Unit 4 Study Guide - Key - Effingham County Schools
... 6. _Frequency____________ (ν) is defined as the number of waves that pass a given point in a specific time. What is its unit? _waves/second or hertz(Hz)___________ 7. Are frequency and wavelength directly or inversely proportional? _inversely_______ 8. A _quantum______________ is the minimum amount ...
... 6. _Frequency____________ (ν) is defined as the number of waves that pass a given point in a specific time. What is its unit? _waves/second or hertz(Hz)___________ 7. Are frequency and wavelength directly or inversely proportional? _inversely_______ 8. A _quantum______________ is the minimum amount ...
EMR and the Bohr Model of the Atom
... effective nuclear charge & distance of electron from nucleus. • Increasing effective charge or decreasing distance from nucleus increases attraction between electron & nucleus – more difficult to remove an electron so ionization energy increases. (Both happen when move across row) • As we move down ...
... effective nuclear charge & distance of electron from nucleus. • Increasing effective charge or decreasing distance from nucleus increases attraction between electron & nucleus – more difficult to remove an electron so ionization energy increases. (Both happen when move across row) • As we move down ...
+l - My CCSD
... – Most sources produce light that contains many wavelengths at once. – However, light emitted from pure substances may contain only a few specific wavelengths of light called a line spectrum (as opposed to a continuous spectrum). – Atomic emission spectra are inverses of atomic absorption spectra. H ...
... – Most sources produce light that contains many wavelengths at once. – However, light emitted from pure substances may contain only a few specific wavelengths of light called a line spectrum (as opposed to a continuous spectrum). – Atomic emission spectra are inverses of atomic absorption spectra. H ...
Physics of Electronics: 2. The Electronic Structure of Atoms (cont.)
... – Notice that the w.f. depends on 3 integers (or quantum numbers) but the energy only in one of them. I.e. several w.f.’s can have the same value of energy. This is called DEGENERACY. ...
... – Notice that the w.f. depends on 3 integers (or quantum numbers) but the energy only in one of them. I.e. several w.f.’s can have the same value of energy. This is called DEGENERACY. ...
Exam #2
... describes the energy of the electron. specifies the momentum for the electron. gives the probability of finding the electron in a region of space. is proportional to the velocity of the electron. is inversely proportional to the distance between the electron and the nucleus. ...
... describes the energy of the electron. specifies the momentum for the electron. gives the probability of finding the electron in a region of space. is proportional to the velocity of the electron. is inversely proportional to the distance between the electron and the nucleus. ...
give and take File
... Find someone in the class to swap with….You give them an answer and they give one to you. (Use each classmate only once. ) Have them initial your answer after you write it down. ...
... Find someone in the class to swap with….You give them an answer and they give one to you. (Use each classmate only once. ) Have them initial your answer after you write it down. ...
Chapter 7: The Quantum Mechanical Model of the Atom I. The
... 1. Bohr s major idea was that the energy states of the atom were _________, and that the amount of energy in the atom was related to the electron s position in the atom. 2. The electrons travel in orbits that are at a fixed distance from the nucleus. ...
... 1. Bohr s major idea was that the energy states of the atom were _________, and that the amount of energy in the atom was related to the electron s position in the atom. 2. The electrons travel in orbits that are at a fixed distance from the nucleus. ...
InorgCh2.1
... The Proton a) Rutherford and Moseley quickly discovered the charge of the nucleus i. Electron beams aimed at an element caused X-rays to be emitted ii. The square root of the X-ray frequency emitted had a linear relationship with about half of the atomic mass of the element iii. This number was clea ...
... The Proton a) Rutherford and Moseley quickly discovered the charge of the nucleus i. Electron beams aimed at an element caused X-rays to be emitted ii. The square root of the X-ray frequency emitted had a linear relationship with about half of the atomic mass of the element iii. This number was clea ...
