Atomic Structure and Periodicity

1. Atomic Structure and Periodicity AP Chemistry

2. Electromagnetic Radiation ROYGBIV

3. Frequency of EM Radiation • c = λν • c: speed of light • λ: wavelength • ν: frequency (Refer to ex. 7.1 in your textbook)

4. The Nature of Matter • The change in energy for a system can be represented by: • ΔE = hν = • h: planck’s constant (6.626 x 10-34Js) • ν: frequency • : wavelength • c: speed of light

5. The Bohr Model • Energy levels available to the electron in the hydrogen atom: • E = -2.178x 10-18 J() • n is an integer • Z is the nuclear charge ΔE = Energy of final state – Energy of initial state

6. Energy Quantization in Hydrogen • ΔE = -2.178 x 10-18 J( - ) • The negative sign simply means that the energy of the electron bound to the nucleus is lower than it would be if the electron were at an infinite distance from the nucleus, where there is no interaction and the energy is zero.

7. Four Quantum Numbers • Principle quantum number (n): Indicates the main energy level occupied by the electron. • Orbital quantum number (l): indicates the sublevel and shape of orbital. • s: spherical (l =0) • p: dumbbells (l =1) • d: lobes (l = 2) • f: undefined (l =3)

8. Four Quantum Numbers • Magnetic quantum number(ml): indicates the orientation of the orbital about the nucleus. ___ ___ ___ ___ ___ -2 -1 0 +1 +2 • Spin quantum number (ms): indicates the state of an electron in an orbital. (+1/2 or -1/2)

9. Example Write the four quantum numbers for the third electron in fluorine’s valence shell. n= ______ l = ______ ml = _______ ms = _______

10. Practice problems • Pg. 337 • 18, 39, 40, 43, 51, 61-63