1. Electron Arrangement Review Unit 3

2. NC Essential Standards Chm.1.1.2 Analyze diagrams related to the Bohr model of the hydrogen atom in terms of allowed, discrete energy levels in the emission spectrum. Describe the electron cloud of the atom in terms of a probability model. Relate the electron configurations of atoms to the Bohr and electron cloud models. Chm.1.1.3 Understand that energy exists in discrete units called quanta Describe the concept of ground and excited states of electrons in an atom 1. When an electron gains an amount of energy equivalent to the energy difference, it moves from its ground state to a higher energy level. 2. When the electron moves to a lower energy level, it releases an amount of energy equal to the energy difference in these levels as electromagnetic radiation (emissions spectrum). Articulate that this electromagnetic radiation is given off as photons. Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency. Use the “Bohr Model for Hydrogen Atom” and “Electromagnetic Spectrum” diagrams from the Reference Tables to relate color, frequency, and wavelength of the light emitted to the energy of the photon. Explain that Niels Bohr produced a model of the hydrogen atom based on experimental observations. This model indicated that: 1. an electron circles the nucleus only in fixed energy ranges called orbits; 2. an electron can neither gain or lose energy inside this orbit, but could move up or down to another orbit; 3. that the lowest energy orbit is closest to the nucleus. Describe the wave/particle duality of electrons.

3. Essential Standard 1.3.2

4. Agenda: 3/3 Objective: To link the electron arrangements concepts for atoms and ions Warm-up: 3 methods to represent electron arrangement Review: –Bohr model –Electromagnetic spectrum –3 methods to write electron arrangement –Valence electrons and electron dot notation –Ions: forming ions and symbols Homework: Study for test on Wednesday Electron arrangement, Bohr, Unit 1 & Unit 2

5. Warm-up: 1s ² 2s ² 2p ⁶ 3s ² 3p ⁶ 4s ² 1s² 2s² 2p ⁶ 3s² 3p ⁶ 4s ² 3d¹º4p⁵ 1.What elements are represented? 2.What is the name of this electron arrangement? 3.Represent the element in two other ways:

6. Energy is related to the Electron’s orbits When an atom is: The electron will: –Start at the –Jump to –Number of jumps is related to Key researchers: Bohr, Plank, Einstein Schrodinger Overview

8. Describe the relationship between wavelength, frequency, and energy. If you have low energy, describe the wavelength and frequency. If you have high energy, describe the wavelength and frequency.

9. Electron Cloud Model Quantum Mechanical Model –Based on determining the probable location of the electron –Within the boundary of the atom, its electrons can be found 90% of the time (based on probability)

10. The electrons travel around the nucleus at high speeds and in complicated patterns.

11. Methods for Writing Electron Arrangements Orbital notation Electron configuration Noble gas notation How are you going to remember the names for each method of writing the electron arrangement?

12. Check your warm-up answers 1s ² 2s ² 2p ⁶ 3s ² 3p ⁶ 4s ² 1s² 2s² 2p ⁶ 3s² 3p ⁶ 4s ² 3d¹º4p⁵ 1.What elements are represented? 2.What is the name of this electron arrangement? 3.Represent the element in two other ways:

13. 1s ² 2s ² 2p ⁶ 3s ² 3p ⁶ 4s ² 1s² 2s² 2p ⁶ 3s² 3p ⁶ 4s ² 3d¹º4p⁵

14. Rules for Electron Arrangement Aufbau: Place the electron at the lowest energy orbital possible. * Pauli’s exclusion principle: Place a maximum of 2 electrons in each orbital. Hund’s rule: Place an electron in each orbital of a sublevel before pairing up. * Check the diagram for the order of increasing energy level

15. Principal Energy Level Location of the Valence electrons

16. Electron Configuration Principal energy level + sublevel Use superscripts to show number of electrons in each sublevel 1s ² 2s ² 2p ⁶ 3s ² 3p ⁶ 4s ²

17. Orbital Notation The orbital is indicated by a line____ wioth the name written below. Arrows represent the electrons. Examples Ne: ___ ___ ___ ___ ___ 1s 2s 2p 2p 2p ___ ___ ___ ___ ___ ___ ___ ___ ___ ___ Note: You must write both the lines and the orbital designations under the lines

18. Noble Gas Notation Short cut method for electron arrangement Use the noble gas in the period above the element Example: Na 1s ² 2s ² 2p ⁶ 3s ¹ -Use Neon -Represent neon’s configuration 1s ² 2s ² 2p ⁶ as [Ne] - Use in Na: [Ne] 3s ¹

19. Arrow Diagram Remembering the order to place the electrons

20. Element Atomic # and Group # Orbital diagramElectron Configuration Noble gas notationValence e- Electron dot Ne Ar Mg Ca N P 0 S F Cl Br

21. Check your electron configuration answers using the Periodic Table Periods S, P, D, F Blocks 18

22. Electron Dot Notation – Maximun number = 8

23. Write the Electron Dot in the correct location for the element

24. Element M? NM? Electron Configuration Atom Electron Configuration Ion Symbol for Ion Ne Ar Mg Ca N P 0 S F Cl Br Forming Ions