Bohr Model and Electron Energy Levels

The video tutorial by Mr. Donahue covers the Bohr model and the energies of principal energy levels. It explains the continuous and line spectra, focusing on how different light sources produce various wavelengths. The Rydberg equation is introduced to calculate the wavelengths of light emitted by hydrogen. Bohr's postulates are discussed, explaining the distinct energy levels of electrons and their transitions. The video also covers energy calculations and the limitations of the Bohr model, highlighting its applicability to hydrogen and its shortcomings for other elements.

What is a continuous spectrum?

• A spectrum with only one color

• A spectrum with only ultraviolet light

• A spectrum with no gaps in wavelengths

• A spectrum with distinct lines

What is the main difference between a continuous spectrum and a line spectrum?

• Continuous spectrum has gaps, line spectrum does not

• Line spectrum is produced by solids, continuous by gases

• Continuous spectrum has no gaps, line spectrum has distinct lines

• Line spectrum is only visible in sunlight

What does the Rydberg equation help to determine?

• The mass of an electron

• The wavelengths of light emitted by hydrogen

• The energy levels of electrons

• The speed of light

According to Bohr's model, what happens when an electron changes energy levels?

• It emits or absorbs a photon

• It loses mass

• It changes into a proton

• It stops moving

Which of the following is NOT one of Bohr's postulates?

• Orbits have specific radii

• Energy is emitted or absorbed when changing orbits

• Electrons have specific energies in orbits

• Electrons can occupy any orbit

What is the ground state of an electron?

• The highest energy state

• The state with the most energy

• The lowest possible energy state

• A state where the electron is not moving

What happens to the energy of an electron as it moves to a higher energy level?

• It becomes more negative

• It becomes zero

• It becomes less negative

• It remains the same

Why does the Bohr model fail for elements other than hydrogen?

• It only works at high temperatures

• It only works for gases

• It does not account for multiple electrons

• It cannot calculate energy levels

What concept introduced by Bohr is still part of the current atomic model?

• Electrons orbit like planets

• Electrons exist in discrete energy levels

• Electrons have no mass

• Electrons are stationary

What is a limitation of the Bohr model?

• It describes electron interactions

• It explains electron wave properties

• It only works for hydrogen

• It accurately describes all elements