All Flashcards
What is the effect of an electron transitioning 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 needed for a transition?
An electron jumps to a higher energy level.
What is the effect of an atom absorbing energy greater than its binding energy?
Ionization: an electron is removed from the atom.
What happens when an element is heated?
Atoms gain energy and electrons jump to higher energy levels. As they return to lower levels, they emit photons, creating an emission spectrum.
What is the effect of shining white light through a gas of a specific element?
The element absorbs specific wavelengths of light, creating dark lines in the absorption spectrum.
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.
Describe the process of photon absorption by an atom.
An atom absorbs a photon with energy equal to the energy difference between two of its energy levels. The electron jumps to a higher energy level.
Describe the process of photon emission by an atom.
An electron drops to a lower energy level, releasing a photon with energy equal to the energy difference between the two levels.
Explain how to identify an element using its emission spectrum.
Analyze the specific frequencies (wavelengths) of light emitted. Each element has a unique emission spectrum, acting as a 'fingerprint'.
Describe how ionization occurs.
An atom absorbs energy greater than or equal to its binding energy, causing an electron to be ejected, forming an ion.
What is the first step in analyzing an unknown gas using absorption spectra?
Shine a continuous spectrum of light through the gas and observe which wavelengths are absorbed. The absorbed wavelengths correspond to the gas's absorption spectrum.