Pick the correct word to complete the sentence: The larger the atom, the (smaller/larger) its first ionization energy.

Verified step by step guidance

1. Understand the concept of ionization energy: Ionization energy is the energy required to remove an electron from an atom in the gaseous state.
2. Recognize the trend in the periodic table: Ionization energy generally increases across a period from left to right and decreases down a group.
3. Consider atomic size: As you move down a group in the periodic table, atoms become larger because they have more electron shells.
4. Relate atomic size to ionization energy: Larger atoms have their outermost electrons further from the nucleus, which means these electrons are less tightly held and require less energy to remove.
5. Conclude the relationship: Therefore, the larger the atom, the smaller its first ionization energy.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It is a key indicator of how strongly an atom holds onto its electrons. Higher ionization energy means that an atom is less likely to lose an electron, while lower ionization energy indicates a greater tendency to lose electrons.

Atomic Size

Atomic size refers to the distance from the nucleus to the outermost electron shell of an atom. As you move down a group in the periodic table, atomic size increases due to the addition of electron shells, which places the outer electrons further from the nucleus and reduces the effective nuclear charge experienced by these electrons.

Trends in Ionization Energy

Ionization energy generally decreases as atomic size increases. This is because larger atoms have their outer electrons further from the nucleus, resulting in a weaker attraction between the nucleus and the outermost electrons. Consequently, it requires less energy to remove an electron from a larger atom compared to a smaller atom.