4.5.3 Energy Levels and Spectra

• What applications rely on discrete energy levels?

  Spectroscopy and lasers
• What are atomic energy levels?

  Specific, discrete energy values
• What is the stability of an electron in the ground state?

  Most stable
• According to the Bohr Model, what type of energy levels can electrons occupy?

  Specific, fixed energy levels
• What happens to an electron when it absorbs a photon in the Bohr Model?

  It jumps to an excited state
• What are discrete energy levels in atomic physics?

  Fixed energy values
• What does energy quantization mean in atomic physics?

  Electrons occupy specific energy levels
• What are discrete energy levels?

  Specific energy values for electrons
• Electrons can only occupy fixed energy levels within an atom due to energy quantization.


  True
• Electrons in excited states emit photons when they return to lower energy levels.


  True
• Electrons can absorb or emit photons to jump between energy levels in the Bohr Model.


  True
• Discrete energy levels signify that electrons cannot possess any energy value between these defined levels
• Discrete energy levels are essential for understanding atomic behavior, light emission, and absorption, enabling technologies like spectroscopy
• Electrons jump between discrete energy levels by absorbing or emitting photons
• Electrons can only occupy specific energy levels
• Absorption spectra show dark lines against a bright background.


  True
• When are emission spectra generated?

  Excited atoms release photons
• What type of photon emission is associated with moderate energy differences?

  Moderately bright line
• The Bohr Model describes electrons orbiting the nucleus in discrete energy levels
• Electrons can only possess fixed energy values
• What are spectral lines formed by?

  Electron transitions
• Match the spectral type with its characteristics:

  Emission ↔️ Bright line on dark background

  Absorption ↔️ Dark line on bright background
• Match the Balmer series line with its corresponding wavelength:

  H-alpha ↔️ 656.3 nm

  H-beta ↔️ 486.1 nm

  H-gamma ↔️ 434.0 nm

  H-delta ↔️ 410.2 nm
• What is the value of the Rydberg constant in the Rydberg Formula?

  $1.097 \times 10^{7} \text{ m}^{ - 1}$
• Order the steps in spectral analysis to determine the composition of a material:

  1️⃣ Generate a spectrum

  2️⃣ Compare spectral lines with known elements

  3️⃣ Identify elemental composition
• The lowest energy level an electron can occupy is called the ground
• The Bohr Model describes electrons orbiting the nucleus in discrete
• The lowest energy level in the Bohr Model is called the ground
• Energy quantization means electrons can only occupy specific energy levels within an atom.


  True
• Match the state with its description:

  Ground State ↔️ Lowest energy state

  Excited State ↔️ Higher energy states
• Discrete energy levels are important for understanding light emission and absorption in atomic behavior.


  True
• A continuous spectrum has distinct gaps between energy levels.

  False
• What process creates absorption spectra?

  Atoms absorb photons
• Spectral lines in emission spectra correspond to photons emitted when electrons drop to lower energy levels.


  True
• The ground state is the lowest energy level an electron can occupy.


  True
• In the Bohr Model, electrons emit photons when they jump to higher energy levels.

  False
• Emission spectra produce bright lines against a dark background because excited atoms release photons.

  True
• Emission spectra produce bright lines on a dark background when electrons fall from higher to lower energy levels.


  True
• What is the most prominent series of spectral lines in the hydrogen spectrum called?

  Balmer series
• The Bohr model explains the hydrogen spectrum by proposing that electrons can only occupy discrete energy levels.


  True