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... ∆E = E higher-energy orbit - E lower-energy orbit = E photon = hν • The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant. λ = h / mν • The quantum mechanical model of the atom assumes that electrons have wave properties. ...
... ∆E = E higher-energy orbit - E lower-energy orbit = E photon = hν • The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant. λ = h / mν • The quantum mechanical model of the atom assumes that electrons have wave properties. ...
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... The photoelectric effect The particle theory or light X-rays Diffraction Photons Electromagnetic ...
... The photoelectric effect The particle theory or light X-rays Diffraction Photons Electromagnetic ...
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... a) Predict three physical properties that would be demonstrated by strontium. b) Compare the chemical reactivity of strontrium and barium. Justify your answer with specific reference to atomic theory. 6. Select the answer to each question from the following key: i) ...
... a) Predict three physical properties that would be demonstrated by strontium. b) Compare the chemical reactivity of strontrium and barium. Justify your answer with specific reference to atomic theory. 6. Select the answer to each question from the following key: i) ...
Gen Chem Ch 5 notes
... ∆E = E higher-energy orbit - E lower-energy orbit = E photon = hν • The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant. λ = h / mν • The quantum mechanical model of the atom assumes that electrons have wave properties. ...
... ∆E = E higher-energy orbit - E lower-energy orbit = E photon = hν • The de Broglie equation relates a particle’s wavelength to its mass, its velocity, and Planck’s constant. λ = h / mν • The quantum mechanical model of the atom assumes that electrons have wave properties. ...
Electro-magnetic radiation (light)
... • 1. Plank: E of light is quantized & depends on frequency • 2. Einstein/photo-electric effect: Light behaves like a particle when it interacts with matter • 3. Emission spectra/Bohr: Potential E. of electrons are quantized in an atom • 4. Debroglie: wave/particle duality of electrons (matter). ...
... • 1. Plank: E of light is quantized & depends on frequency • 2. Einstein/photo-electric effect: Light behaves like a particle when it interacts with matter • 3. Emission spectra/Bohr: Potential E. of electrons are quantized in an atom • 4. Debroglie: wave/particle duality of electrons (matter). ...
Fall Final Review Honors
... atom. Rutherford’s nuclear model-dense, positive nucleus surrounded by negative electrons. Bohr’s planetary model-electrons move in circular orbits in specific energy levels. Schrödinger’s electron cloud model-electrons move within orbitals not in specific orbits. (Chadwick then added neutrons to th ...
... atom. Rutherford’s nuclear model-dense, positive nucleus surrounded by negative electrons. Bohr’s planetary model-electrons move in circular orbits in specific energy levels. Schrödinger’s electron cloud model-electrons move within orbitals not in specific orbits. (Chadwick then added neutrons to th ...
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... Subshell (l), s-p-d-f, gives the shape of region Orbital (m), gives the orientation in space of the shapes Spin (s), clockwise or counterclockwise ...
... Subshell (l), s-p-d-f, gives the shape of region Orbital (m), gives the orientation in space of the shapes Spin (s), clockwise or counterclockwise ...
ZCT 104 Test II solution
... 20. Which of the following statements are correct? I(T) Frank-Hertz experiment shows that atoms are excited to discrete energy levels II(T) Frank-Hertz experimental result is consistent with the results suggested by the line spectra III (T) The predictions of the quantum theory for the behaviour of ...
... 20. Which of the following statements are correct? I(T) Frank-Hertz experiment shows that atoms are excited to discrete energy levels II(T) Frank-Hertz experimental result is consistent with the results suggested by the line spectra III (T) The predictions of the quantum theory for the behaviour of ...
Information in Radio Waves
... Part 2: Analyzing the Bohr model In neutral Hydrogen, electrons can jump from one energy state to another. If in a vacuum, then the only energy inputs or outputs will be from photons of light (EM radiation). Given the following relationships determine the frequency of the emission line from the H1 t ...
... Part 2: Analyzing the Bohr model In neutral Hydrogen, electrons can jump from one energy state to another. If in a vacuum, then the only energy inputs or outputs will be from photons of light (EM radiation). Given the following relationships determine the frequency of the emission line from the H1 t ...
APS Science Curriculum Unit Planner
... Our perception of the modern model of the atom has developed over time and allows us to make predictions about how chemicals will act when combined. ...
... Our perception of the modern model of the atom has developed over time and allows us to make predictions about how chemicals will act when combined. ...
