CHEM 1000 Lecture Notes - Lecture 5: Flame Test, Valence Electron

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17 Nov 2017
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Light and Electron Configuration
Light- Electromagnetic Radiation
Gamma, x-rays, ultra-violet, infrared, microwaves, radio
Wavelength increases from left to right; Energy increases from right to left.
Bohr (1913)
Electrons have certain specified amounts of energy
Electrons arrange into different energy levels
Flame test: different elements give different colors to a flame
When light emitted from a solid substance passes through a prism, it produces a
continuous spectrum of colors.
When light from a gaseous substance passes through a prism, it produces a line
spectrum.
Each element has a unique spectrum
Line spectra and Energy Levels
A tiny unit of energy produced or absorbed when a electron makes a transition
from one energy level to another. (QUANTUM)
Excited State- gives the energy level
Energy absorbed- Ionization
Ground state- n=1 (Starting point)
Schrodinger (1913)- Calculated the probability of finding an electron in a given volume
of space
Orbitals- various shaped volumes of space (Electron Cloud)
S orbitals- Spherical P orbitals- peanut shaped
Electron Arrangement: The Quantum Model
Principle Energy Levels (Shells): Roughly correlate to the distance that an
electron is from an atom’s nucleus.
Sublevels (Subshells): Each principle energy level is divided into sublevels.
Orbitals: Regions in space that represent a high probability of locating an
electron. Each sublevel has one or more orbitals.
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