Problem 27 - Chemistry The Molecular Science

Question

Energy is emitted from an atom when an electron moves from a(n) _________ state to the ________ . The energy of the emitted radiation corresponds to the __________ between the two energy levels.

Step-by-Step Solution

Answer

Electrons emit energy moving from an excited state to the ground state; emission equals the energy difference.

Step 1: Understanding Electron Transition

Electrons in an atom can be in various energy levels or states. When an electron transitions from one energy level to another, energy is either absorbed or emitted depending on the direction of the transition.

Step 2: Identifying Initial State

If an electron moves to a lower energy state, it means it's moving from an excited state. The excited state is any state higher in energy than the lowest possible energy state.

Step 3: Identifying Final State

The electron moves to the ground state when it is in the lowest energy state possible. The ground state is the most stable state of an atom.

Step 4: Calculating Energy Difference

The energy of the emitted radiation is equal to the difference between the two energy levels involved in the transition. This energy difference is responsible for the emission of radiation.

Step 5: Filling in the Blanks

Using the understanding from the above steps, the blanks can be filled as follows: Energy is emitted from an atom when an electron moves from an excited state to the ground state. The energy of the emitted radiation corresponds to the energy difference between the two energy levels.

Key Concepts

Excited State

Electrons orbit around the nucleus of an atom and can be found at different energy levels. When an electron absorbs energy, it moves to a higher energy level, which is known as the excited state. This state is temporary and unstable because it requires external energy to maintain.
In the excited state, electrons have higher energy than in their normal positions. This can be compared to climbing a hill—energy is needed to go up, and it's not a place you stay naturally for long.
For example, when you provide heat or light to an atom, its electrons can jump to higher energy levels and enter excited states. Excited states are critical because they precede processes like the emission of light and other forms of radiation as electrons return to lower energy levels.

Ground State

The ground state is the lowest energy state an electron can occupy in an atom. This is the most stable and natural state for electrons, where they tend to remain unless given extra energy to leave.
When an electron falls back from an excited state to the ground state, it releases the energy it previously absorbed. This release is what produces visible light, among other radiations.
Think of the ground state as the "home" level for electrons. It's like the flat land at the bottom of the hill. Since it requires no extra energy supply, electrons prefer staying here. Additionally, the ground state aligns with nature's tendency to default to a minimum energy configuration.

Energy Levels

Energy levels in atoms are like stepping stones. Electrons can "jump" between these steps by absorbing or emitting energy. Each level has a specific energy value, and electrons prefer to occupy the lowest available space.
When an electron transitions from one energy level to another, it either absorbs or releases a packet of energy, often in the form of light. This energy packet is known as a photon.

• Higher energy levels: These are like top steps requiring more energy to reach.
• Lower energy levels: Easier to reach with less energy needed.
• Transitioning: The move between these levels is what causes emission or absorption of energy.

It's important to understand that the energy difference between levels determines the color and type of light emitted during these transitions. Therefore, energy levels are crucial in understanding atomic behavior and the behavior of light.