Section 2 Notes
... describe the motion of particles like electron as waves which supports quantum theory. ...
... describe the motion of particles like electron as waves which supports quantum theory. ...
Quantum Number
... • De Broglie's hypothesis was soon confirmed in experiments that showed electron beams could be diffracted or bent as they passed through a slit much like light could. • The waves produced by an electron confined in its orbit about the nucleus sets up a standing wave of specific wavelength, energy a ...
... • De Broglie's hypothesis was soon confirmed in experiments that showed electron beams could be diffracted or bent as they passed through a slit much like light could. • The waves produced by an electron confined in its orbit about the nucleus sets up a standing wave of specific wavelength, energy a ...
Activity 17 Follow-up
... very reactive. When the sodium reacts with the water it takes the place of one of the hydrogen atoms. This happens because sodium is more reactive than the hydrogen it is replacing. Reactivity is largely due to the atomic radius of an element and the valence. Larger metals lose their outer electrons ...
... very reactive. When the sodium reacts with the water it takes the place of one of the hydrogen atoms. This happens because sodium is more reactive than the hydrogen it is replacing. Reactivity is largely due to the atomic radius of an element and the valence. Larger metals lose their outer electrons ...
What do the quantum numbers l and m determine
... Hydrogen atom is a very simple system which is why it has so many degenerate orbitals. Quantum mechanics of other atoms shows one additional feature. The energy now depends on n and l. For a given n the energy increases with increasing l. 2s < 2p 3s < 3p <3d 4s < 4p < 4d < 4f etc. Each energy level ...
... Hydrogen atom is a very simple system which is why it has so many degenerate orbitals. Quantum mechanics of other atoms shows one additional feature. The energy now depends on n and l. For a given n the energy increases with increasing l. 2s < 2p 3s < 3p <3d 4s < 4p < 4d < 4f etc. Each energy level ...
Chapter 7 Quantum Theory of the Atom
... Light Waves, Photons, and the Bohr Theory To understand the formation of chemical bonds, you need to know something about the electronic structure of atoms. Because light gives us information about this structure, we begin by discussing the nature of light. Then we look at the Bohr theory of the sim ...
... Light Waves, Photons, and the Bohr Theory To understand the formation of chemical bonds, you need to know something about the electronic structure of atoms. Because light gives us information about this structure, we begin by discussing the nature of light. Then we look at the Bohr theory of the sim ...
Quantum Mechanics I. Introduction Just before 1900, the classical
... temperature, all objects emit radiation. C. Classical theory, modeling the atoms as harmonic oscillators, resulted in the “ultraviolet catastrophe”. Max Planck, in order to reproduce the experimental results, had to assume that each oscillator could only have an integral number of units of energy, r ...
... temperature, all objects emit radiation. C. Classical theory, modeling the atoms as harmonic oscillators, resulted in the “ultraviolet catastrophe”. Max Planck, in order to reproduce the experimental results, had to assume that each oscillator could only have an integral number of units of energy, r ...
The Atomic Theory of Matter
... • The rest of the subatomic particles were found when scientists made theories on where the electrons were in an atom. In 1910, a scientist named Rutherford examined the effects of passing alpha rays through a gold foil a few thousand atoms thick. He found that most passed right through the gold foi ...
... • The rest of the subatomic particles were found when scientists made theories on where the electrons were in an atom. In 1910, a scientist named Rutherford examined the effects of passing alpha rays through a gold foil a few thousand atoms thick. He found that most passed right through the gold foi ...
LOYOLA COLLEGE (AUTONOMOUS), CHENNAI – 600 034
... 27. a) Write the Schroedinger equation to be solved for H atom and solve it for its energy using a simple solution, which assumes the wave function to depend only on the distance r and not on θ and φ. b) The wave function of 1s orbital of Li2+ is Ψ1s = (1/√π) (Z/a0)3/2 exp(-Zr/a0), where a0 is the m ...
... 27. a) Write the Schroedinger equation to be solved for H atom and solve it for its energy using a simple solution, which assumes the wave function to depend only on the distance r and not on θ and φ. b) The wave function of 1s orbital of Li2+ is Ψ1s = (1/√π) (Z/a0)3/2 exp(-Zr/a0), where a0 is the m ...
