Structure 1.3

• ROYGBIV: Infored, Red, Orange, Green, Blue, Indigo, Violet, Ultra Violent
• Ultraviolet (UV) light has a shorter wavelength than visible light but longer than X-rays.
• X-ray has a very short wavelength compared to UV light.
• Energy Emitted: The energy absorbed in the same
• Infrared radiation has lower frequencies and less energy than visible light.
• Chromium electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵
• Limit of convergence corresponds to the ionization energy: The minimum amount of energy required to remove 1 mole of electrons from the ground state of 1 mole of gaseous atoms.
• Copper Electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d10
• The first ionisation energy of an element is always greater than its second ionisation energy because it requires more energy to remove another electron from a positively charged atom.
• Left to right on the perodic table: Increase number of protons

  Increase nuclear pull

  INcrease energy required to remove 1st electron
• Steps to find wavelength: Converting first ionization energy from kilojoules to joules

  divide by avogadro's number = variable 1

  variable 1/planks constant = variable 2

  speed of light/ variable 2
• First Ionization energy formula: x (g) —> x+ (g) + e-
• High first ionization: harder to remove the electron
• Absorption line spectrum: occurs when the light is absorbed by the atoms in the gas.
• relative percentage abundance formula: isotope 1(x) + isotope 2(100-x) = isotope 1 relative mass x 100

  solve for x = isotope 1 percentage

  isotope 1 percentage - 100 = isotope 2 percentage
• Emission light: Occurs when an electron is emitted from an atom or ion.