Degeneracy vs. Energy Level Scaling for Hydrogen
... this e↵ect and give the same potential energy for each shell. The total energy of the system is linear in the filling fraction ⌫, representing the number of filled energy levels. Each electron within a given shell contributes equally, while a totally filled shell contributes 2E0 . Figure 1 shows how ...
... this e↵ect and give the same potential energy for each shell. The total energy of the system is linear in the filling fraction ⌫, representing the number of filled energy levels. Each electron within a given shell contributes equally, while a totally filled shell contributes 2E0 . Figure 1 shows how ...
Chemical Change
... The chemical properties of elements are related to the energy changes that take place when atoms lose, gain or share electrons to obtain a filled valence shell. ...
... The chemical properties of elements are related to the energy changes that take place when atoms lose, gain or share electrons to obtain a filled valence shell. ...
Honors Chemistry
... 8. What is a line-emission spectrum and how is it different from a continuous spectrum? A line-emission spectrum is emitted light that gives off separated frequencies of electromagnetic radiation when passed through a prism. A continues spectrum is an emission of a continuous range of frequency of ...
... 8. What is a line-emission spectrum and how is it different from a continuous spectrum? A line-emission spectrum is emitted light that gives off separated frequencies of electromagnetic radiation when passed through a prism. A continues spectrum is an emission of a continuous range of frequency of ...
GY 111 Lecture Note Series Elemental Chemistry
... sometimes help to imagine that they do. They are assigned to different energy levels or electron shells. Each successive level is at a higher energy level than the previous one and each energy level contains a different maximum number of electrons: ...
... sometimes help to imagine that they do. They are assigned to different energy levels or electron shells. Each successive level is at a higher energy level than the previous one and each energy level contains a different maximum number of electrons: ...
QM-01
... • Wave-particle duality- matter can behave both like particles as well as waves. Louis de Broglie • If a particle of mass m moves with a velocity v then it behaves like a matter wave having a wavelength λ given by, λ= ...
... • Wave-particle duality- matter can behave both like particles as well as waves. Louis de Broglie • If a particle of mass m moves with a velocity v then it behaves like a matter wave having a wavelength λ given by, λ= ...
Quantum Numbers - Evan`s Chemistry Corner
... o ℓ =0 is called s o ℓ =1 is called p o ℓ =2 is called d o ℓ =3 is called f o For ℓ >3, the sublevels are named alphabetically, (g, h, and i), but there are no atoms with electrons in these locations. ...
... o ℓ =0 is called s o ℓ =1 is called p o ℓ =2 is called d o ℓ =3 is called f o For ℓ >3, the sublevels are named alphabetically, (g, h, and i), but there are no atoms with electrons in these locations. ...
Solid State Physics
... Ionic Bonding Consider two different atoms, such as Ga and As joined by a covalent bond. The functions come from different orbitals. The C constants would be different. The wave function still spreads between the atoms, but the probability is that the shared electron will be nearer to one atom th ...
... Ionic Bonding Consider two different atoms, such as Ga and As joined by a covalent bond. The functions come from different orbitals. The C constants would be different. The wave function still spreads between the atoms, but the probability is that the shared electron will be nearer to one atom th ...
Lecture 5: The Hydrogen Atom (continued). In the previous lecture
... The Spin of the Electron. Introduction. With high resolution spectrometers one finds many spectral lines split into two. This is called fine structure. The first attempt at an explanation of the fine structure was made by Sommerfeld in 1916, even before the birth of quantum mechanics. Developing the ...
... The Spin of the Electron. Introduction. With high resolution spectrometers one finds many spectral lines split into two. This is called fine structure. The first attempt at an explanation of the fine structure was made by Sommerfeld in 1916, even before the birth of quantum mechanics. Developing the ...
Figure 7.18 The 3d orbitals
... Experiments with "excited" atoms of H produced emission spectra - always a discrete set of lines at certain wavelengths White light dispersed by a prism or diffraction grating: - we see ROYGBIV – a continuous spectrum from 750 nm to 400 nm When a gas-filled tube is charged with current, only certain ...
