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- https://chem.libretexts.org/Bookshelves/General_Chemistry/General_Chemistry_Supplement_(Eames)/Quantum_Chemistry/Discovery_of_QuantizationHe assumed that the lines in the spectrum come from electrons moving from one stable orbit to another, and the wavelength of the light emitted equals the energy difference of the orbits.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/21%3A_Spectra_and_Structure_of_Atoms_and_Molecules/21.01%3A_Prelude_to_SpectroscopyAbsorption of an appropriate quantity of energy can raise the hydrogen atom from a lower to a higher energy level, while emission of electromagnetic radiation corresponds to a change from a higher to ...Absorption of an appropriate quantity of energy can raise the hydrogen atom from a lower to a higher energy level, while emission of electromagnetic radiation corresponds to a change from a higher to a lower energy level. Although Bohr’s theory is quantitatively accurate only for hydrogen, his idea of energy levels is useful for all other atoms and even for molecules.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/Concept_Development_Studies_in_Chemistry_(Hutchinson)/05_Quantum_Energy_Levels_in_Atomshe atomic molecular theory provides us a particulate understanding of matter. Each element is characterized as consisting of identical, indestructible atoms with atomic weights which have been determi...he atomic molecular theory provides us a particulate understanding of matter. Each element is characterized as consisting of identical, indestructible atoms with atomic weights which have been determined. Compounds consists of identical molecules, each made up from a specific number of atoms of each of the component elements. We also know that atoms have a nuclear structure, meaning that all of the positive charge and virtually all of the mass of the atom are concentrated in a nucleus.
- https://chem.libretexts.org/Courses/Western_Washington_University/Biophysical_Chemistry_(Smirnov_and_McCarty)/04%3A_Spectroscopy_-_Types_Key_Features_Examples/4.01%3A_Spectroscopy-_Basic_Elements_and_PrinciplesIn this Chapter, we will introduce a general notion of spectroscopy as a method and of its most basic type of data, a spectrum. We will also introduce the most basic features of each spectroscopic sig...In this Chapter, we will introduce a general notion of spectroscopy as a method and of its most basic type of data, a spectrum. We will also introduce the most basic features of each spectroscopic signal (spectral line or resonance): position, intensity and width/lineshape. Lastly, we will take a look at a relationship between quantum chemistry features of a sample (energy levels of electrons and other quantized particles) and spectral properties of such a sample.
- https://chem.libretexts.org/Bookshelves/Physical_and_Theoretical_Chemistry_Textbook_Maps/Physical_Chemistry_(LibreTexts)/01%3A_The_Dawn_of_the_Quantum_Theory/1.05%3A_The_Rydberg_Formula_and_the_Hydrogen_Atomic_SpectrumThis page discusses Rydberg's theory and Balmer's formula for predicting hydrogen spectrum wavelengths, highlighting Balmer's 1885 formula for visible wavelengths and Rydberg's generalization for all ...This page discusses Rydberg's theory and Balmer's formula for predicting hydrogen spectrum wavelengths, highlighting Balmer's 1885 formula for visible wavelengths and Rydberg's generalization for all atomic spectra, including the Lyman series in the ultraviolet. The Lyman series corresponds to transitions to the n=1 orbit, with relevant formulas and values mentioned. Various sequentially named series are outlined, emphasizing that atomic spectra provide insights into atomic structure.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/05%3A_Electrons_in_Atoms/5.01%3A_Electromagnetic_SpectrumThis page discusses the nature of waves, highlighting that they represent energy beyond just water. It critiques Rutherford's atomic model for not addressing electron behavior and notes early 20th-cen...This page discusses the nature of waves, highlighting that they represent energy beyond just water. It critiques Rutherford's atomic model for not addressing electron behavior and notes early 20th-century experiments showcasing light's dual wave-particle nature. Additionally, it details visible light's wavelength (400-700 nm) and speed (3.
