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Chapter 5: Problem 51

Suppose you could see into solid objects at the atomic level. Explain, based on what you see, why solid NaCl would not be called a molecular substance whereas solid \(\mathrm{H}_{2} \mathrm{O}\) would.

Short Answer

Expert verified
When observed at the atomic level, solid NaCl has an ionic structure with sodium and chloride ions arranged in a 3D lattice, held together by electrostatic attractions between the oppositely charged ions. There are no discrete molecular units in NaCl. In contrast, solid \(\mathrm{H}_{2} \mathrm{O}\) (ice) consists of individual water molecules with covalent bonding between oxygen and hydrogen atoms, forming distinct molecular units with specific shapes. Therefore, NaCl is not considered a molecular substance, while \(\mathrm{H}_{2} \mathrm{O}\) is.

Step by step solution

01

Understand the atomic structures of NaCl and \(\mathrm{H}_{2} \mathrm{O}\)

Sodium chloride (NaCl) has an ionic structure, where sodium and chloride ions are arranged in a regular, repeating 3D lattice. In this lattice, each sodium ion is surrounded by chloride ions, and each chloride ion is surrounded by sodium ions. The attractive forces between the positive sodium ions and the negative chloride ions hold the structure together. On the other hand, water (\(\mathrm{H}_{2} \mathrm{O}\)) has a covalent molecular structure. It consists of individual water molecules, where each oxygen atom is covalently bonded to two hydrogen atoms, forming the H-O-H structure.
02

Compare the bonding in NaCl and \(\mathrm{H}_{2} \mathrm{O}\)

In NaCl, the bonding is ionic, which results from the electrostatic attraction between oppositely charged ions. This type of bonding is non-directional, meaning that the force of attraction is equal in all directions. As a result, there are no discrete units or molecules in the NaCl lattice structure. Conversely, in solid \(\mathrm{H}_{2} \mathrm{O}\) (ice), the bonding within each water molecule is covalent, involving the sharing of electrons between the oxygen and hydrogen atoms. Covalent bonds are directional and strong, creating distinct molecules with specific shapes.
03

Explanation of why NaCl is not a molecular substance and \(\mathrm{H}_{2} \mathrm{O}\) is

Based on the difference in atomic structures and bonding, we can explain why NaCl is not considered a molecular substance, while \(\mathrm{H}_{2} \mathrm{O}\) is. In NaCl, there are no discrete molecules, and the attractive forces holding the solid together are ionic bonds resulting from the electrostatic attractions between oppositely charged ions. Thus, we cannot identify discrete molecular units in the NaCl lattice. In contrast, solid \(\mathrm{H}_{2} \mathrm{O}\) has discrete water molecules with covalent bonding holding the hydrogen and oxygen atoms together. These distinct molecular units with specific shapes help define \(\mathrm{H}_{2} \mathrm{O}\) as a molecular substance.

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