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Chapter 10: Problem 103

Explain why sodium is malleable, but sodium chloride is brittle.

Short Answer

Expert verified
Sodium is malleable due to its metallic bonding which allows the layers of atoms to slide past one another without breaking the bonds. Sodium chloride is brittle because of its ionic structure. When stress is applied, ions of the same charge are pushed next to each other causing repulsion and breaking off of ions, resulting in brittleness.

Step by step solution

01

Understand the structure of sodium

Sodium (Na) is a metal with a simple structure - it consists of closely packed layers of atoms. The electrons in the outer shell of sodium atoms are free to move, forming a 'sea' of delocalized electrons. This is known as metallic bonding.
02

Explain malleability of sodium

Due to the metallic bonding, when a stress is applied to sodium, the layers of atoms can slide past each other. The bonds between atoms are not broken, just moved, this allows the metal to change shape without breaking. This is the reason why sodium is malleable.
03

Understand the structure of sodium chloride

Sodium chloride (NaCl) is an ionic compound. It has a giant ionic structure with each sodium ion surrounded by six chloride ions and each chloride ion surrounded by six sodium ions. The ionic bonds between these ions are very strong.
04

Explain brittleness of sodium chloride

When a stress is applied to sodium chloride, the layers of ions try to slide past each other, but the action brings ions of similar charges into close proximity, which causes a strong repulsion. These repulsions cause the layers to separate and the ions to break off, leading to the brittle nature of sodium chloride.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Metallic Bonding
In metals like sodium, the atoms are arranged in a closely packed structure. The electrons in the outer shell of these atoms are not bound tightly and, instead, move freely throughout the structure. This creates what we call a 'sea of delocalized electrons.'

These free-moving electrons are crucial to metallic bonding. They act as a glue, holding the metal atoms together. This bonding allows metals to conduct electricity and heat efficiently. The delocalized nature of the electrons also contributes to other unique properties of metals.
  • Creates strong but flexible bonds.
  • Allows atoms to move without breaking the bond.
  • Enables metals to be shaped into different forms.
Ionic Compounds
Ionic compounds consist of ions that are bonded together by electrostatic forces. Sodium chloride (NaCl) is a classic example. It is formed by the transfer of electrons from sodium (Na) to chlorine (Cl), resulting in a crystal lattice of positively charged sodium ions (Na鈦�) and negatively charged chloride ions (Cl鈦�).

In these compounds, the ions are arranged in a repeating pattern, creating a stable but intricate structure. The bonds between ions are very strong, making ionic compounds generally less volatile. However, these strong bonds do not allow for flexibility.
  • Strong electrostatic attraction between oppositely charged ions.
  • High melting and boiling points.
  • Solids at room temperature and brittle.
Malleability
Metals like sodium are known for their malleability, which means they can be hammered or pressed into different shapes without breaking. This property is due to the nature of metallic bonding.

When stress is applied to a metal, the layers of atoms can slide over one another. The delocalized electrons act as a cushion, maintaining metallic bonds as the layers shift. This movement allows metals to be bent or shaped without shattering.
  • Atoms can move past each other easily.
  • Delocalized electrons maintain attraction.
  • Prevents breakage under stress.
Brittleness
Brittleness is a characteristic of materials like sodium chloride, where the structure is rigid and unable to withstand stress without breaking. The brittleness of ionic compounds stems from their rigid lattice structure.

When stress is applied, the like-charged ions are forced closer together, causing repulsive forces that lead to a fracture. Unlike metals, the ionic bonds do not permit sliding of ions without breaking, making the material brittle.
  • No ability for ions to shift without resistance.
  • Repulsion between like-charged ions leads to breakage.
  • Rigid structure cannot absorb energy or stress well.

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