
The first ionization energy of and atoms follow the order:
A.
B.
C.
D.
Answer
511.8k+ views
Hint:Ionisation energy is the minimum amount of energy required to remove an electron from an isolated gaseous atom to form monovalent cation. Ionisation energy depends upon the size of the atom, half-filled and fully filled configuration and nuclear charge.
Complete answer:
First ionisation energy of all the elements (like and depends upon electronic configuration.First of all, is an electropositive element, or alkali metal and belongs to the first group of the periodic table. Size of is larger than that of other elements and lesser force of attraction between the nucleus and outermost electrons. So its ionisation energy becomes less than that of other elements. But as we move from left to right in a period, nuclear charge increases and atomic size decreases thus ionisation energy increases.
Along the period, ionisation energy increases then the order of elements i.e. but the actual order of is , the reason being half filled configuration of nitrogen followed by oxygen due to its smaller size than boron.
Thus half-filled and fully filled configurations are more stable. They have extra stability.
Hence the correct answer is option B.
Note:: The force of attraction between the nucleus and outermost electron increases with increase in nuclear charge. Greater is the nuclear charge, greater will be the energy required to pull the electron from the atom. Hence, with increase in nuclear charge ionization enthalpy increases. However, the effective nuclear charge experienced by a valence electrons in an atom will be less than the actual charge on the nucleus due to a phenomenon known as `shielding effect’ or `screening effect’ where the force of attraction by the nucleus on the valence electron is reduced due to the repulsive forces exerted by the inner shell electrons.
Complete answer:
First ionisation energy of all the elements (like
Along the period, ionisation energy increases then the order of elements i.e.
Thus half-filled and fully filled configurations are more stable. They have extra stability.
Hence the correct answer is option B.
Note:: The force of attraction between the nucleus and outermost electron increases with increase in nuclear charge. Greater is the nuclear charge, greater will be the energy required to pull the electron from the atom. Hence, with increase in nuclear charge ionization enthalpy increases. However, the effective nuclear charge experienced by a valence electrons in an atom will be less than the actual charge on the nucleus due to a phenomenon known as `shielding effect’ or `screening effect’ where the force of attraction by the nucleus on the valence electron is reduced due to the repulsive forces exerted by the inner shell electrons.
Recently Updated Pages
Master Class 11 Accountancy: Engaging Questions & Answers for Success

Master Class 11 Social Science: Engaging Questions & Answers for Success

Master Class 11 Economics: Engaging Questions & Answers for Success

Master Class 11 Physics: Engaging Questions & Answers for Success

Master Class 11 Biology: Engaging Questions & Answers for Success

Class 11 Question and Answer - Your Ultimate Solutions Guide

Trending doubts
The non protein part of an enzyme is a A Prosthetic class 11 biology CBSE

What is a zygomorphic flower Give example class 11 biology CBSE

The deoxygenated blood from the hind limbs of the frog class 11 biology CBSE

What is the function of copulatory pads in the forelimbs class 11 biology CBSE

Which of the following is nitrogenfixing algae a Nostoc class 11 biology CBSE

Renal portal system of frog is significant in A Quick class 11 biology CBSE
