THE PERIODIC TABLE

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THE PERIODIC TABLE
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THE SCIENTISTS

• Stanislao Cannizzarro (1860)
• Italian
• Founded a method for measuring atomic masses

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2. Dmitri Mendeleev (1869)

• Russian
• Arranged elements in order of increasing atomic
  mass.
• Observed that properties were arranged
  periodically
• Was able to predict the existence of elements
  based on gaps in his table.

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3. Moseley (1911)

•  Found that elements varied by the number of
  protons in the nucleus.
•  Arranged elements based on atomic number.

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PERIODIC LAW

• PERIODIC LAW states that the physical and
  chemical properties of the elements are functions
  of their ATOMIC NUMBER.

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PERIODICITY

• A repeating/ predictable pattern of properties of
  atoms as a function of their position on the
  periodic table.
• Periodicity is a result of the ELECTRON
  CONFIGURATION of atoms and shows that elements
  within the same GROUP/ FAMILY on the periodic
  table tend to have similar PROPERTIES.

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ALKALI METALS

• Group IA
• s1 electron configuration
• Combine vigorously with non-metals
• Extremely reactive
• Not found in nature as free elements
• Produce basic solutions when dropped into water.
• soft

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ALKALINE EARTH METALS

• Group IIA
• s2 electron configuration
• Harder than group I metals
• Not found as free elements, but are commonly
  found in nature in compounds
• Very reactive not as reactive as alkali

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TRANSITION METALS

• D- block
• Good conductors
• Lustrous
• Hard/ dense solids (except Hg)
• Form colored solutions.
• Palladium, platinum and gold are non-reactive.

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P-BLOCK

• Lots of variation in properties
• Includes metals, metalloids, and non-metals.
• HALOGENS
• most reactive non-metals
• p5 electron configuration

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NOBLE GASES

• Least reactive non-metals
• p6 electron configuration
• Full octet

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F-BLOCK

• LANTHANIDE SERIES
• Rare earth elements
• Shiny metals
• ACTINIDE SERIES
• Unstable and radioactive
• Th-Np found in nature
• All others are man made