Deduce the reason why silicon dioxide has high melting point, taking into consideration what you know about it's structure and type of bonding.

1. ### Understanding the Structure of Silicon Dioxide

Silicon dioxide (SiO₂), commonly known as quartz, has a tetrahedral structure where each silicon atom is covalently bonded to four oxygen atoms. This arrangement forms a three-dimensional network of strong covalent bonds throughout the crystal lattice.

2. ### Type of Bonding

The bonding in silicon dioxide is characterized by:

• Strong covalent bonds formed between silicon and oxygen atoms.
• The presence of a continuous network of these bonds, resulting in a highly stable structure.

3. ### Analysis of Melting Point

The high melting point of silicon dioxide can be attributed to:

• The strength of covalent bonds: Covalent bonds possess substantial bond energy, meaning a considerable amount of heat is required to overcome these bonds.
• Network solid characteristics: As a covalently bonded network solid, SiO₂ does not have individual molecules, but rather a lattice that requires breaking many strong bonds, leading to its high melting point.

4. ### Summary

In summary, the high melting point of silicon dioxide is directly related to its tetrahedral network structure and the robust covalent bonding throughout the material. The significant energy needed to break these bonds accounts for the material's elevated melting temperature, making it one of the highest among non-metal compounds.

Final Answer

Silicon dioxide (SiO₂) has a high melting point due to its strong covalent network structure, requiring substantial energy to disrupt the extensive bonding throughout the crystal lattice.