Periodic Trends. Atomic Size (Radius) As you go down in a group on the periodic table, the atomic size increases. Bigger = More electron Shells.

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Presentation transcript:

Periodic Trends

Atomic Size (Radius) As you go down in a group on the periodic table, the atomic size increases. Bigger = More electron Shells

As you go across the periodic table, the atomic radius decreases. 3 p+ 9p+ 3 e - 9 e - Bigger – Less Attraction Smaller – More Attraction Atomic Radius is found on Table S of Reference Tables Li F 2

Ionization Energy Ionization Energy = the energy needed to remove a valence electron. Metals = giving Non-Metals = greedy

Electronegativity Electronegativity = the desire of an atom for an electron.

Valence Electrons As you go down a group, the valence electrons remain the same.

Valence Electrons Bonding: Group 11 + ionNa 1+ Group 22 + ionMg 2+ Group 14 four covalent bonds (carbon) Group ion w/ metal covalent w/nonmetal Group ion Group 18 no bondingstable octet

Reactivity Reactivity = how fast the element reacts. Metallic  gives electronsNa + ion Nonmetallic  gets electronsF - ion Semimetals  can give or get electrons Noble Gases  don’t react

Noble Gas: Don’t React

Transition Metals Sc  Ti  Inner shells (lower energy level) fill before completing higher outer levels. (d-sublevel) Properties don’t change much as you go across. Make compounds with color. Some have multiple oxidation states Cr, Mn, Ti, V Electrons for bonding come from 2 outer shells.

Transition Metals

Radioactive Elements Elements beyond Bi (#84-114) Also Tc & Pm

Man Made Elements Not found in nature Unstable Beyond Uranium (# Also Tc & Pm