Question #a3f82

1 Answer
Aug 1, 2017




sodium , lithium and potassium are highly electropositive elements placed in #1^(st)# group in periodic table.
all these three have something in common . if you look at the electronic configuration of these elements (alkali metals) its identical.
here we got electronic configuration of all the three.
shell | K| L | M | N
Lithium (Li) | 2 | 1 |
Sodium (Na) | 2 | 8 | 1
potassium (K) | 2 | 8 | 8 | 1.

This data shows something identical in all that is presence of 1 #e^(-)# in valence shell. these #e^(-)# are present in s shell [refer aufbau principle].
This is the reason that they readily give #e^(-)# from their valence shell since they got just 1 #e^(-)# in valence shell which makes them a bit unstable in atom form. stability can be attained by forming ions .
so these have a greater tendency to form cations. and give up their #e^(-)# easily.

every atom wants to attain a sense of nobility so it requires to either gain or lose electrons . losing 1 electron doesn't require much energy lose #( p^(+) vs e ^(-))#. .