2. Light is an electromagnetic wave EM wave- a form of energy that exhibits wavelike behavior as it travels through space All the forms of EM radiation form the electromagnetic spectrum

3. Properties of EM waves Speed- all forms of EM radiation travel at 3 x 10 8 m/s in a vacuum Wavelength-the distance between 2 consecutive waves Frequency- the # of waves that pass a stationary pt. in one second Amplitude- the height of a wave measured from the origin to its crest

4. Photoelectric Effect Refers to the emission of electrons from a metal when light of a specific frequency (or energy) shines on the metal

5. Particle Description of Light Quantum- the minimum quantity of energy that can be lost or gained by an atom This relationship is expressed as: E = hv Where E = energy h= Planck’s constant v= frequency of light

6. The Dual Nature of Light Light exhibits many wavelike properties but can also be thought of as a stream of particles called photons. Photon- a particle of EM radiation having zero mass and carrying a quantum of energy

7. Bohr’s Model The electron can circle the nucleus only in allowed paths or orbits In an orbit, an electron has a fixed energy The lowest energy state is closest to the nucleus An electron can move to a higher orbital if it gains the amount of energy equal to the difference in energy between the initial orbit and the higher energy orbit

8. Line Emission Spectra The lowest energy state of an electron is the ground state. A state in which that atom has a higher energy potential is called an excited state. As the excited electron falls back to its ground state, it releases EM radiation of an energy that corresponds to the amount of energy gained to reach the excited state.

9. energy of emitted photon = (atom energy before) - (atom energy after)

10. When the EM radiation released is passed through a prism or diffraction grating- it is separated into a series of specific frequencies of visible light. This is referred to as a line emission spectra

12. DeBroglie’s Idea Suggested that electrons could also have a wave nature much like light. This was based on the fact that:  Electrons can be diffracted (bending)  Electrons exhibit interference (overlapping that results in a reduction of energy)

13. It is impossible to determine simultaneously both the position and velocity of an electron.

14. Schrodinger’s Wave Equation Laid the foundation for modern quantum theory. Quantum Theory describes mathematically the wave properties of electrons. The solutions to this equation give only the probability of finding an electron at a given location.

15. Electrons do not travel in neat orbits They exist in three- dimensional regions called orbits that indicate the probable location of an electron.

16. The location of electrons within the atom can be described using quantum numbers:  Principle  Orbital (Angular Momentum)  Magnetic  Spin

17. Principle Quantum Number Gives the principle energy level n= 1, 2, 3, etc. Maximum # of Electrons for Orbitals: 1 st - 2 2 nd – 8 3 rd – 18 4 th - 32

18. Orbital Quantum Number Tells the shape or type of orbital s orbital is doughnut shaped p orbital is dumbbell shaped

19. Suborbital# of electrons# of orbitals s21 p63 d105 f147

20. Magnetic Quantum Number Designates specific regions of space w/in each energy sublevel (s, p, d, f) Ex. p sublevel has 3 orbitals (p x, p y, p z )

21. Spin Quantum Number Designates direction of electron spin Electrons w/in an orbital spin in opposite directions

22. Governing Rules and Principles Pauli Exclusion Principle- only 2 electrons in each orbital Aufbau Principle- electrons must occupy lower energy orbitals first Hunds Rule- a second electron can not be added to an orbital until each orbital in a sublevel contains an electron

24. Summary: Principle Energy Level OrbitalsMax. Electrons 1s2 2s p8 3s p d18 4s p d f32