ATOMIC PHYSICS REVISION NOTES:
... The eigenvalues of j 2, l2 and s2 are j (j +1)h2, l(l +1)h2 and s(s+1)h2; (s = 1=2), respectively so that the splitting is proportional to (j (j + 1) ? l(l + 1) ? s(s + 1)) The states of the electrons are denoted as nflgj ; where n is the principle quantum number, flg is a code which indicates th ...
... The eigenvalues of j 2, l2 and s2 are j (j +1)h2, l(l +1)h2 and s(s+1)h2; (s = 1=2), respectively so that the splitting is proportional to (j (j + 1) ? l(l + 1) ? s(s + 1)) The states of the electrons are denoted as nflgj ; where n is the principle quantum number, flg is a code which indicates th ...
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... (a) Calculate the three lowest energy levels for an electron trapped in an infinitely deep square well potential of width = 0.1 nm (about the diameter of a hydrogen atom in its ground state). (b) If a photon were emitted when the electron jumps from the n = 2 state to the n = 1 state, what would ...
... (a) Calculate the three lowest energy levels for an electron trapped in an infinitely deep square well potential of width = 0.1 nm (about the diameter of a hydrogen atom in its ground state). (b) If a photon were emitted when the electron jumps from the n = 2 state to the n = 1 state, what would ...
Chem 2 AP Ch 7 MC Review Key
... 18. Which electronic transition requires the addition of the most energy? [The only one where ni < nf] A) n=1 to n=3 D) n=4 to n=1 B) n=5 to n=2 E) n=5 to n=1 C) n=2 to n=3 19. Electromagnetic radiation behaves like particles when it A) travels through space B) is absorbed by matter C) interacts wit ...
... 18. Which electronic transition requires the addition of the most energy? [The only one where ni < nf] A) n=1 to n=3 D) n=4 to n=1 B) n=5 to n=2 E) n=5 to n=1 C) n=2 to n=3 19. Electromagnetic radiation behaves like particles when it A) travels through space B) is absorbed by matter C) interacts wit ...
Unit 5 Notes - Har
... Schrödinger’s equation: Schrödinger applied the principles of wave mechanics to derive information of about the electron. He used Heisenberg’s concept of the say that the probability of finding the electron was equal to the square of the amplitude of the wave of the electron, ||2. The solution to h ...
... Schrödinger’s equation: Schrödinger applied the principles of wave mechanics to derive information of about the electron. He used Heisenberg’s concept of the say that the probability of finding the electron was equal to the square of the amplitude of the wave of the electron, ||2. The solution to h ...
orbital quantum number
... Note how Table 6.1 is set up. For n=1, the only allowed possibilities are ℓ=mℓ=0. For this case, Beiser lists the three solutions R, , and . For n=2, ℓ can be either 0 or 1. If ℓ=0 then mℓ=0. If ℓ=1 then mℓ=0 and mℓ=1 are allowed. The solutions for mℓ=1 are the same. Beiser tabulates the three ...
... Note how Table 6.1 is set up. For n=1, the only allowed possibilities are ℓ=mℓ=0. For this case, Beiser lists the three solutions R, , and . For n=2, ℓ can be either 0 or 1. If ℓ=0 then mℓ=0. If ℓ=1 then mℓ=0 and mℓ=1 are allowed. The solutions for mℓ=1 are the same. Beiser tabulates the three ...
Light33i
... why atoms emit only certain wavelengths. First of all, what is the size of a typical atom? Let’s take water (although that is a molecule, we know a lot about water: its mass density: 1 gm / 1 cc, it is H2O so it has 18 grams/mole, and we know Avagadro’s ...
... why atoms emit only certain wavelengths. First of all, what is the size of a typical atom? Let’s take water (although that is a molecule, we know a lot about water: its mass density: 1 gm / 1 cc, it is H2O so it has 18 grams/mole, and we know Avagadro’s ...
Physics Week 15(Sem. 2)
... equal to 0 the shape is a basic sphere and for l equal to 1 it is called a dumbbell shape. ...
... equal to 0 the shape is a basic sphere and for l equal to 1 it is called a dumbbell shape. ...
Basic Chemistry - Biology with Radjewski
... • Electronegativity—the attractive force that an atomic nucleus exerts on electrons • It depends on the number of protons and the distance between the nucleus and electrons. ...
... • Electronegativity—the attractive force that an atomic nucleus exerts on electrons • It depends on the number of protons and the distance between the nucleus and electrons. ...
Review-Semester Final (Part I)
... 6. Compare/contrast elements, compounds and mixtures ( smallest unit, how is it broken down?-physical or chemical changes, examples, pure or nonpure?) ...
... 6. Compare/contrast elements, compounds and mixtures ( smallest unit, how is it broken down?-physical or chemical changes, examples, pure or nonpure?) ...
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.