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Name ____________ Chapter 11 and 12-2 Review/Study Guide for Test 1. List the major discovery or accomplishment associated with of each of the following scientists: a. Democritus – named the atom b. Dalton – said the atom was positively charged, had his atomic theory (all atoms of the same element are the same, atoms of different elements are different, everything is made up of atoms) c. Thomson – discovered the electron through the cathode-ray tube experiment d. Rutherford – discovered the nucleus through the gold foil experiment e. Bohr – said electrons follow definite paths outside the nucleus. 2. How can you distinguish between isotopes? By their mass numbers. 3. What makes an atom neutral? If it has an equal number of protons and electrons. 4. How does an atom become an ion? By gaining or losing electrons. 5. What happens to the electrons in the atom when it becomes an ion? They are gained or lost to another atom. 6. What is an isotope? When atoms of the same element have different numbers of neutrons from each other. 7. What determines the identity of an element? The number of protons in the nucleus (the atomic number) 8. How do you calculate the atomic mass of an element? It is the weighted average of the mass numbers of all of the isotopes. 9. What is an atom? The smallest particle into which an element can be divided and still be the same substance. 10. Why do scientists say that most of the mass of an atom is located in the nucleus? The mass of a proton is 1, the mass of a neutron is 1 and the mass of an electron is almost 0 amu. Protons and neutrons are found in the nucleus and electrons are outside of the nucleus. 11. Honors only: Calculate the atomic mass of silver, which occurs naturally as 52 percent silver-107 and 48 percent silver-109. Show your work. Round to the nearest hundredth. 0.52 x 107 = 55.64 55.64 + 52.32 = 107.96 0.48 x 109 = 52.32 12. State the charge, location and mass of each of the particles found in an atom. Protons – positive, in the nucleus, 1 Neutrons – neutral, in the nucleus, 1 Electrons – negative, electron cloud, almost 0 P5 N6 13. Draw a Bohr diagram for Boron-11. 5 electrons on the outside, 2 on the first shell, 3 on the second 14. What is a strong force? The force keeping the nucleus together. 15. What is the electromagnetic force? The force attracting the protons to the neutrons. 16. Fill in the missing parts of the chart. – HONORS Element Symbol / Ion S -2 Co +2 Ga Na + Atomic Mass Mass Number Atomic Number Charge # of Protons # of Neutrons # of Electrons 32.064 32 16 -2 16 16 18 58.9332 59 27 +2 27 32 25 69.723 70 31 0 31 39 31 22.9898 23 11 +1 11 12 10 ACADEMIC Element Symbol Atomic Mass Mass Number Atomic Number # of Protons # of Neutrons # of Electrons S 32.064 32 16 16 16 16 Co 58.9332 59 27 27 32 27 Ga 69.723 70 31 31 39 31 Na 22.9898 23 11 11 12 11 17. Explain the difference between a group and a period on the periodic table of elements. A group shares similar properties and is a vertical column. A period is a horizontal row and changes from metals to metalloids to nonmetals moving across the table. 18. Why are neither the alkali metals nor the alkaline-earth metals found uncombined in nature? They are very reactive. 19. Why is the element hydrogen not part of a group? It only has 1 valence electron and has properties of a nonmetal. 20. Fill in the information on the chart about the major groups on the periodic table. Group Number and Group Name Group 1 Group Contains Number of Valence Electrons Reactivity Shared Properties Metal 1 Very reactive Soft, silver colored, shiny, low density Metals 2 Reactive Silver-colored, more dense Metals 1 or 2 Varies in reactivity Shiny, good conductors, higher densities than groups 1 and 2 Group 13 Metalloids and metals 3 Somewhat reactive Solid at room temperature Group 14 Metals, metalloids and nonmetals Metals, metalloids, and nonmetals Metals, metalloids and nonmetals 4 Somewhat reactive Solid at room temperature 5 Somewhat reactive All but N solid at room temperature 6 Reactive All but O solid at room temperature Nonmetals 7 Very reactive Poor conductors Nonmetals 8 Not reactive Colorless, odorless, gases at room temperature Group 2 Group 3 - 12 Group 15 Group 16 Group 17 Group 18 21. Color on the periodic table the location of the metals, nonmetals and metalloids. Check textbook page 304.