electron structure of the atom chapter 7. 7.1 electromagnetic radiation and energy
TRANSCRIPT
Electromagnetic Radiation
• EM Radiation travels through space as an oscillating waveform.
• EM Radiation travels through a vacuum at a constant speed of 3.00×108 m/s
Mathematical Relationships
υλ = cυ = Frequency of the light (1/s, or Hz)λ = Wavelength of light (nm or m)c = CONSTANT, Speed of light (3.00×108 m/s)
Mathematical Relationships
Ephoton=hυ Ephoton=(hc)/λυ = Frequency of the light (1/s, or Hz)λ = Wavelength of light (nm or m)c = CONSTANT, Speed of light (3.00×108 m/s)h = Planck’s Constant (6.626×10-34 J×s)Ephoton = Energy of a single photon (J)
Example
• Assume we want to determine the frequency of orange light and the energy of a single photon of this light.
• Orange light = 600 nm = 6.00×10-7 m• υλ = c, therefore υ = c/λ• = 5.00×1014 Hz• Ephoton=hυ=(6.626×10-34 J×s)(5.00×1014
Hz)• Ephoton=3.31×10-19 J
PROBLEM
• Calculate the frequency and photon energy for an X-ray of wavelength 1.00 nm.
• X-Ray= 1.00 nm = 1.00×10-9 m• υλ = c, therefore υ = c/λ• = 3.00×1017 Hz• Ephoton=hυ=(6.626×10-34 J×s)(3.00×1017
Hz)• Ephoton=1.99×10-16 J
PROBLEM
• What color is laser with a frequency of 6.0×1014 Hz?
• therefore • = 5.00×10-7 m = 500 nm• 500 nm = Green Light
Bohr Model of the Atom
• Propsed by Niels Bohr• Explains the Emission
Spectrum of Hydrogen• Relies of quantitized
energy levels.• Does not work for
atoms with more than one electron.
Orbitals and Orbits
• Bohr’s model had electrons orbit in tight paths, but this only worked for Hydrogen.
• Schrödinger expanded the model by using 3 dimensional orbitals
Energy Levels and Orbital Shape
• Electrons are still in quantitized energy levels.
• Orbitals of roughly the same size are in the same overarching, or principal, energy level.
• There are four ground state orbital geometries: s, p, d and f.
Naming Orbitals
• Orbitals are named for their principal energy level and their orbital geometry.
• The n=1 principal energy level has only one geometry, s.
• The n=2 principal energy level has two geometries, s and p.
• n=3 is composed of s, p, and d• n=4 is composed of s, p, d and f.
Rules for Filling in Orbitals
• Ground State Atoms have the same number of electrons as protons.
• Aufbau Principle – Start with the lowest energy level.
• Pauli Exclusion Principle – Max of two electrons in each orbital with opposite spins
• Hund’s Rule – Electrons are distributed in orbitals of the same energy as to maximize the number of unpaired electrons.
Electron Configurations
• Orbital diagrams are informative but take a lot of space.
• Electron Configurations are a shorthand for these diagrams.
• Though they convey the same information, they do not show sublevel organization.
Valance Electrons
• Valance Electrons are those electrons in the last filled principal energy level.
• Core Electrons are those below the valance level.
• Valance Electrons for Main Group Elements are those in the highest s and p orbitals.
• Main Elements in the same group have the same number of valance electrons.
Ion Electron Configurations
• Ion charges are as they are due to the role of orbitals.
• Ions are stable at 1+, 2+, or such because that gets the electron configuration to a completed principal energy shell (for main group elements).
• Na (1+) is isoelectronic with Neon (a completed n=2)
Valance Electrons and Chemistry
• Valance electrons are the ones participating in chemical reactions.
• Compounds are stabilized by reaching a filled principal energy level.
• We will return to this next chapter.