Identify the type of interactions involved in each of the following processes taking place during the dissolution of sodium chloride (NaCl) in water.I. Solvent-solvent interactionsII. Solute-solute interactionsIII. Solute-solvent interactionsA. Interactions between the ions of sodium chlorideB. Interactions involving dipole-dipole attractionsC. Interactions formed during hydrationD. Interactions involving ion-ion attractionsE. Interactions associated with an exothermic process during the dissolution of sodium chlorideF. Interactions between the water moleculesG. Interactions formed between the sodium ions and the oxygen atoms of water molecules

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09-12-2019
Chemistry

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Identify the type of interactions involved in each of the following processes taking place during the dissolution of sodium chloride (NaCl) in water.I. Solvent-solvent interactionsII. Solute-solute interactionsIII. Solute-solvent interactionsA. Interactions between the ions of sodium chlorideB. Interactions involving dipole-dipole attractionsC. Interactions formed during hydrationD. Interactions involving ion-ion attractionsE. Interactions associated with an exothermic process during the dissolution of sodium chlorideF. Interactions between the water moleculesG. Interactions formed between the sodium ions and the oxygen atoms of water molecules

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sabriledesma13 sabriledesma13 · Answer 1 · 2019-12-11T03:32:32+01:00

Answer:

A. Interactions between the ions of sodium chloride (solute-solute interactions).

B. Interactions involving dipole-dipole attractions (solvent-solvent interactions).

C. Interactions formed during hydration (solute-solvent interactions).

D. Interactions involving ion-ion attractions (solute-solute interactions).

E. Interactions associated with an exothermic process during the dissolution of sodium chloride (solute-solvent interactions).

F. Interactions between the water molecules (solvent-solvent interactions).

G. Interactions formed between the sodium ions and the oxygen atoms of water molecules (solute-solvent interactions).

Explanation:

The solution process takes place in three distinct steps:

Step 1 is the separation of solvent molecules.

Step 2 entails the separation of solute molecules.

These steps require energy input to break attractive intermolecular forces; therefore, they are endothermic.

Step 3 refers to the mixing of solvent and solute molecules. This process can be exothermic or endothermic.

If the solute-solvent attraction is stronger than the solvent-solvent attraction and solute-solute attraction, the solution process is favorable, or exothermic (ΔHsoln < 0). If the solute-solvent interaction is weaker than the solvent-solvent and solute-solute interactions, then the solution process is endothermic (ΔHsoln > 0).

In the dissolution of sodium chloride, this process is exothermic.