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Slide 2 / 163ChemistryThe Periodic Table2015-11-16www.njctl.org

Slide 3 / 163Table of Contents: The Periodic TableClick on the topic to go to that section· Periodic Table· Periodic Table & Electron Configurations· Effective Nuclear Charge· Periodic Trends: Atomic Radius· Periodic Trends: Ionization Energy· Periodic Trends: Electronegativity· Periodic Trends: Metallic Character

Slide 4 / 163The Periodic TableReturn to Tableof Contents

Slide 5 / 163Identifying Properties of AtomsNow that we know where(or approximately where)to find the parts of atoms,we can start tounderstand how thesefactors all come togetherto affect how we view theelements.

Slide 6 / 163Identifying Properties of AtomsWe can look at them as individual yetinteracting chemicals, and we areable to group them based, not only onthe properties they present when inisolation, but also the properties theyreveal when exposed to otherelements or compounds.

Slide 7 / 163"Periodic" Table of ElementsThe Periodic Table of Elementscontains physical and chemicalinformation about every elementthat matter can be made of in theUniverse.The Pillars of Creation, part of theEagle Nebula shown to the right,*is a cloud of interstellar gases7,000 light years from Earth madeup of the same gaseous elementsfound on the Periodic Table.Courtesy of Hubble Telescope*NASA recently captured this image; however, the Pillars of Creation no longer exists.The Eagle Nebula was destroyed by a Supernova around 6000 years ago, but fromour viewpoint, it will be visible for another 1000 years.

Slide 8 / 163"Periodic" Table of ElementsWhy is one of the most useful tools ever created by humanscalled the "Periodic Table"?When scientists were organizing the known elements, theynoticed that certain patterns of chemical and physical behaviorkept repeating themselves.These elementsare all shinymetals and reactviolently in water.These elementsare all verystable gases.

Slide 9 / 163"Periodic" Table of ElementsThese patterns were so predictable that Dmitri Mendeleev, thescientist who formulated the Periodic Law, was actually able topredict the existence of elements #31 and #32 and theirapproximate masses before they were discovered based on theexisting patterns of known elements.Gallium, 31GaGermanium, 32GeMendeleev's work preceded the discovery of subatomic particles.

Slide 10 / 163"Periodic" Table of Elements

Slide 11 / 163History of the Periodic TableMendeleev argued that elementalproperties are periodic functions of theiratomic weights.We now know that element properties areperiodic functions of their atomic number.Atoms are listed on the periodic table inrows, based on number of protons.

Slide 12 / 163Periodic TableThe periodic table is made of rows and columns:Rows in the periodic table are called Periods.Columns in the periodic table are called Groups.Groups are sometimes referred to as Families, but "groups" ismore traditional.

Slide 13 / 163groups1periods234567*7**6***

Slide 14 / 1631 The elements in the Periodic Table are arranged from leftto right in order of increasing .A massB number of neutronsC number of protonsD number of protons and electrons

Slide 15 / 1632 What is the atomic number for the element inperiod 3, group 16?

Slide 16 / 1633 What is the atomic number for the elementin period 5, group 3?

Slide 17 / 163Groups of ElementsEnjoy Tom Lehrer'sFamous Element Song!

Slide 18 / 163Metals, Nonmetals, and MetalloidsThe periodic table can be divided into metals (blue) andnonmetals (yellow) . A few elements retain some oftheproperties of metals and nonmetals, they are called metalloids(pink).metals me Sita Ge AslloSb TeidsBnonmetals?

Slide 19 / 163Special GroupsNoble GasesTransition MetalsHalogensAlkaline Earth MetalsAlkali MetalsSome groups have distinctive properties and are given special names.

