
Concept explainers
(a)
Interpretation:
The element with the highest
Concept introduction:
The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by IE.
Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high.
The ionization energy of an element increases along the period because the electrons are held by high effective nuclear charge. The value of ionization energy decreases down the group because the valence electrons are much farther from the nucleus and therefore experience weaker forces of attraction.
(a)

Answer to Problem 8.59P
Na will have the highest value of
Explanation of Solution
The first ionization energy is determined by the removal of an electron from the neutral parent atom. The value of the second ionization for all the elements will be higher than that of
The
After the removal of an electron,
For the second ionization energy,
The atomic number of Mg is 12 so it’s ground state electronic configuration is
For the second ionization energy,
The atomic number of
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows:
The first ionization energy is determined by the removal of an electron from the neutral parent atom. The value of the second ionization for all the elements will be higher than that of
(b)
Interpretation:
The element with the highest
Concept introduction:
The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by IE.
Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high.
The ionization energy of an element increases along the period because the electrons are held by high effective nuclear charge. The value of ionization energy decreases down the group because the valence electrons are much farther from the nucleus and therefore experience weaker forces of attraction.
(b)

Answer to Problem 8.59P
Explanation of Solution
The first ionization energy is determined by the removal of an electron from the neutral parent atom. The value of the second ionization for all the elements will be higher than that of
The atomic number of
After the removal of an electron,
For the second ionization energy,
The atomic number of
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows:
For both sodium and potassium, the second electron is removed from a stable noble gas configuration but because the size of sodium is smaller than potassium the second ionization energy of sodium will be greater than potassium.
The atomic number of
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows:
In case of iron, the first ionization energy is high because the first electron is removed from the fully filled
(c)
Interpretation:
The element with the highest
Concept introduction:
The ionization energy is the amount of energy required to remove the most loosely bound valence electrons from an isolated neutral gaseous atom. It is represented by IE.
Its value varies with the ease of removal of the outermost valence electron. If the outermost electron is removed very easily then the value of ionization energy is very small. If the electron is removed with quite a difficulty then the value of ionization energy will be very high.
The ionization energy of an element increases along the period because the electrons are held by high effective nuclear charge. The value of ionization energy decreases down the group because the valence electrons are much farther from the nucleus and therefore experience weaker forces of attraction.
(c)

Answer to Problem 8.59P
Explanation of Solution
Down the group the ionization energy decreases. Scandium is a placed in the 4th period, magnesium is placed in the 3rd period and beryllium is placed 2nd period. Therefore, among
The atomic number of
For the first ionization energy, the change in electronic configuration is as follows:
For the second ionization energy, the change in electronic configuration is as follows:
The size of
The atomic number of
After the removal of an electron,
For the second ionization energy, the change in electronic configuration is as follows:
It is expected that
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Chapter 8 Solutions
Loose Leaf for Chemistry: The Molecular Nature of Matter and Change
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