Describe with reasons which atom in each of the following pairs has higher ionisation energy?
a) Mg and Al
b) B and Al
c) Al and Si
Answers
In option (a) Mg & Al ----→ Mg has higher ionization energy.
Reason :- Mg has greater ionization energy than Al because of it's configuration 2s²,2p⁶,3s² .We know that s orbital has greater penetration power so it is hard to remove electron from 3s orbital on compare to 3p orbital. Also Mg has stable electronic configuration. fully filled 3 s orbital.
In option (b) B & Al----→ Aluminium has higher ionization energy
Reason :- The size of atom of Boron is much smaller then Aluminum.
Thus the aluminum has the high nuclear charge as a result of which it required a large amount of energy to convert into a positively charged ion on compare to boron. Hence Aluminium has higher ionization energy.
In option (c) Al & Si -----→ Silicon has higher ionization energy
Reason :- The size of the atom of the silicon is smaller then Aluminum due to its nuclear charge , Thus large amount of energy is required to convert silicon into a positively charged on compare to Al. Hence it has the higher ionization energy then aluminum .
Hope it Helps :-)
Answer:
The higher ionization energy in each of the following atoms are :-
In option (a) Mg & Al ----→ Mg has higher ionization energy.
Reason :- Mg has greater ionization energy than Al because of it's configuration 2s²,2p⁶,3s² .We know that s orbital has greater penetration power so it is hard to remove electron from 3s orbital on compare to 3p orbital. Also Mg has stable electronic configuration. fully filled 3 s orbital.
In option (b) B & Al----→ Aluminium has higher ionization energy
Reason :- The size of atom of Boron is much smaller then Aluminum.
Thus the aluminum has the high nuclear charge as a result of which it required a large amount of energy to convert into a positively charged ion on compare to boron. Hence Aluminium has higher ionization energy.
In option (c) Al & Si -----→ Silicon has higher ionization energy
Reason :- The size of the atom of the silicon is smaller then Aluminum due to its nuclear charge , Thus large amount of energy is required to convert silicon into a positively charged on compare to Al. Hence it has the higher ionization energy then aluminum .