Question

Which of the following electronic transitions could lead to the emission of light from an atom? \(1 s \longrightarrow 4 p \longrightarrow 3 d \longrightarrow 5 f \longrightarrow 4 d \longrightarrow 2 p\)

Short answer

The transitions 4p to 3d, 5f to 4d, and 4d to 2p could lead to the emission of light.

Step-by-step solution

Understand Electronic Transitions

Electronic transitions occur when an electron moves from one energy level to a lower one in an atom, releasing energy in the form of a photon. This process is called 'emission'. The energy emitted can be observed as light.

Analyze the Given Transitions

Each transition involves an electron falling to a lower energy level, starting from the 1s orbital to the 4p, then to 3d, followed by 5f, then to 4d, and finally to 2p. We need to identify which of these transitions corresponds to a drop to a lower energy level and could, therefore, lead to the emission of light.

Identify the Emissions

The transitions from an electron at higher to lower energy levels are as follows: - 4p to 3d- 5f to 4d- 4d to 2pThese transitions could lead to the emission of photons, visible as light.

Key concepts

Emission of Light

The phenomenon of emission of light occurs in an incredibly small, though massively important, theater: the interior of an atom. This production of light is actually a physical manifestation of energy being released. When an excited electron within an atom falls to a lower energy level, it loses energy in the form of a photon, a particle of light.

This isn't a random process, however. Specific amounts of energy correspond to precise wavelengths of light, which is why we can see distinct colors in fireworks or neon lights. These characteristic colors come from electrons in different atoms making transitions between specific energy levels and emitting photons at certain wavelengths. Hence, when we discuss the emission of light, we are actually talking about electronic transitions that produce discernible colors, depending on the energy difference between the initial and final states of the electrons.

Electron Energy Levels

The invisible rungs on the ladder of an atom are its electron energy levels, also known as electron shells. Electrons in atoms reside in these energy levels. The levels closest to the nucleus have the lowest energy, and as you move away from the nucleus, each level represents a higher potential energy that an electron can have.

Electrons seek the most stable (or lowest-energy) configuration possible, but they can be excited to higher levels when energy is supplied. When they return to their lower energy states, the excess energy is released as light. Think of it like a ball rolling down a hill, it gains speed (or energy) going up the hill and loses it coming down—the same principle applies, but with electrons releasing light as they 'roll down' to lower energy levels.

• Lowest energy level is closest to the nucleus
• Higher energy levels are further away
• Energy absorbed to move up, light emitted moving down

Atomic Orbital Transitions

While the term 'energy levels' may evoke a simpler picture of neatly ordered shelves, the reality is more complex. Within each energy level, there are sublevels made up of different atomic orbitals designated as s, p, d, f, and so on. Just as each room in a house serves a different purpose, each type of orbital has a different shape and energy.

Transitions can happen between these orbitals when electrons gain or lose energy. Our textbook exercise showed a sequence where electrons fall from higher-energy orbitals to lower ones. The transition of an electron from a 4p orbital to a 3d orbital, or a 5f to a 4d are examples of such processes that result in light emission. The shape and complex interactions within these orbitals influence the exact energy changes involved, which in turn dictate the specific colors of light we can observe. When these transitions are understood and characterized, they can tell us an immense amount about the identity and properties of different elements, even those in distant stars!

• Orbitals are sublevels within energy levels
• Designated as s, p, d, f, etc., each with unique shapes and energies
• Transitions between orbitals release or absorb energy resulting in the emission or absorption of light