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Step-by-Step Explanation
Step 1: Identify the Key Properties in the Question
The question highlights a type of solid that:
Reflects visible light.
Has electrical conductivity that decreases with an increase in temperature.
Exhibits a high melting point.
These three characteristics are typical properties of metals.
Step 2: Recognize the Bond Type Responsible for These Properties
In metals, the atoms are held together by metallic bonding. This bonding model explains that the metal cations are arranged in a lattice, surrounded by a “sea” of delocalized electrons. These electrons can move freely, giving rise to the excellent electrical and thermal conductivity of metals.
Step 3: Explain How Metallic Bonding Leads to the Mentioned Properties
Reflection of Light:
The free electrons interact with incoming visible light, allowing metals to efficiently reflect it. This is why metals have a lustrous (shiny) appearance.
Electrical Conductivity Decreases with Temperature:
As temperature increases, the metal lattice ions vibrate more vigorously. This increased vibration impedes the flow of electrons, causing the electrical conductivity to drop.
High Melting Point:
Metallic bonds are generally very strong due to the strong electrostatic attraction between the positive metal ions and the sea of delocalized electrons, leading to high melting points.
Step 4: Conclude and Confirm the Correct Answer
Given the properties described, the bonding responsible for such a solid must be metallic bonding. Therefore, the correct answer is metallic bonding.
