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Thursday, October 31, 2013 D-day As you enter, take out your 5.1 & 5.3 reading guides and prepare for a quiz. Review of special groups Important info (hint, hint) • Alkali metals – Group ?? – 1 valence electron – VERY reactive to water and oxygen. • Alkaline Earth metals – Group ?? – Too reactive to occur naturally in nature as pure elements. – NOT as reactive as alkali metals. • Halogens – Only group which has all three states of matter at STP. (what is STP?) – Most reactive nonmetals. – These elements are all brightly colored. • Noble Gases – Have their valence shell filled. – VERY unreactive (inert). • Radioactive Elements- no naturally occurring stable isotope (what is an isotope?). – These elements loose neutrons and protons and emit them as particles. – All manmade elements are radioactive. • Transuranium elements- element with an atomic number above 92 (uranium). • Diatomic elements- two atoms of the same element bonded together. – “BrINClHOF” – Place a dot on your periodic table to indicate these elements are diatomic. Periodic Trends • Jigsaw activity – At the end we will regroup and review the material. Block 3 Groups Group 1 Group 2 Group 3 Alexis Michael R. Allison SkyLynn Bianca Andrea Kayla Tyler Jacob Skylar Amanda Cassie Kollin Group 4 Group 5 Group 6 Adam Laura Christen Nephy Carly Beth Gabbi Shelby Michael H. Ross Aimee Julie Jigsaw groups Group 1 Group 2 Group 3 Alexis Shelby Amanda Michael R. Gabbi Cassie Allison Beth Skylar Group 4 Group 5 Group 6 SkyLynn Carly Kollin Adam Jacob Michael H. Laura Tyler Ross Group 7 Group 8 Christen Kayla Aimee Nephy Andrea Julie Bianca Block 4 Groups Group 1 Group 2 Group 3 Alex Cal Bri YingYing Hope Avery Simran Josh Trevor Brooke Addison Kim Stephen Jigsaw Groups Group 1 Group 2 Alex Avery Kim Trevor Cal Hope Brooke Group 3 Group 4 Bri Josh Addison Ying Ying Simran Stephen Atomic Radius • Half the distance between the nuclei of two atoms of the same element when the elements are joined. • Trend- Size increases from top to bottom within a group and decreases from left to right in a period. • Why? Ionization energy • Amount of energy needed to strip an electron from the valence shell of an atom. • Trend- Ionization energy decreases from top to bottom in a group and increases from left to right in a period. • Why? – Electron Shielding Ionic Radii • As atoms gain and lose electrons, their radius changes accordingly. • Cations- always smaller than the atoms from which they form. – Why? • Anions- always larger than the atoms from which they form? – Why? Electronegativity • Ability of an atom to gain electrons when in a compound. – Based on ionization energy and other factors. • Trend- Decreases from top to bottom of a group and increase from left to right. – Where in the reference tables can you find electronegativity? • Why do we see this trend?