(b) Write the chemical equation that represents the process of lattice energy for the case of NaCl.

검증된 단계별 안내

Identify the ions involved in the formation of NaCl: sodium ion \( \text{Na}^+ \) and chloride ion \( \text{Cl}^- \).

Understand that lattice energy is the energy released when gaseous ions combine to form an ionic solid.

Write the chemical equation for the formation of solid NaCl from its gaseous ions: \( \text{Na}^+ (g) + \text{Cl}^- (g) \rightarrow \text{NaCl} (s) \).

Recognize that this equation represents the exothermic process where lattice energy is released.

Remember that lattice energy is a measure of the strength of the forces between the ions in an ionic solid.

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

주요 개념

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

Lattice Energy

Lattice energy is the energy released when gaseous ions combine to form an ionic solid. It is a measure of the strength of the forces between the ions in an ionic compound. For NaCl, lattice energy reflects the stability of the Na+ and Cl- ions in the solid state compared to their gaseous forms.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of positively charged cations and negatively charged anions. In the case of NaCl, sodium (Na) loses an electron to become Na+, while chlorine (Cl) gains an electron to become Cl-. The electrostatic attraction between these oppositely charged ions leads to the formation of a stable ionic lattice.

Chemical Equation

A chemical equation is a symbolic representation of a chemical reaction, showing the reactants and products involved. For lattice energy, the equation typically illustrates the formation of NaCl from its constituent ions: Na+(g) + Cl-(g) → NaCl(s). This equation highlights the transition from gaseous ions to a solid ionic compound, emphasizing the energy change associated with the process.