Unit III – The Periodic Table
12/5/2016Learning Target: Classify elements according to their location onthe Periodic Table This is a brief review of that information.Identify the following as being an alkalai metal,alkaline earth metal, transition metal, semi-conductor(aka metalloid), halogen, or noble gas: Germanium Tungsten Potassium Radon Strontium Uranium Silicon Beryllium Palladium Iodine Whichof the following are main-groupelements? Magnesium Vanadium Antimony Lead Neptunium Cesium Rutherfordium Boron Indium1
12/5/2016Section 1:Who’s Who?Learning Target: Explain the development of Periodic Law 1817– Dobereiner Grouped elements in TRIADS Three elements with similar properties 1865– Newlands Arranged by increasing atomic MASS. Law of Octaves Similar propertiesover EIGHT elements 1870– Mendeleev Created an 8Column table basedon ATOMIC MASS Elements withsimilar propertieswere in the samecolumn Problems w/ Mendeleev’s table:1.Some elements did not fit the order hedescribed.Ex: Tellurium (Te) and Iodine (I): he put them out oforder in terms of atomic mass, but did this so they were inthe same column as elements with similar properties (hebroke his own rules)2.There were gaps in the table BUT he was able to predict the properties andmasses of the unknown elements veryaccurately.2
12/5/2016 1913– Moseley 1944 Studied X-ray spectra ofelements and noticed theycorrelated with atomic number Arranged elements withincreasing ATOMIC NUMBER PERIODIC–Glenn Seaborg Lastrearrangement ofthe periodic table –created the actinideseriesLAW: Properties of the elements are a(periodic) function of theiratomic number18171865DobereinerNewlandsTriadsLaw ofOctaves187019131944MendeleevMosleySeaborgFirst 8columntablePeriodic LawActinideSeriesSection 2 Atomicproperties are determined byELECTRON CONFIGURATION. Ex. 1s2 2s2 2p6 3s2 3p3 Therefore thetable is designed on thebasis of electron configuration 3
12/5/2016 ValenceElectrons: Electrons that arefound in an atom’s outer most shell Determines chemical properties of anatom These are the electrons that can begained, lost or shared when formingcompounds OCTETRULE 8 electrons in the outer energy level renders anatom UNREACTIVE Unreactive Very Stable So which elements are considered unreactive?A: The Noble Gases Atomsreact with other atoms so all atomsend up with FULL OUTER ENERGYLEVELS (i.e. compounds)1. They may add electrons2. They may lose electrons3. They may share electrons4
12/5/2016 Don’tSection 3forget your color-codedperiodic table It identifies the Groups Periods Main Group ElementsLearning Target: Identify properties of metals,nonmetals and metalloids Italso classifies elements as Metals: Alkali metals Alkaline Earth metals Transition metals Metals–On the LEFT of the stairs– On the RIGHT of the stairs Metalloids – Attached to stairs Nonmetals Lanthanide Series Actinide Series Other Metals Nonmetals: Noble gases Halogens Other nonmetals Metalloids: semiconductorsMETALSNONMETALS1. Typically Solids1. Gasses or BRITTLE solids2. Shiny2. Dull3. Conduct Heat andElectricity3. Insulators4. Tendency when forming 4. Tendency when formingcompounds to losecompounds to GAIN orouter electronsSHARE electronsRULE of THUMB Metals: 3 or fewer outer energy level electronsNonmetals: 5 or more outer energy level electronsMetalloids: Properties of both Metals and Nonmetals aka Semiconductors5
12/5/2016 WhatSection 4is a trend? Apredictable change in aparticular directionLearning Target: Describe element trends on thePeriodic Table (FOCUSON MAIN GROUPELEMENTS)Atomic Radii ½ the distance betweenthe nuclei of identical atomsthat are bonded togetherAtomic Radii increasefrom top to bottom and fromright to left on the periodictableIncreasesIncreases Radius d/2 PeriodicTableIncreases as you move down dueto electron shielding electrons in the inner energylevels are between the nucleusand the outer electrons andtherefore are shielded frombeing pulled away **More energy levels as you godown PT6
12/5/2016 Decreases as you go right due toincreasing charge of the nucleus(**means increases as you go left due todecreasing charge of nucleus) although more electrons are also presentthey are at the same distance from thenucleus b/c they are in the same energylevel Stronger force of attraction, pullingelectrons closer—making radius smaller Gallium Thallium Yttrium Strontium Helium Neon Hafnium VanadiumIons Atomor group of atoms that has apositive or negative charge Positive charge occurs when atom loseselectrons Thisprocess that results in an ionrequires energy—this process is referredto as ionization Ex: Na : Sodium that has lost an electron, andnow has 10 e Negative charge occurs when atom gainselectrons Ex: Cl-: Chlorine that has gained an electron,and now has 18 e-Ionization Energyrequired to remove oneelectron from a neutral atom of anelement This happens when compounds form Ionization energy tends to increasefrom bottom to top and left to rightIncreasesIncreases EnergyPeriodicTable7
12/5/2016 Asyou move across, the nucleusgets larger and holds theelectrons more tightlyTHEREFORE harder to remove RequiresMORE energy (higherionization energy) Asyou move down, the outermost electrons are farther awayfrom the nucleus THEREFOREeasier to remove Iron Cobalt Cesium Rhenium Sulfur Tin Iodine Bismuth RequiresLESS energy (lowerionization energy)8
Learning Target: Identify properties of metals, nonmetals and metalloids Don’t forget your color-coded periodic table It identifies the Groups Periods Main Group Elements It also classifies elements as Metals: Alkali metals Alkaline Earth metals Transition metals Lantha
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Periodic Table and Bonding I. Handout: Periodic Table and Bonding Notes II. Periodic Properties and the Development of the Periodic Table i. Mendeleev's First Periodic table I. The first periodic table was arranged by Dimitri Mendeleev in 1869. i. He was a professor of Chemistry. at the University of St. Petersburg in Russia and was
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History of Periodic Table 1869: Dmitri Mendeleev organized the periodic table based on atomic weights “Father of the Periodic Table” 1913: Henry Moseley rearranged the periodic table based on the positive charges in the nucleus Lead to the periodic law: the states that a periodic pattern appears in
