A completed review turned in at the time of the exam will result in 10 bonus points. (I will not take this late and I want a old school on paper submission) This review covers chapters one through six. The exam will be set up just like all the tests you have taken this semester. The questions reflect what will be important to carry over to the 2nd trimester of this course. You will be issued a periodic table to use on the exam. You will also be allowed to use your calculator. 1. What are the three particles that make up an atom? What are their charges? Where are they located within the atom? 2. What is the difference between an isotope and an atom? 3. How many protons, neutrons, and electrons are in the following isotopes? a. Sodium – 23 b. Calcium – 40 c. Silicon – 39 d. Silicon – 40 4. Determine the number of atoms in the following: a. 5.40 grams boron b. 0.250 mole sulfur c. 0.02550 g platinum d. 0.0384 mol potassium 5. Determine the mass of each of the following: a. 3.0 mol aluminum b. 2.56 x 1024 atoms lithium c. 1.380 mol nitrogen d. 1.05 x 1018 atoms mercury 6. Determine the number of moles in each of the following: a. 40.1 g calcium b. 2.25 x 1025 atoms zinc c. 2.6500 g iron d. 150 g sulfur e. 50 atoms barium 7. Name and describe the phenomenon that proves light is a wave. 8. Name and describe the phenomenon that proves light is a particle. 9. List the seven parts of the electromagnetic spectrum from longest to shortest wavelength. (include the colors of visible light) 10. How many electrons can each sub orbital hold? 11. How many orientations do each of the following orbitals have? a. s b. p c. d d. f 12. Write the orbital notation, electron configuration notation, and noble gas notation for the following elements: a. Potassium b. Sulfur c. Tungsten 13. Who developed the first periodic table that allowed for the prediction of properties of unknown elements? 14. Explain why atomic radii decrease across the periods but increase down the groups. 15. Use the electronegativity difference between phosphorus and iodine to indicate what type of bond is formed.