Slide 20 / 163Alkali MetalsGroup 1 Alkali Metals(very reactive metals)

Slide 21 / 163Alkaline Earth MetalsGroup 2 Alkaline Earth Metals(reactive metals)

Slide 22 / 163Groups 3 - 12 Transition Metals(low reactivity, typical metals)Transition Metals

Slide 23 / 163Group 16 Oxygen Family(elements of fire)

Slide 24 / 163HalogensGroup 17 Halogens(highly reactive, nonmetals)

Slide 25 / 163Noble GasesGroup 18 Noble Gases (nearly inert)

Slide 26 / 163Noble GasesTransition MetalsHalogensAlkaline Earth MetalsAlkali MetalsMajor Groups of the Periodic Table

Slide 27 / 1634 To which group on the periodic table does Iodinebelong?ANoble GasesBAlkali MetalsCTransition MetalsDHalogens

Slide 28 / 1635 To which group on the periodic table does Neonbelong?AAlkali MetalsBTransition MetalsCNoble GasesDAlkaline Earth Metals

Slide 29 / 1636 To which group on the periodic table doesFluorine belong?AAlkali MetalsBTransition MetalsCNoble GasesDHalogens

Slide 30 / 1637 To which group on the periodic table does Ironbelong?AAlkali MetalsBTransition MetalsCHalogensDAlkaline Earth Metals

Slide 31 / 1638 To which group on the periodic table doesBeryllium belong?AAlkali MetalsBTransition MetalsCHalogensDAlkaline Earth Metals

Slide 32 / 1639 Two elements are studied. One with atomicnumber X and one with atomic number X 1. It isknown that element X is a Noble Gas. Whichgroup on the periodic table is X 1 in?ATransition MetalsBHalogensCAlkali MetalsDThere is no way to tell

Slide 33 / 163Periodic Table & ElectronConfigurationsReturn to Tableof Contents

Slide 34 / 163. . . we now know that elements in the same groups, with thesame chemical propertieshave very similar electron configurations.Noble GasesTransition MetalsHalogensHow an elementreacts depends onhow its electrons arearranged. . .Alkaline Earth MetalsThe elements arearranged by groups withsimilar reactivity.Alkali MetalsPeriodic Table & Electron Configuration

Slide 35 / 163Periodic Table & Electron Configuration1A 2A1 2}3B 4B 5B 6B 7B3 4 5 6 7 88B3A 4A 5A 6A 7A13 14 15 16 178A181B 2B9 10 11 12There are two methods for labeling the groups, the older methodshown in black on the top and the newer method shown in blue onthe bottom.

Slide 36 / 163Periodic Table & Electron ConfigurationClick here to view an Interactive Periodic Tablethat shows orbitals for each ElementClick here for an electron orbital game.

Slide 37 / 163Group NamesGroup NameGroup #ElectronConfigurationAlkali Metals1s1 endingVery reactiveAlkaline EarthMetals2s2 endingReactive3-12 (d block)ns2, (n-1)dendingInner TransitionMetalsf blockns2, (n-2)fendingHalogens17s2p5 endingHighly reactiveNoble Gases18s2p6 ewhatreactive, typicalmetalsSomewhatreactive,radioactive

Slide 38 / 16310 The highlighted elements below are in the .A s blockB d blockC p blockD f block

Slide 39 / 16311 The highlighted elements below are in the .A s blockB d blockC p blockD f block

Slide 40 / 16312 The highlighted elements below are in the .A s blockB d blockC p blockD f block

Slide 41 / 16313 Elements in each group on the Periodic Table havesimilar .A massB number of neutronsC number of protons and electronsD electron configurations

Slide 42 / 16314 The electron configuration ending ns2p6 belongs in whichgroup of the periodic table?A Alkali MetalsB Alkaline Earth MetalsC HalogensD Noble Gases

Slide 43 / 16315 An unknown element has an electron configurationending in s2. It is most likely in which group?AAlkaline Earth MetalsBHalogensCAlkali MetalsDTransition Metals

Slide 44 / 163Periodic Table with f block in PlaceHere is the Periodic Table with the f block in sequence.Why isn't this the more commonly used version of the d2p3p4p5p6p7p

Slide 45 / 163Shorthand ConfigurationsNoble Gas elements are used to write shortened electronconfigurations.To write a Shorthand Configuration for an element:(1) Write the Symbol of the Noble Gas element fromthe row before it in brackets [ ].(2) Add the remaining electrons by starting at the sorbital of the row that the element is in until theconfiguration is complete.

