Periodic Table of Elements Objectives: Describe the arrangement of the PTE Explain characteristics of families and trends on the table
1869 Dmirtri Mendeleev Organized by atomic mass Predicted undiscovered elements
1913 Organized by atomic number Fixed Mendeleev’s problems Henry Moseley 1913 Organized by atomic number Fixed Mendeleev’s problems
Metals, nonmetals and metalloids Organization Metals, nonmetals and metalloids
True Configuration
Groups (families)—columns Periods--rows Groups and Periods Groups (families)—columns Periods--rows
Periodic Law Properties of elements repeat periodically when the elements are arranged by increasing atomic number
First Ionization Energy Terms Valence Electrons— Electrons in the outermost energy level Atomic radius Distance from nucleus to outer boundary First Ionization Energy Energy required to remove an e- from a neutral atom
Increases LEFT and DOWN Periodic Trends Atomic Radius Increases LEFT and DOWN
First Ionization energy: Trends First Ionization energy: Increases RIGHT and UP
Electronegativity Tendency of an atom to attract e- Affected by both atomic number and atomic radius (distance valence e- are from nucleus)
Group #= number of valence e- (except He) More Trends Group #= number of valence e- (except He) Families have similar reactivity since they have the same number of valence e- Period Number= # of energy levels
Dots represent valence e- Lewis Dot Structures Dots represent valence e-
Fill in your Table Group Number Period Number Color Metals one color, nonmetals anther color and metalloids another color Make a key at the top of your Periodic Table
On Your Own Atomic Radius: Which is bigger? H or Li, Ca of Mn, Pt or Ag, Ne or Ar How many valence e-? Mg Al Si Ar Cl C B Rb How many energy levels? Rb K Na Mg Bi P S F Which has a lower Ionization energy? Ca or K, Al or P, Ga of Be, Cs or Se Which has a higher electronegativity? For Ne, Ar or N, Be or Mg, As, or S Lewis Dot Structure: Draw it! For the ones where you identified the number of Valence e- up above.