Sodium melts at 98 °C, and magnesium melts at 650 °C. Account for the higher melting point of magnesium using the electron-sea model.

Verified step by step guidance

Step 1: Understand the electron-sea model. The electron-sea model is a model of metallic bonding in which cations are considered to be fixed points within a 'sea' of mobile electrons.

Step 2: Consider the atomic structure of sodium and magnesium. Sodium has one valence electron, while magnesium has two. This means that magnesium can contribute more electrons to the 'sea' of delocalized electrons than sodium.

Step 3: Understand the relationship between the number of delocalized electrons and the strength of metallic bonds. The more delocalized electrons, the stronger the metallic bonds. This is because the delocalized electrons can move freely and interact with a greater number of positive ions, creating a stronger bond.

Step 4: Apply this understanding to the given problem. Because magnesium contributes more delocalized electrons than sodium, it has stronger metallic bonds. This means that more energy (in the form of heat) is required to break these bonds and melt magnesium.

Step 5: Conclude that the higher melting point of magnesium compared to sodium can be explained by the electron-sea model. The greater number of delocalized electrons in magnesium leads to stronger metallic bonds and a higher melting point.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron-Sea Model

The electron-sea model describes metallic bonding as a structure where electrons are delocalized and free to move throughout a lattice of positively charged metal ions. This 'sea' of electrons allows metals to conduct electricity and contributes to their malleability and ductility. The strength of the metallic bond, influenced by the number of delocalized electrons, plays a crucial role in determining the melting point of metals.

Metallic Bonding Strength

The strength of metallic bonds varies among different metals, primarily due to the number of valence electrons that can participate in the electron-sea. Magnesium, with its two valence electrons, forms stronger metallic bonds compared to sodium, which has one. This increased bonding strength in magnesium results in a higher melting point, as more energy is required to overcome these bonds during the melting process.

Melting Point and Atomic Structure

The melting point of a substance is influenced by its atomic structure and the type of bonding present. In metals, a higher melting point typically indicates stronger metallic bonds and a more stable lattice structure. Magnesium's higher melting point compared to sodium can be attributed to its greater atomic mass and the stronger interactions between its ions and the delocalized electrons, leading to a more stable arrangement that requires more energy to disrupt.

Recommended video:

Guided course