As the temperature rises and the kinetic energy of solid particles increases, the energy supplied by heat overcomes the forces of attraction between the particles. Eventually, the particles break free from their fixed positions and begin to move more freely, resulting in the solid melting into a liquid.
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Increased kinetic energy, typically from heating, causes the molecules in a solid to vibrate more vigorously, weakening the intermolecular forces holding them in a fixed lattice structure. As these forces weaken, the molecules become less ordered, eventually overcoming the solid’s cohesive forces and transitioning into the more disordered liquid state, resulting in melting.
When the kinetic energy of a solid increases, typically due to heating, the particles within the solid begin to move more quickly and vibrate more intensely. This increased movement disrupts the orderly arrangement of particles in the solid’s structure. As the temperature continues to rise, the particles gain enough energy to overcome the forces holding them in fixed positions.
As the intermolecular forces weaken, the solid starts to lose its rigidity, allowing the particles to move more freely. Once the kinetic energy reaches a certain level, the particles break free from their fixed positions, and the solid begins to melt. This transition from solid to liquid state occurs at the melting point, where the increased kinetic energy enables the particles to flow past one another, leading to the melting of the solid.