CH 4 SEC 2: Book Notes
... specific electron with a photon knocks the electron off its course. As a result, there is always a basic uncertainty in trying to locate an electron (or any other particle). The Schrödinger Wave Equation (DO NOT NEED TO KNOW) Atomic Orbitals and Quantum Numbers ~ In the Bohr atomic model, electrons ...
... specific electron with a photon knocks the electron off its course. As a result, there is always a basic uncertainty in trying to locate an electron (or any other particle). The Schrödinger Wave Equation (DO NOT NEED TO KNOW) Atomic Orbitals and Quantum Numbers ~ In the Bohr atomic model, electrons ...
Learning Goals
... 2. Light as a Particle- why believe idea that there are particle and wave like properties to objects, role of probability in this interpretation • Write down the mathematical description of a classical electromagnetic wave, and relate the terms in the expression to the velocity, wavelength, and freq ...
... 2. Light as a Particle- why believe idea that there are particle and wave like properties to objects, role of probability in this interpretation • Write down the mathematical description of a classical electromagnetic wave, and relate the terms in the expression to the velocity, wavelength, and freq ...
Chemistry - Unit 6 What do you need to know?? This chapter is on
... has integral (meaning they must be an integer) values from 0 to (n-1) for each value n instead of being listed as a numerical value, 'l' is referred to by a letter (s = 0, p = 1, d = 2, f = 3) defines the shape of the orbital The third quantum number m1 has integral values between 1 and -1 i ...
... has integral (meaning they must be an integer) values from 0 to (n-1) for each value n instead of being listed as a numerical value, 'l' is referred to by a letter (s = 0, p = 1, d = 2, f = 3) defines the shape of the orbital The third quantum number m1 has integral values between 1 and -1 i ...
5 Electrons in Atoms
... Both of the known values in the problem are expressed with significant figures, so the answer must ...
... Both of the known values in the problem are expressed with significant figures, so the answer must ...
Radiation Equilibrium (in Everything Including Direct Semiconductors)
... But how about hν = Eg/2 or any other energy inside the band gap? After all, photons with these energies can not be created in the semiconductor, while they have a certain density according to Plancks formula. Well, as in the free electron gas model (which does not have band gaps after all) we have m ...
... But how about hν = Eg/2 or any other energy inside the band gap? After all, photons with these energies can not be created in the semiconductor, while they have a certain density according to Plancks formula. Well, as in the free electron gas model (which does not have band gaps after all) we have m ...
![ChemChapter_4[1]Light](http://s1.studyres.com/store/data/001894151_1-323884b777914f52c04d2bb917d4088a-300x300.png)
Light and Energy AP Style
... Only for hydrogen atoms and other monoelectronic species. Why the negative sign? To increase the energy of the electron you make it further to the nucleus. the maximum energy an electron can have is zero, at an infinite distance. ...
... Only for hydrogen atoms and other monoelectronic species. Why the negative sign? To increase the energy of the electron you make it further to the nucleus. the maximum energy an electron can have is zero, at an infinite distance. ...
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends
... 8. DRAW energy level diagrams showing the relative orderings of the orbitals (similar to those in questions 4,6 and 7) and fill them with the correct numbers of electrons to indicate the ground state configurations of the following atoms: a) Nitrogen (N) ...
... 8. DRAW energy level diagrams showing the relative orderings of the orbitals (similar to those in questions 4,6 and 7) and fill them with the correct numbers of electrons to indicate the ground state configurations of the following atoms: a) Nitrogen (N) ...
Quantum Numbers, Orbitals, Electron Configurations, Periodic Trends
... 8. DRAW energy level diagrams showing the relative orderings of the orbitals (similar to those in questions 4,6 and 7) and fill them with the correct numbers of electrons to indicate the ground state configurations of the following atoms: a) Nitrogen (N) ...
... 8. DRAW energy level diagrams showing the relative orderings of the orbitals (similar to those in questions 4,6 and 7) and fill them with the correct numbers of electrons to indicate the ground state configurations of the following atoms: a) Nitrogen (N) ...
Section 11.3 Atomic Orbitals
... Atomic Orbitals •The dots indicate the nodes, or points of zero lateral (sideway) displacement, for a given wave. •There are limitations on the allowed wavelengths of the standing wave. •Each end of the string is fixed, so there is always anode at each end • There must be a whole number of half wave ...
