Choose the larger atom in each pair. a. P or O b. Si or Sn c. S or Sb d. B or N

검증된 단계별 안내

Step 1: Understand the concept of atomic size. Atomic size generally increases as you move down a group in the periodic table and decreases as you move across a period from left to right.

Step 2: Compare the atomic sizes for each pair by locating them on the periodic table. For pair (a) P or O, both are in the same period, so compare their positions across the period.

Step 3: For pair (b) Si or Sn, note that they are in the same group. Atomic size increases as you move down a group, so compare their positions vertically.

Step 4: For pair (c) S or Sb, they are in different periods and groups. Consider both the group and period trends to determine which is larger.

Step 5: For pair (d) B or N, both are in the same period. Compare their positions across the period to determine which 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 the same period show trends in size and reactivity. Understanding these relationships allows for accurate comparisons of atomic sizes among different elements.