Question

In the box below, draw and label an atomic/molecular level picture of the bonding in iron (Fe) that can be used to explain iron's properties (mp 1811 K, grey solid at room temp. shiny, malleable, ductile, conducts electricity). Use your drawing to explain how the bonding in iron leads to the observed melting point (1811 K).

Answer 1

The properties of iron, including its high melting point, malleability, ductility, and electrical conductivity, are due to its metallic bonding, where delocalized electrons create a “sea” that facilitates these characteristics and strong interatomic attraction results in high melting points.

Step-by-step explanation:

To explain the properties of iron (Fe) such as its melting point (mp) of 1811 K, its solid state at room temperature, and its ability to conduct electricity and appear shiny, we refer to the metallic bonding model. Iron's atoms are arranged in a crystal structure, surrounded by a “sea” of delocalized electrons that can move freely. This is the key to iron being , ductile, and an excellent conductor of electricity and heat. The delocalized electrons also facilitate metallic luster, as they can absorb and emit light.

The melting point of iron being high is a reflection of the strength of its metallic bonds. A significant amount of energy is required to overcome these bonds and transition iron from a solid to a liquid state. Compared with other metals on the periodic table, iron's melting point indicates strong metallic bonding, lending it high durability and versatility as a material.