NaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions. (b) Use the ionic radii given in Figure 7.8 to estimate the Na─Cl and K─F distances.

검증된 단계별 안내

Identify the ionic radii for Na^+ and Cl^- from Figure 7.8.

Identify the ionic radii for K^+ and F^- from Figure 7.8.

Add the ionic radius of Na^+ to the ionic radius of Cl^- to estimate the Na─Cl distance.

Add the ionic radius of K^+ to the ionic radius of F^- to estimate the K─F distance.

Compare the estimated distances to understand the difference in separation between the cations and anions in NaCl and KF.

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주요 개념

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

Ionic Radii

Ionic radii refer to the effective size of an ion in a crystal lattice, which is influenced by its charge and the surrounding ions. Cations are typically smaller than their neutral atoms due to the loss of electrons, while anions are larger due to the gain of electrons. Understanding ionic radii is crucial for estimating distances between ions in ionic compounds.

Crystal Structure

Crystal structure describes the orderly arrangement of ions in a solid, which determines the properties of the material. In the case of NaCl and KF, both adopt a face-centered cubic lattice structure, where each ion is surrounded by six oppositely charged ions. This arrangement is essential for understanding how ionic distances are calculated based on the positions of cations and anions.

Ionic Bonding

Ionic bonding occurs when electrons are transferred from one atom to another, resulting in the formation of positively charged cations and negatively charged anions. The electrostatic attraction between these oppositely charged ions leads to the formation of ionic compounds like NaCl and KF. This concept is fundamental for understanding the interactions that dictate the distances between ions in a crystal lattice.