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Mastering Chemistry Quiz #3

Study quietly for your quiz - spelling counts! Write "Element Quiz #3" at the top of the paper in portrait layout with your name. Electron configurations, Aufbau Principle, and orbital diagrams explained.

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Mastering Chemistry Quiz #3

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  1. Element Quiz #3 • Quietly study for your quiz – spelling counts! • Make sure you write “Element Quiz #3” at the top of the paper, portrait layout, and your name & bell. • Number 1 – 11. • Directions: Given the name or symbol, provide the opposite.

  2. Element Quiz #3 • Lead • Mn • Neon • Hg • Nickel • Mg Lithium Mo Nitrogen P Oxygen

  3. Electron Configuration Follow along in Text Chapter 3 Section 3 Pgs. 90 - 99

  4. Orbitals • Regions around a nucleus where electrons are located that correspond to specific energy levels • Called electron cloud because no definite boundaries

  5. Electron States • Ground State: Lowest possible energy level • Excited State: Electron gains energy & moves to a higher level • Energy in the form of light is emitted when an electron loses energy & falls to a lower level

  6. Aufbau Principle • Aufbau means “building up” in German • Electrons fill orbitals that have the lowest energy first • The Diagonal Rule follows the Aufbau Principle

  7. Shorthand (Noble Gas) Configuration • The Noble Gases can be used to fill in the first part of the electron configuration of atoms of the following period S = 1s2 2s2 2p6 3s2 3p4 and Ne =1s2 2s2 2p6 so S = [Ne] 3s2 3p4

  8. Closure Complete the below nuclear equations on your exit slip. 1. → + 1 4 0 218 59 238 n e Po He U Co 0 -1 84 2 27 92 2. → + 3. + → 14 4. C undergoes beta decay 6

  9. Orbital Diagrams Follow along in Text Chapter 3 Section 3 Pgs. 90 - 99

  10. Orbital Diagrams • Uses arrows to represent each electron and lines to represent each sublevel • Can be determined from Electron Configuration

  11. Pauli Exclusion Principle • Wolfgang Pauli discovered that no more than 2 electrons can occupy a single orbital • No two electrons in an atom will have all the same quantum numbers, which tell an electrons location in an atom

  12. Orbital Diagrams • Each sublevel is represented by a line above the orbital’s name 1s 2s 2p

  13. Sublevels • Divisions of orbitals • Each type of orbital has its own amount of sublevels 0 -1 0 1 s - orbital p - orbitals -2 -1 0 1 2 d - orbitals -3 -2 -1 0 1 2 3 f - orbitals

  14. 1s2 2s2 2p6 Orbital Diagrams • Electrons are put on each line and the number of electrons for each sublevel is a superscript

  15. Hund’s Rule • Each line of a sublevel must have one electron on it before the electrons are paired 1 2 3 4 5 8 6 9 7 10 1s2 2s2 2p6

  16. Orbital Diagrams • Counting these electrons, you can tell that this element is… Neon (Ne) 1s2 2s2 2p6

  17. Hund’s Rule • So for Oxygen, the orbital diagram would be 1 2 3 4 5 8 6 7 1s2 2s2 2p4

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