Organizing the Elements: The Periodic Table (PT)



5309235-20320000Organizing the Elements: The Periodic Table (PT)Development of the Periodic Tablefrom Steven Hawkings’ Universe: Cosmic Alchemya) As you view the video segment on the periodic table, jot down the answers to the following questions. Short answers only.1) Where and when was Mendeleev born? _______________________________________________________________________________________________2) What sparked Mendeleev interest in chemistry?______________________________________________________________________________________________3) What properties of the elements did Mendeleev list before he began to organize the elements? __________________________________________________________________4) Explain the process Mendeleev used to help design the first periodic table. __________________________________________________________________5) How was Mendeleev able to predict properties of the yet to be discovered elements? __________________________________________________________________6) How is the modern Periodic Table organized? ________________________________________________________________________________________________b) Overview of the Periodic TableDeveloped by Russian scientist Dimitri Mendeleev (1869)Revised based on the work of Henry Mosley (1913) and Glenn Seaborg (1940’s)Revised or Modern Periodic Law: The properties of the elements are periodic function of their atomic number. This means that theElements are arranged by INCREASING atomic number.Predictable & repeating pattern to the elements’ properties (characteristics)Elements in the same horizontal row (PERIOD) have the same number of energy levels (where the electrons are found). The PERIOD Number on the side of the PT is the same as the number of energy levels. Period 1: ______ energy levelPeriod 4: ______ energy levelsElements in the same vertical column (GROUP) have similar chemical properties due to the same number of electrons in outermost energy level. In the electron configuration, the number of electrons in the outermost energy level is the number on the right in the configuration for the ‘tall’ groups (exception: He in group 18)Group 1: _____ electron in the outermost energy levelGroup 2: _____ electrons in the outermost energy levelGroup 14: _____ electrons in the outermost energy levelGroup 17: _____ electrons in the outermost energy level Four Basic types of Elements:1234567891011121314151617181HHe2LiBeBCNOFNe3NaMgAlSiPSClAr4KCaScTiVCrMnFeCoNiCuZnGaGeAsSeBrKr5RbSrYZrNbMoTcRuRhPdAgCdInSnSbTeIXe6CsBaLa-LuHfTaWReOsIrPtAuHgTlPbBiPoAtRn7FrRaAc-LrRfDbSgBhHsMtKey: Each type of element has certain properties associated with it.MetalMetalloidNonmetalNoble gasThe most active metal and nonmetal on the PT are the two F’s in opposite corners! ___&___Special Names of Groups on the Periodic Table: Group 1: __________________________________Group 2: __________________________________ (2 names= group 2)Groups 1& 2 are so active/ reactive (unstable), these elements are always found in compounds and never alone.Groups 3- 11 ________________________________Solutions of compounds containing these elements are usually colorful.CuSO4 (aq) : ___________________________CoCl2 (aq) : ____________________________Group 17: __________________________________ Has elements which are found in all three phases of matter, (s, l & g)Group 18: __________________________________ Very stable (non-reactive, inert) due to having 8 electrons in outermost energy level except for Helium (He), which has 2 electrons.c) Color Coding the PT on your Reference Tables- use your notes and the PTs around the room to help you1) On the left side, copy the following to remind yourself that vertical columns are called GROUPS and horizontal rows are called PERIODS:G P E R I O DOUP2) Using a brown pencil, color lightly the elements, which are liquids.3) Using a yellow pencil, color lightly the elements, which are gases.4) Using an orange pencil, add two stripes to the Noble gases to remind yourself that they are found alone as Monatomic molecules.5) Using a purple pencil, color over lightly the elements’ symbols, which always come in pairs, The “BrINClHOF” or “GEN-INE”. You should be able to still see the symbol!6) Using a green pencil, lightly color the metalloids. Remember Al and Po are metals and NOT metalloids. Metalloids touch one full side along the dark “crack” on the right side of the PT.7) Using a red pencil, lightly color groups 1 & 2 to remind yourself that these elements are so reactive that they are never found alone in nature, only in compounds.8) Using a blue pencil, lightly color groups 3 to 11, the Transition elements/metals, to remind you, that these elements often form colorful compounds and solutions.9) Using an arrow to help, label the groups 1, 2, 17 & 18 with their special names. 10) Use a bracket ( { ) to help label groups 3 & 11, the Transition elements/ metals.11) At the top of the PT, label the left side metals and the right side NONMETALS. 