Group Reactivity & Properties
Ever wonder why sodium explodes in water whilst lithium just fizzes? It's all about reactivity patterns in the periodic table, and understanding these will help you predict how elements behave.
Group 1 metals (alkali metals) like lithium, sodium, and potassium are surprisingly light - they actually float on water! They're soft enough to cut with a knife and become even softer as you go down the group. These metals are brilliant electrical conductors and stay shiny until oxygen gets to them.
The real excitement happens with their chemical properties. These metals become increasingly reactive as you move down Group 1 because their outer electron gets further from the nucleus and easier to lose. Lithium gently fizzes in water, sodium rushes about vigorously, and potassium burns with a beautiful lilac flame.
Group 7 elements (halogens) work completely differently - they become less reactive going down the group. Fluorine is pale yellow and extremely dangerous, chlorine is pale green, bromine is orange-brown, and iodine appears grey as a solid but purple as a vapour. Unlike Group 1, halogens want to gain electrons rather than lose them.
Quick Tip: Remember that Group 1 gets more reactive going down, whilst Group 7 gets less reactive - opposite patterns!