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Name:____________________________ Date:___________ Period:____ Review Chemistry I Honors Unit 3: Atomic Theory and Structure Define each of the following terms: 1. atom: 2. proton: 3. electron: 4. neutron: 5. nucleus: 6. average atomic mass: 7. isotope: 8. mass number: 9. atomic number: 10. Avogadro’s number: 11. molar mass: Circle or write in the correct answer: 12. Which of the following was originally a part of Dalton's atomic theory, but had to be revised later based on new experimental evidence? (circle all that apply) A. B. C. D. Atoms are tiny indivisible particles. Atoms of the same element are identical. Atoms of different elements can sometimes be identical. Compounds are made by combining atoms. 13. Consider J.J. Thomson’s cathode ray tube experiment. Briefly describe what occurred that gave evidence of electrons in all atoms. ___________________________________________________________________ ___________________________________________________________________ 1 14. Which of the following is FALSE about subatomic particles? A. B. C. D. Electrons are negatively charged and are the lightest subatomic particle. Protons are positively charged and have nearly the same mass as neutrons. Neutrons have no charge and have no mass. The mass of a neutron nearly equals the mass of a proton. 15. All atoms are neutral because the number of __________________ always equals the number of __________________ in every atom. Fill in the chart with a charge and mass: Proton Neutron Electron Charge (+ , – , or 0 ) ____ ____ ____ Rutherford Gold Foil Experiment gold atom expected results gold atom actual results 16. What observations in this experiment by led to the theory that atoms are mostly empty space, and that almost all of the mass of the atom is contained in a tiny, dense nucleus? ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ ___________________________________________________________________ 17. Based on Rutherford’s discovery of the nucleus, which model of the atom is thought to be true? A. B. C. D. Protons, electrons, and neutrons are evenly distributed throughout the atom. The nucleus is made of protons, electrons, and neutrons. Electrons are located around the nucleus and occupy most of the volume. The nucleus is made of electrons and protons. 2 18. All atoms of the same element have the same ____. A. B. C. D. number of neutrons number of protons mass numbers mass 19. What are atoms of the same element with different numbers of neutrons? A. B. C. D. ions atoms numbers of electrons isotopes 20. Explain why isotopes of the same element are not considered different elements. ___________________________________________________________________ ___________________________________________________________________ 21. Element X has an atomic number of 35 and a mass number of 75. Which of the following is correct? A. B. C. D. 35 protons, 35 neutrons, and 70 electrons 35 protons, 75 neutrons, and 35 electrons 75 protons, 35 neutrons, and 40 electrons 35 protons, 40 neutrons, and 35 electrons 22. In which of the following is the number of neutrons correctly represented? A. F has 9 neutrons. B. As has 108 neutrons. C. Mg has 12 neutrons. D. U has 238 neutrons. 23. The weighted average atomic mass of the element chlorine is 35.45 amu, but the mass number of a chlorine-37 atom is 37. So how is the average atomic mass of an element different from the mass number of an atom? ___________________________________________________________________ ___________________________________________________________________ 24. Which of the following statements about atoms is FALSE? A. B. C. D. Atoms of the same element can have different masses. Isotopes of an element have different numbers of protons. The nucleus of an atom has a positive charge. Atoms are mostly empty space. 3 25. Which of the following statements about atoms and subatomic particles is FALSE? A. B. C. D. Protons have a positive charge. Electrons are negatively charged and have a mass of 1. The nucleus of an atom is positively charged. Neutrons are located in the nucleus of an atom. 26. 15 moles of sodium and 15 moles of carbon have the same number of _________. A. B. C. D. atoms grams molecules ALL of the above 27. _____________________ is the particles or energy emitted from an atomic nucleus when it is unstable due to stronger ________________ repulsive forces than ______________ attractive forces. 28. Draw a line to match the name to the Greek symbol to the description to the symbol for each type of radiation: Name/Type Greek letter Alpha particle Description Symbol Helium nucleus Beta particle Energy Gamma ray Electron 29. The three radioactive emissions from question 2 were shot from the left side of Figure 1. Cross out the symbol of each emission in the boxes based of the ability of different materials to stop the emission from penetrating. Single sheet of paper Single sheet of Aluminum Foil three feet of concrete concretese 4 30. The element silver has two naturally occurring isotopes: silver-107 has an isotopic mass of 106.905 amu and a relative abundance of 51.84% silver-109 has an isotopic mass of 108.905 amu and a relative abundance of 48.16% Calculate the average atomic mass of the element silver. (SHOW ALL WORK) 31. The fictitious element Z has two naturally occurring isotopes, Z-310 and Z-313. The average atomic mass of Z is found to be 311.02 amu. Which of the three isotopes of the fictitious element Z is more abundant? Z-310 or Z-313 or equal abundance (circle one) How could you tell? _____________________________________________________________ Calculations and Mole Conversions SHOW ALL WORK BOX your answer molar mass 32. What is the molar mass of CaF2 ? 33. What is the molar mass of Fe3(PO4)2 ? ______________________________________________________________________ particle ↔ mole 34. Convert 4.50 moles of Fe to atoms of Fe. 35. Convert 4.03 x 1022 molecules of water to moles of water. 5 Calculations and Mole Conversions SHOW ALL WORK BOX your answer gram ↔ mole 36. Convert 0.300 moles of S to grams of S. 37. Convert 652 g Sn(CO3)2 to moles of Sn(CO3)2 . (MM = 238.73 g/mol) ______________________________________________________________________ particle ↔ gram 38. What is the mass in grams of 3.42 x 1024 atoms of C ? 39. How many atoms of aluminum are in a 5.60 g sheet of aluminum foil? 40. How many molecules are in 237 g H2O (one cup of water)? (MM = 18.02 g/mol) 6 Calculations and Mole Conversions SHOW ALL WORK BOX your answer Mix of all Mole Conversion Types 41. How many atoms are in 1.85 mol Pb? 42. How many molecules are in 120 g H2O2? (MM = 34.02 g/mol) 43. How many moles is 2.12 x 1024 molecules of PABA (sun block ingredient)? 44. What is the mass in grams of 4.78 x 1022 molecules of capsaicin, C18H27NO3? (MM = 305.41 g/mol) (capsaicin makes chili peppers hot!!) [Extra] What mass of gold would have the same number of atoms as 1000. g lead? 7