12) Under Groups #1, #2, #13, #14, #15, #16, #17 & #18 draw the electron dot diagram, using “X” to represent the kernel. (Remember elements in the same vertical group have the same number of valence electrons so they have the same electron dot diagram. They will also have similar chemical properties because of the valence electrons)d) Properties of Element TypesElement TypePhysical PropertiesChemical PropertiesMetalSide of PT:__________about 2/3 of all elements- Malleable (aluminum foil)- Ductile (copper wire)- Luster (aluminized glass = a mirror!)- Excellent conductors of heat and electricity (wires + toasters)- Large atomic radius (big atoms)- Phase @ 25oC: ___________except: ________________- Silver in color except for:- Low electronegativity- Lose electrons when forming bonds- Form + charged ions (called CATIONS)- Low ionization energy- Tend to tarnish or rust or form a patina (oxide coating) in the presence of oxygen- Group 1 and 2 metals react violently with waterNonmetalSide of PT:__________about 1/3 of all elements- Brittle (sulfur can be crushed to a powder)- Dull (don’t reflect light well)- Poor conductors of heat and electricity (except for certain forms of carbon)- Small atomic radius (small atoms)- Phase @ 25oC: __________________________________Only Liquid: ______________Gases: - Come in a variety of colors & colorless- High electronegativity- Gain electrons when forming bonds with metals to form ionic bonds- Form – charged ions (called ANIONS)- Share electrons with other nonmetals to form covalent bonds- Form molecules when bonded to other nonmetals- Group 17 nonmetals (halogens) are extremely corrosive- High ionization energyMetalloid- Found along the crack in the PT, except for Al & Po (dog food),which are metals a full side must touch the crack- Sometimes conduct electricity (semiconductors)- Used to make computer microchips- Some have Luster (like metals)- Brittle (like nonmetals)- Photovoltaic (produce electricity from light)- Used to make solar energy panels- Phase @ 25oC: ___________- Gain electrons from metals- Lose electrons to nonmetalsNoble Gas-Group 18- Low boiling points- All gases at room temperature- Poor conductors of heat and electricity- Completely chemically nonreactive - No electronegativity (no bonds form)- Extremely high ionization energyMetallic and Nonmetallic Character1) Metallic Character: metals lose electrons due to low ionization energy. The element with the least ionization energy (Fr) is the most metallic, because it will lose electrons more easily than any other metal. When comparing metals, the lower the ionization energy, the more metallic character the element has. You can find ionization energy values on Reference Table S.Example: Ca has an ionization energy of 590 kJ/mol, and K has an ionization energy of 419 kJ/mol. If you heat both metals up, K will lose its electron first, as it requires less energy. K has more metallic character than Ca.Note: The total quantity of Francium on this planet (Earth) has been estimated to be just enough to fit inside a small pen cap. Being so rare, we will not be using Fr during this course for any other reason than as the most metallic element.2) Nonmetallic Character: nonmetals tend to gain electrons due to high electronegativity. The element with the highest electronegativity (F) is the most nonmetallic, because it will gain electrons more easily than any other nonmetal. When comparing nonmetals, the higher the electronegativity, the more nonmetallic character the element has. You can find electronegativity values on Reference Table S.Example: O has an electronegativity of 3.5 and Cl has an electronegativity of 3.2. Since O has a greater attraction to electrons than Cl does, it is more likely to gain electrons from a metal than Cl is. O has greater nonmetallic character than Cl.e) Common Element Names and Symbols (based on Reference Table S) SymbolNameSignificance/UseSymbolNameSignificance/UseHHydrogenLightest element, flammableCoCobaltMagnetic alloysHeHeliumBalloons, radioactivityNiNickelCoins, alloysLiLithiumBattery technologyCuCopperWires, pipes, alloysCCarbonLife, plastics, energyZnZincGalvanized steel, batteriesNNitrogenLife, atmosphereBrBromineCleaning propertiesOOxygenLife, atmosphere, oxidesKrKryptonHeadlampsFFluorineMost nonmetallic elementAgSilverJewelry, alloysNeNeonAdvertising signsSnTinAlloys, toxic heavy metalNaSodiumExplosive metal, makes saltIIodineDisinfectantMgMagnesiumLightweight metal, flaresXeXenonFlashbulbsAlAluminumStructural lightweight metalBaBariumRadiocontrast for X-raysSiSiliconMicrochip technologyWTungstenLight bulb filamentsPPhosphorousLife, incendiary devicesAuGoldJewelry, conductor, alloysSSulfurMatches, gunpowderHgMercuryAmalgams, thermostatsClChlorineCleaning propertiesPbLeadX-ray blankets, toxicArArgonGas in windowsFrFranciumMost metallic elementKPotassium Nutrition, explosive metalRnRadonCarcinogenic gasCaCalciumBones, minerals (limestone)UUraniumNuclear reactor fuelf) Important Definitions to Know for Periodic Table UnitPERIODIC TABLE: PROPERTIES OF ELEMENTS and TRENDSElectronegativity: _____________________________________________________________________________________________________________- found on Reference Table S- For Metals (left side of PT) it tends to be _______- For Nonmetals (right side of PT) it tends to be ______Ionization Energy: ____________________________________________________________________________________________________________- found on Reference Table S- For Metals (left side of PT) it tends to be _______- For Nonmetals (right side of PT) it tends to be ______Atomic Radii:________________________________________________________________________________________________________________- found on Reference Table S- radii ____________ as you go across the Periodic Table Left Right - radii ____________ as you go down Periodic TableReactivity: As a metal: _____________________________________________________Most reactive Metal = _____________________________As a nonmetal: __________________________________________________Most reactive Nonmetal = __________________________g) Trends in an “atomic shell” instead of a nutshell!TrendDown A Group (top to bottom)Reason for TrendAcross a Period(L R)Reason for TrendAtomic NumberNumber of Valence ElectronsAtomic Radius Metallic Characteristics (Reactivity/Activity as a metal loses electrons)Non-Metallic Characteristics (Reactivity/Activity as a non-metal gains electrons)Electronegativity (EN)Ionization Energy (IE)h) Forming Ions: An ionic bond forms when a metal loses valence electrons to a nonmetal forming a positive ion and the nonmetal, which gained the electrons, forms a negative ion. These oppositely charged ions then attract to each other. By losing or gaining electrons, each ion formed gets 8 valence electrons.Metals: lose valence electrons when forming positive ions called: _____________ # electrons lost = _____________ This is known as oxidation.For lithium (Li) Bohr Model of the neutral atom Bohr Model of the “+ ion” What happens to the size of the metal atom when it forms an + ion? ________This is known as the ionic radius. Ionic radius of a metal ion is _____________ then its neutral atom.(Memory hook- lose weight, get a smaller waist; lose electrons get __________)Nonmetals: gain valence electrons when forming negative ions called: ___________ # electrons gained = ___________ This is known as reduction.For fluorine (F):Bohr Model of the neutral atom Bohr Model of the ion “-ion” What happens to the size of the nonmetal atom when it forms an - ion? ________ This is known as the ionic radius. Ionic radius of a nonmetal ion is ____________ then its neutral atom.(Memory hook- gain weight, get a larger waist; gain electrons get __________)I) PERIODIC TABLE WORKSHEETI. Determine the Principle Energy Level (PEL) and the number of valence electrons for the following elements.(PEL = Period #)ElementPEL# Valence ElectronsLiMgAlGeNSeClKrII. Use the trend for atomic radii to III. Use the trend for electronegativity determine the larger atom of the pair. (EN) to determine which atom of the pair Circle the larger element (You can look has the higher electronegativity. Circleup the radii on Reference Table S also) the element with the higher EN (You1) O or S2) N or O3) Mg or P4) Cl or I5) P or N can look up the EN on Ref. Table S also)1) N or O2) O or S3) P or As4) Mg or Na5) Li or BeIV. Using the periodic table, determine the charge of the ion formed from the element listed and indicate if the radius of the ion is Larger (L) or Smaller (S) than the neutral atom. Remember to use the FIRST charge listed for nonmetals.ELEMENTCHARGESize: L or SELEMENTCHARGESize: L or S1) Mg5) Br2) Na6) O3) S7) Sc4) H8) NPeriodic Table in Review:Which two elements are the only liquids?________and __________Which group, name and number, exists as monatomic molecules of gas? Group #: ____________Name: ______________________3) Which group, name and number, contains elements, which are solids, liquids and gases? Group #: ____________Name: ______________________Which elements exist as diatomic molecules? ___________________________Which elements are gases on the periodic table? ______________________________________________________________Which elements are metalloids and where are they found? _______________________________________________________________________________Which element is the most reactive metal? ______ reactive nonmetal? _______Even though iodine’s mass is less than tellurium, why was iodine (I) placed in group 17, after tellurium (Te)? _________________________________________Why is hydrogen (H) placed on top of Group 1 metals when H is not a metal?_____________________________________________________________Which elements form compounds whose aqueous solutions are colorful?________________________________________________________________Which metal groups are so reactive, they are never found alone, only in compounds?Group #: ___Name: ___________________________________Group #: ____Name: __________________________________12) Metals form __________ charge ions by (losing or gaining) electrons, whose size is ________________ then the neutral atom. Loss of electrons is known as (oxidation or reduction). [circle the correct term in the ( )]13) Nonmetals form __________ charge ions by (losing or gaining) electrons, whose size is ________________ then the neutral atom. Gain of electrons is known as (oxidation or reduction). [circle the correct term in the ( )] ................
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