2. Subatomic particle chargelocationmass Other feature proton+Nucleus 1 amu Defines the element -atomic no. neutron0Nucleus 1 amu Change no. to form isotopes electron-Electroncloud ~0~0~0~0 atom’s volume -dictates reactivity

3. Rutherford Thompson Dalton Democritus Gold Foil Experiment Cathode Ray Tube 4 Parts of Atomic Theory Coined the term “atom”

4. F 19 9 Atomic mass Atomic number Chemical Symbol A charge would be noted at the top right of a chemical symbol if the atom carries a charge ( - or + )

5. What does this mean? O 16 Oxygen-16

6. Isotopes are the same element but differ in their amount of neutrons C CC 12 C 6 7 13 6 7 12

7. Multiply the mass of each isotope by its abundance to get the weighted average. Ex.: Boron is 80.20% boron-11 (atomic mass 11.01 amu) and 19.80% boron-10 (atomic mass 10.01 amu). What is the average atomic mass of boron? (11.01amu)(80.20%) + (10.01amu)(19.80%) = 100 % =10.81 amu

8. (C=3.0 x 10 8 m/s) As frequency increases, wavelength decreases

10. E = h∙f and λ = c f  wavelength (λ)  frequency (f )  Energy (E)  Planck’s constant (h) c=3.0 x 10 8 m/s speed of light h=6.63 x 10 -34 joule-sec

11. 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d 6f 7s 7p 7d 7f Sublevels fill in order of increasing energy. 1s2s2p3s3p4s3d4p5s4d5p6s4f5d6p7s5f6d7p

13. 22 2 8 10 2 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 2 electron configuration             __ __ __ 1s 2s 2p 3s 3p 4s 3d For Ti:

14.  Electron(s) in higher energy levels than at ground state.  Energy is emitted when the electron(s) return to ground state.

15.  Mendeleev- grouped elements into 7 columns by increasing atomic mass  Moseley- determined atomic number using x-rays  Today’s Periodic Law- The properties of the elements are a periodic function of their atomic numbers.

16.  Atomic radii ◦ Increase down groups ◦ Decrease across periods  Ionization energy and electronegativity ◦ Decreases down groups ◦ Increases across periods  Reactivity ◦ Increases down metal groups ◦ Increases up nonmetal groups

17.  Atoms that have gained or lost electrons Na 1s 2 2s 2 2p 6 3s 1 Na + 1s 2 2s 2 2p 6

18. What do the following symbols stand for? Show the units for each of the above symbols. 1. f 2. 3. h 4. c 5. E Write the two formulas using the above symbols frequency wavelength Planck’s constant Speed of light energy Hz, s -1, 1/s m, nm J∙s m/s J =c /f =c /f E=h∙f

19. What is the energy of one photon of light with a wavelength of 546nm? E=h∙f f=c/λ c=3.0 x 10 8 m/s h=6.63 x 10 -34 joule∙sec f= 3.0 x 10 8 m/s x 10 9 nm = 5.49 x 10 14 s -1 546 nm 1 m E = (6.63 x 10 -34 joule∙sec)(5.49 x 10 14 s -1 ) = 3.64 x 10 -19 J

20. How many protons, electrons, and neutrons are in the following elements? Ca Hg Co Na + 20 p, 20 e, 20 n 80 p, 80 e, 121 n 27 p, 27 e, 32 n 11 p, 10 e, 12 n

21. Write the electron configuration for the following elements. S Na Au 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 1 4f 14 5d 10 1s 2 2s 2 2p 6 3s 2 3p 4 1s 2 2s 2 2p 6 3s 1

22. Two isotopes of copper occur naturally, 63 Cu (atomic mass 62.9296 amu; abundance 69.17%) and 65 Cu (atomic mass 64.9278; abundance 30.83%). What is the average atomic mass of copper? (62.9296amu)(69.17%)+(64.9278amu)(30.83%) 100% = 63.5456 = 63.55 amu