Light Emission Spectra and Electron Energy Levels in Atoms

The video explains how each element emits a unique emission spectrum due to the arrangement of electrons and their energy levels. Using the Bohr model, it describes how electrons absorb energy, move to excited states, and release energy as photons when returning to ground states. The energy of these photons determines their color in the visible spectrum, with higher energy photons having shorter wavelengths. The unique spectra of elements, akin to fingerprints, are used for identification.

What determines the unique emission spectra of each element?

• The temperature of the element

• The size of the atom

• The arrangement of electrons and their energy levels

• The number of protons in the nucleus

What happens when an electron absorbs energy?

• It moves to a higher energy level

• It remains in the same energy level

• It moves to a lower energy level

• It emits a photon

How is the energy of a photon related to its wavelength?

• Exponentially proportional

• Not related

• Inversely proportional

• Directly proportional

What color of light is associated with higher energy photons?

• Red

• Green

• Blue

• Violet

Which end of the spectrum is associated with longer wavelengths?

• Violet

• Blue

• Red

• Green

What happens when electrons drop in multiple steps from an excited state?

• They release a single high-energy photon

• They release multiple lower-energy photons

• They absorb more energy

• They remain in the excited state

How are light spectra used in science?

• To determine the speed of light

• To identify elements and substances

• To measure temperature

• To calculate atomic mass