CHEMISTRY 113 EXAM 3(A)
... A. reflection of light by metal surface B. ejection of electrons by a metal when struck by light C. acceleration of electrons in vacuum by the electric field D. effect of the electric field on the emission of light 3. The frequency of electromagnetic radiation required to promote an electron from n= ...
... A. reflection of light by metal surface B. ejection of electrons by a metal when struck by light C. acceleration of electrons in vacuum by the electric field D. effect of the electric field on the emission of light 3. The frequency of electromagnetic radiation required to promote an electron from n= ...
Chapter 6
... The Uncertainty Principle •Heisenberg showed that the more precisely the momentum of a particle is known, the less precisely is its position known: •In many cases, our uncertainty of the whereabouts of an electron is greater than the size of the atom itself! ...
... The Uncertainty Principle •Heisenberg showed that the more precisely the momentum of a particle is known, the less precisely is its position known: •In many cases, our uncertainty of the whereabouts of an electron is greater than the size of the atom itself! ...
Chapter 4
... Development of a New Atomic Model • There were some problems with the Rutherford model…It did not answer: – Where the e- were located in the space outside the nucleus – Why the e- did not crash into the nucleus – Why atoms produce spectra (colors) at specific wavelengths when energy is added ...
... Development of a New Atomic Model • There were some problems with the Rutherford model…It did not answer: – Where the e- were located in the space outside the nucleus – Why the e- did not crash into the nucleus – Why atoms produce spectra (colors) at specific wavelengths when energy is added ...
The Wave Nature of Matter - Waterford Public Schools
... • The square of a wave function (2) gives the probability of finding an electron in a particular infinitesimally small volume of space in an atom • Because we are treating electrons as waves (not particles), we cannot pinpoint the specific location of an electron! • Instead, mathematical solutions ...
... • The square of a wave function (2) gives the probability of finding an electron in a particular infinitesimally small volume of space in an atom • Because we are treating electrons as waves (not particles), we cannot pinpoint the specific location of an electron! • Instead, mathematical solutions ...
Electrons in Atoms 5.1 Worksheet
... Niels Bohr proposed that electrons move in specific orbits around the nucleus. In these orbits, each electron has a fixed energy called an energy level. A quantum of energy is the amount of energy needed to move an electron from one energy level to another. The Quantum Mechanical Model The quantum m ...
... Niels Bohr proposed that electrons move in specific orbits around the nucleus. In these orbits, each electron has a fixed energy called an energy level. A quantum of energy is the amount of energy needed to move an electron from one energy level to another. The Quantum Mechanical Model The quantum m ...
Atomic Structure 1. Historical perspective of the model of the atom a
... of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or rearranging atoms. b.) In 1910, Ernest Rutherford passed alpha particles through gold foil which showed t ...
... of the same type of element have the same chemical properties, compounds are formed by two or more different types of atoms, and that a chemical reaction involves either, joining, separating, or rearranging atoms. b.) In 1910, Ernest Rutherford passed alpha particles through gold foil which showed t ...
Electrons as waves
... Electrons as waves • Scientists accepted the fact that light has a dual wave- particle nature. • De Broglie pointed out that in many ways the behavior of the Bohr’s quantized electron orbits was similar to the known behavior of waves. • Electrons should be thought of as having a dual wave-particle n ...
... Electrons as waves • Scientists accepted the fact that light has a dual wave- particle nature. • De Broglie pointed out that in many ways the behavior of the Bohr’s quantized electron orbits was similar to the known behavior of waves. • Electrons should be thought of as having a dual wave-particle n ...
Quantum Numbers (6.5-9)
... atom that are at the same energy level. Note that to have the same energy, the orbitals must be on the same energy level as well as be the same type of orbital (n and l values are equal). A 2s orbital is not degenerate (e.g., the same energy) with a 2p or a 1s orbital. The ml values are entirely dep ...
... atom that are at the same energy level. Note that to have the same energy, the orbitals must be on the same energy level as well as be the same type of orbital (n and l values are equal). A 2s orbital is not degenerate (e.g., the same energy) with a 2p or a 1s orbital. The ml values are entirely dep ...
