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Electron Affinity the Energy Associated with Adding an Electron to an Atom

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Electron Affinity the Energy Associated with Adding an Electron to an Atom UMass Boston, Chem 115 CHEM 115 Periodic Trends (Ch. 7), and The Lewis Structure Model (Ch. 8) Lectures 21 and 22 Prof. Sevian April 22 is Earth Day. In honor of it, I offer some suggestions for ways to reduce your carbon footprint. Reduce paper usage. Print on the back of scrap paper when you need to print. Agenda Chapter 7 z Periodic properties z Ionization energy z Atomic radius z Others z Interpreting measured properties of elements in light of their electronic configurations z (+) Core = nucleus + (all but the outer shell of electrons) z (-)V) Va lence = the ou termos t s he ll o f e lec trons z Effective nuclear charge = (Total electrons) – (Core electrons) = Zeff z Coulombic force of attraction between core (+) and valence (-) z Building a logical explanation 2 © H. Sevian 1 UMass Boston, Chem 115 Convert monthly bills over to automated electronic bills What We’ve Observed So Far instead of bills mailed to you. z Noble gases (Group VIIIA) z High ionization energies compared to other Groups z Within same group, ionization energy is smaller as atomic number increases z All elements in ggproup have comp lete shell electron config urations (outermost s- and p-subshells are completely filled) z Alkali metals (Group IA) z Low ionization energies compared to other Groups z Within same group, ionization energy is smaller as atomic number increases z All elements in group have one electron in outermost s-subshell z +1 charged ions of Alkali metals (Group IA) z The alkali metals have the same second ionization energy behavior as noble g ases z Electron configurations same as noble gases z Trends down a group all follow the same pattern z The trend in the property is that it increases or decreases as you go down the group z The reason is that the most loosely bound electron is less tightly held to the atom These are all trends that occur within the same group. What about trends across a period? To be able to explain further, we need Coulomb’s law. Zeff = Z – S Core vs. Valence S = screening constant S is approximately equal to the One way to view an atom or ion number of core electrons (Note: not drawn to scale!) Nucleus Book calls (protons and this Zeff neutrons) CORE + All complete charged inner shells of electrons Outer electrons VALENCE beyond all SHELL complete inner – shells charged Image modified from http://www.badastronomy.com/bad/movies/thecore_review.html © H. Sevian 2 UMass Boston, Chem 115 Zeff = Z – S = 11 – 10 = 1 Example: Sodium Atom Z = 11 (the atomic number) S = approximately equal to the A neutral sodium atom has 11 protons number of core electrons = 10 and 11 electrons Electronic configuration is 1s2 2s2 2p6 3s1 (Note: not dra wn to scale!) 11 protons and Book calls some neutrons this Z eff (charge: +11) CORE All complete Net +1 inner shells of charge electrons ((gcharge: -10) 1s2 2s2 2p6 3s1 Outer electrons VALENCE beyond all SHELL complete inner Net -1 shells (charge: -1) charge Image modified from http://www.badastronomy.com/bad/movies/thecore_review.html Zeff = Z – S = 12 – 10 = 2 Example 2: Magnesium Atom Z = 12 (the atomic number) S = approximately equal to the A neutral magnesium atom has 12 protons number of core electrons = 10 and 12 electrons Electronic configuration is 1s2 2s2 2p6 3s2 (Note: not dra wn to scale!) 12 protons and some neutrons (charge: +12) CORE All complete Net +2 inner shells of charge electrons ((gcharge: -10) 1s2 2s2 2p6 3s2 Outer electrons VALENCE beyond all SHELL complete inner Net -2 shells (charge: -2) charge Image modified from http://www.badastronomy.com/bad/movies/thecore_review.html © H. Sevian 3 UMass Boston, Chem 115 Clicker question #1 What is the effective nuclear charge (Zeff) of silicon, Si? (A) +1 (B) +2 (C) +3 (D) +4 (E) +5 7 Remove your name from mailing lists to reduce the amount of junk mail you receive. Core vs. Valence An abbreviated periodic table (showing only the s- and p-blocks) H He Zeff = 1-0 Zeff = 2-0 Li Be B C N O F Ne Zeff = 3-2 Zeff = 4-2 Zeff = 5-2 Zeff = 6-2 Zeff = 7-2 Zeff = 8-2 Zeff = 9-2 Zeff = 10-2 Na Mg Al Si P S Cl Ar Zeff = 11-10 Zeff = 12-10 Zeff = 13-10 Zeff = 18-10 KCa GaGeAsSeBrKr 8 © H. Sevian 4 UMass Boston, Chem 115 Eat less meat Recall Coulomb’s Law Force of attraction (or repulsion): z Increases when magnitudes of charges increase z Decreases as distance between charges increases Charge on proportionality positive part Charge on constant negative part k Q Q F = + − r2 Force of distance attraction between parts To reason using Coulomb’s law, you must talk about the magnitudes