Electron Configuration Notes
... • electrons move around nucleus in orbits similar to how planets orbit the sun • energy levels for electrons are quantized Major developments that put Bohr’s Model into question: Einstein: Light energy exhibits properties of matter. Matter and energy are different forms of the same thing. De Broglie ...
... • electrons move around nucleus in orbits similar to how planets orbit the sun • energy levels for electrons are quantized Major developments that put Bohr’s Model into question: Einstein: Light energy exhibits properties of matter. Matter and energy are different forms of the same thing. De Broglie ...
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Chem 150 Problem Set Introductory Quantum Chemistry 1
... a) According to the Bohr model an electron in the ground state of a hydrogen atom orbits the nucleus at a specific radius of 0.53 x 10-10 m. In the quantum mechanical description of the hydrogen atom, the most probable distance of the electron from the nucleus is 0.53 x 10 -10 m. Why are these two s ...
... a) According to the Bohr model an electron in the ground state of a hydrogen atom orbits the nucleus at a specific radius of 0.53 x 10-10 m. In the quantum mechanical description of the hydrogen atom, the most probable distance of the electron from the nucleus is 0.53 x 10 -10 m. Why are these two s ...
Midterm review
... Boundary conditions: Ends tied down standing wave More nodes higher energy 4. 2D waves for a square or round drum have degenerate sets (i.e. two or more waves have the same energy. They are the same wave only rotate in space. Schrödinger Equations: 3D wavefunctions (r) or Orbitals ...
... Boundary conditions: Ends tied down standing wave More nodes higher energy 4. 2D waves for a square or round drum have degenerate sets (i.e. two or more waves have the same energy. They are the same wave only rotate in space. Schrödinger Equations: 3D wavefunctions (r) or Orbitals ...
Matter and Energy Identify a chemical physical change Identify a
... b. Is larger with same charge c. Is smaller with opposite charge d. Is larger with opposite charge ...
... b. Is larger with same charge c. Is smaller with opposite charge d. Is larger with opposite charge ...
Orbitals and Quantum Numbers
... the properties of atomic orbitals and the properties of electrons in orbitals) 1) The principle quantum number (n) indicates the main energy level occupied by the electron ...
... the properties of atomic orbitals and the properties of electrons in orbitals) 1) The principle quantum number (n) indicates the main energy level occupied by the electron ...
1 pt
... What is the name of the term given to the minimum quantity of energy that can be lost or gained by an atom? ...
... What is the name of the term given to the minimum quantity of energy that can be lost or gained by an atom? ...
Quantum Numbers and Atomic Orbitals
... • We are not parOcularly interested in electron configuraOons (will not be on exam) • BUT – core and valence electrons are ...
... • We are not parOcularly interested in electron configuraOons (will not be on exam) • BUT – core and valence electrons are ...
the principle quantum number
... • Map to determine location of the electrons….. • (Methods for denoting earrangement for an atom: orbital notation) ...
... • Map to determine location of the electrons….. • (Methods for denoting earrangement for an atom: orbital notation) ...
Document
... Exact position and exact momentum cannot both be known simultaneously De Broglie's Hypothesis λ = h/mv Particles have wave lengths; proof came from diffraction of electron beam Schroedinger's Wave Equation ∂2Ψ/∂x2 + ∂2Ψ/∂y2 + ∂2Ψ/∂z2 + 8π2m/h2(E-V)Ψ = 0 ...
... Exact position and exact momentum cannot both be known simultaneously De Broglie's Hypothesis λ = h/mv Particles have wave lengths; proof came from diffraction of electron beam Schroedinger's Wave Equation ∂2Ψ/∂x2 + ∂2Ψ/∂y2 + ∂2Ψ/∂z2 + 8π2m/h2(E-V)Ψ = 0 ...
Electron Configurations
... how electrons will be arranged in the atom is Hund’s rule, which states that the most stable arrangement of electrons is that which allows the maximum number of unpaired electrons. This arrangement minimizes electron-electron repulsions. Here’s an analogy. In large families with several children, it ...
... how electrons will be arranged in the atom is Hund’s rule, which states that the most stable arrangement of electrons is that which allows the maximum number of unpaired electrons. This arrangement minimizes electron-electron repulsions. Here’s an analogy. In large families with several children, it ...
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... Impacting electrons cause electrons in core (lowest energy) states to be knocked out. For high Z atoms, these are very tightly bound states (K shells), so require high energies (many keV) to eject them Spectrum shows sharp peaks, due to emission of photons by outer electrons falling to vacated core ...
... Impacting electrons cause electrons in core (lowest energy) states to be knocked out. For high Z atoms, these are very tightly bound states (K shells), so require high energies (many keV) to eject them Spectrum shows sharp peaks, due to emission of photons by outer electrons falling to vacated core ...
Chapter 2
... 3. An x-ray has a wavelength of 0.13 nm. Calculate the energy (in J) of one photon of this radiation. ...
... 3. An x-ray has a wavelength of 0.13 nm. Calculate the energy (in J) of one photon of this radiation. ...
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.