All Flashcards
Define a photon.
A photon is a discrete packet of light energy.
What is an atom's emission spectrum?
The specific frequencies of light an element emits when its atoms transition from higher to lower energy states.
What is an atom's absorption spectrum?
The specific frequencies of light an element absorbs when its atoms transition from lower to higher energy states.
Define binding energy.
The minimum energy required to remove an electron from an atom.
What is ionization?
The process where an electron is removed from an atom, creating an ion.
Define ground state.
The lowest energy level of an atom.
Describe the process of photon absorption by an atom.
An atom absorbs a photon with energy equal to the difference between two energy levels, causing an electron to jump to a higher energy level.
Describe the process of photon emission by an atom.
An electron drops to a lower energy level, emitting a photon with energy equal to the energy difference between the levels.
What is the first step in identifying an element using its spectrum?
Analyze the emission or absorption spectrum to identify the unique set of spectral lines.
What is the process of ionization?
An atom absorbs energy greater than its binding energy, resulting in the removal of an electron and the formation of an ion.
What is the process of electron transition to a higher energy level?
The electron absorbs a photon with the exact amount of energy needed to move to the higher energy level.
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.