INORG CHEM LEC

• Hydrogen


  Colorless, Odorless and Tasteless
• Hydrogen 


  Electron configuration is 1s1 (similar to the electron configuration of group 1 elements)
• Hydrogen


  Classified as a non-metal
• The elemental form of H is H2
• H2 is small and non-polar so the H atoms can only attract each other through weak London Forces.
• Hydrogen


  No Neutrons
• H2


  Hydrogen
• Diatomic Elements (Have No Fear Of Ice Cold Beer)

  Hydrogen, Nitrogen, Fluorine, Oxygen, Iodine, Chlorine, Bromine
• N2


  Nitrogen
• F2


  Fluorine
• O2


  Oxygen
• I2 Chemical Name


  Iodine
• CL2 Chemical Name


  Chlorine
• Br2 Chemical Name


  Bromine
• Isotopes


  same number of proton but different mass number; therefore different number of neutron
• 3 Hydrogen Isotopes

  Protium, Deuterium, Tritium
• Protium


  has only 1 mass number (most abundant)
• Deuterium


  has 2 mass number
• Tritium


  has 3 mass number
• H is the most abundant element on the universe and accounts for 89% of all atoms.
• Most commercial H2 is obtained as a by product of petroleum refining
• Hydrogen as a fuel source: • Light (Low Density) • Clean burning • Plenty of abundant H in water
• Hydrogen


  • Third most abundant element in earth’s crust in combination with other elements
• Hydrogen


  Forms covalent bonds with both non metals and metalloids
• Hydrogen


  follows duet rule
• Hydrogen


  • Produced by the process of Lindé method.
• Uses of Hydrogen

  • Inflating balloons
  • Welding torches (H burns with oxygen and produces high temperature).
  • Used in Haber Process (Nitrogen Fixation) for the production of Ammonia
• Group 1A: Alkali Metals

  The melting point, boiling point and densities of 1A metals are low and they are generally a soft metal.
• Group 1A: Alkali Metals

  Li, Na, K
• Group 1A Alkali Metals


  Outer shell contains only one s electron
• Group 1A Alkali Metals


  • Very active metals, increases activity as atomic weight increases.
• Group 1A General Properties

  • Never found in nature in free state.
  • Readily reacts with water and forms hydroxides that are strongly basic except LiOH (Lithium Hydroxide)
  • Upon reaction with oxygen, lithium forms the normal oxide (Li2O), sodium forms peroxides (Na2O2) and potassium, rubidium and cesium form superoxides (MO2)
  • Reacts with hydrogen to form hydrides and with HALOGENS, to form halides.
  • All salts of alkali metals are water soluble.
• Group 1A General Rule

  SALTS OF ALKALI METAL ARE MORE SOLUBLE THAN ANY SALTS OF ANY PERIODIC GROUP (with exception to Li).
• Lithium

  • earth stone, "Lithos"
• Lithium

  Lightest of all metals
• Bridge Element

  • element of the 2nd period that has the same properties of the element of the 3rd group of the next group.
• Bridge Element of Li

  Mg (Magnesium)
• Small size of the Li cation:

  • Strong polarizing power
  • Forms bond with highly covalent character
• Li Properties

  • Anode (+) in Battery due to ease of oxidation.
  • Heat exchanger in air conditioner.
  • For Mania, Depressant effect and diuretic.
• Brand Names for Lithium

  1. Eskalith - Li2CO3 (Lithium Carbonate)
  2. Quilonium R- Lithase