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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