Test 1: Frequency, Wavelength, Electronegativity, etc.

• M = x10^6
• k = x10^3
• d = 10^-1
• n = x10^-9
• c = x10^-2
• m = x10^-3
• µ = x10^-6
• The properties of radiation are described by three parameters:

  1. Wavelength
  2. Frequency
  3. Amplitude
• wavelength (λ), or distance between two successive peaks
• frequency (ν) is the number of waves that pass through a point per second.
• amplitude (A) is the maximum displacement from equilibrium position to either side of it.
• Electromagnetic spectrum - all forms of electromagnetic radiation arranged according to wavelength or frequency
• Visible light has a range of wavelengths from about 400 nm to 750 nm
• Infrared radiation has longer wavelength than visible light but shorter wavelength than radio waves
• Ultraviolet light has shorter wavelength than visible light but longer than X-ray
• X-ray has very short wavelength compared with ultraviolet light
• Gamma ray has even smaller wavelength than x-ray
• Radio waves have very long wavelengths compared with other types of EM radiation
• X-ray has short wavelengths compared with visible light
• speed of light = C = 3.00 x 10^8 m/s
• C = λv
• V = c/λ
• E = hc/λ
• h = 6.626 x 10^-23 J/s-1
• Quantized states - discrete energy levels
• Continum states - smooth transition between levels
• work = φ
• KE = hc - φ
• φ (work) is either gained or absorbed
• Rydberg Equation: λ = [R(1/n1^2 - 1/n2^2)]^-1
• R = 1.1 x 10^7 m-1
• KE = hc / λ-φ
• n1 is always smaller than n2
• Paschen (infared wavelengths): n=3
• Balmer (visible wavelengths): n=2
• Luman (ultraviolet wavelengths): n=1
• Ground state energy is closest to the nucleus
• Excited states occur between states due to emission or absorbtion of energy
• Bohr Energy (hydrogen atom): E = k/n^2
• k = Rhc (-2.179 x 10^-18 J)