Consider this set of ionization energies. IE 1 = 578 kJ/mol IE 2 = 1820 kJ/mol IE 3 = 2750 kJ/mol IE 4 = 11,600 kJ/mol To which third-period element do these ionization values belong?

All right. Hello everyone. So this question says to consider this set of ionization energy ie one is equal to 578 kilojoules per more ie two is equal to 1979 kg joules per mole ie three is equal to 2963 kg joules per mole. An ie four is equal to 6180 kg joules per mole to which fourth period element do these ionization values belong. Option A is gallium. Option B says Germanium option C says calcium and option D says potassium. All right. So when considering the set of ionization energies provided, we can see that as the number of electrons being removed increases. So does the value of the ionization energy. But there is a remarkable difference between two ionization energy values in particular because the difference between the third and the fourth ionization energies is remarkable compared to the difference between the other ionization energies in this set. Now recall that such a drastic difference in the ionization energy indicates that the fourth electron is actually a core electron that gets removed. So this means that the fourth period element in question contains three valent electrons. And the value of the fourth ionization energy corresponds to the removal of a core electron. Now, because there are only three valence electrons. The valence electronic configuration would be NS two NP one to yield a total of three vent electrons. Now, because the valence configuration is NS two NP one, this means that the fourth period element is in group or column three A. So now let's consider the locations of the elements listed in our answer choices. Starting off with potassium, potassium is found in group one A mm, calcium is found in group two A. Now Germanium, on the other hand is found in group four A whereas gallium is in group three A and there you have it. So our answer here is going to be option a in the multiple choice. And the reason for this is because gallium is the fourth period element in this list belonging to group three A and therefore having three valence electrons. So with that being said, thank you so very much for watching. And I hope you found this helpful.

Ch.8 - Periodic Properties of the Elements

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Tro 4th Edition

Ch.8 - Periodic Properties of the Elements

Problem 78

Chapter 8, Problem 78

Consider this set of ionization energies. IE₁ = 578 kJ/mol IE₂ = 1820 kJ/mol IE₃ = 2750 kJ/mol IE₄ = 11,600 kJ/mol To which third-period element do these ionization values belong?

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Identify the pattern in the ionization energies: Notice the large jump between IE3 and IE4.

Recall that a large increase in ionization energy typically indicates the removal of an electron from a new, inner shell.

Determine the number of valence electrons: The large jump after IE3 suggests that the element has 3 valence electrons.

Identify the third-period element with 3 valence electrons: In the periodic table, elements in the third period with 3 valence electrons are in Group 13.

Conclude the element: The third-period element in Group 13 is Aluminum (Al).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of an element's reactivity and can vary significantly among different elements. Generally, ionization energy increases across a period in the periodic table due to increasing nuclear charge, which holds electrons more tightly.

Trends in Ionization Energies

Ionization energies exhibit specific trends in the periodic table. As you move from left to right across a period, ionization energy tends to increase due to the greater effective nuclear charge experienced by the outer electrons. Conversely, as you move down a group, ionization energy decreases because the outer electrons are further from the nucleus and experience more shielding from inner electrons.

Identification of Elements

To identify an element based on its ionization energies, one can compare the given values to known ionization energies of elements in the same period. The significant jump in ionization energy values, particularly between IE3 and IE4, suggests that the element has a stable electron configuration after losing three electrons, indicating it is likely a non-metal in the third period, such as phosphorus or sulfur.