Interpretation:
The smallest ion should be identified.
Concept Introduction:
Energy required to remove an electron from an individual atom in gas phase defined as its ionization energy.
Answer to Problem 43CR
a.
Explanation of Solution
Order in which orbitals fill to produce the atoms in periodic table as follows:
There are only one
Thus,
Thus,
Thus,
Thus,
Thus,
First ionization energy of neutral atoms vary as follows:
As the energy levels grow up from top to bottom in one group of elements, removal energy of the final electron reduces as attraction of the final electron to the nucleus decreases.
From left to right of a period ionization energy increases. Thus metals tend to remove electrons easily than nonmetals.
Ionization energies of different ions vary as follows:
All above five ions have achieved the noble gas configuration of
Positive charge increment of the nucleus tends to pull the electrons towards the nucleus and ions get smaller than the neutral atom and cause more difficult to remove another electron. Opposite happens for anions. More negative charge cause repulsion of most distinct electrons and also the atomic size increases. Because of that it’s more easier to remove another electron from anion than cation whose having same valance electrons.
Ionization energy of anions < Ionization energy of cations
(Have more minus charge) (Have more plus charge)
Thus, (a)
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Chapter 12 Solutions
Introductory Chemistry: A Foundation
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