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Electrons in Atoms 13.3 Physics and the Quantum Mechanical Model
13.1 Models of the Atom Atomic orbitals 13.2 Electron Arrangement in Atoms
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Physics in Chemistry Speed of light, c = 3 x 108 m/s c = c =
= wavelength (m) = frequency (Hz) (Hertz = s-1) Also = frequency Electromagnetic spectrum p. 373
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Atomic emission spectra =
Group of wavelengths of energy emitted by electrons falling down to lower energy levels after being excited Unique for each element Ground state vs. Excited state E = h E = energy (J) (Joule) Planck’s constant, h = x Js Photoelectric effect = Metals eject electrons when light shines on them Proves the particle concept of the dual wave-particle behavior of light
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Example: A popular radio station broadcasts with a frequency of 94
Example: A popular radio station broadcasts with a frequency of 94.7 MHz. What is the wavelength of the broadcast?
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deBroglie’s equation =
Calculate the wavelength of a moving particle, like an electron = h / mv = wavelength (m) h = Planck’s constant (Js) m = mass (g) v = velocity (m/s) Heisenberg Uncertainty Principle = You cannot know both the velocity (speed) and position (location) of a particle at the same time
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Atomic Orbitals Describe the location of electrons
Orbital = region of space Principle quantum # (n) = energy level n = 1, 2, 3, 4, 5 … with increasing distance from the nucleus Energy Sublevels = s, p, d, f (see p ) s sphere 1 orbital max 2 electrons p dumbbell 3 (x, y, z) 6 d clover leaf f Max 2 electrons in each orbital
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Order of filling orbitals (p.135)
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Pauli Exclusion Principle: Hund’s Rule:
Aufbau Principle: Electrons enter orbitals of lowest energy first Pauli Exclusion Principle: Atomic orbital can have at most 2 electrons Hund’s Rule: For orbitals of equal energy, 1 electron enters each orbital until all orbitals have 1 electron with parallel spins
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Electron Configuration and Orbital Notation
Si Ni Ar B Cr and Cu Al, Ge, Sb, Po
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Noble gas shorthand notation
Valence electrons and electron dot structure Link s, p, d, f blocks to periodic table
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