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Answer:
Is iron more metallic or aluminum? Never thought about it? Now is the time to actually think and know about it then! You have possibly always followed the modern periodic table of elements. In this chapter, we will look at the modern periodic table of elements and get into the details of the properties of the same. It is interesting to learn the changes in the various properties of the elements within the periodic table.
Explanation:
Modern Periodic Table of Elements
The modern periodic law states that the physical and chemical properties of the elements are the periodic function of the atomic numbers. The various elements with similar properties repeat after certain regular intervals. This repetition occurs when you arrange the elements in order of their increasing atomic numbers.
Modern Periodic Table of elements
Modern Periodic Table
Atomic Mass or Atomic Number: What affects the properties?
Atomic mass depends upon the number of protons and neutrons in the nucleus. On the other hand, the atomic number implies the number of electrons in the extranuclear part of the number of protons in the nucleus.
Since the nucleus is deep-seated in an atom and is also shielded by electrons in the extranuclear part, therefore, the atomic mass has little effect on the chemical properties of the elements. Electrons are exposed to the environment. Hence, they can interact with the reagent. As a result, the physical and chemical properties of the elements depend upon their atomic numbers rather than the atomic masses.
Read about the Historical Development of the Periodic Table.
Cause of Periodicity in the Periodic Table
According to the Modern periodic law, the properties of the elements repeat after certain regular intervals when these elements are arranged in order of their increasing atomic numbers. This is how the modern periodic table of elements is designed.
The cause of periodicity in properties is the repetition of similar outer electronic configuration after certain regular intervals. All the elements of group IA or 1 i.e. alkali metals have a similar outer electronic configuration, i.e. ns1 where n refers to the number of outermost principal shells. It is because of the similarity in the electronic configuration that all the elements have similar properties.
All the halogens i.e. elements of group VIIA or 17 have similar outer electronic configuration i.e. ns2 np6 and hence, possesses similar properties. All the elements of group 0 or 18 have a similar electronic configuration, i.e ns2 np5 and hence, possess similar properties.
Read about the Metallic and Non-Metallic Characters here.
Long Form of Periodic Table
The long form of the periodic table is based upon the electronic configuration of the elements. It is the present form or the modern periodic table of elements. The modern periodic table of elements consists of 18 vertical columns and 7 horizontal rows. We obtain these by arranging the elements in order of their increasing atomic numbers.
The scientists have made this arrangement in a very peculiar way. It keeps all the elements with similar electronic configuration under each other in the same vertical column. Groups are these vertical columns. On the other hand, periods are the horizontal rows.
Modern Periodic Table of elements
Learn more about D and F Block elements here.
Groups in the Periodic Table
The 18 vertical columns in the modern or long form of the periodic table are the groups.
Each of the group consists of a number of elements having the same electronic configuration of the outermost shell.
These groups are numbered from 1 to 18.
Periods in the Periodic Table
The long form of the periodic table consists of 7 periods.
These are numbered as 1, 2, 3, 4, 5, 6 and 7 from top to bottom.
The first period consists of only two elements – Hydrogen and Helium.
The 2nd and 3rd period consists of 8 elements each. On the other hand, the 4th and 5th consists of 18 elements each while the sixth period consists of 32 elements.
The 7th period is incomplete and like the 6th period would have a maximum of 32 electrons.
In the long form of the periodic