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Lecture

Main Periodic Table Ideas - Larsen.pdf

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Department
Chemistry
Course
CHE 2C
Professor
Lawrence Marx
Semester
Spring

Description
The 10 Things You Need To Know For Dr Larsens ClassDescriptive Chemistry Courtesy of Rachelle Hamblin superorganized student 51612 1 Group 1Alkali Metals a Name The metals and their oxides react with water to form OH thus creating a basic solution b Atomic Radius INCREASES down the group and DECREASES left to right c Electronegativity DECREASES down the group and INCREASES left to right d Ionization Energy DECREASES down the group and INCREASES left to righte Metallic Character INCREASES down the group and DECREASES left to right think more metallic towards the metals on the left side of the periodic table f Reactions with H All metals react with H to form ionic hydrides where H 2gbehaves like the halogens i 2MH 2MH222g Reactions with O Forms Oxide Ion O Peroxide Ion O or Superoxide Ion 2O 2i Oxides 1 2LiO 2LiO 22ii Peroxides 1 2NaO NaO 2 22iii Superoxides 1 KO KO 2 22 CsOCsO 223 RbORbO 22h Reactions with HO The Alkali Metals are powerful reducing agents meaning 2they really want to be oxidized that reduce HO and release H They form 22gstrong bases in aqueous solutions i 2M2HO2MOHH 22ii Note These metals oxides can also dissolve in water to give a basic solution 1 Ex LiHO2Li2OH 222 Ex 2NaOHO4Na4OHO 2222 3 Ex 4KO2HO4K 4OH3O222i Reactions with N Only Li reacts with N at room temperature i 6LiN2LiN 23j Reactions with Halogens Forms ionic halides i 2MX2MX 2 2 Group 2Alkaline Earth Metalsa Name Alkaline The metals and their oxides react with water to form OH thus creating a basic solution Earth They are more insoluble than their counterparts in group one and do not decompose upon heating
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