The end
... b/ One milliwatt of light of wavelength 4,560A is incident on a caesium surface. Calculate the electron current liberated and the minimum stopping voltage necessary to reduce this current to zero. Work function of caesium is 1.93 volts. Assume a quantum efficiency of 0.5 % (that means only 0,5 % of ...
... b/ One milliwatt of light of wavelength 4,560A is incident on a caesium surface. Calculate the electron current liberated and the minimum stopping voltage necessary to reduce this current to zero. Work function of caesium is 1.93 volts. Assume a quantum efficiency of 0.5 % (that means only 0,5 % of ...
Atomic Structure
... Later it was proposed that light behaves as either as waves or particles. This property is also a characteristic of all matter. Niels Bohr Atomic structure was analogues to planetary system. Studied line ...
... Later it was proposed that light behaves as either as waves or particles. This property is also a characteristic of all matter. Niels Bohr Atomic structure was analogues to planetary system. Studied line ...
Writing Electron Configuration
... Quantum numbers define the location of electrons in an atomic orbital. This helps us understand why different atoms exhibit certain properties, such as size and reactivity. Quantum numbers are written like this: (2,1,-1,-½) where (n, /, m/, ms) They are like an “address” ...
... Quantum numbers define the location of electrons in an atomic orbital. This helps us understand why different atoms exhibit certain properties, such as size and reactivity. Quantum numbers are written like this: (2,1,-1,-½) where (n, /, m/, ms) They are like an “address” ...
CHEMISTRY
... become IONS- they have a charge. Ex. a Hydrogen atom that loses it’s electron is called a hydrogen ion, H+, or a proton. ...
... become IONS- they have a charge. Ex. a Hydrogen atom that loses it’s electron is called a hydrogen ion, H+, or a proton. ...
Key Concepts for Exam #2
... If the frequency of incident light is above the threshold frequency, then as the intensity of light increases, the kinetic energy of ejected electrons remains constant and the number of electrons increases. In addition, as the frequency of light increases, the kinetic energy of ejected electrons inc ...
... If the frequency of incident light is above the threshold frequency, then as the intensity of light increases, the kinetic energy of ejected electrons remains constant and the number of electrons increases. In addition, as the frequency of light increases, the kinetic energy of ejected electrons inc ...
Practice Test 2
... 19. In a far galaxy, the average atomic mass of an oxygen atom is 16.5 amu. Based upon the assumption of the existence of only two oxygen isotopes 16O and 18O (with atomic masses corresponding to their mass numbers), the natural abundance of the 18O isotope is A) 15% C) 75% B) 25% D) 85% E) none 20. ...
... 19. In a far galaxy, the average atomic mass of an oxygen atom is 16.5 amu. Based upon the assumption of the existence of only two oxygen isotopes 16O and 18O (with atomic masses corresponding to their mass numbers), the natural abundance of the 18O isotope is A) 15% C) 75% B) 25% D) 85% E) none 20. ...
Document
... • Can be extended to “hydrogen-like” atoms – Those with one electron – Ze2 needs to be substituted for e2 in equations • Z is the atomic number of the element ...
... • Can be extended to “hydrogen-like” atoms – Those with one electron – Ze2 needs to be substituted for e2 in equations • Z is the atomic number of the element ...
Atomic Physics
... 2. Certain orbits are stable and no radiation is emitted while the electron is in these orbits. (Classically, a charge moving in a circle would radiate electromagnetic energy.) 3. If an electron jumps from one orbit to another, the energy difference would appear as an emitted photon. That is, ...
... 2. Certain orbits are stable and no radiation is emitted while the electron is in these orbits. (Classically, a charge moving in a circle would radiate electromagnetic energy.) 3. If an electron jumps from one orbit to another, the energy difference would appear as an emitted photon. That is, ...
CH 28 – Atomic Physics
... 2. Certain orbits are stable and no radiation is emitted while the electron is in these orbits. (Classically, a charge moving in a circle would radiate electromagnetic energy.) 3. If an electron jumps from one orbit to another, the energy difference would appear as an emitted photon. That is, ...
... 2. Certain orbits are stable and no radiation is emitted while the electron is in these orbits. (Classically, a charge moving in a circle would radiate electromagnetic energy.) 3. If an electron jumps from one orbit to another, the energy difference would appear as an emitted photon. That is, ...
Covalent Bonds
... The central atom is often the 1st atom in the formula. c. Carbon is ALWAYS central. d. Hydrogen/halogens are always terminal (on end). ...
... The central atom is often the 1st atom in the formula. c. Carbon is ALWAYS central. d. Hydrogen/halogens are always terminal (on end). ...
H-atom, emission spectra
... Electron loses energy to a photon - gives off light Electron goes to a lower energy level 13.6eV 13.6eV losing energy | E | nf 2 ni 2 ...
... Electron loses energy to a photon - gives off light Electron goes to a lower energy level 13.6eV 13.6eV losing energy | E | nf 2 ni 2 ...
Modeling the Hydrogen Atom - The Supercomputing Challenge
... Our project is modeling a hydrogen atom. Because no one knows the exact shape or properties of an atom, we used the most accepted atomic theories in our model. These two theories include the Quantum Mechanics theory and the planetary theory otherwise known as Bohr’s Atomic Model. The planetary model ...
... Our project is modeling a hydrogen atom. Because no one knows the exact shape or properties of an atom, we used the most accepted atomic theories in our model. These two theories include the Quantum Mechanics theory and the planetary theory otherwise known as Bohr’s Atomic Model. The planetary model ...
study note 1 06
... Use de Broglie's wave equation to explain why large objects do The huge m means a very small wavelength. not seem like waves Through a diffraction experiment. (showing destructive and constructive How can the wave properties of light be shown? interference) (as in fig. 6.16) Give an example showing ...
... Use de Broglie's wave equation to explain why large objects do The huge m means a very small wavelength. not seem like waves Through a diffraction experiment. (showing destructive and constructive How can the wave properties of light be shown? interference) (as in fig. 6.16) Give an example showing ...
Franck-Hertz experiment with Ne-tube Related Topics
... where U is the applied voltage, and A and C the work function voltages of the anode and cathode respectively. As the excitation energy E is determined from the voltage differences at the minima, the work function voltages are of no significance here. According to the classical theory the energy leve ...
... where U is the applied voltage, and A and C the work function voltages of the anode and cathode respectively. As the excitation energy E is determined from the voltage differences at the minima, the work function voltages are of no significance here. According to the classical theory the energy leve ...
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.