(b) Which has the larger sixth ionization energy, Se or Br?

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Identify the electron configurations of Se (Selenium) and Br (Bromine) in their ground states. This will help in understanding how many electrons each element has in its various shells.

Understand the concept of ionization energy, which is the energy required to remove an electron from a gaseous atom or ion. The sixth ionization energy refers to the energy needed to remove the sixth electron.

Analyze the electron configuration after removing five electrons from each element, which will give you the electron configuration relevant to the sixth ionization energy.

Consider the stability of the resulting ion after removing five electrons. Elements with a more stable electronic configuration after electron removal generally have higher ionization energies.

Compare the effective nuclear charge (the net positive charge experienced by electrons in the outermost shell) of the resulting ions. A higher effective nuclear charge typically leads to a higher ionization energy.

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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 energy required to remove an electron from a gaseous atom or ion. It is a key concept in understanding the reactivity and stability of elements. Generally, ionization energy increases across a period due to increasing nuclear charge and decreases down a group due to increased electron shielding.

Trends in Ionization Energy

Ionization energy exhibits specific trends in the periodic table. As you move from left to right across a period, ionization energy increases, while it decreases as you move down a group. This is due to the balance between nuclear attraction and electron shielding, which affects how tightly electrons are held by the nucleus.

Comparison of Elements

When comparing elements like selenium (Se) and bromine (Br), it is essential to consider their positions in the periodic table. Bromine is to the right of selenium, indicating it has a higher nuclear charge and generally higher ionization energies. However, the sixth ionization energy specifically refers to the energy required to remove the sixth electron, which can be influenced by the electron configuration and stability of the resulting ion.