Slide 46 / 163Shorthand ConfigurationsExample: Sodium (Na)Electron Configuration:1s22s22p63s1Neon's electron configurationShorthand Configuration:[Ne] 3s1

Slide 47 / 163Fill in Shorthand ConfigurationsElementShorthand ConfigurationSlide for Answers

Slide 48 / 16316 What would be the expected "shorthand" electronconfiguration for Sulfur (S)?A [He]3s23p4B [Ar]3s24p4C [Ne]3s23p3D [Ne]3s23p4

Slide 49 / 16317 What would be the expected "shorthand" electronconfiguration for vanadium (V) ?A [He]4s23d1B [Ar]4s23d104p1C [Ar]4s23d3D [Kr]4s23d1

Slide 50 / 16318 Which of the following represents an electronconfiguration of a 5p4

Slide 51 / 16319 The electron configuration [Ar]4s23d5 belongs in whichgroup of the periodic table?ABCDAlkali MetalsAlkaline Earth MetalsTransition MetalsHalogens

Slide 52 / 16320 Which of the following represents an electronconfiguration of an alkaline earth metal?ABCD[He]2s1[Ne]3s23p6[Ar]4s23d2[Xe]6s2

Slide 53 / 16321 The element iridium is found in a higher abundance inmeteorites than in Earth's crust. One specific layer ofEarth associated with the end of the Cretaceous Periodhas an abnormal abundance of iridium, which ledscientists to hypothesize that the impact of a massiveextraterrestrial object caused the extinction of thedinosaurs 66 million years ago. Using the PeriodicTable, choose the correct electron configuration d7D[Xe]6s25f146d7

Slide 54 / 16322 The element tin has been known for a long and waseven mentioned in the Old Testament of the Bible.During the Bronze Age, humans mixed tin and copper tomake a malleable alloy called bronze. Tin's symbol isSn, which comes from the Latin word "stannum." Whichof the following is tin's correct electron Kr]5s24d105p2D[Kr]5s25d105p2

Slide 55 / 16323 Chemical elements with atomic numbers greater than92 are called transuranic elements. They are allunstable and decay into other elements. All werediscovered in the laboratory by using nuclear reactorsor particle accelerators, although neptunium andplutonium were also discovered later in nature.Neptunium, number 93, and plutonium, number 94,were synthesized by bombarding uranium-238 withdeuterons (a proton and neutron). What is plutonium'selectron Rn]7s26d105f6D[Rn]7s25f6

Slide 56 / 163StabilityWhen the elements were studied, scientists noticed that, when put inthe same situation, some elements reacted while others did not.The elements that did not react were labeled "stable" because they didnot change easily. When these stable elements were grouped together,periodically, they formed a pattern.Today we recognize that this difference in stability is due to electronconfigurations.Based on your knowledge and the electron configurations of argonand zinc, can you predict which electron is more stable?ArgonZinc1s2 2s2 2p6 3s2 3p61s2 2s2 2p6 3s2 3p6 4s2 3d10

Slide 57 / 163StabilityElements of varying stability fall into one of 3 categories. The moststable atoms have completely full energy levels. Full Energy Level Full Sublevel (s, p, d, f) Half Full Sublevel ( d , f )51234567677

Slide 58 / 163StabilityNext in order of stability are elements with full sublevels. Full Energy Level Full Sublevel (s, p, d, f) Half Full Sublevel ( d , f )51234567677

Slide 59 / 163StabilityFinally, the elements with half full sublevels are also stable, but not asstable as elements with fully energy levels or sublevels. Full Energy Level Full Sublevel (s, p, d, f) Half Full Sublevel ( d , f )51234567677

Slide 60 / 16324 The elements in the periodic table that havecompletely filled shells or subshells are referred toas:Anoble gases.Bhalogens.Calkali metals.Dtransition elements.

Slide 61 / 16325 Alkaline earth metals are more stable thanalkali metals because.Athey have a full shell.Bthey have a full subshell.Cthey have a half-full subshell.Dthey contain no p orbitals.

