Quantum Theory of Atoms and Molecules
... Atomic motion. Quantum mechanical description of the translational, vibrational and rotational behaviour of isolated molecules. Solution of the Schrödinger equation and form of wavefunctions for simple harmonic oscillator and rigid rotor. Heat capacities. Comparison with classical behaviour. Deficie ...
... Atomic motion. Quantum mechanical description of the translational, vibrational and rotational behaviour of isolated molecules. Solution of the Schrödinger equation and form of wavefunctions for simple harmonic oscillator and rigid rotor. Heat capacities. Comparison with classical behaviour. Deficie ...
Document
... Only orbits that fit n electron wavelengths are allowed Explains the stability of the atom Energy quantization correct for single e– atoms (H, He+, Li++) However, it is fundamentally incorrect ...
... Only orbits that fit n electron wavelengths are allowed Explains the stability of the atom Energy quantization correct for single e– atoms (H, He+, Li++) However, it is fundamentally incorrect ...
atomic physics
... 2. The electrons can only orbit stably, without radiating, in certain orbits (called the "stationary orbits”) at a certain discrete set of distances from the nucleus. These orbits are associated with definite energies and are also called energy shells or energy levels. In these orbits, the electron' ...
... 2. The electrons can only orbit stably, without radiating, in certain orbits (called the "stationary orbits”) at a certain discrete set of distances from the nucleus. These orbits are associated with definite energies and are also called energy shells or energy levels. In these orbits, the electron' ...
Atomic Physics 4
... • electrons are either in lowest energy state (ground state) or certain allowed levels (excited state). ...
... • electrons are either in lowest energy state (ground state) or certain allowed levels (excited state). ...
slides
... I found it particularly beautiful in the presentation of the complex structure that you have left all modellmässig considerations to one side. The model-idea now finds itself in a difficult, fundamental [prinzipiellen] crisis, which I believe will end with a further radical sharpening of the opposit ...
... I found it particularly beautiful in the presentation of the complex structure that you have left all modellmässig considerations to one side. The model-idea now finds itself in a difficult, fundamental [prinzipiellen] crisis, which I believe will end with a further radical sharpening of the opposit ...
Chem 1151
... (5) Titration with solutions of KBrO3 can be used to determine the concentration of As(III) in an unknown sample. What is the molarity of As(III) if 33.45 mL of 0.125M KBrO3 is needed to titrate 50.0 mL of the As(III) solution? The balanced chemical equation is H3AsO3(aq) + BrO3-(aq) Br -(aq) + 3H ...
... (5) Titration with solutions of KBrO3 can be used to determine the concentration of As(III) in an unknown sample. What is the molarity of As(III) if 33.45 mL of 0.125M KBrO3 is needed to titrate 50.0 mL of the As(III) solution? The balanced chemical equation is H3AsO3(aq) + BrO3-(aq) Br -(aq) + 3H ...
Quantum theory
... • Each pair in a sublevel has a different place in space • Due to the interactions of the e- within a sublevel on each other • Try to be as far from each other as possible due to the fact they are all same charge • The space occupied by one pair of e- is called an orbital • Designated by quantum nu ...
... • Each pair in a sublevel has a different place in space • Due to the interactions of the e- within a sublevel on each other • Try to be as far from each other as possible due to the fact they are all same charge • The space occupied by one pair of e- is called an orbital • Designated by quantum nu ...
3D Schrödinger Eq.
... Schrodinger’s solution for multi-electron atoms What’s different for these cases? Potential energy (V) changes! (Now more protons AND other electrons) V (for q1) = kqnucleusq1/rn-1 + kq2q1/r2-1 + kq3q1/r3-1 + …. Need to account for all the interactions among the electrons Must solve for all electro ...
