Atomic Structure and Electron Configurations Multiple Choice PSI
... D. all of the above 21. Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A. 3f C. 3p B. 3d D. 3s 22. Which one of the following is an incorrect orbital notation? A. 4f C. 3s B. 2d D. 2p 23. There are __________ sub-orbitals in the 3rd shell. A. 25 B. 4 ...
... D. all of the above 21. Which of the orbitals below do not exist due to the constraints upon the angular quantum number? A. 3f C. 3p B. 3d D. 3s 22. Which one of the following is an incorrect orbital notation? A. 4f C. 3s B. 2d D. 2p 23. There are __________ sub-orbitals in the 3rd shell. A. 25 B. 4 ...
Chap30-DrJJ - 2 slides
... In the Bohr model, a photon is emitted when the electron drops from a larger, higherenergy orbit to a smaller, lower energy orbit. In a hydrogen atom, electrons’ total (kinetic & potential) energy can have only certain allowed values corresponding different orbits (stationary state or orbits) of the ...
... In the Bohr model, a photon is emitted when the electron drops from a larger, higherenergy orbit to a smaller, lower energy orbit. In a hydrogen atom, electrons’ total (kinetic & potential) energy can have only certain allowed values corresponding different orbits (stationary state or orbits) of the ...
No Slide Title - Rubin Gulaboski
... • However, a charged particle moving in a circular path should lose energy. • This means that the atom should be unstable according to Rutherford’s theory. • Bohr noted the line spectra of certain elements and assumed the electrons were confined to specific energy states. These were called orbits. ...
... • However, a charged particle moving in a circular path should lose energy. • This means that the atom should be unstable according to Rutherford’s theory. • Bohr noted the line spectra of certain elements and assumed the electrons were confined to specific energy states. These were called orbits. ...
Many-Electron Atoms Thornton and Rex, Ch. 8
... Many-Electron Atoms For many-electron atoms there is now orbit-orbit and spin-spin interactions, in addition to spin-orbit interactions. Consider simplest case of 2 electrons with L1, S1 and L2, S2. Only “good” quantum number is ...
... Many-Electron Atoms For many-electron atoms there is now orbit-orbit and spin-spin interactions, in addition to spin-orbit interactions. Consider simplest case of 2 electrons with L1, S1 and L2, S2. Only “good” quantum number is ...
Many-Electron Atoms Thornton and Rex, Ch. 8
... Many-Electron Atoms For many-electron atoms there is now orbit-orbit and spin-spin interactions, in addition to spin-orbit interactions. Consider simplest case of 2 electrons with L1, S1 and L2, S2. Only “good” quantum number is ...
... Many-Electron Atoms For many-electron atoms there is now orbit-orbit and spin-spin interactions, in addition to spin-orbit interactions. Consider simplest case of 2 electrons with L1, S1 and L2, S2. Only “good” quantum number is ...
Chapter 3 Make up Test 2004
... Read carefully for questions 28-30: Experiments reveal that all oxygen atoms have six protons. However, they may have atomic masses of 16, 17, or 18. ______28. The nucleus of each carbon atom contains: A. neutrons and electrons B. protons and electrons C. neutrons and protons D. electron energy leve ...
... Read carefully for questions 28-30: Experiments reveal that all oxygen atoms have six protons. However, they may have atomic masses of 16, 17, or 18. ______28. The nucleus of each carbon atom contains: A. neutrons and electrons B. protons and electrons C. neutrons and protons D. electron energy leve ...
Chapter 6 and 7 Reading Guide Electronic Structure of Atoms and
... Be sure to read “A Closer Look” on page 260. Follow the diagram for a clear understanding of effective nuclear charge. This concept is critical to understanding periodic trends. Section 7.3 Define the following terms: non-bonding atomic radius (van der Waal’s radius): ...
... Be sure to read “A Closer Look” on page 260. Follow the diagram for a clear understanding of effective nuclear charge. This concept is critical to understanding periodic trends. Section 7.3 Define the following terms: non-bonding atomic radius (van der Waal’s radius): ...
Help Sheet
... Increases as you move DOWN, Small in full or ½ full orbitals Decreases as you move DOWN, High in full or ½ full orbitals Decreases as you move DOWN, High in almost full orbitals, low in full orbitals Metal or a non-metal (ox. no. of +1 and –1) Metal w/ox. no. of +1, increase reactivity down table, R ...
