Cheat Sheet – Periodic Table .docx



Periodic TableOrganization of elementsPeriods: horizontal rows across the periodic tableGroups/families: vertical columns in the periodic tableElements in the same group have the same number of valence electrons and have other similar properties.Types of ElementsMetalsNonmetalsMetalloids/Semi-metalsDuctile – roll into wiresMalleable – flatten into thin sheetsBrittle – break easilyHave some properties of metals and some of nonmetalsConductive of heat and electricityPoor conductors of heat and electricitySemi-conductors (often used for computers)Shiny lusterLacks lusterDepends on the elementTend to lose electrons and become cationsTend to gain electrons and become anionsCan either gain or lose electrons depending on the environmentLeft of the staircase; make up about 2/3 of the periodic tableRight of the staircase; include S, P, O, N, C, H, Se, and groups 17 and 18Along the staircase:B, Si, Ge, As, Sb, Te (exceptions: Al, Po)Evolution of the Periodic TableFirst Periodic TableArranged by Dmitry Mendeleev in 1839.Elements were arranged by increasing atomic mass and were grouped by properties.Modern Periodic TableElements are arranged by atomic numberPeriodic Law: When elements are arranges in order of increasing atomic number, their chemical and physical properties show a periodic pattern.Periodic Trends and PatternsAtomic RadiusThe distance from the nucleus to the outermost electron. [picometers]More energy levels are added as you move down a group…atoms become larger.The nucleus is more attractive (stronger) as you move across a period…pulls the electrons in closer which makes the atom smaller.First Ionization EnergyThe energy required to remove the outermost electron from an atom [kJ/mol]Smaller atoms hold their electrons tighter which make them harder to remove.Larger atoms have a loose grip on their electrons, making them easier to remove.ElectronegativityThe ability of an atom to attract electrons in a chemical bond. [no units]Noble gases do not have an electronegativity value; they will not bond with anything.Small atoms have strong nuclei, which can attract electrons towards themselves.Large atoms have weaker nuclei, which cannot attract electrons towards themselves.Electron AffinityThe amount of energy released when an atom gains an electron. [kJ/mol]Chlorine has the greatest electron affinity.Ionic RadiusThe radius of a cation or anion. [picometers]Cations (lose electrons) become smaller.Anions (gain electrons) become bigger. Specific Group PropertiesGroup #NameAppearanceValance e-ReactivityPhase(s)1AlkaliVery soft, shiny metals1Most reactive metalsSolids2Alkali EarthSoft, shiny metals2Moderately ReactiveSolids3-12TransitionStrong, shiny metalsVariedSomewhat reactiveSolids17HalogensHard, shiny7Most reactive nonmetalsAll phases18Noble GasesAll are gases8Not reactive (inert)GasesMost Reactive Metal (Francium–Fr)Large atom, low ionization energy, low electronegativityMost Reactive Nonmetal (Fluorine–F)Small atom, high ionization energy, high electronegativity ................
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