Slide 62 / 16326 The elements in the periodic table which lackone electron from a filled shell are referred toas .Anoble gasesBhalogensCalkali metalsDtransition elements

Slide 63 / 163Electron Configuration ExceptionsThere are basic exceptions in electron configurations in the d- and f-sublevels.These fall in the circled areas on the table below.123456767

Slide 64 / 163Electron Configuration ExceptionsChromiumExpect: [Ar] 4s2 3d4Actually: [Ar] 4s1 3d5For some elements, in order to exist in a more stable state, electronsfrom an s sublevel will move to a d sublevel, thus providing thestability of a half-full sublevel. Tosee why this can happen we needto examine how "close" d and s sublevels are.1234567Cr67

Slide 65 / 163Energies of Orbitals(It's kind of like borrowing acup of sugar from a neighbor).7f7d7EnergyBecause of how close the fand d orbitals are to the sorbitals, very little energy isrequired to move an electronfrom the s orbital(leaving it half full) to the f or dorbital, causing them to alsobe half f

Slide 66 / 163Electron Configuration ExceptionsCopperExpected: [Ar] 4s2 3d9Actual: [Ar] 4s1 3d10Copper gains stability when an electron from the 4sorbital fills the 3d orbital.1234567Cu67

Slide 67 / 16327 The electron configuration for Copper (Cu) isA [Ar] 4s24d9B [Ar] 4s14d9C [Ar] 4s23d9D [Ar] 4s13d10

Slide 68 / 16328 What would be the shorthand electron configuration forSilver (Ag)?A [Kr]5s25d9B [Ar]5s14d10C [Kr]5s24d9D [Kr]5s14d10

Slide 69 / 16329 What would be the shorthand electron configuration forMolybdenum (Mb)?A [Kr]5s25d4B [Ar]5s24d4C [Kr]5s14d5D [Kr]5s24d4

Slide 70 / 163Effective Nuclear Charge andCoulomb's LawReturn to Tableof Contents

Slide 71 / 163Periodic TrendsThere are four main trends in the periodic table:····Radius of atomsElectronegativityIonizatioin EnergyMetallic CharacterThese four periodic trends are all shaped by the interactions betweenthe positive charge of the atomic nucleus and the negative charge ofelectrons. How do these charges interact with each other?

Slide 72 / 163Periodic TrendsRemember that like charges repel and opposite charges attract. Thepositive protons are attracted to the negative electrons. The negativeelectrons, on the other hand, are repelled by neighboring electrons.

Slide 73 / 163Atom DiagramsAtoms of an element are often depicted showing total number ofelectrons in each energy level, like the diagram below:For example, Neon's electronconfiguration:1s22s22p610 2 electronsin inner energy levels8 electronsin the outer energy level.These outer electrons arecalled valence electrons.

Slide 74 / 16330 How many valence electrons does magnesium have?A 2B 8C 10D 1212

Slide 75 / 16331 Which of the following elements has the largest amountof inner shell electrons: aluminum, silicon or phosphorus?A AlB SiC PD They all have the same number of inner shellelectrons.

Slide 76 / 163Effective Nuclear ChargeIn a multi-electron atom, electrons are both attracted to the positivenucleus and repelled by other electrons.The nuclear charge that an electron experiences depends on bothfactors. For example, the valence electron of sodium is attracted tothe positive nucleus but is repelled by the negative inner electrons.-111 There is one valence electron.There are 11 protons in the nucleus. This attractsthe valence electron with a charge of 11 .10-There are 10 inner shell electrons. These repelthe valence electron with a charge of 10-.The total charge on the valence electron is: 11 -10 1

Slide 77 / 163Effective Nuclear ChargeThe inner shell electrons prevent the valence electron from feelingthe full attractive force of the positive protons. In other words, theinner electrons are shielding the valence electrons from the nucleus.11 10-1These 10 inner electrons preventthe 1 valence electron from feelingthe full attractive force of the 11protons.