... Increases as you move DOWN, Small in full or ½ full orbitals Decreases as you move DOWN, High in full or ½ full orbitals Decreases as you move DOWN, High in almost full orbitals, low in full orbitals Metal or a non-metal (ox. no. of +1 and –1) Metal w/ox. no. of +1, increase reactivity down table, R ...
Energy and Matter - Hicksville Public Schools
... The excited state is short living. According to the Bohr model of the atom, hydrogen’s atomic emission spectrum = bright line spectrum, results from electrons dropping from higher-energy atomic orbits (excited state) to lower-energy atomic orbits (ground state). ...
... The excited state is short living. According to the Bohr model of the atom, hydrogen’s atomic emission spectrum = bright line spectrum, results from electrons dropping from higher-energy atomic orbits (excited state) to lower-energy atomic orbits (ground state). ...
Problem 1 Tritium (3H) is a radioactive isotope of hydrogen. The
... because the nucleus is not really a point charge. Assume the proton is a uniformly distributed spherical charge cloud of radius R = 1 fermi. Neglect fine structure. H INT: Find the potential both inside and outside R and subtract the Coulomb potential to get H ′ . You can simplify the subsequent cal ...
... because the nucleus is not really a point charge. Assume the proton is a uniformly distributed spherical charge cloud of radius R = 1 fermi. Neglect fine structure. H INT: Find the potential both inside and outside R and subtract the Coulomb potential to get H ′ . You can simplify the subsequent cal ...
Early Modern Physics
... l=hc/pc = 1240 ev*nm/97 MeV = 13 Fermi p=50 GeV/c (electron or proton) gives .025 fm (size of proton: 1 F) P460 - Early Modern ...
... l=hc/pc = 1240 ev*nm/97 MeV = 13 Fermi p=50 GeV/c (electron or proton) gives .025 fm (size of proton: 1 F) P460 - Early Modern ...
Basic Atomic Theory
... • Mathematically gravitational force similar to Coulomb forces • Strength of Coulomb forces much larger than gravitational • +ve and –ve charges cause attractive and repulsive interactions. ...
... • Mathematically gravitational force similar to Coulomb forces • Strength of Coulomb forces much larger than gravitational • +ve and –ve charges cause attractive and repulsive interactions. ...
Seeing Atoms and Electrons in Motion - The Munich
... LMU München / MPI Quantenoptik / Munich-Centre for Advanced Photonics (MAP) ...
... LMU München / MPI Quantenoptik / Munich-Centre for Advanced Photonics (MAP) ...
Quantum Mechanics
... • If electrons (and other particles) can act like waves, what else can they do? • They can setup standing waves – Waves with particular wavelength/frequency that appear to not be travelling ...
... • If electrons (and other particles) can act like waves, what else can they do? • They can setup standing waves – Waves with particular wavelength/frequency that appear to not be travelling ...
Chapter 7
... • Travel in waves that can be described by their wavelength (lamda –l) and frequency (n- nu) • In a vacuum, travel at the speed of light, c = 3 x 108 m/s ...
... • Travel in waves that can be described by their wavelength (lamda –l) and frequency (n- nu) • In a vacuum, travel at the speed of light, c = 3 x 108 m/s ...
Some Quantum Considerations II
... Which of the following statements is false? a. Longer wavelength radiation carries higher energies. b. Light can be considered to be made up of particles called photons. c. All material objects have some wave characteristics. d. Electrons can be viewed as standing waves in an atom. e. Bohr’s model o ...
... Which of the following statements is false? a. Longer wavelength radiation carries higher energies. b. Light can be considered to be made up of particles called photons. c. All material objects have some wave characteristics. d. Electrons can be viewed as standing waves in an atom. e. Bohr’s model o ...
Early Modern Physics
... l=hc/pc = 1240 ev*nm/97 MeV = 13 Fermi p=50 GeV/c (electron or proton) gives .025 fm (size of proton: 1 F) P460 - Early Modern ...
... l=hc/pc = 1240 ev*nm/97 MeV = 13 Fermi p=50 GeV/c (electron or proton) gives .025 fm (size of proton: 1 F) P460 - Early Modern ...
Review Sheet Filled Out
... Electrons closest to the nucleus have the least amount of energy Electrons farthest away from the nucleus have the most energy – valence e Have a negative charge Have insignificant mass and volume Reside in the 99.996% of the atom outside the nucleus Can’t tell where an electron is at any ...
... Electrons closest to the nucleus have the least amount of energy Electrons farthest away from the nucleus have the most energy – valence e Have a negative charge Have insignificant mass and volume Reside in the 99.996% of the atom outside the nucleus Can’t tell where an electron is at any ...
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.