Examine diagrams for the electron population of the composite s–d band for three metals in question 6. Which metal has the highest melting point? (LO 12.7) (a) Metal 1 (b) Metal 2 (c) Metal 3

Verified step by step guidance

1. Examine the energy diagram for the electron population of the composite s–d band for the three metals.
2. Identify the bonding and antibonding states in the diagram. The bonding states are below the dashed line, and the antibonding states are above it.
3. Observe the proportion of electrons in the bonding and antibonding states for each metal. Metal I has all electrons in the bonding state, Metal II has a mix of bonding and antibonding electrons, and Metal III has more electrons in the bonding state than in the antibonding state.
4. Recall that a higher proportion of electrons in the bonding state generally leads to stronger metallic bonding and thus a higher melting point.
5. Determine which metal has the highest proportion of electrons in the bonding state, as this metal will have the highest melting point.

Key Concepts

s–d Band Theory

The s–d band theory describes the electronic structure of metals, focusing on the interaction between s and d orbitals. In this context, the bonding and antibonding states formed by these orbitals influence the metal's properties, including conductivity and melting point. The distribution of electrons in these bands can indicate the stability and strength of metallic bonds.

Melting Point and Bonding Strength

The melting point of a metal is closely related to the strength of its metallic bonds, which are influenced by the electron configuration in the bonding and antibonding states. Metals with a higher population of electrons in bonding states typically exhibit stronger interactions between atoms, leading to higher melting points. Thus, analyzing the electron population in the s–d bands can help predict which metal will have the highest melting point.

Electron Configuration and Stability

Electron configuration refers to the arrangement of electrons in an atom's orbitals. In metals, a stable electron configuration in the bonding states contributes to lower energy and greater stability. The diagrams provided show how the distribution of electrons in bonding versus antibonding states can affect the overall stability of the metal, which is a key factor in determining its melting point.