Trends In The Periodic Table (Atomic Radius (Atomic Radius decreases…
Trends In The Periodic Table
"Half the distance between the nuclei of 2 atoms of the same element that are joined together by the same covalent bond."
Atomic Radius decreases across a period
This is due to an increase in nuclear charge and the lack of an increase in the screening effect.
Atomic Radius increases going down a group
This is due to the increase in Energy Levels (shells) and the screening effect of the inner electrons
The screening effect refers to how the further the electron is from the nucleus,the less of the positive charge it feels,as other electrons are in the way and are far closer,meaning the outer electrons aren't being pulled as much.
"The energy required to remove an electron from an ion with one positive charge in the gaseous state."
"The minimum required energy to detach the most loosely bound electron from a neutral gaseous atom."
Ionisation Energy decreases going down a group
This is due to increasing atomic radius and the screening effect of inner electrons
Ionisation Energy increases crossing a period
This is due to a higher nuclear charge,and a decreasing atomic radius (lack of screening effect)
"The relative attraction that an atom in a molecule has for the shared pair of electrons in a covalent bond."
If an Electronegativity difference is greater than 1.7,it's indicating an ionic bond.
If less than or equal to 1.7,it indicates a covalent bond.
If greater than 0.4 but less than 1.7,it is a polar covalent
If less than or equal to 0.4,it indicates it is non polar