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.

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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

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