Atomic Line Spectra

• EM spectrum is CONTINUOUS; Atomic Line Spectra is NOT CONTINUOUS leading to specific colored lines.
• Electric discharge EXCITES gas atoms, transferring energy to the electron; When an electron is RELAXED, drops to a lower energy level leading to LIGHT emission.
• The Atomic Line Spectra is NOT CONTINUOUS leading to specific colored lines.
• The series of colored lines means, the line spectrum IS the atomic spectrum
• The EMISSION of light is at SPECIFIC WAVELENGTHS, meaning that the atomic spectrum is specific to a SPECIFIC ELEMENT.
• The Tungsten (W) filaments are found in OLD lights = SMALL percentages of light are available.
• In the Hydrogen Line Spectrum, Hydrogen has 1 PROTON and 1 ELECTRON, meaning there are several observable lines - visible, UV, and IR regions.
• If Hydrogen has 1 ELECTRON, 


  then it must explain how this ONE subatomic particle has several lines
• The Rydberg Equation calculates the lines of the Hydrogen atom. The formula below is: (n - BOTH positive integers, R∞ = 1.09 x 10^7m-1) $1/λ =$$R∞ (1/n1^2 - 1/n2^2)$