Chapter 8 - Chapter 8 Electron Configurations Lecture...

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Chapter 8: Electron Configurations Lecture Outline ± What's The Point ? ² By examining how electrons organize themselves in atoms, we can egin to nderstand trends in chemical reacti it and str ct re begin to understand trends in chemical reactivity and structure. ± Periodic Table Revisited any- lectron Atoms ± Many Electron Atoms ± Electron Configurations ± Periodic Trends ± Atomic Structure and Chemical Reactivity ± Reading : Entire Chapter omework Problems 11(12) 21(22) 23(24) 27(28a b) 33(34) ± Homework Problems : 11(12), 21(22), 23(24), 27(28a,b), 33(34), 39(40), 53(54a,c), 55(56b,d), 59(60a), 76(77), 78(79a,d), 80(81a,b), 82(83), 86(87b,c) hemSkill Builder 93 6 11 1 11 2 Due Wed Oct 11 (Your Slide No. 1 CHEM 1035 Fall 2007 Silberberg Chapter 8 ± ChemSkill Builder : 9.3-9.6, 11.1, 11.2. Due Wed Oct 11. (Your scores will be downloaded sometime on Thursday, Oct 12.) Today's Periodic Table Review: Chapter 2 Slide 17 ± Review: Chapter 2, Slides 18-20. ² Each column is called a group (18 groups) ² Each row is called a period (7 periods) ± Early periodic table (Mendeleev) ² Groups combined elements with similar "maximum valences." ² alence describes the ratio of combinations (PCl VCl Valence describes the ratio of combinations (PCl 5 , VCl 5 ). ² Predicted the future discovery of "Missing" elements. ² Elements were ordered by their masses. ± Modern table 1 234567891 01 1 1 21 3 1 41 5 1 61 71 8 Metals Metalloids on etals Slide No. 2 CHEM 1035 Fall 2007 Silberberg Chapter 8 Non-metals 8.1 From Quantum Theory to Chemistry uantum theory gives us: ± Quantum theory gives us: ² Location and behavior or electrons in atoms ² Orbital energies ² Orbital shapes ± Quantum theory explains: ² whether elements are metals, metalloids, or nonmetals ² the tendency of an atom to form ions ² trends in atomic and ionic size ² hemical reactivity chemical reactivity ² colors of atoms and molecules ² interactions of atoms and molecules with light ² magnetic properties of solids ² etc. ± The _____________________ is the key to relating chemical and Slide No. 3 CHEM 1035 Fall 2007 Silberberg Chapter 8 physical properties to electron distribution. 8.2 The Electron Spin Quantum Number uantum Number ± m s =__________ ________ Quantum Number ² Needed to describe atoms that have more than one __________ ² allowed values are +½ ( , clockwise) and –½ ( , counterclockwise) ± Pauli Exclusion Principle ² No two electrons in an atom can have the same ________________ • (n, l , m , m ) l s ² There can be at most ___ electrons in one orbital (same n, l , m l ) but then they have to have opposite _____ (different value for m s ) xample: ± Example: ² The 1s level has n = 1, l = 0, and m l = 0. ² Two electrons can go into the 1s level . .. one "up" and one "down" ² These two electrons would be: • (n = 1, l = 0, m l = 0, m s = ____) • (n = 1, l = 0, m l = 0, m s = ____) Slide No. 4 CHEM 1035 Fall 2007 Silberberg Chapter 8 ² This "configuration" describes the two electrons in the _______ atom!
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Example of the Pauli Principle ow many electrons in an atom can have the sublevel ± How many electrons in an atom can have the sublevel designation 4 p ?
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Chapter 8 - Chapter 8 Electron Configurations Lecture...

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