of the9 charges (Q+ and Q-) and the separation of the charges (r). Summary of Ionization Energy Trends Ionization energy trends: • Increases from left to right across a period (row) • Decreases from top to bottom down a group (()column) From Chemistry & Chemical Reactivity 5th edition by Kotz / Treichel. C 2003. Reprinted with permission of Brooks/Cole, a division of Thomson Learning: www.thomsonrights.com. Fax 800-730-2215. © H. Sevian 5 UMass Boston, Chem 115 Explaining trends in ionization energy z Group trend z For the halogens, the ionization energy decreases as atomic number increases. z This is because… …the effective nuclear charge is the same (+7) for all the halogens, but the most loosely bound electron is in an energy level whose radius is larger as atomic number is larger, thus it is held less strongly due to greater r. z Period trend z For period 3, the ionization energy generally increases as atomic number increases. z This is because… …the most loosely bound electron is in the same energy level for all of them (more or less the same r away from the nucleus), but the effective nuclear charge increases as atomic number is larger, thus the most loosely bound electron is more tightly held as atomic number increases. The next time a light bulb burns out, replace it with a fluorescent bulb. Chemical Explanations In general, there are only a few basic concepts on which the logical steps of chemical explanations are built. The importance of size and charge (Coulomb’s law) 1. Core vs. valence in a single atom or ion The core is always positively charged and consists of all the protons plus the electrons that don’t participate in any action. All the electrons that participate in any action are in the valence shell. Comparisons are made based on magnitude of charges and distance separating the charges. (Note: it is possible to have competing effects.) 2. Charge density of an ion If two particles have equal charge but are different in size, the smaller one has greater charge density (more charge packed into a smaller space). Generally, something with greater charge density can have a stronger effect (e.g., it can get closer to oppositely charged particles, so the force of attraction will be greater) 3. Partial (polarizable) charge (next semester…) 12 © H. Sevian 6 UMass Boston, Chem 115 Periods vs. Groups Comparing two elements in the same group: z Identify the trend in the property from top to bottom elements in the same group z Use # of shells argument to explain the trend z Different number of compp,()lete shells, so size (radius) of cores is different z Core charges are the same because valence electrons same z Arguments are usually based on distance between core and valence (r), or most loosely bound electron, being different while Q+ and Q- are the same Comparing two elements in the same period: z Identify the trend in the property from left to right elements in the same period z Use Zeff arggpument to explain the trend z Same number of complete shells, so size (radius) of cores is the same z Different charges in nucleus, but same number of core electrons, leads to different core charge (Zeff) z Different numbers of electrons in valence z Arguments are usually based on Q+ (core charge) and Q- (valence charge) being different while distance between core and valence (r) is nearly the same 13 Atomic Radius Comparisons 1. TddTrend down any g iven group? 2. Trend across any given period? 3. Wha t happens to ra dii if these atoms become ions? From Chemistry & Chemical Reactivity 5th edition by Kotz / Treichel. C 2003. Reprinted with permission of Brooks/Cole, a division of Thomson Learning: www.thomsonrights.com. Fax 800-730-2215. © H. Sevian 7 UMass Boston, Chem 115 Radii of Cations and Anions vs. Neutral Atoms Gray = atoms Red = cations Blue = anions Summary of Atomic Radii Trends Atomic radius generally: z Increases down a group (column) z Decreases across a period (row) © H. Sevian 8 UMass Boston, Chem 115 Clicker question #2 Which answer is the correct completion of this statement? As you go from left to right across a period in the periodic table, the atomic radius… (A) decreases because the effective nuclear charge increases. (B) decreases because the effective nuclear charge decreases. (C) increases because the e ffec tive nuc lear c harge increases. (D) increases because the effective nuclear charge decreases. 17 Electron affinity The energy associated with adding an electron to an atom z Electron affinities in kJ/mol z The more negative the electron affinity, the more exothermic. Therefore, the greater attraction the atom has for the electron to be added. z Trend: As you go from left to right across a row, the electron affinity generally ________ © H.
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