Models of the Atom:
... All elements are composed of submicroscopic, indivisible particles called atoms Atoms of the same element are identical. Atoms of different elements are not the ...
... All elements are composed of submicroscopic, indivisible particles called atoms Atoms of the same element are identical. Atoms of different elements are not the ...
IntroQuantumNuclearp..
... like matter and waves simultaneously 1927 experimental evidence: electrons (particles) moving through slits formed diffraction patterns (like waves) deBroglie Wavelength & frequency: ...
... like matter and waves simultaneously 1927 experimental evidence: electrons (particles) moving through slits formed diffraction patterns (like waves) deBroglie Wavelength & frequency: ...
Review for Chapter 3: Atoms, Electrons and Periodic Trends Text
... significant and means that electrons probably do not move in fixed, perfectly predictable paths as Bohr suggested. 4c) Einstein supported Planck’s idea that energy had particle-like properties and was quantized, so energy came in certain amounts. Einstein found that light (a form of energy) is also ...
... significant and means that electrons probably do not move in fixed, perfectly predictable paths as Bohr suggested. 4c) Einstein supported Planck’s idea that energy had particle-like properties and was quantized, so energy came in certain amounts. Einstein found that light (a form of energy) is also ...
Chapter 5
... Electrons occupy the lowest possible energy levels or orbitals The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of four quantum numbers. Hund’s Rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly oc ...
... Electrons occupy the lowest possible energy levels or orbitals The Pauli Exclusion Principle states that no two electrons in the same atom can have the same set of four quantum numbers. Hund’s Rule: Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly oc ...
schoa - Schieck
... a) Using the analogy of a shooting range with a gun, bullet, and paper target, what does each item represent in the experiment? (see N:p. 163-4) b) Using the shooting range analogy, why were the results so startling? 3. How did Rutherford infer that the nucleus was: a) very small (compared to the si ...
... a) Using the analogy of a shooting range with a gun, bullet, and paper target, what does each item represent in the experiment? (see N:p. 163-4) b) Using the shooting range analogy, why were the results so startling? 3. How did Rutherford infer that the nucleus was: a) very small (compared to the si ...
ATOMIC STRUCTURE NOTES n hcZ E ℜ
... Where the radial wavefunction passes through zero is a radial node. Where the angular wavefunction passes thru zero is an angular node or nodal plane. 1s (n=1, l=0, ml=0) decays exponentially with distance from the nucleus and never passes thru zero. An orbital with Quantum Numbers n and l in genera ...
... Where the radial wavefunction passes through zero is a radial node. Where the angular wavefunction passes thru zero is an angular node or nodal plane. 1s (n=1, l=0, ml=0) decays exponentially with distance from the nucleus and never passes thru zero. An orbital with Quantum Numbers n and l in genera ...
Document
... Q. What is the de Broglie wavelength of an electron that has a kinetic energy of 100 eV? After an electron is accelerated in 100 V potential difference, its kinetic energy is 100 eV. eV unit has to be converted into SI unit, Joule. 1 eV = 1.6 x 10-19 J ...
... Q. What is the de Broglie wavelength of an electron that has a kinetic energy of 100 eV? After an electron is accelerated in 100 V potential difference, its kinetic energy is 100 eV. eV unit has to be converted into SI unit, Joule. 1 eV = 1.6 x 10-19 J ...
Midterm Review Sample Content Questions
... 17. Which of the ions in problem 15 are anions? How would you recognize an anion? 18. What is the significance of Rutherford’s gold foil experimentation? 19. What is the significance of the Plum pudding model of the atom? 20. Bohr is known for the “planetary model” of the atom – what does this mean? ...
... 17. Which of the ions in problem 15 are anions? How would you recognize an anion? 18. What is the significance of Rutherford’s gold foil experimentation? 19. What is the significance of the Plum pudding model of the atom? 20. Bohr is known for the “planetary model” of the atom – what does this mean? ...
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.