The following diagrams represent the electron population of the composite s–d band for three metals—Ag, Mo, and Y:
Which diagram corresponds to which metal? (LO 12.7) (a) Ag = 3, Mo = 1, Y = 2 (b) Ag = 2, Mo = 1, Y = 3 (c) Ag = 2, Mo = 3, Y = 1 (d) Ag = 1, Mo = 2, Y = 3

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Step 1: Understand the electron configuration of each metal (Ag, Mo, Y).

Step 2: Identify the number of electrons in the s and d bands for each metal.

Step 3: Analyze the given energy diagram and note the distribution of electrons in bonding and antibonding states.

Step 4: Compare the electron distribution in the diagram with the expected electron configurations of Ag, Mo, and Y.

Step 5: Match the diagram to the metal based on the electron population in the s-d band.

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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For metals, the arrangement of electrons in the s and d orbitals is crucial for understanding their chemical properties and bonding behavior. The specific filling of these orbitals influences the metal's conductivity, reactivity, and overall electronic structure.

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In molecular orbital theory, bonding orbitals are formed when atomic orbitals combine constructively, leading to lower energy states, while antibonding orbitals result from destructive interference, leading to higher energy states. The occupancy of these orbitals determines the stability and reactivity of the metal. Understanding how electrons populate these orbitals is essential for predicting the behavior of metals in various chemical contexts.

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Metallic bonding occurs due to the attraction between positively charged metal ions and delocalized electrons that are free to move throughout the structure. This delocalization allows metals to conduct electricity and heat efficiently. The strength and nature of metallic bonds can vary among different metals, influencing their physical properties and the arrangement of electrons in their s-d bands.

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