An alloy is a homogeneous mixture of two or more metals or a metal and a non-metal. It is prepared by melting the primary metal and dissolving other elements in it in definite proportions before cooling to room temperature. Alloys generally have lower electrical conductivity and melting points compared to pure metals.
What is an alloy, and how is it prepared? How do the electrical conductivity and melting point of alloys compare to those of pure metals?
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An alloy is a mixture of two or more elements, where at least one is a metal. Alloys are prepared by melting the constituent metals together and then cooling to form a solid solution. This process can involve varying proportions of different metals to achieve desired properties. In general, alloys exhibit improved characteristics compared to pure metals. Electrical conductivity may vary, but alloys often maintain good conductivity. The melting point of alloys is typically lower than that of pure metals due to the disruption of regular atomic arrangements, making them more malleable and adaptable for various applications.