Problem 12 - Chemistry An Atoms First Approach

Question

In going across a row of the periodic table, electrons are added and ionization energy generally increases. In going down a column of the periodic table, electrons are also being added but ionization energy decreases. Explain.

Step-by-Step Solution

Answer

In summary, the ionization energy generally increases across a row of the periodic table due to the increased effective nuclear charge experienced by outer electrons and constant distance between the electron and nucleus. However, it decreases down a column due to the increased distance between the outermost electron and the nucleus, as well as the electron shielding effect caused by an increased number of inner electron shells.

Step 1: Understanding Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion. Factors that influence ionization energy include the effective nuclear charge experienced by the electron, the distance between the electron and the nucleus, and electron shielding.

Step 2: Trend Across a Row (Left to Right)

In going across a row of the periodic table, electrons are added, and the atomic number increases, which means the number of protons in the nucleus also increases. As a result, the effective nuclear charge experienced by the outer electrons increases. The increased positive charge in the nucleus attracts the electrons more strongly, making it more difficult to remove them. Furthermore, as we move across a row, the electrons are added to the same energy level, so the distance between the electron and nucleus remains relatively constant. Thus, ionization energy generally increases from left to right across a row in the periodic table.

Step 3: Trend Down a Column (Top to Bottom)

In going down a column of the periodic table, electrons are also being added, but ionization energy decreases. This trend can be explained by considering the distance between the outermost electron and the nucleus, as well as the electron shielding effect. As we move down a group, each subsequent element has an additional electron shell, meaning that the outermost electrons are further away from the nucleus. The increased distance between the outer electrons and the nucleus reduces the attractive force between them, making it easier to remove an electron, hence decreasing ionization energy. Additionally, as we move down a group, the increased number of electron shells results in an increase in electron shielding. The inner electron shells shield the outer electrons from the full attractive force of the positively charged nucleus. This shielding effect further decreases the ionization energy as we move down a column of the periodic table. In conclusion, ionization energy trends in the periodic table can be explained by understanding factors such as effective nuclear charge, distance between electrons and nucleus, and electron shielding effects. Ionization energy generally increases across a row and decreases down a column due to these factors.