Slide 78 / 163Effective Nuclear ChargeEffective nuclear charge is the amount of charge that the outerelectron actually feels.The formula for effective nuclear charge is:Zeff Z - SZ is the atomic number (the number of protons).S is the shielding constant, the number of inner electrons thatshields the valence electrons from the protons.1011 For sodium:Zeff 11 - 10 1

Slide 79 / 163Effective Nuclear ChargeBeryllium, boron and carbon are all in the same period of theperiodic table. Compare their shielding constants.BerylliumMove for2 answer.BoronCarbonMove for2 answer.Move for2 answer.

Slide 80 / 163Effective Nuclear ChargeElements in the same period will have the same shielding constantbecause their valence electrons are located in the same energy level.Beryllium4 Boron5 Carbon6 Each has a different atomic number. Boron and carbon have differentsubshells from beryllium. BUT, they are all in the same energy level, sothey have the same number of shielding electrons.

Slide 81 / 163Effective Nuclear ChargeNow look at effective nuclear charge. Compare the values forberyllium, boron and carbon.BerylliumMove for2 answer.BoronCarbonMove for3 answer.Move for4 answer.What do these values tell you?

Slide 82 / 16332 What is the shielding constant, S, for Boron(B)?

Slide 83 / 16333 What is the effective nuclear charge, Z eff on electrons inthe outer most shell for Boron?

Slide 84 / 16334 What is the shielding constant, S, for Aluminum (Al)?

Slide 85 / 16335 What is the effective nuclear charge on electrons inthe outer most shell for Aluminum?

Slide 86 / 16336 Which of the following would have the highest effectivenuclear charge?A AluminumB PhosphorusC ChlorineD Neon

Slide 87 / 16337 In which subshell does an electron in an arsenic (As)atom experience the greatest shielding?A 2pB 4pC 3sD 1s

Slide 88 / 16338 Two elements are studied: one with atomic number X andone with atomic number X 1. Assuming element X is nota noble gas, which element has the larger shieldingconstant?A Element XB Element X 1C They are both the same.D More information is needed.

Slide 89 / 16339 Two elements are studied: one with atomic number X andone with atomic number X 1. It is known that element Xis a noble gas. Which element has the larger shieldingconstant?A Element XB Element X 1C They are both the same.D More information is needed.

Slide 90 / 16340 In which subshell does an electron in a calcium atom experiencethe greatest effective nuclear charge?A 1sB 2sC 2pD 3s

Slide 91 / 16341 Compare the following elements: potassium, cobalt andselenium. Which atom feels the strongest attractive forcebetween the nucleus and the valence electrons?A KB CoC SeD They all experience the same magnitude of force.

Slide 92 / 163Coulomb's LawThe magnitude of the force between the protons in the nucleusand electrons in the orbitals can be calculated usingCoulomb's Law.F kq1 q2r2k Coulomb's constantq1 the charge on the first objectq2 the charge on the second objectr2 the distance between the two objects

Slide 93 / 16342 According to Coulomb's Law, the stronger the charge ofthe objects, the the force between the objects.A strongerB weakerF kq1 q2r2

Slide 94 / 16343 According to Coulomb's Law, the greater the distancebetween two objects, the the force between theobjects.A strongerB weakerF kq1 q2r2

Slide 95 / 163HydrogenApplying Coulomb's Law to atoms provides useful information aboutthose atoms.Consider hydrogen. Zeff for hydrogen is 1.Zeff 1 proton - 0 inner electronZeff 11 The charge between the valenceelectron and the nucleus is 1e.Plugging this into Coulomb's Law:F kq1 q2r2kZeff(e)2F r2F ke2r2

Slide 96 / 163HeliumNow let's apply Coulomb's Law to helium.Zeff for hydrogen is 2.Zeff 2 protons - 0 inner electronZeff 22 The charge between the valenceelectron and the nucleus is 2e.Plugging this into Coulomb's Law:F kq1 q2r2kZeff(e)2F r2k(2e)2F r2

Slide 97 / 163Hydrogen vs HeliumNow we can compare hydrogen and helium.HydrogenThe force between the valenceelectron and the nucleus is:F ke2r2HeliumThe force between the valenceelectrons and the nucleus is:k(2e)2F r2(Initially, the radius is the same for both since bothhave valence electrons in the same energy level.)The force between the nucleus and the electrons in helium is muchlarger than the force between the nucleus and the electron inhydrogen.How does this affect the radii of the atoms?

Slide 98 / 163LithiumZeff Z - SZeff 3 -23 Zeff 1Plugging this into Coulomb's Law:F kq1 q2r2kZeff(e)2F r2F ke2r2

Slide 99 / 163Lithium vs HydrogenLithiumHydrogen3 1 F ker22F ke2r2The Zeff is the same for both atoms. However, lithium has valenceelectrons in a higher energy level.How does this affect the radii of the atoms?

Slide 100 / 163BerylliumZeff Z - SZeff 4 -24 Zeff 2Plug this into Coulomb's Law.F kq1 q2r2Slidek(2e)for 2F answer.r2

Slide 101 / 163Lithium vs BerylliumLithium3 F ke2r2Beryllium4 k(2e)2F r2How do the radii of beryllium and lithium compare?

Slide 102 / 16344 What is Zeff for Boron (B)?5

Slide 103 / 16345 Compare the radial size of boron to lithium andberyllium.A Li Be BB Li Be BC Li B BeD Be Li B

Slide 104 / 16346 What is Zeff for Carbon (C)?6

Slide 105 / 16347 Compare the radial size of carbon to boron and nitrogen.A C N BB C N BC B C ND B C N

Slide 106 / 16348 Which of the following equations correctly calculates theCoulombic force between the valence electrons and thenucleus of an oxygen atom?A F k(2e)2/r2B F k(4e)2/r2C F k(6e)2/r2D F k(8e)2/r2

Slide 107 / 16349 Give the atomic number of the smallest element in the2nd period.

Slide 108 / 163Periodic Trends: Atomic RadiusReturn to Tableof Contents

Slide 109 / 16350Atomic Radii TrendWhattypeis theirtheanswerstrendherein atomicStudentssize across a period?What is the trend in atomic size down a group?(Pull the box away to see the answers.)

Slide 110 / 16351 Across a period from left to right Zeff .AincreasesBdecreasesCremains the same

Slide 111 / 16352 Down a group from top to bottom Zeff .AincreasesBdecreasesCremains the same

Slide 112 / 16353 Atomic radius generally increases as we move.A down a group and from right to left across aperiodBup a group and from left to right across aperiodCdown a group and from left to right across aperiodDup a group and from right to left across aperiod

Slide 113 / 16354 Which one of the following atoms has the smallestradius?A OB FC SD Cl

Slide 114 / 16355 Which one of the following atoms has thelargest radius?A CsBAlC BeD Ne

Slide 115 / 16356 Which one of the following atoms has thesmallest radius?A FeB NC SD I

Slide 116 / 16357 Of the following, which gives the correct orderfor atomic radius for Mg, Na, P, Si and Ar?AMg NaBAr SiCSi DNa P PP Si Na Ar Mg Si Ar Mg Na P Mg Ar

Slide 117 / 16358 Which of the following correctly lists the fiveatoms in order of increasing size (smallest tolargest)?AO F S Mg BaBF O S Mg BaCF O S Ba MgDF S O Mg Ba

Slide 118 / 16359 Two elements are studied. One with atomicnumber X and one with atomic number X 1.Assuming element X is not a Noble Gas, whichelement has the larger atomic radius?AElement XBElement X 1CThey are both the same.DMore information is needed.

Slide 119 / 16360 Two elements are studied. One with atomic numberX and one with atomic number X 1. It is known thatelement X is a Noble Gas. Which element has thelarger atomic radius?AElement XBElement X 1CThey are both the same.DMore information is needed.

