Energy Levels and Light Absorption
... • Consider an electron in an atom with quantum number n = n1. How many electrons in this atom can have the quantum number n1? n1 • Pauli exclusion says no two electrons can be in exactly the same state ...
... • Consider an electron in an atom with quantum number n = n1. How many electrons in this atom can have the quantum number n1? n1 • Pauli exclusion says no two electrons can be in exactly the same state ...
PowerPoint Presentation - Chapter 15
... His formula required that light could only be absorbed or emitted in discrete chunks or quanta, whose energy depended on the ...
... His formula required that light could only be absorbed or emitted in discrete chunks or quanta, whose energy depended on the ...
Ionic And Covalent Bonds
... c. Be able to calculate the average atomic mass of a set of isotopes. d. Be able to draw a picture (or write a clear description) that represents each different model of the atom. e. Know the difference between an atom, ion, and isotope. f. Be able to count the number of protons, neutrons, and elect ...
... c. Be able to calculate the average atomic mass of a set of isotopes. d. Be able to draw a picture (or write a clear description) that represents each different model of the atom. e. Know the difference between an atom, ion, and isotope. f. Be able to count the number of protons, neutrons, and elect ...
File
... The concept of discrete energy levels can be demonstrated with a 3-way light bulb. A 40/75/115 watt bulb can only shine light at those three wattage's, and when you switch from one setting to the next, the power immediately jumps to the new setting instead of just gradually increasing. It is the fac ...
... The concept of discrete energy levels can be demonstrated with a 3-way light bulb. A 40/75/115 watt bulb can only shine light at those three wattage's, and when you switch from one setting to the next, the power immediately jumps to the new setting instead of just gradually increasing. It is the fac ...
Review for Test II
... F. Microwaves G. Radio waves Classical vs Quantum physics for matter and light ...
... F. Microwaves G. Radio waves Classical vs Quantum physics for matter and light ...
lecture notes, page 2
... • Similar to the angular momentum quantum number, l, ms describes the magnitude of an angular momentum. However, ms completes the description of an __________________ and is NOT dependent on the orbital. The property of electron spin was first proposed by S. Goudsmit and G. Uhlenbeck in 1925 to exp ...
... • Similar to the angular momentum quantum number, l, ms describes the magnitude of an angular momentum. However, ms completes the description of an __________________ and is NOT dependent on the orbital. The property of electron spin was first proposed by S. Goudsmit and G. Uhlenbeck in 1925 to exp ...
wave-particle duality
... The flux of particles arriving at the slits can be reduced so that only one particle arrives at a time. Interference fringes are still observed! Wave-behaviour can be shown by a single atom. Each particle goes through both slits at once. A matter wave can interfere with itself. Hence matter-waves ar ...
... The flux of particles arriving at the slits can be reduced so that only one particle arrives at a time. Interference fringes are still observed! Wave-behaviour can be shown by a single atom. Each particle goes through both slits at once. A matter wave can interfere with itself. Hence matter-waves ar ...
Quantum Mechanics
... L = L = l (l + 1) , where l = 1, 2,3,..., n − 1 The permitted values of the component of L in a given direction, say the z-direction: Lz = m , where m = −l , −l + 1,...0,...l − 1, l . This quantum number can be zero or a positive or negative integer up to, but no larger in magnitude than l. This qua ...
... L = L = l (l + 1) , where l = 1, 2,3,..., n − 1 The permitted values of the component of L in a given direction, say the z-direction: Lz = m , where m = −l , −l + 1,...0,...l − 1, l . This quantum number can be zero or a positive or negative integer up to, but no larger in magnitude than l. This qua ...
WAVE-PARTICLE DUALITY
... The flux of particles arriving at the slits can be reduced so that only one particle arrives at a time. Interference fringes are still observed! Wave-behaviour can be shown by a single atom. Each particle goes through both slits at once. A matter wave can interfere with itself. Hence matter-waves ar ...
