We have discussed all periodic properties like size/ atomic radius, ionization enthalpy, electron gain enthalpy and electronegativity separately. All of them are interrelated to each other. In this post we will try to find relation between all periodic properties.
The secret of every property of an element lies within its atom. So you must have to consider the structure of an atom and arrangement of its subatomic particles.
When you go towards right in a period, number of orbits remains the same but the increasing number of protons makes nucleus stronger, therefore the size of atom decreases, as a result of which EN increases. As you know, it is easier to add an extra electron to a more electronegative element, hence the EGE decreases. And since ionisation is just opposite to EGE, the IE increases on going towards right in a period.
When you go downwards in a group, number of orbits increases, hence the size of atom increases which diminishes the power of nucleus and that’s why it becomes easier to remove an outermost electron from the neutral atom that means IE decreases. Since electron gain is opposite to the ionization so, EGE increases downward. And because of increased size it becomes difficult for nucleus to attract bonding electrons that means EN decreases downwards in a group.
You have seen that how subatomic particles play an imp role in deciding the nature of an atom, which in turn decides the nature of an element. Electrons are the most important part of an atoms life. They decide its stability and help it to achieve octet. The electrons that help in bonding are special electrons. These special electrons are called Valence electrons. In the next post we will learn more about Valence electrons.
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