(b) Which element in the periodic table has the largest ionization energy? Which has the smallest?

Verified step by step guidance

1. 1. Ionization energy is the energy required to remove an electron from an atom or ion. It is an indication of how tightly an atom holds onto its electrons. The larger the ionization energy, the harder it is to remove an electron.
2. 2. In general, ionization energy increases from left to right across a period (horizontal row) in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, which means the positive charge of the nucleus increases. This stronger positive charge pulls the electrons in the atom closer to the nucleus, making them harder to remove.
3. 3. Ionization energy also generally decreases from top to bottom down a group (vertical column) in the periodic table. This is because as you move down a group, the electrons are further from the nucleus and are therefore easier to remove.
4. 4. Therefore, the element with the largest ionization energy is typically found in the top right corner of the periodic table (excluding the noble gases). This is because it is furthest to the right (so it has a high nuclear charge) and at the top (so the electrons are close to the nucleus).
5. 5. Conversely, the element with the smallest ionization energy is typically found in the bottom left corner of the periodic table. This is because it is furthest to the left (so it has a low nuclear charge) and at the bottom (so the electrons are far from the nucleus).

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of how strongly an atom holds onto its electrons. Generally, ionization energy increases across a period from left to right due to increasing nuclear charge and decreases down a group as the distance between the nucleus and the outermost electrons increases.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Key trends include ionization energy, electronegativity, and atomic radius. Understanding these trends helps in predicting the behavior of elements, including which will have the highest or lowest ionization energies.

Noble Gases and Alkali Metals

Noble gases, located in Group 18 of the periodic table, typically have the highest ionization energies due to their stable electron configurations. In contrast, alkali metals in Group 1 have the lowest ionization energies because they have a single electron in their outermost shell, which is easily removed. This distinction is crucial for identifying the elements with the largest and smallest ionization energies.