All Flashcards
Label the energy level diagram showing electron transitions.
1: Ground State, 2: Excited State, 3: Absorption Transition, 4: Emission Transition.
Label the key components of a generic emission spectrum.
1: Wavelength, 2: Intensity, 3: Spectral Lines, 4: Continuous Spectrum (if present).
Label the key components of a generic absorption spectrum.
1: Wavelength, 2: Intensity, 3: Dark Lines (Absorption Lines), 4: Continuous Spectrum.
Label the parts of a hydrogen emission spectrum.
1: Balmer Series, 2: Specific Wavelengths, 3: Intensity of Lines.
Label the parts of a hydrogen absorption spectrum.
1: Balmer Series, 2: Specific Wavelengths, 3: Dark Absorption Lines.
What are the key differences between emission and absorption spectra?
Emission spectra show bright lines at specific wavelengths emitted by an element. Absorption spectra show dark lines at specific wavelengths absorbed by an element.
Compare the binding energy of an electron in the ground state versus an excited state.
Ground state: Highest binding energy, hardest to remove electron. Excited state: Lower binding energy, easier to remove electron.
Compare high frequency photons to low frequency photons in terms of energy.
High frequency photons: Larger energy transitions. Low frequency photons: Smaller energy transitions.
Compare absorption and emission in terms of energy change of the atom.
Absorption: Atom gains energy. Emission: Atom loses energy.
Compare the appearance of emission and absorption spectra.
Emission spectra: Bright lines on a dark background. Absorption spectra: Dark lines on a continuous spectrum.
What is the effect of an electron transitioning from a higher to a lower energy level?
Emission of a photon with energy equal to the energy difference between the levels.
What is the effect of an atom absorbing a photon with the exact energy difference between two energy levels?
The electron jumps to the higher energy level.
What is the effect of an atom absorbing energy greater than its binding energy?
Ionization: an electron is ejected from the atom, creating an ion.
Cause: An element is heated. What is the effect?
Effect: The element emits light at specific frequencies, creating its emission spectrum.
Cause: White light passes through a cool gas. What is the effect?
Effect: The gas absorbs specific wavelengths, creating dark lines in the spectrum (absorption spectrum).
What happens when an electron in an atom transitions to a lower energy level?
A photon is emitted with energy equal to the energy difference.