Metallic bonding is the electrostatic attractive force between positively charged metal ions and delocalized electrons. Imagine a 'sea' of electrons freely moving around positive metal ions. This electron mobility is what gives metals their excellent electrical and thermal conductivity. The strength of metallic bonds influences properties like melting point and hardness. Stronger metallic bonds mean higher melting points and harder metals!
Match the term with its definition:
| Term | Definition |
|---|---|
| 1. Delocalized Electrons | A. The ability of a metal to be hammered into thin sheets. |
| 2. Metallic Bond | B. Electrons that are not associated with a single atom or bond. |
| 3. Malleability | C. The ability of a metal to be drawn into wires. |
| 4. Ductility | D. A measure of how easily a metal conducts electricity. |
| 5. Electrical Conductivity | E. The electrostatic attraction between positive metal ions and a sea of delocalized electrons. |
Complete the following paragraph using the words: positive, sea, strong, electrons, conductivity.
Metallic bonding involves a "____" of delocalized ______. These electrons are not bound to individual atoms, allowing them to move freely. This free movement is responsible for the metal's high electrical ______. The metal ions are ______ charged and held together by the attraction to the delocalized electrons. A metal with a high melting point likely has ______ metallic bonds.
Explain how the number of valence electrons affects the strength of a metallic bond and resulting properties of the metal. Provide an example. 🤔
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