Test 1 Guide
... 1) Neutrons have almost no mass (in amu) and no charge. 2) The fact that 2 different elements may have atoms with the same atomic mass violates Dalton’s atomic theory. 3) Deuterium differs from hydrogen in the number of protons it has. 4) In the quantum mechanical model of the atom, electrons are co ...
... 1) Neutrons have almost no mass (in amu) and no charge. 2) The fact that 2 different elements may have atoms with the same atomic mass violates Dalton’s atomic theory. 3) Deuterium differs from hydrogen in the number of protons it has. 4) In the quantum mechanical model of the atom, electrons are co ...
Document
... 1/λ = 1.097 x 107 m-1 (1/22-1/n2) E = hc/λ = 2.178 x 10-18 J (1/22-1/n2) Later work showed several series of lines E = 2.178 x 10-18 J (1/n22-1/n12 ) (n2
... 1/λ = 1.097 x 107 m-1 (1/22-1/n2) E = hc/λ = 2.178 x 10-18 J (1/22-1/n2) Later work showed several series of lines E = 2.178 x 10-18 J (1/n22-1/n12 ) (n2
Modern Model of the Atom Student Notes and Assignment
... The ways in which electrons are arranged around the nuclei of atoms are called ELECTRON CONFIGURATIONS. The rules that govern the way the electrons fill the atomic orbitals are: 1. AUFBAU PRINCIPLE - electrons enter orbitals of the lowest energy levels first 2. PAULI EXCLUSION PRINCIPLE - an atomic ...
... The ways in which electrons are arranged around the nuclei of atoms are called ELECTRON CONFIGURATIONS. The rules that govern the way the electrons fill the atomic orbitals are: 1. AUFBAU PRINCIPLE - electrons enter orbitals of the lowest energy levels first 2. PAULI EXCLUSION PRINCIPLE - an atomic ...
CHEMISTRY 113 EXAM 3(A)
... A. reflection of light by metal surface B. ejection of electrons by a metal when struck by light C. acceleration of electrons in vacuum by the electric field D. effect of the electric field on the emission of light 3. The frequency of electromagnetic radiation required to promote an electron from n= ...
... A. reflection of light by metal surface B. ejection of electrons by a metal when struck by light C. acceleration of electrons in vacuum by the electric field D. effect of the electric field on the emission of light 3. The frequency of electromagnetic radiation required to promote an electron from n= ...
7.4 The Wave Nature of Matter * 7.5 Quantum Mechanics and the Atom
... • Since we can not determine the exact location and velocity of an electron at the same time, experimentation has been done over time to identify the most likely places that the electrons exist in an atom. These locations are called orbitals. • Schrödinger's equation can be used derive the energies ...
... • Since we can not determine the exact location and velocity of an electron at the same time, experimentation has been done over time to identify the most likely places that the electrons exist in an atom. These locations are called orbitals. • Schrödinger's equation can be used derive the energies ...
Quantum Numbers Primer The quantum numbers
... Consider the hydrogen atom. When the electron occupies the n = 1 orbital (the lowest value allowed), the atom is at the lowest energy and the radius is the smallest. We call this lowest energy state the ground state. We can promote an electron in the n = 1 energy level to a higher level; such as n = ...
... Consider the hydrogen atom. When the electron occupies the n = 1 orbital (the lowest value allowed), the atom is at the lowest energy and the radius is the smallest. We call this lowest energy state the ground state. We can promote an electron in the n = 1 energy level to a higher level; such as n = ...
Topic 7: Atomic and nuclear physics 7.1 The atom
... 1. Electrons that are accelerating (and here we have centripetal acceleration) are known to radiate light energy. The electrons in Rutherford’s model should, therefore lose energy and spiral into the nucleus in a matter of nanoseconds. Rutherford’s model, then, cannot explain why stable atoms exist. ...
... 1. Electrons that are accelerating (and here we have centripetal acceleration) are known to radiate light energy. The electrons in Rutherford’s model should, therefore lose energy and spiral into the nucleus in a matter of nanoseconds. Rutherford’s model, then, cannot explain why stable atoms exist. ...
Chem 101A Exam 4 Concepts Chapter 7 – Modern Atomic Theory
... Chem 101A Exam 4 Concepts Chapter 7 – Modern Atomic Theory Use formulas that relate energy of photon, frequency, wavelength, speed of light, and the Rydberg Equation Notable scientists and their contributions: Rutherford, Bohr, Planc, de Broglie, Heisenberg, Schrödinger. The four Quantum ...
