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Chapter 11: Problem 35

Classify the solid states in terms of crystal types of the elements in the third period of the periodic table. Predict the trends in their melting points and boiling points.

Short Answer

Expert verified
The third period elements' crystal structures are unique for each, including body-centered cubic, face-centered cubic, diamond cubic, simple cubic, orthorhombic, and monoclinic structures. Melting and boiling points increase from Sodium to Aluminum, peak at Silicon due to its covalent structure, then decrease towards Argon.

Step by step solution

01

Identify the Elements in the Third Period

The elements found in the third period of the periodic table are Sodium (Na), Magnesium (Mg), Aluminum (Al), Silicon (Si), Phosphorus (P), Sulfur (S), Chlorine (Cl), and Argon (Ar).
02

Classify the Crystal Structures

Each of these elements adopts a unique crystal structure: Sodium and Magnesium adopt a body-centered cubic structure; Aluminum adopts a face-centered cubic structure; Silicon and Argon adopt a diamond cubic structure; Phosphorus takes up a simple cubic structure; Sulfur has an orthorhombic structure; Chlorine has a monoclinic structure.
03

Predict the Trends in Melting Points

The melting points of these elements typically increase from Sodium to Aluminum as the metallic bonding strengthens with increasing nuclear charge. Silicon, a semi-metal, has a very high melting point due to its giant covalent structure. After Silicon, the melting point decreases up to Argon, since these elements form molecular structures that are held together through Van der Waals forces which are far less strong than metallic or covalent bonds.
04

Predict the Trends in Boiling Points

The boiling points follow a similar trend with the melting points. Silicon has the highest boiling point and Argon has the lowest, due to it being a noble gas.

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Most popular questions from this chapter

Carbon and silicon belong to Group 4 A of the periodic table and have the same valence electron configuration \(\left(n s^{2} n p^{2}\right) .\) Why does silicon dioxide \(\left(\mathrm{SiO}_{2}\right)\) have a much higher melting point than carbon dioxide \(\left(\mathrm{CO}_{2}\right) ?\)

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