Question

As a metal such as lead melts, what happens to (a) the average kinetic energy of the atoms and (b) the average distance between the atoms?

Short answer

As a metal like lead melts, (a) the average kinetic energy of the atoms increases due to the temperature rise and faster atomic movement, and (b) the average distance between the atoms increases as the material transitions from a closely packed solid-state lattice to a less ordered liquid state with increased repulsion forces.

Step-by-step solution

Understand the concept of kinetic energy

Kinetic energy is the energy of motion. In the context of atoms, it directly relates to the speed at which the atoms are moving within the material.

Consider the effect of temperature

When a metal melts, the temperature increases, meaning the atoms have more energy. As the atoms gain more energy, they move faster. This results in an increase in the average kinetic energy of the atoms.

Final answer for (a)

As a metal such as lead melts, the average kinetic energy of the atoms increases. #b) The average distance between the atoms#

Understand the concept of atomic spacing

The average distance between the atoms refers to the space between individual atoms within the material.

Consider the transition from solid to liquid state

As a metal melts, it transitions from a solid state to a liquid state. In the solid state, the atoms are arranged in a fixed, closely packed lattice. In the liquid state, the atoms lose their fixed positions and flow freely, which means the arrangement becomes less ordered.

Account for the increase in energy

In the liquid state, the atoms have more energy and move more rapidly, causing the atoms to collide and repel each other. This leads to an increase in the average distance between the atoms due to the increased repulsion forces.

Final answer for (b)

As a metal such as lead melts, the average distance between the atoms increases.

Key concepts

Kinetic Energy in Melting Metals

Kinetic energy is a fundamental concept in physics, representing the energy that an object possesses due to its motion. When we think about metals like lead undergoing a phase transition from solid to liquid, we need to consider the behavior of the atoms. As the temperature of the metal increases during melting, the atoms gain energy, causing them to vibrate and move more vigorously.
This increase in motion translates directly to an increase in kinetic energy. As a result, as metal melts, the average kinetic energy of the atoms within the metal increases, signifying faster-moving particles.

Phase Transition from Solid to Liquid

The phase transition from solid to liquid is a fascinating phenomenon, particularly in metals such as lead. In a solid state, metal atoms are arranged in a structured, closely packed lattice. However, during melting, the atoms absorb energy and overcome the rigid lattice structure, transitioning into a liquid form.
Atoms in a liquid state flow more freely and are less ordered compared to their solid counterparts. This change is significant in understanding the nature of metals at different temperatures. One can visualize this transition as moving from a regimented marching band (solid) to a lively dance floor (liquid), highlighting less order and more movement.

Atomic Spacing During Melting

One important aspect of the melting process is the change in atomic spacing. The term 'atomic spacing' refers to the distance between atoms in a material. In the solid state, atoms are tightly packed in a fixed structure; however, when a metal like lead melts, the atoms shift into a more random distribution.
As the temperature rises, the increased energy causes atoms to move more rapidly and frequently collide, inducing repulsion forces that increase the distance between them. This increase in atomic spacing is crucial as it indicates a shift towards the liquid state, allowing atoms greater freedom to move and occupy a larger volume.