... The flux of particles arriving at the slits can be reduced so that only one particle arrives at a time. Interference fringes are still observed! Wave-behaviour can be shown by a single atom. Each particle goes through both slits at once. A matter wave can interfere with itself. Hence matter-waves ar ...
wlq10
... • Messenger series of lectures, Cornell University, 1964 • Lecture 6: ‘Probability and Uncertainty – the quantum mechanical view of nature’ • The Character of Physical Law - Penguin • see the later series of Douglas Robb memorial lectures (1979) online ...
... • Messenger series of lectures, Cornell University, 1964 • Lecture 6: ‘Probability and Uncertainty – the quantum mechanical view of nature’ • The Character of Physical Law - Penguin • see the later series of Douglas Robb memorial lectures (1979) online ...
Welcome to Physics 112N
... • Newton – Laws of Motion – Law of Gravitation – Kepler’s Laws follow from these general ...
... • Newton – Laws of Motion – Law of Gravitation – Kepler’s Laws follow from these general ...
The Periodic Table OL Page 1 of 2 G. Galvin Name: Periodic Table
... No. of neutrons in an atom = Mass Number (A) – Atomic Number (Z) Defn: Isotopes are atoms of the same element (i.e. they have the same atomic number) which have different mass numbers due to the different number of neutrons in the nucleus. Defn: Relative atomic mass (Ar) is the average of the mass ...
... No. of neutrons in an atom = Mass Number (A) – Atomic Number (Z) Defn: Isotopes are atoms of the same element (i.e. they have the same atomic number) which have different mass numbers due to the different number of neutrons in the nucleus. Defn: Relative atomic mass (Ar) is the average of the mass ...
Chemistry Unit IV – The Electron
... 4. Notice the lines are ______________ for Ultraviolet, thus there is ____________ energy. a. Likewise, IR lines are ______________, so they have the ______________ energy. 5. Consider an electron falling from n = ___ to n = ___ energy level. a. What is its wavelength? b. What color is this light? F ...
... 4. Notice the lines are ______________ for Ultraviolet, thus there is ____________ energy. a. Likewise, IR lines are ______________, so they have the ______________ energy. 5. Consider an electron falling from n = ___ to n = ___ energy level. a. What is its wavelength? b. What color is this light? F ...
Micro_lect13
... Each electron needs a minimum energy to escape the cathode. This is called f If Equant is less than f, the electron can’t escape If Equant is greater than f, the electron escapes & the f quantum energy in excess of f becomes electron KE ...
... Each electron needs a minimum energy to escape the cathode. This is called f If Equant is less than f, the electron can’t escape If Equant is greater than f, the electron escapes & the f quantum energy in excess of f becomes electron KE ...
Atoms in Combination: The Chemical Bond
... Metal loses eNonmetals gain eElectrostatic attraction holds the crystal ...
... Metal loses eNonmetals gain eElectrostatic attraction holds the crystal ...
QUASICLASSICAL AND QUANTUM SYSTEMS OF ANGULAR FOR QUANTUM-MECHANICAL MODELS WITH SYMMETRIES
... for describing certain problems concerning the quantum dynamics of systems of angular momenta, including also the spin systems. The underlying groups are SU(2) and its quotient SO(3, R). The proposed scheme is applied in two different contexts. Firstly, the purely group-algebraic framework is applie ...
... for describing certain problems concerning the quantum dynamics of systems of angular momenta, including also the spin systems. The underlying groups are SU(2) and its quotient SO(3, R). The proposed scheme is applied in two different contexts. Firstly, the purely group-algebraic framework is applie ...
![The Structure of the Atom [Режим совместимости]](http://s1.studyres.com/store/data/001854271_1-ef1245c1f375ab31b64ec8e56383a02e-300x300.png)
The Structure of the Atom [Режим совместимости]
... • ℓ is related to the shape of electron orbitals, and • the number of values of ℓ states how many different orbital types or electron subshells there are in a particular electron shell ℓ, the angular momentum quantum number = 0,1,2...(n – 1) ...
... • ℓ is related to the shape of electron orbitals, and • the number of values of ℓ states how many different orbital types or electron subshells there are in a particular electron shell ℓ, the angular momentum quantum number = 0,1,2...(n – 1) ...
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.