... Experiments with "excited" atoms of H produced emission spectra - always a discrete set of lines at certain wavelengths White light dispersed by a prism or diffraction grating: - we see ROYGBIV – a continuous spectrum from 750 nm to 400 nm When a gas-filled tube is charged with current, only certain ...
Chapter 2.2 and 7 Notes
... So waves act like matter…can matter act like waves? It turns out that matter does act like ...
... So waves act like matter…can matter act like waves? It turns out that matter does act like ...
Modeling Single Electron Transistor Sensitivity for Read
... Energy spacing must be greater then thermal smearing ...
... Energy spacing must be greater then thermal smearing ...
III. Quantum Model of the Atom
... Pauli Exclusion Principle No two electrons in an atom can have the same 4 quantum numbers. Each e- has a unique “address”: ...
... Pauli Exclusion Principle No two electrons in an atom can have the same 4 quantum numbers. Each e- has a unique “address”: ...
IB Phys..
... – 2. A diffraction grating or prism is used to determine what frequencies pass through the gas and which are absorbed. ...
... – 2. A diffraction grating or prism is used to determine what frequencies pass through the gas and which are absorbed. ...
AP Chemistry
... 6.3.1 Monochromatic light = light of a single wavelength 6.3.2 Spectrum = when radiation from a source is separated into its different wavelengths 6.3.2.1 Continuous spectrum = rainbow of colors, containing light of all wavelengths 6.3.2.2 Some radiation sources give off light with only a few, speci ...
... 6.3.1 Monochromatic light = light of a single wavelength 6.3.2 Spectrum = when radiation from a source is separated into its different wavelengths 6.3.2.1 Continuous spectrum = rainbow of colors, containing light of all wavelengths 6.3.2.2 Some radiation sources give off light with only a few, speci ...
Notes 7
... is the nuclear screening constant. (See the table on page Justification for this large approximation is: ...
... is the nuclear screening constant. (See the table on page Justification for this large approximation is: ...
Answers
... 6) How are the photoelectric effect and an LED similar/different? The photoelectric effect involves a metal and an LED involves a semiconductor. Otherwise they use reverse processes, where one electron kicks out one photon or the reverse. The photon only appears before or after, but the electron doe ...
... 6) How are the photoelectric effect and an LED similar/different? The photoelectric effect involves a metal and an LED involves a semiconductor. Otherwise they use reverse processes, where one electron kicks out one photon or the reverse. The photon only appears before or after, but the electron doe ...
Honors Chemistry
... 10. What is meant by an electron having dual wave-particle nature, where were these electrons described as being located, and who suggested this theory? Sometimes light acts like a wave and some other times like a particle. To understand what light is one must take both characteristics into consider ...
... 10. What is meant by an electron having dual wave-particle nature, where were these electrons described as being located, and who suggested this theory? Sometimes light acts like a wave and some other times like a particle. To understand what light is one must take both characteristics into consider ...
Bohr model
In atomic physics, the Rutherford–Bohr model or Bohr model, introduced by Niels Bohr in 1913, depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity. After the cubic model (1902), the plum-pudding model (1904), the Saturnian model (1904), and the Rutherford model (1911) came the Rutherford–Bohr model or just Bohr model for short (1913). The improvement to the Rutherford model is mostly a quantum physical interpretation of it. The Bohr model has been superseded, but the quantum theory remains sound.The model's key success lay in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen. While the Rydberg formula had been known experimentally, it did not gain a theoretical underpinning until the Bohr model was introduced. Not only did the Bohr model explain the reason for the structure of the Rydberg formula, it also provided a justification for its empirical results in terms of fundamental physical constants.The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems (see below for application), the Bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atom. A related model was originally proposed by Arthur Erich Haas in 1910, but was rejected. The quantum theory of the period between Planck's discovery of the quantum (1900) and the advent of a full-blown quantum mechanics (1925) is often referred to as the old quantum theory.