Quantum Numbers
... atom that are at the same energy level. Note that to have the same energy, the orbitals must be on the same energy level as well as be the same type of orbital (n and l values are equal). A 2s orbital is not degenerate (e.g., the same energy) with a 2p or a 1s orbital. The ml values are entirely dep ...
... atom that are at the same energy level. Note that to have the same energy, the orbitals must be on the same energy level as well as be the same type of orbital (n and l values are equal). A 2s orbital is not degenerate (e.g., the same energy) with a 2p or a 1s orbital. The ml values are entirely dep ...
Quantum Notes
... proposed in 1905 that light has a dual nature (wave-like and particle-like) • Matter can gain or lose energy only in small, specific amounts called quanta •A quantum is the minimum amount of energy that can be gained or lost by an atom ...
... proposed in 1905 that light has a dual nature (wave-like and particle-like) • Matter can gain or lose energy only in small, specific amounts called quanta •A quantum is the minimum amount of energy that can be gained or lost by an atom ...
Energy levels of various orbitals MEMORIZE ! 1s < 2s < 2p < 3s < 3p
... 2. Give the orbital notations for electrons in orbitals with the following set of quantum # (a) n = 2, l = 1, ml = 1 (b) n = 4, l = 3, ml = -2 (c ) n =3, l = 2, ml = -1 Ans 2p 4f 3d ...
... 2. Give the orbital notations for electrons in orbitals with the following set of quantum # (a) n = 2, l = 1, ml = 1 (b) n = 4, l = 3, ml = -2 (c ) n =3, l = 2, ml = -1 Ans 2p 4f 3d ...
Baby-Quiz
... don’t all the photoelectrons have the same kinetic energy when they leave the metal’s surface? 4. What property of the emitted electrons depends on the intensity of incident light?What property of the emitted photoelectrons depends on the frequency of incident light? ...
... don’t all the photoelectrons have the same kinetic energy when they leave the metal’s surface? 4. What property of the emitted electrons depends on the intensity of incident light?What property of the emitted photoelectrons depends on the frequency of incident light? ...
The study of biology can help you better understand
... Write noble gas notation for electrons configuration for the following atoms: d orbital can hold maximum 10 electrons. K ________________________________________________________________ Ca ________________________________________________________________ ...
... Write noble gas notation for electrons configuration for the following atoms: d orbital can hold maximum 10 electrons. K ________________________________________________________________ Ca ________________________________________________________________ ...
The Modern Atomic Model
... • Showed electrons in controlled orbits. (like planets) – often called “Planetary Model”. • Experiments greater than 1 electron systems failed to reproduce this motion. ...
... • Showed electrons in controlled orbits. (like planets) – often called “Planetary Model”. • Experiments greater than 1 electron systems failed to reproduce this motion. ...
Electromagnetic Radiation
... relates to size and energy of the orbital. 2. Angular Momentum QN ( integer l or )= 0 to n 1) : relates to shape of the orbital. 3. Magnetic QN (integer m l or m = + l to l) : relates to orientation of the orbital in space relative to other orbitals. 4. Electron Spin QN : (ms = +1/2, 1/2) : ...
... relates to size and energy of the orbital. 2. Angular Momentum QN ( integer l or )= 0 to n 1) : relates to shape of the orbital. 3. Magnetic QN (integer m l or m = + l to l) : relates to orientation of the orbital in space relative to other orbitals. 4. Electron Spin QN : (ms = +1/2, 1/2) : ...
II. Units of Measurement
... to just how precisely we can know both the position and velocity of a particle at a given time. ...
... to just how precisely we can know both the position and velocity of a particle at a given time. ...
Electrons in Atoms
... When electrons occupy orbitals of the same shape on the same energy level, one e- enters each orbital until all orbitals contain an e- of the same spin direction B. Electron Configuration Notations (1s22s2) and Orbital Notation 1. Electron Configuration is a method of using the quantum mechanical mo ...
... When electrons occupy orbitals of the same shape on the same energy level, one e- enters each orbital until all orbitals contain an e- of the same spin direction B. Electron Configuration Notations (1s22s2) and Orbital Notation 1. Electron Configuration is a method of using the quantum mechanical mo ...
Atomic orbital
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. Orbitals for ℓ > 3 continue alphabetically, omitting j (g, h, i, k, …).Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively.