For the following crystals, explain how their melting points are related to the bonding forces and the crystal structure.

a)Copper,Cu
b)Water,H20
c)Sodium chloride,NaCl
d)Diamond,C

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To understand how the melting points of crystals are related to bonding forces and crystal structure, let's break it down for each of the given examples:

a) Copper (Cu):
Copper is a metal with metallic bonding. Metallic bonds occur between the positively charged metal ions and the delocalized electrons. These bonds are strong and result in high melting points. Additionally, copper has a face-centered cubic crystal structure, which allows for strong bonding between adjacent atoms. Hence, copper has a relatively high melting point.

b) Water (H2O):
Water is a molecular compound with covalent bonding. Covalent bonds occur when atoms share electrons. In the case of water, oxygen shares electrons with two hydrogen atoms. The intermolecular forces between water molecules, known as hydrogen bonding, play a critical role in determining the melting point. Hydrogen bonds are relatively weaker compared to metallic bonds, resulting in a lower melting point for water compared to metals.

c) Sodium chloride (NaCl):
Sodium chloride is an ionic compound composed of positively charged sodium (Na+) ions and negatively charged chloride (Cl-) ions. Ionic bonds occur due to the electrostatic attraction between these oppositely charged ions. The strong electrostatic forces between adjacent ions require a high amount of energy to overcome, thus resulting in a high melting point for sodium chloride.

d) Diamond (C):
Diamond is a covalent network solid composed entirely of carbon atoms. Each carbon atom forms strong covalent bonds with four neighboring carbon atoms, resulting in a three-dimensional network structure. These covalent bonds are incredibly strong, making diamond one of the hardest substances known and giving it an exceptionally high melting point.

In summary, the bonding forces and crystal structures significantly affect the melting points of crystals. Metallic bonding and covalent network structures tend to result in high melting points due to the strength of the bonds involved. Covalent bonding in molecular compounds and ionic bonding in salts also contribute to relatively high melting points, although they are generally lower than those of metals and covalent network solids.