer to the nucleus and more tightly bound to it. 2nd, moving down a column in the periodic table, outermost electrons become less tightly bound to the nucleus. This happens because of the number of filled principal energy levels (which shield the outermost electrons from attraction to the nucleus) increases downward within each group. These trends give details of the periodicity observed in the elemental properties of atomic radius, electron affinity, and the electronegativity and ionization energy.

Periodic Law

Periodic law, in chemistry, the generalization that there is a recurring pattern in the properties of the elements when they are arranged in order of increasing atomic number- that is the total number of protons in the atomic nucleus. Periods of the periodic table illustrate these relationships. Initial discovery was made by the Dmitry I. Mendeleyev in the mid-19th century has been of inestimable value in the development of chemistry.

It was not actually recognized until the second decade of the 20th century that the order of elements in the periodic system is that of their atomic numbers, integers of which are equal to the positive electrical charges of the atomic nuclei expressed in electronic units. In the subsequent years great progress was made in explaining the periodic law in terms of the electronic structure of atoms and molecules. This clarification has been increased the value of the law, which is used that much today that it was at the beginning of the 20th century, when it expressed only known relationship among the elements.

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