Trends of the Periodic Table

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Presentation transcript:

Trends of the Periodic Table Representative elements (main group) only—so, transition and inner transition metals are not included in the trends Group/family: column of periodic table Period: row of the periodic table

Atomic Radius: (atoms without charge) ½ the distance across atom Decreases left to right (across a period) because of the pull from the nucleus as the outer energy level fills Increase top to bottom (down a group) because of the additional energy level

Atomic Radius…examples What’s bigger? sodium or chlorine? hydrogen or potassium? What’s smaller? potassium or nickel? fluorine or bromine?

Ionization Energy: The energy required to remove the valence electron from an atom Increases left to right (across period) because the electron is closer to the nucleus Decrease going down a group because the electron is further from the nucleus

Ionization Energy…examples Which has a greater ionization energy? sodium or chlorine? hydrogen or potassium? Which has a smaller ionization energy? potassium or nickel? fluorine or bromine?

Electronegativity increases across a period Electronegativity: The ability of an atom to attract electrons in a chemical bond Electronegativity increases across a period Electronegativity decreases down a group H 2.1 Li 1.0 Be 1.5 B 2.0 C 2.5 N 3.0 O 3.5 F 4.0 Na 0.9 Mg 1.2 Al Si 1.8 P S Cl K 0.8 Ca Ga 1.6 Ge As Se 2.4 Br 2.8 Rb Sr In 1.7 Sn Sb 1.9 Te I Cs 0.7 Ba Tl Pb Bi

Electronegativity…examples Which has a greater electronegativity? sodium or chlorine? hydrogen or potassium? Which has a smaller electronegativity? potassium or nickel? fluorine or bromine?