12.3
Spektroskopia molekularna: absorpcja i emisja
Cząsteczki posiadają dyskretne poziomy energii zwane stanami kwantowymi. W przeciwieństwie do atomów, które mają prostsze poziomy energii, cząsteczki…
W cząsteczce istnieją dyskretne stany energetyczne zwane stanami kwantowymi. Każdy stan kwantowy – czy to elektronowy, wibracyjny czy rotacyjny – jest unikalny, ma określoną wartość energii i jest oddzielony od innych tego typu przerwami energetycznymi.
Po pochłonięciu fotonu promieniowania elektromagnetycznego cząsteczka może zostać wzbudzona do wyższego poziomu energetycznego. W efekcie ulega relaksacji na niższy poziom energetyczny poprzez emisję fotonu.
Cząsteczka może absorbować lub emitować tylko fotony o określonych energiach, które pasują do przerw energetycznych między tymi poziomami energii. Tak więc każde przejście jest zależne od częstotliwości lub długości fali.
W związku z tym w cząsteczce zachodzą różne rodzaje wzbudzenia, w zależności od długości fali promieniowania.
Na przykład fotony w obszarze mikrofalowym są absorbowane w celu zmiany wewnętrznej rotacji wiązania, podczas gdy te w obszarze podczerwieni posiadają energię potrzebną do zmiany częstotliwości wibracji wiązania.
Fotony w zakresie widzialnym UV mogą wzbudzać elektrony do wyższych stanów energii elektronowej.
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Q1: What are quantum states in molecules?
Quantum states are discrete energy levels that exist in molecules, each with a definite energy value. These states can be electronic, vibrational, or rotational, and are separated from one another by specific energy gaps. Unlike continuous energy, molecules can only occupy these distinct quantum states, making energy absorption and emission frequency-dependent processes.
Q2: How does a molecule absorb and emit photons?
A molecule absorbs a photon of electromagnetic radiation when its energy matches the gap between two quantum states, exciting the molecule to a higher energy level. When the excited molecule returns to a lower energy state, it emits a photon with energy equivalent to that gap. This process ensures each transition is wavelength- or frequency-dependent, allowing only specific photons to be absorbed or emitted.
Q3: Why do different wavelengths of radiation affect molecules differently?
Different radiation wavelengths correspond to different energy levels in molecules. Microwave photons possess energy to alter internal bond rotation, infrared photons change bond vibration frequencies, and ultraviolet and visible photons can excite electrons to higher electronic energy states. The varying magnitudes of energy gaps between rotational, vibrational, and electronic levels determine which wavelengths are absorbed during each type of transition.
Q4: What is the relationship between energy gaps and photon wavelength?
The energy of an absorbed or emitted photon is equivalent to the energy gap between two quantum states involved in a molecular transition. Since photon energy is inversely related to wavelength, larger energy gaps require shorter wavelengths and higher-frequency radiation. This direct relationship ensures that each specific transition in a molecule corresponds to a unique wavelength of electromagnetic radiation.
Q5: What types of molecular changes occur during photon absorption?
When a molecule absorbs a photon, three types of changes can occur depending on the radiation energy: rotation around a bond can change, the frequency of bond vibration can increase, or an electron can transition from its ground state to an excited state. Molecules with conjugated double bonds are particularly susceptible to electronic excitation by ultraviolet and visible photons.
Q6: How do electronic, vibrational, and rotational energy levels differ in molecules?
Molecules possess three distinct types of energy levels: electronic, vibrational, and rotational. Each type has its own set of discrete quantum states separated by characteristic energy gaps. The energy gaps between electronic levels are largest, followed by vibrational gaps, and then rotational gaps, which are smallest. These differences determine which wavelengths of radiation interact with each type of molecular motion.
Q7: Why must photon energy match specific molecular transitions?
Molecules can only absorb or emit photons whose energy exactly matches the energy gap between two quantum states. This quantized nature of molecular energy means that photons with incorrect energy cannot cause transitions. The specificity of this matching process is fundamental to spectroscopy and explains why molecular electronic transitions occur only at particular wavelengths.