... Chem 101A Exam 4 Concepts Chapter 7 – Modern Atomic Theory Use formulas that relate energy of photon, frequency, wavelength, speed of light, and the Rydberg Equation Notable scientists and their contributions: Rutherford, Bohr, Planc, de Broglie, Heisenberg, Schrödinger. The four Quantum ...
Lecture 17: Bohr Model of the Atom
... • What is a standing wave? • A standing wave is a motion in which translation of the wave does not occur. • In the guitar string analogy (illustrated), note that standing waves involve nodes in which no motion of the string occurs. • Note also that integer and halfinteger values of the wavelength co ...
... • What is a standing wave? • A standing wave is a motion in which translation of the wave does not occur. • In the guitar string analogy (illustrated), note that standing waves involve nodes in which no motion of the string occurs. • Note also that integer and halfinteger values of the wavelength co ...
Schrödinger`s Wave Mechanical Model
... No intermingling between the two This all changed with the start of the 20th century and the work of Max Planck. Planck – Observed radiations emitted from solid bodies heated to incandescence (glowing). This could not be explained by classical physics, which said that matter could absorb or emit a ...
... No intermingling between the two This all changed with the start of the 20th century and the work of Max Planck. Planck – Observed radiations emitted from solid bodies heated to incandescence (glowing). This could not be explained by classical physics, which said that matter could absorb or emit a ...
Chapt. 5: Quantum Theory of the Hydrogen Atom
... -so, the better we know the position of an object, the worse we know the velocity (p = mv) of the object -not an issue in the macroscopic world, but the limitation is ...
... -so, the better we know the position of an object, the worse we know the velocity (p = mv) of the object -not an issue in the macroscopic world, but the limitation is ...
November 18
... C(speed of light 3x 108 m/s)=(lambda[wavelength in meters])(frequency in Hertz) Energy in Joules = h (plank’s constant 6.6 x 10-34) x frequency Example problem: Given that red light has a wavelength of 700 x 10-9 meters, what is the frequency and how much energy does it have? To find frequency, use ...
... C(speed of light 3x 108 m/s)=(lambda[wavelength in meters])(frequency in Hertz) Energy in Joules = h (plank’s constant 6.6 x 10-34) x frequency Example problem: Given that red light has a wavelength of 700 x 10-9 meters, what is the frequency and how much energy does it have? To find frequency, use ...
CH7 handout is here.
... o Line Spectra and the Rydberg Equation o Bohr Model of the Hydrogen Atom o Energy Levels of the Hydrogen Atom 7.3The Wave-Particle Duality of Matter and Energy o Wave Nature of Electrons and Particle Nature of Photons o Heisenberg's Uncertainty Principle 7.4The Quantum-Mechanical Model of the Atom ...
... o Line Spectra and the Rydberg Equation o Bohr Model of the Hydrogen Atom o Energy Levels of the Hydrogen Atom 7.3The Wave-Particle Duality of Matter and Energy o Wave Nature of Electrons and Particle Nature of Photons o Heisenberg's Uncertainty Principle 7.4The Quantum-Mechanical Model of the Atom ...
Matter and Energy Identify a chemical physical change Identify a
... Heisenberg Uncertainty Principle Hund’s rule Pauli exclusion Principle Ground and excited state Sublevels s p d f ...
... Heisenberg Uncertainty Principle Hund’s rule Pauli exclusion Principle Ground and excited state Sublevels s p d f ...
Which scientist developed the quantum mechanical model of the
... What is the correct number of electrons in the outermost energy level of an oxygen atom? A) B) C) D) ...
... What is the correct number of electrons in the outermost energy level of an oxygen atom? A) B) C) D) ...
3. Represents an atom that has four valence electrons.
... no others)? (I) Only orbits of specific radii, corresponding to certain definite energies, are permitted for electrons in an atom. (II) An electron in a permitted orbit has a specific energy and is an "allowed" energy state. (III) Energy is only emitted or absorbed by an electron as it moves from on ...
... no others)? (I) Only orbits of specific radii, corresponding to certain definite energies, are permitted for electrons in an atom. (II) An electron in a permitted orbit has a specific energy and is an "allowed" energy state. (III) Energy is only emitted or absorbed by an electron as it moves from on ...
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.