Slide 120 / 163Summary of Atomic Radius Trends· Across a period, effective nuclear charge increases while energylevel remains the same. The force of attraction between thenucleus and valence electrons gets stronger. Valence electronsare pulled in tighter, so radius gets smaller.F kq1 q2r2This value gets larger, so force islarger. (Radius is smaller.)· Down a period, effective nuclear charge remains the same whilethe energy level increases. The increased distance from thenucleus to valence electrons makes the force of attractiondecrease. Electrons are not held as tightly, so radius gets larger.F kq1 q2r2This value gets larger, so force issmaller. (Radius is larger.)Click here for an animation on the atomic radius trend.

Slide 121 / 163Periodic Trends:Ionization EnergyReturn to Tableof Contents

Slide 122 / 163.Ionization EnergyAtoms of the same element have equal numbers ofprotons and electrons.Neutral Oxygen --- 8 ( ) protons and 8 (-) electronsNeutral Magnesium --- 12 ( ) protons and 12 (-) electrons-- 8 8- 8 -80 charge-Neutral atom

Slide 123 / 163Ionization EnergyThe ionization energy is the amount of energy required toremove anelectron from an atom.Removing an electron creates a positively charged atom called acation.Calcium cation1e- 20 - 19CaCa e- 1 charge

Slide 124 / 163Ionization EnergyThe ionization energy is the amount of energy required toremove anelectron from an atom. Removing an electron creates a positivelycharged atom called a cation.The first ionizationenergy is the energyrequired to removethe first electron.CaCa e -The second ionizationenergy is the energyrequired to removethe second electron,etc.Ca 1e1e-Ca2 e-

Slide 125 / 16361 If an electron is removed from a sodium (Na) atom, whatcharge does the Na cation have?

Slide 126 / 16362 If two electrons are removed from a Magnesium (Mg)atom, what charge does the Mg cation have?

Slide 127 / 163Lithium vs BerylliumApplying Coulomb's Law helps us to understand how ionizationenergy changes among elements.Lithium3 F ke2r2Beryllium4 k(2e)2F r2Which atom is held together more closely?

Slide 128 / 163Lithium vs BerylliumLithiumBeryllium3 4 F ke2r2k(2e)2F r2Since beryllium holds onto its electrons tighter, it will require moreenergy to take away an electron. The ionization energy of beryllium ishigher than lithium.

Slide 129 / 163Ionization Energy and Coulomb's LawAs the force increases, the atom holds onto electrons tighter. Theseelectrons will require more energy (ionization energy) to take themaway than an atom with a lower force.As force increases, ionization energy increases.Think back to atomic radius. How does atomic radius relate toCoulomb's Law? How does it relate to ionization energy?

Slide 130 / 163Trends in First Ionization EnergiesCompare ionization energies for magnesium, aluminum andsilicon.First, find Coulomb's equation for each. Then, order the elementsin increasing ionization energy.MagnesiumPull fork(2e)2F answerr2AluminumPull fork(3e)2F answerr2SiliconPull fork(4e)2F answerr2Increasing order of ionization energies: PullMgfor answerAl SiHow does ionization energy change as you go across a period?

Slide 131 / 163energ/mol)ioniza ti o nergy (kJasingIncreIonization energyincreases across aperiod.n EnIonizatioAcross a period, Zeffincreases and the forceon electrons increases.This makes it harder foran electron to be takenaway.yTrends in First Ionization Energiesation energyIncreasing ioniz

Slide 132 / 163Trends in First Ionization EnergiesCompare ionization energies for sodium and potassium.First, find Coulomb's equation for each. Then, order the elementsin increasing ionization energy.Sodium2kePullF foranswer r2PotassiumPull forke2F answerr2answerIncreasing order of ionization energies: PullK forNaHow does ionization energy change as you go down a group?

Slide 133 / 163Click here for an animation onIonization Energyener gat i onkJ/mol)i oni zasingIncreIonization energydecreases as you godown a period.rgy (on EnetiaiznIoDown a group, Zeff staysthe same but the extraenergy levels make theradius larger which makethe force less. It is easierto take electrons away.yTrends in First Ionization EnergiesIncreasing ionization energy

Slide 134 / 163Trends in First Ionization EnergiesHowever, there are two apparent discontinuities in this trend.