... Atomic Orbitals •The dots indicate the nodes, or points of zero lateral (sideway) displacement, for a given wave. •There are limitations on the allowed wavelengths of the standing wave. •Each end of the string is fixed, so there is always anode at each end • There must be a whole number of half wave ...
Quantum Theory
... •V is the potential energy and is a function of x, y and z. The probability of finding the electron decreases as you move away from the center of the nucleus. ...
... •V is the potential energy and is a function of x, y and z. The probability of finding the electron decreases as you move away from the center of the nucleus. ...
Chapter 4 Arrangement of Electrons in Atoms
... • If light could behave as both a wave and a particle, then could an electron (a particle) also behave as both a particle and a wave ????????????? • He said “_________” because…. – Since electrons could only exist at specific energies, and E can be equated to frequency (E = hν), they have ...
... • If light could behave as both a wave and a particle, then could an electron (a particle) also behave as both a particle and a wave ????????????? • He said “_________” because…. – Since electrons could only exist at specific energies, and E can be equated to frequency (E = hν), they have ...
Atomic Theory and Periodicity Questions
... (a) State the Heisenberg uncertainty principle as it related to the determining the position and momentum of an object. (b) What aspect of the Bohr theory of the atom is considered unsatisfactory as a result of the Heisenberg uncertainty principle? (c) Explain why the uncertainty principle or the wa ...
... (a) State the Heisenberg uncertainty principle as it related to the determining the position and momentum of an object. (b) What aspect of the Bohr theory of the atom is considered unsatisfactory as a result of the Heisenberg uncertainty principle? (c) Explain why the uncertainty principle or the wa ...
CH 6 electrons in atoms
... Another consequence of this wave particle duality is the Heisenberg uncertainty principle. This uncertainty is a fundamental limitation of nature, not a result of the crudeness of measuring devices. This leads to a different picture of the electron in the atom. Bohr’s definite orbits are replaced b ...
... Another consequence of this wave particle duality is the Heisenberg uncertainty principle. This uncertainty is a fundamental limitation of nature, not a result of the crudeness of measuring devices. This leads to a different picture of the electron in the atom. Bohr’s definite orbits are replaced b ...
Chapter 07
... Note that this relation also applies to electromagnetic radiation: mc = h / , or h = mc , and since E = h and = c / , ...
... Note that this relation also applies to electromagnetic radiation: mc = h / , or h = mc , and since E = h and = c / , ...
Chapter7Part3
... (for example: the path of a thrown ball) (for example: the motion of an electron in an atom) the path of the ball is given by - the electron is moving so fast and it has such a its position and its velocity at small mass, that its path cannot be predicted various times we think of the ball as moving ...
... (for example: the path of a thrown ball) (for example: the motion of an electron in an atom) the path of the ball is given by - the electron is moving so fast and it has such a its position and its velocity at small mass, that its path cannot be predicted various times we think of the ball as moving ...
Indiana University Physics P301: Modern Physics Review Problems
... problems are intended to review the material since the last exam. 1. Consider a square well having an infinite wall at x = 0 and a wall of height U0 at x = L. (a) For the case E < U0 , obtain solutions to the Schrodinger equation inside the well (0 < x < L) and in the region beyond (x > L) that sati ...
... problems are intended to review the material since the last exam. 1. Consider a square well having an infinite wall at x = 0 and a wall of height U0 at x = L. (a) For the case E < U0 , obtain solutions to the Schrodinger equation inside the well (0 < x < L) and in the region beyond (x > L) that sati ...
Bohr Model of the Atom
... changing energy states, a photon would be emitted with energy equal to that change Bohr (1913) argued that perhaps electrons in the atom may also behave in this way. Electrons don’t radiate with just any energy, but rather must do so in a quantised fashion. He developed the following theory of the a ...
... changing energy states, a photon would be emitted with energy equal to that change Bohr (1913) argued that perhaps electrons in the atom may also behave in this way. Electrons don’t radiate with just any energy, but rather must do so in a quantised fashion. He developed the following theory of the a ...
atomic physics
... (called as Bohr model or Rutherford-Bohr model). It was a simple model of hydrogen atom, but it solved the problems coming from the classical EM theory. ...
... (called as Bohr model or Rutherford-Bohr model). It was a simple model of hydrogen atom, but it solved the problems coming from the classical EM theory. ...