Chem unit 1 study guide

Where does an atom get its size from?
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Periodic table familiesAlkali metals, Alkali Earth metals, Boron, Carbon, Nitrogen, Chalcogen, Halogen, and Nobel gases. The bottom row has Lanthanoids and Actinoides.GroupsVertical columns on the periodic tablePeriodA horizontal row of elements in the periodic tableionization energy/Electronegativity trendMore upper rightAtomic Radii trendbottom left is bigger1st ionization energyThe energy required to remove a valence electron from another atomElectronegativityability of an atom to attract electrons from another atomatomic radiusdetermines size of atomDetermine number of electrons used for bondinghow to write an electron configuration and determine an elementUse the filing order and count the total exponentsBe able to write noble gas configuration and valence electron config.Noble gas config: atomic # - [last Ng element] ex: 34Se = [Ar] (18) 4s2 3d10 4p4 (16) Valence electron config: same as Ng config but w/out noble gasdetermine the number of valence electrons.bring valence electron config and count the exponents of same period as og.Know the significance of a valence electron.outer electrons used for bondingenergy sublevelss=2 p=6 d=10 f=14determine the oxidation state of an element.Natural charge of an elementOxidation state chargesGroup 1: +1 Group 2: +2 Group 3-12: +2 and 1 more Group 13: +3 Group 14: +4 Group 15: -3 Group 16: -2 Group 17: -1 Group 18: 0write a CER for atomic radius trend.1. state claim (which is bigger) 2. locate group for both 3. smaller element has greater nuclear charge bc it pulls more valence electrons 4.This makes it smaller 5. Therefore, bigger electron is larger.Energy ringsEvery period represents the # of them in every element