Slide 135 / 163Discontinuity #1The first is betweenGroups 2 and 13 (3A).As you can see on the chartto the right, the ionizationenergy actually decreasesfrom Group 2 to Group 13elements. The electronremoved for Group 13elements is from a p orbitaland removing this electronactually adds stability.The electron removed is farther from nucleus, there is a smallamount of repulsion by the s electrons.The atom gains stability by having a full s orbital, and anempty p orbital.

Slide 136 / 163Discontinuity #1More energy is required to remove an electron from Group 2elements than Group 13 elements. Draw the orbital diagrams forGroup 2 Boron and Group 13 Beryllium to illustrate why.Boron1sBeryllium1s2s2p2s2pThe atom gains stability by having a full s orbital, and anempty p orbital.

Slide 137 / 16363Discontinuity #2Students type their answers hereThe second is betweenGroups 15 and 16.Using your knowledge ofelectron configurations andthe stability of atomsexplain why the firstionization energy for aGroup 16 element wouldbe less than that for aGroup 15 element in thesame period.

Slide 138 / 16364 Of the elements below, has thelargest first ionization energy.A LiB KC RbD H

Slide 139 / 16365 Of the following atoms, which has the largest firstionization energy?A BrB OC CD P

Slide 140 / 16366 Of the following elements, which has the largestfirst ionization energy?ANaBAlCSeDCl

Slide 141 / 16367 Which noble gas has the lowest first ionizationenergy (enter the atomic number)?

Slide 142 / 163Periodic Trends:ElectronegativityReturn to Tableof Contents

Slide 143 / 163ElectronegativityElectronegativity is the ability of an atom to attract other electrons.Using Coulomb's Law, an atom with

Nov 19, 2015 · Alkali Metals 1 s1 ending Very reactive Alkaline Earth Metals 2 s2 ending Reactive Transition Metals 3-12 (d block) ns2, (n-1)d ending Somewhat reactive, typical metals Inner Transition Metals f block ns2, (n-2)f ending Somewhat reactive, radioactive Halogens 17 s2p5 endi

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Slide della Presentazione del libro elettronico (e-book) "EMOZIONI – storia, biologia, psicologia e loro influenza sulle scelte" (proiettate in occasione della Presentazione del libro svolta a Guardia Lombardi il 9 Maggio 2015) Slide 19 Slide 20 Slid 21 Slide 22 Slide 23 Slide 24 5.

PowerPoint Slides, Computer, LCD projector, Easel, Flip Chart, and Markers . II. Training Session Content . a. PowerPoint Slides Slide 3-1: Chapter Overview Slide 3-2: Getting Started Slide 3-3: Assertiveness Slide 3-4: Hypervigilance Slide 3-5: Personal Agency Slide 3-6: Trigger Slide

Slide 17- Adding Pizzazz: Clip Art Slide 18- Adding Pizzazz: Photos Slide 19- Adding Pizzazz: Navigating Windows to Copy/Paste Slide 20- Adding Pizzazz: Photos & Clip Art Using Copy/Paste Slide 21- Adding Pizzazz: WordArt Slide 22- Adding Pizzazz: Borders Slide 23-Moving Graphics & Clip Art

8 Quantum dots 163 8.1 Sources 163 8.2 Introduction 163 8.3 Quasi-zero dimensional systems [1,2] 163 8.4 The single-particle eigen-spectrum of a quantum dot [3] 165 8.4.1 Zero fleld limit 165 8.4.2 High fleld limit 166 8.5 Conductance of a quantum dot 167 8.6 McEuen et al [2] 169 8.6.1 Magnetic fleld dependence of resonant peaks [1,2] 169

Slide guide for 1-4 pipe. Slide welded to pipe with bolt down axial guide base. MODEL PTFE SLIDE GUIDE STANDARD AND PRE-INSULATED Slide guides can come in a variety of configura-tions. Listed below are various options for PTFE slide supports, pre-insulated PTFE slide sup-ports, and base options. 1-4” pipe diameter Maximum 2” insulation