Trends in the periodic table

Question	Answer
1st Ionisation energy (groups)	X(g) ---> X+(g) + e- Going down a group decreases as the outer electron is further away and is shielded by inner shells
Atomic radius (groups)	Atomic radius increases down the group as an extra inner shell of electrons is added per period the more electron shells the bigger the radius
Melting & Boiling points (group 1 & 2)	Decrease down the group Distance between nucleaus and electrons increases so weaker bonds less energy required to break them
Melting & Boiling points (Halogens & Noble gases)	The molecule gets bigger and the intermolecular forces get stronger and more energy is required to overcome them
Electrical conductivity	Increases as metallic character increases
From left to right across a period	1st ionisation energy increases atomic radius decreases electronegativity increases
Down a group	1st ionisation energy decreases atomic radius increases electronegativity decreases increase in metallic character

Resource summary

	Created by Holly Bamford over 8 years ago