... Schrodinger’s solution for multi-electron atoms What’s different for these cases? Potential energy (V) changes! (Now more protons AND other electrons) V (for q1) = kqnucleusq1/rn-1 + kq2q1/r2-1 + kq3q1/r3-1 + …. Need to account for all the interactions among the electrons Must solve for all electro ...
topics in atomic physics - University of Missouri
... reflects the predilection of the authors toward certain aspects of the subject. This one is no exception. It reflects our belief that a thorough understanding of the unique properties of the hydrogen atom is essential to an understanding of atomic physics. It also reflects our fascination with the d ...
... reflects the predilection of the authors toward certain aspects of the subject. This one is no exception. It reflects our belief that a thorough understanding of the unique properties of the hydrogen atom is essential to an understanding of atomic physics. It also reflects our fascination with the d ...
Chapter 6.8 - Periodic Trends
... Electrons in the orbitals are attracted to the protons in the nucleus. One might think that each electron in the Na atom would experience the pull of all 11 of its electrons. But this is not the case. The effective nuclear charge is less than 11 due to shielding effects. Which of the following state ...
... Electrons in the orbitals are attracted to the protons in the nucleus. One might think that each electron in the Na atom would experience the pull of all 11 of its electrons. But this is not the case. The effective nuclear charge is less than 11 due to shielding effects. Which of the following state ...
Raman spectroscopy
... Electronic energy levels of a molecule gives much more information about the structure of molecules ...
... Electronic energy levels of a molecule gives much more information about the structure of molecules ...
What is Matter - watertown.k12.wi.us
... freely moving charged particles, (electrons & ions) It is perhaps the most common phase of matter in the Matter is made up of ...
... freely moving charged particles, (electrons & ions) It is perhaps the most common phase of matter in the Matter is made up of ...
Document
... c. Speed of light (c) is a constant, so νλ is also a constant ν (nu) and λ (lambda) must be inversely proportional ...
... c. Speed of light (c) is a constant, so νλ is also a constant ν (nu) and λ (lambda) must be inversely proportional ...
Niels Bohr, greatest physicist of the 20th century
... Never express yourself more clearly than you think. We are suspended in language in such a way that we cannot say what is up and what is down. The word “reality” is also a word, a word which we must learn to use correctly. When it comes to atoms, language can be used only as in poetry. The poet, too ...
... Never express yourself more clearly than you think. We are suspended in language in such a way that we cannot say what is up and what is down. The word “reality” is also a word, a word which we must learn to use correctly. When it comes to atoms, language can be used only as in poetry. The poet, too ...
Ch. 5 Electrons in Atoms
... - Waves and particles were seemingly opposites, yet light exhibits both characteristics ...
... - Waves and particles were seemingly opposites, yet light exhibits both characteristics ...
The Quantum Numbers
... If two negatively charged particles occupy the same orbital, how do they keep from repelling one another? It is possible the electrons spin in opposite directions and therefore, produce opposite magnetic fields that attract rather than repel one another. Scientist refer to these possible spins as (+ ...
... If two negatively charged particles occupy the same orbital, how do they keep from repelling one another? It is possible the electrons spin in opposite directions and therefore, produce opposite magnetic fields that attract rather than repel one another. Scientist refer to these possible spins as (+ ...
BCK0103-15 Quantum physics (3-0-4) - nuvem
... General goals: The main goal of this course is to present to the student the main concepts of the quantum theory, with the perspective of comprehending the basic phenomena which originate at the atomic scale, their effects and technological applications. ...
... General goals: The main goal of this course is to present to the student the main concepts of the quantum theory, with the perspective of comprehending the basic phenomena which originate at the atomic scale, their effects and technological applications. ...
o Positive charge • Electrons
... Atomic mass (u) = average mass of atoms of isotopes as the occur naturally To calculate: o Divide percentages by 100 to find natural abundances o Atomic mass = (abundance 1 x mass 1) + (abundance 2 x mass 2) ...
... Atomic mass (u) = average mass of atoms of isotopes as the occur naturally To calculate: o Divide percentages by 100 to find natural abundances o Atomic mass = (abundance 1 x mass 1) + (abundance 2 x mass 2) ...
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.