Choose the larger atom in each pair. a. Al or In b. Si or N c. P or Pb d. Si or Cl

검증된 단계별 안내

Identify the periodic trend: Atomic size increases as you move down a group in the periodic table and decreases as you move across a period from left to right.

Compare Al and In: Both are in Group 13, but In is below Al, so In is larger.

Compare Si and N: Both are in Period 2, but Si is to the left of N, so Si is larger.

Compare P and Pb: P is in Group 15 and Period 3, while Pb is in Group 14 and Period 6. Pb is much lower in the periodic table, so Pb is larger.

Compare Si and Cl: Both are in Period 3, but Si is to the left of Cl, so Si is larger.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Atomic Size

Atomic size refers to the distance from the nucleus to the outermost electron shell of an atom. Generally, atomic size increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.

Periodic Trends

Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, ionization energy, and electronegativity, which help predict the behavior of elements in chemical reactions and their relative sizes.

Comparison of Elements

When comparing elements, it is essential to consider their positions in the periodic table. Elements in the same group typically have similar properties, while those in different groups may vary significantly. Understanding these relationships allows for accurate predictions about which atom is larger based on their respective group and period placements.