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Concept explainers
(a)
Interpretation:
The element having the larger ionization energy among Li and N needs to be determined.
Concept introduction:
Ionization energy can be defined as the amount of energy needed to remove an electron form an atom or an ion.
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Answer to Problem 64A
N has the largest ionization energy.
Explanation of Solution
The elements with the smaller ionic radius or the elements in the further right in the period have the larger ionization energy.
N has the
Therefore, as N is placed right in comparison with Li, Hence, N has the larger ionization energy.
(b)
Interpretation:
The element that has the larger ionization energy among Kr and Ne needs to be determined.
Concept introduction:
Ionization energy can be defined as the amount of energy needed to remove an electron form an atom or an ion.
(b)
![Check Mark](/static/check-mark.png)
Answer to Problem 64A
Ne has the larger ionization energy.
Explanation of Solution
Kr has the atomic number of 36 and the electronic configuration [Ar] 3d10 4s24p6. Kr is present in Group 18 i.e. in p-block. And Ne has an atomic number of 10 and electronic configuration [He] 2s24p6, located in group 18i.e. in p-block..
In the periodic table, the size of elements increases and ionization energy decreases down the group.
Due to this, Ne has a smaller size since its electrons are held closer to the nucleus of the atom than that of Kr. Hence, Ne has a larger ionization energy.
(c)
Interpretation:
The element having the larger ionization energy among Cs and Li needs to be determined.
Concept introduction:
Ionization energy can be defined as the amount of energy needed to remove an electron form an atom or an ion.
(c)
![Check Mark](/static/check-mark.png)
Answer to Problem 64A
Li has the larger ionization energy.
Explanation of Solution
Cs has the atomic number of 55 and the electronic configuration [Xe] 6s1. Ce is present in Group 1 i.e. in s-block. And Li has an atomic number of 3 and electronic configuration [He] 2s2located in group 1 i.e. in s-block.
In the periodic table, the size of elements increases and ionization energy decreases down the group. Due to this, Li has a smaller size since its electrons are held closer to the nucleus of the atom than that of Cs. Hence, Li has a larger ionization energy.
Chapter 6 Solutions
Glencoe Chemistry: Matter and Change, Student Edition
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