![Semester 1 Exam Review Part 1](http://s1.studyres.com/store/data/015571451_1-09a7f8a8d81812948fd30f468fd0fecf-300x300.png)
Semester 1 Exam Review Part 1
... atomic number is equal to the number of protons in the nucleus A = Atomic Number These are all equal to each P = Proton Number other E = Electron Number ...
... atomic number is equal to the number of protons in the nucleus A = Atomic Number These are all equal to each P = Proton Number other E = Electron Number ...
Pre-AP Chemistry
... Focus on the following topics for the semester exam, being sure to relate terminology to concepts to calculations, as well as unifying principles between these topics. Questions will be focused on, but not limited to the specific items listed. Topics 1. science and chemistry 2. branches/courses in c ...
... Focus on the following topics for the semester exam, being sure to relate terminology to concepts to calculations, as well as unifying principles between these topics. Questions will be focused on, but not limited to the specific items listed. Topics 1. science and chemistry 2. branches/courses in c ...
Review 2nd KEY
... c. a combination of px and py orbitals. b. a px orbital. d. a combination of an s and a px orbital. ____ 3. For an electron in an atom to change from the ground state to an excited state, a. energy must be released. b. energy must be absorbed. c. radiation must be emitted. d. the electron must make ...
... c. a combination of px and py orbitals. b. a px orbital. d. a combination of an s and a px orbital. ____ 3. For an electron in an atom to change from the ground state to an excited state, a. energy must be released. b. energy must be absorbed. c. radiation must be emitted. d. the electron must make ...
Solutions to the exam itself are now available.
... would be spherical, and if you circled these, you were not penalized as long as you also circled Si and Cl.) (f) The Cr4+ ion in the compound CrO2 is exploited in magnetic audio and video recording tape. The electron configuration of Cr4+ is [Ar] 3d2. The question here is simple: which four electron ...
... would be spherical, and if you circled these, you were not penalized as long as you also circled Si and Cl.) (f) The Cr4+ ion in the compound CrO2 is exploited in magnetic audio and video recording tape. The electron configuration of Cr4+ is [Ar] 3d2. The question here is simple: which four electron ...
Chapter 12 Worksheet
... metal is irradiated with 254-nm light, what is the maximum kinetic energy (kJ/mol) the released electrons can have? 7. Consider the following transitions. Which will emit light with a longer wavelength? a. n = 4 n = 2 or n=3 n=2 b. n = 3 n = 1 or n=1 n=3 c. n = 5 n = 3 or n=3 n=1 8. Calc ...
... metal is irradiated with 254-nm light, what is the maximum kinetic energy (kJ/mol) the released electrons can have? 7. Consider the following transitions. Which will emit light with a longer wavelength? a. n = 4 n = 2 or n=3 n=2 b. n = 3 n = 1 or n=1 n=3 c. n = 5 n = 3 or n=3 n=1 8. Calc ...
Light - UDChemistry
... • Find the frequency of purple light (wavelength 455 nm). • Solution: c = ln, or n = c/l Wavelength must be in meters, since c is in m/s: 455 nm = 4.55x10-7 m n = (3.00x108 m/s)/(4.55x10-7 m) = 6.59x1014s-1 ...
... • Find the frequency of purple light (wavelength 455 nm). • Solution: c = ln, or n = c/l Wavelength must be in meters, since c is in m/s: 455 nm = 4.55x10-7 m n = (3.00x108 m/s)/(4.55x10-7 m) = 6.59x1014s-1 ...
III. Quantum Model of the Atom
... Rutherford Model - Nuclear model 1912-1913 Rutherford gathered physicists, including Neils Bohr to work on WHY atoms don’t collapse (negative eattract positive p+) ...
... Rutherford Model - Nuclear model 1912-1913 Rutherford gathered physicists, including Neils Bohr to work on WHY atoms don’t collapse (negative eattract positive p+) ...
Chapter 3 Atomic Structure
... When electrons are in the lowest energy state, they are said to be in the ground state. When a flame or other source of energy is absorbed by the electrons, they are promoted to a higher energy state (excited state). When an electron in an excited state returns to a lower energy state, it emits a ph ...
... When electrons are in the lowest energy state, they are said to be in the ground state. When a flame or other source of energy is absorbed by the electrons, they are promoted to a higher energy state (excited state). When an electron in an excited state returns to a lower energy state, it emits a ph ...
Physics 107 Exam #3 October 13, 1994 Your name: Multiple Choice
... 3. Molecules of a dilute gas which are identical, distinguishable particles obey statistics. (a) Maxwell-Boltzmann, (b) Bose-Einstein, (c) Fermi-Dirac, (d) Rayleigh-Jeans. 4. We cannot think of the electron as orbiting the nucleus in any conventional sense because (a) the Pauli exclusion principle p ...
... 3. Molecules of a dilute gas which are identical, distinguishable particles obey statistics. (a) Maxwell-Boltzmann, (b) Bose-Einstein, (c) Fermi-Dirac, (d) Rayleigh-Jeans. 4. We cannot think of the electron as orbiting the nucleus in any conventional sense because (a) the Pauli exclusion principle p ...
Honors Midterm Review – 2015-16
... _________ responsible for the uncertainty principle which states that it is impossible to know (with any great degree of certainty) both the location and velocity of an electron) _________ responsible for the planetary model of the atom, where electrons traveled in distinct paths around the nucleus ...
... _________ responsible for the uncertainty principle which states that it is impossible to know (with any great degree of certainty) both the location and velocity of an electron) _________ responsible for the planetary model of the atom, where electrons traveled in distinct paths around the nucleus ...
Lecture 1 (Bohr model of the atom)
... • In 1913 Niels Bohr proposed a pre-QM model to explain the spectra emitted by H atoms • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year yo ...
... • In 1913 Niels Bohr proposed a pre-QM model to explain the spectra emitted by H atoms • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next year yo ...
Unit 4: Atoms and Nuclei
... • In 1913 Niels Bohr proposed a pre-QM model to explain the spectra emitted by H atoms • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next yea ...
... • In 1913 Niels Bohr proposed a pre-QM model to explain the spectra emitted by H atoms • In this theory electrons are considered to be point objects in orbit around the nucleus • It gives a 1st order explanation of the spectral lines, & remains a useful treatment of electron behaviour • Next yea ...
Atomic Physics
... A hydrogen atom emits a photon of wavelength 657.7 nm. From what energy state to what lower energy state did the electron jump? ...
... A hydrogen atom emits a photon of wavelength 657.7 nm. From what energy state to what lower energy state did the electron jump? ...
The principal quantum number (n) cannot be zero. The allowed
... electrons in the atom. The only information that was important was the size of the orbit, which was described by the n quantum number. Schrödinger's model allowed the electron to occupy three-dimensional space. It therefore required three coordinates, or three quantum numbers, to describe the orbita ...
... electrons in the atom. The only information that was important was the size of the orbit, which was described by the n quantum number. Schrödinger's model allowed the electron to occupy three-dimensional space. It therefore required three coordinates, or three quantum numbers, to describe the orbita ...
Ch. 4-2 PowerPoint
... behave as both a particle and a wave. What about electrons? Louis De Broglie stated that electrons could be considered waves confined to a space around an atomic nucleus. ...
... behave as both a particle and a wave. What about electrons? Louis De Broglie stated that electrons could be considered waves confined to a space around an atomic nucleus. ...
quantum number
... number… zip code… the whole business. • These items describe the location of your residence. ...
... number… zip code… the whole business. • These items describe the location of your residence. ...
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.