Quater 3 - Periodic Table- TRENDS

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Periodic Table Basics:

• Ordered by Atomic Number (# of Protons)
• Columns are groups (Tend to have the same valence electrons)
• Rows are periods (Same amount of orbitals)
• Main Groups: (Divided by staircase on the right hand side. In yellow in the picture above)
  • Metals- On the left side of the staircase.
  • Reactive
  • Ductile and Malleable
  • Usually good conductors
  • Usually solid at room temperature
  • Nonmetals- On the right of the staircase.
  • Brittle (Will break easily)
  • Not always solid at room temperature
  • Some of them are diatomic (Exist in pairs of atoms).
  • Do not conduct electricity.
  • Metalloids- Touching the staircase. (Yellow elements above)
  • Can act like either a metal or a nonmetal depending on the conditions.

Other Groups: (Location on picture in parentheses)

• Alkaline: (Dark blue on left)
  • Group 1 (1 valence electron)
  • Very reactive with water
  • Very soft
• Alkaline Earth: (Light purple on left)
  • Group 2 (2 valence electrons)
  • Also reactive with water
  • Also soft
• Transition Metals: (Red in the middle)
  • Groups 3-12 (Random amounts of valence electrons)
  • Traditional metals like Copper
  • Good conductors
  • Hard
• Nonmetals: (Turquoise next to the yellow staircase)
  • Groups 13-16 (3-6 valence electrons)
  • Same characteristics as above for nonmetals
  • Can be named more specifically by the element at the top of the group
• Halogens: (Lime green on the far right)
  • Group 17 (7 valence electrons)
  • Gasses
  • Diatomic
• Noble Gasses: (Dark turquoise on the right end)
  • Group 18 (8 valence electrons)
  • Stable (Non-reactive)
  • Gasses

Periodic Trends:

• Atomic Radius:
  • Radius of an atom. Distance from the nucleus to its farthest orbital
  • Increases from Right to left, and top to bottom on the table.
  • Francinium (Fr) has the largest Atomic Radius.
• Electronegativity:
  • Attraction of an atom to electrons
  • Atoms will even attract its own electrons, pulling its orbitals farther in.
  • Decreseres Atomic Radius
  • Increases from left to right, and bottom to top on the table.
  • Does not affect Group 18
  • Categorized by a number 1-4 (4 being the strongest attraction)
  • Fluorine (F) has the most attraction (4)
• Ionization energy:
  • The amount of energy for an atom to take another atom’s electrons. To become an Ion.
  • Atoms will attract not just it’s own electrons, but other atom’s electrons.
  • Most atoms want 8 valence electrons so that's what they want to pull.
  • Increases from left to right, and bottom to top on the table.
  • Directly related to Electronegativity.
  • Also does not affect group 18.
  • Fluorine(F) is as
  • Elements on the far left just easily give up electrons, rather than taking them.

Next Unit: Unit 4- Bonding