(c) Would you expect salts like NaCl, which have singly charged ions, to have larger or smaller lattice energies compared to salts like CaO which are composed of doubly-charged ions?

검증된 단계별 안내

insert step 1> Consider the concept of lattice energy, which is the energy required to separate one mole of an ionic solid into its gaseous ions. It is influenced by the charges of the ions and the distance between them.

insert step 2> Recall that lattice energy is directly proportional to the product of the charges of the ions. This means that higher charges on the ions will result in a larger lattice energy.

insert step 3> Compare the charges of the ions in NaCl and CaO. NaCl is composed of Na^+ and Cl^- ions, each with a charge of ±1. CaO is composed of Ca^2+ and O^2- ions, each with a charge of ±2.

insert step 4> Analyze the effect of ion charges on lattice energy. Since CaO has ions with higher charges compared to NaCl, the lattice energy of CaO is expected to be larger.

insert step 5> Conclude that salts like CaO, with doubly-charged ions, generally have larger lattice energies compared to salts like NaCl, which have singly charged ions.

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주요 개념

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Lattice Energy

Lattice energy is the amount of 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. Higher lattice energy indicates stronger ionic bonds, which typically results in higher melting points and greater stability of the compound.

Charge of Ions

The charge of ions significantly influences lattice energy. Ions with higher charges create stronger electrostatic attractions between them, leading to greater lattice energy. For example, doubly charged ions like Ca²⁺ and O²⁻ will interact more strongly than singly charged ions like Na⁺ and Cl⁻, resulting in a higher lattice energy for compounds formed from doubly charged ions.

Ionic Size

The size of the ions also affects lattice energy. Smaller ions can get closer together, increasing the electrostatic attraction and thus the lattice energy. In contrast, larger ions have a greater distance between them, which can reduce the strength of the ionic bond. Therefore, the combination of ion charge and size is crucial in determining the overall lattice energy of a salt.