1. Unanswered Questions Rutherford’s model did not address the following questions: 1. What is the arrangement of electrons in the atom? 2. What keeps the electrons from converging on the nucleus? 3. What accounts for the differences in chemical behavior among elements?

2. Bohr Model of the Atom Electrons movement around the nucleus is restricted to a particular circular orbit. The “Planetary” model. Each orbit is associated with a certain amount of energy The larger the orbit (farther away from the nucleus) the greater the energy In order to move from one orbit to the next, an electron has to absorb a quantum of energy Bohrs model was limited to explaining the behavior of hydrogen The minimum amount of energy required to move an electron from one level to another

3. Quantum Mechanical Model Like Bohr, electrons energies are limited to a certain value Unlike Bohr, electrons do not travel in prescribed paths. Electrons travel within a particular volume of space surrounding the nucleus The probability of finding an electron in a particular region of space is represented as a cloud of electrons.

4. Organization of Electrons in an Atom Energy Levels (aka principal quantum numbers) n=1,2,3,4,5,6,7 Energy levels increase as distance from the nucleus increases Sublevels (s,p,d,f) Volume of space defined by a collection of orbitals Orbitals Shapes Sharp, principal, diffuse, and fundamental

5. Ground-State Electron Configuration Arrangement of electron in an atom at rest  The lowest energy arrangement is the most stable Three Rules that govern how electrons can be arranged in an atom: Aufbau Principle Each electron occupies the lowest energy orbital available Pauli Exclusion Principle A maximum of two electrons can occupy a single orbital Hund’s Rule Electrons with the same spin must occupy each orbital before electrons with opposite spins can occupy each orbital

6. Orbital Filling Sequence (subshell) (Energy Level)

7. Orbital Filling Diagram Electron Configuration Fluorine (atomic #9) 225 Orbital Diagram

9. Nobel Gas Configuration To shorten the amount of writing required to represent the configuration of elements with large numbers of electrons, the symbol for the noble gas that directly precedes an element can represent all of the electrons up to that point. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 [Ar] 4s2 Long HandShort Hand

10. Exceptional Electron Configurations Not all electron configurations abide by Aufbau’s principle. Half-filled sub-levels are not as stable as filled sublevels, but they are more stable than other configurations. Ex. Chromium According to AufbauMore stable configuration 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 4

11. Chemical Behavior Related to the Arrangement of Electrons In the early 1900’s scientist observed that when they heated elements in a flame, the elements emitted colored light. Analysis of the light led scientist to determine that the arrangement of electrons in an atom is related to the elements chemical behavior.

12. Understanding Light – Characteristics of Waves C A 1 sec D E Using the word bank below, match the words to the lettered parts of the diagram B = 3/s FrequencyAmplitudePeak TroughWavelength

13. Waves Characteristics Wavelength ( ) the shortest distance between two equivalent points on a wave. ( unit of measure: meters, centimeters, or nanometers) Frequency (v ) the number of waves that pass a given point per second. (unit of measure: Hz, waves/second, /s, s -1 ) c v Waves c= v Speed of Light (c) = 3.0 x 10 8 m/s

14. Relationship Between Wavelength and Frequency c= v Frequency Wavelength

15. Electromagnetic Spectrum Electromagnetic radiation – Form of energy that exhibits wave-like behavior. Electromagnetic spectrum – encompasses all forms of electromagnetic radiation. The only differences between each form is their characteristic wavelengths and frequencies. White Light – a continuous spectrum of colors, each with a unique wavelength and frequency.

16. The Electromagnetic Spectrum Which of the following waves has the longest wavelength? Which has the greatest frequency?

17. Line Spectra

18. Einstein’s Contribution E photon =hv Explained that electromagnetic radiation behaves both like waves and particles. Photon – a particle of electromagnetic radiation with no mass that carries a quantum of energy.

19. E quantum =hv E = energy h = Planck’s constant=6.626 x 10 -34 J V = frequency Relationships between wavelength, frequency and Energy Frequency Wavelength Energy Frequency Energy Wavelength

20. Electrons as Waves (Louis de Broglie) de Broglie proposed the idea that all particles have wavelengths Wavelengths of large bodies are too small to observe and therefore principals of classical physics best describes their movement Quantum mechanics provides a more suitable explanation of the movement of subatomic particles

21. Photoelectric Effect Electrons are emitted from a metal’s surface when light of a certain minimum frequency of 1.14 x 10 15 Hz shines on the surface. (Conversion of light energy to electrical energy)

22. Heisenberg Uncertainty Principle Premise: It is impossible to make any measurement on an object without disturbing the object. The position of electron can be determined by shooting photons at electrons in an atom It is impossible to know precisely both the velocity and position of a particle at the same time