Lecture 14
... En = -R/n2, with E0 = ħ2/2ma02 = 13.6 eV The example we gave in Lecture 13 corresponds to n=2, l=1, m=0. The energy level diagram starts at -13.6 eV, which is the binding energy of the ground state n = 1, and continues with -3.4 eV, which is the binding energy of the first excited state, and so on. ...
... En = -R/n2, with E0 = ħ2/2ma02 = 13.6 eV The example we gave in Lecture 13 corresponds to n=2, l=1, m=0. The energy level diagram starts at -13.6 eV, which is the binding energy of the ground state n = 1, and continues with -3.4 eV, which is the binding energy of the first excited state, and so on. ...
Wave Particle Duality
... Later in the nineteenth century, James Clerk Maxwell discovered that light was actually an electromagnetic wave – a wave of oscillating magnetic and electric fields. This was proven experimentally by Heinrich Hertz. ...
... Later in the nineteenth century, James Clerk Maxwell discovered that light was actually an electromagnetic wave – a wave of oscillating magnetic and electric fields. This was proven experimentally by Heinrich Hertz. ...
Trends in the Periodic Table
... • Radius of an atom always decreases when it loses an electron (becomes a cation +) – A whole energy level may be lost, or – There is less electron-electron repulsion (pushing away) between the electrons in different energy levels • The radius of an atom always increases when it gains an electron ...
... • Radius of an atom always decreases when it loses an electron (becomes a cation +) – A whole energy level may be lost, or – There is less electron-electron repulsion (pushing away) between the electrons in different energy levels • The radius of an atom always increases when it gains an electron ...
Draw atomic models showing the appropriate number of electrons
... 7. Any electron in the outermost occupied shell of an atom 8. Atoms with a positive or negative charge due to loss or gain of electrons ...
... 7. Any electron in the outermost occupied shell of an atom 8. Atoms with a positive or negative charge due to loss or gain of electrons ...
CHEMISTRY MIDTERM REVIEW
... energy level sublevel quantum ionization energy atomic radius electronegativity 28. List all the types of electromagnetic radiation in increasing WAVELENGTH. 29. List the colors of visible light in decreasing ENERGY. 30. Draw the 1s, 2s, 2p, 3s, and 3p orbitals on the same set of axes. 31. What is t ...
... energy level sublevel quantum ionization energy atomic radius electronegativity 28. List all the types of electromagnetic radiation in increasing WAVELENGTH. 29. List the colors of visible light in decreasing ENERGY. 30. Draw the 1s, 2s, 2p, 3s, and 3p orbitals on the same set of axes. 31. What is t ...
Chem 2 AP Ch 7 MC Review
... C) Yes, fluorescent materials emit a broad spectrum of light. D) Yes, after storing enough visible light energy, the fluorescent material can emit ultraviolet light. ...
... C) Yes, fluorescent materials emit a broad spectrum of light. D) Yes, after storing enough visible light energy, the fluorescent material can emit ultraviolet light. ...
Chapter 7
... This model is a very simplified view of the hydrogen atom that cannot possibly be correct but it is amazingly accurate in the determinations of the energy levels of the electron in hydrogen. Efforts to extend this model to other atoms failed…the fully theory of quantum mechanics came along short ...
... This model is a very simplified view of the hydrogen atom that cannot possibly be correct but it is amazingly accurate in the determinations of the energy levels of the electron in hydrogen. Efforts to extend this model to other atoms failed…the fully theory of quantum mechanics came along short ...
Fall Exam 1
... demonstrated the existence of more than one charge. neutrons. B. proved that Thomson’s “plum D. determined the charge on a single pudding” model of the atom’s electron. structure was correct. 19. Nobel prize winner Ernest Rutherford conducted an experiment with gold foil and alpha particles, leading ...
... demonstrated the existence of more than one charge. neutrons. B. proved that Thomson’s “plum D. determined the charge on a single pudding” model of the atom’s electron. structure was correct. 19. Nobel prize winner Ernest Rutherford conducted an experiment with gold foil and alpha particles, leading ...
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.