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PSU CHEM 110 - Periodic Properties of the Elements

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Chapter 7: Periodic Properties of the ElementsChapter 7: Periodic Properties of the ElementsReality Check: Exam 1!Basis for Periodic PropertiesGroups and PeriodsAtomic SizeWhich is the largest element in the periodic table?Effective Nuclear ChargePractice ProblemElectron Configurations of IonsIonic SizeIon Channels: Size Matters!Ionization EnergyPeriodic Trends in First Ionization EnergyPeriodic Trends in First Ionization EnergyExceptions to the TrendTransition MetalsPractice ProblemWhat You Should Know (By the end of Friday’s Class)What You Should Know (By the end of Friday’s Class)What You Should Know (By the end of Friday’s Class)Chapter 7: Periodic Properties of the ElementsCH110 FA11 SAS 1Prepare for Recitation September 15thALEKS Objective 3 due September 13thANGEL Quiz 3, September 15thLecture 7: September 7thLecture 8: September 9thLecture 9: September 12thYou are advised to read ahead for all three lecturesand see the BIG PICTURE FIRST.Read: Ch. 2.5 – 2.8; Ch. 7.1 – 7.6; Ch. 8.1 – 8.4Additional Preparation*: Packet 2: 4,5BLB 6: 70,71c,74,75; Packet 6: 10-14BLB 7: 11,31,41,48acd,53,94; Packet 7: 1-12BLB 8: 22,25; Packet 8: 1,2*ALEKS work is necessary but not sufficient for exam level preparation! Do not neglect the packet!Chapter 7: Periodic Properties of the ElementsCH110 FA11 SAS 2By the end of Today’s Lecture you should know:Screening EffectsPeriodic Properties: atomic and ion sizes Isoelectronic series Electron configurations of ions Ionization energies Electron affinities (well, this is Friday…)How does the periodic table reflect the electronic structure of atoms?How do I know what ions an atom might form?Remember: structure affects function!How does an atoms family help me to predict its chemistry?What does the periodic table have to do with ionic bonding? KEY QUESTIONS: THE BIG PICTUREReality Check: Exam 1!CH110 FA11 SAS 3When and where is Exam 1?What do I bring to Exam 1?PencilsStudent IDCalculatorAbsolutely NO text-programmable calculators or wireless devices (yes, this includes your i-Phone) We will check!Note: We will provide the data sheet and periodic table, exactly as they appear in your course packet.Basis for Periodic PropertiesCH110 FA11 SAS 4• Electron configurations determine:-organization of the periodic table-properties are ‘periodic’and categorize…• Elemental properties … which are determined by:– size (__) and shape (__) of orbitals– atomic number (__________)- Atomic sizes- Ionization energies- Electron affinities- Reactivity• Chemists examine periodic properties experimentally by measuring:Groups and PeriodsCH110 FA11 SAS 5Properties repeat periodically.What electrons control the chemistry of the elements?Why do groups have similar properties? Some groups to remember the names of:Atomic SizeCH110 FA11 SAS 6Observation:Observation:WHY? − as n increases orbital _____ increases− as n increases, orbitals energy becomes:WHY? − number of ________ increases− added valence electrons shield ineffectivelyWhich is the largest element in the periodic table?CH110 FA11 SAS 7Two simple rules to usually be right:1) Look at n, which determines the ______2) For a given n, look at ______________Effective Nuclear ChargeCH110 FA11 SAS 8Case study: 11NaThe more e-the harder it is for the valence e-to “see” the nucleus (due to _________ ).Left to right across a period, Zeff_________What is Zefffelt by valence e-?Zeff=Practice ProblemCH110 FA11 SAS 9In which subshell does an electron experience the greatest effective nuclear charge in a many-electron atom? A. 3f B. 3p C. 3d D. 3s E. 4sElectron Configurations of IonsCH110 FA11 SAS 10How do elements form ions? Observation: Main group atoms tend to form ions with filled _____________ .Do core electrons participate in chemistry of reactions? e−Na Cl1s22s22p63s11s22s22p63s23p5core electrons valence electronsNa+Cl−1s22s22p61s22s22p63s23p6“complete octets”Ionic SizeCH110 FA11 SAS 11cations are _________ than parent atomsNa Na+1.54Å 0.97Åanions are _________ than parent atomsCl Cl−0.99Å 1.81ÅIon Channels: Size Matters!CH110 FA11 SAS 12Voltage gated potassium channels must selectively allow K+ions through the cell membrane, while preventing Na+or Ca2+from passing through.They accomplish this by detecting the difference in size between the ions!Ionization EnergyCH110 FA11 SAS 13_______ electrons are more easily removedbecause electrons further from the nucleus are _____ stable.Definition:M(g) →M+(g) + e-I1First ionization energyM+(g) →M+2(g) +e-I2Second ionization energyEXAMPLE: Mg1st I.E. = 735 kJ/mol2nd I.E. = 1445 kJ/mol3rd I.E. = 7730 kJ/molPeriodic Trends in First Ionization EnergyCH110 FA11 SAS 14Quantitative look at group 1A: I1(kJ/mol)•Li 520 •Na I.E. 496 size•K _______ 419 ________•Rb 403 •Cs 376Periodic Trends in First Ionization EnergyCH110 FA11 SAS 15Ionization going across a period:1st I.E. (kJ/mol)Na Mg Al Si P S Cl Ar490 735 580 780 1060 1005 1225 1550Exceptions to the TrendCH110 FA11 SAS 16It requires energy to remove electrons from atoms. It is much harder (requires more energy) to remove electrons from:1)2)Transition MetalsCH110 FA11 SAS 17• s electrons are part of the valence electrons but are lost _____ during ionization• will lose d electrons ______ valence s e-are gone• transition metal ions can have _______chargesEXAMPLES:Ag [Kr] 5s14d10Ag+Fe [Ar] 4s23d6Fe2+Fe3+Cu [Ar] 4s13d10Cu+Cu2+Practice ProblemCH110 FA11 SAS 18Below are successive ionization energies of an atom. Which atom is it?I1= 578 kJ/molI2= 1820 kJ/molI3= 2750 kJ/molI4= 11,600 kJ/molA) SB) LiC) MgD) NeE) AlWhat You Should Know (By the end of Friday’s Class)CH110 FA11 SAS 19Periodicity of Atomic Size• How does size vary going down a group in the periodic table and why? (look at n and radius)• How does size vary going across the periodic table and why? (look at Zeff and shielding)• What is effective nuclear charge? What affects this? Which atoms/orbitalsexperience it more?• Compare sizes of cations to parent ions.• Compare sizes of anions to parent ions.• Know how the size of isolectronic series are affected by shielding.What You Should Know (By the end of Friday’s Class)CH110 FA11 SAS 20Ionization Energy• What is the definition?• What is the sign of ionization energy?• Why?• Know how IE varies going down a family and across the periodic table.Electron


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PSU CHEM 110 - Periodic Properties of the Elements

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