Regents Chemistry PRACTICE PACKET. Unit 2: Atomic Theory

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1 *STUDENT* *STUDENT* Regents Chemistry PRACTICE PACKET Unit 2: Atomic Theory

Name History of Atomic Theory Period Fill in the missing information in the chart below: Name of Researcher Equipment/ Experiment Sketch of Model Major Idea/Discovery N/A All atoms of a given element

3 Name History of Atomic Theory Period Fill in the missing information in the chart below: Name of Researcher Equipment/ Experiment Sketch of Model Major Idea/Discovery N/A All atoms of a given element are identical in mass and properties Thomson Rutherford N/A Electrons travel around the nucleus in welldefined paths called orbits (like planets in a solar system) N/A Electrons have distinct amounts of energy and move in areas called orbitals Developed after the famous discovery that energy can behave as both waves & particles 3 Copyright 2015 Tim Dolgos

6 Atomic Structure Worksheet **Assume all are neutral atoms! Fill in the blanks in the following worksheet. Please keep in mind that the isotope represented by each space may NOT be the most common isotope or the one closest in atomic mass to the value on the periodic table. Atomic Atomic Protons Neutrons Electrons Mass symbol number number C W 183 Cr Md 259 Se Notice there are two different atoms of zirconium (Zr) listed. These different versions are called ISOTOPES. What one subatomic particle is different from one isotope to the other? 6 Copyright 2015 Tim Dolgos

7 Atomic Theory- Neutral Atoms and their subatomic parts **IMPORTANT**If the mass number is not given to you, round the atomic mass that you find on the Periodic Table for that element. How many protons, neutrons, and electrons are present in the following neutral atoms? vanadium P = N = e = potassium nitrogen platinum argon helium What is the name of the element that has neutral atoms that contain: 5 protons? 16 electrons? 17 protons? 32 electrons? 25 protons? 1 electron? 82 protons? 8 electrons? 92 protons? 2 electrons? 7 Copyright 2015 Tim Dolgos

8 Complete the following chart: (assume the overall charge on all atoms = 0.except the last one!) Element Symbol Atomic Number # of Protons # of Neutrons Hydrogen 1 Mass Number (amu) # of Electrons He 4 Na 12 Potassium Rb 86 Carbon 6 Xenon At Copper 64 Ne Lithium Ion Li Copyright 2015 Tim Dolgos

9 P, n, e of ions **IMPORTANT**If the mass number is not given to you, round the atomic mass that you find on the Periodic Table for that element. Write the full chemical symbol for the ion with: 1) 12 protons and 10 electrons: P = N = e = 2) 74 protons and 68 electrons: 3) 95 protons and 89 electrons: 4) 33 protons and 36 electrons: Determine the number of p, n, e for the following ions: Cu 2+ Li + O 2- p = n = e = Cl - Al 3+ I 7+ # protons # electrons # neutrons Atomic # Mass # Lithium Phosphorus Vanadium Krypton Barium Uranium Copyright 2015 Tim Dolgos

10 For the following atoms/ions determine the number of protons, neutrons, electrons, mass number, and nuclear charge. ATOM or ION? PROTONS NEUTRONS ELECTRONS MASS NUMBER NUCLEAR CHARGE 15 N Cu +2 8 B O F Pb 208 Pb Ag +1 Zn +2 Mg S -2 Question: Which of the above atoms are isotopes of one another? Explain how you know this. 10 Copyright 2015 Tim Dolgos

11 ATOM or ION? PROTONS NEUTRONS ELECTRONS MASS NUMBER NUCLEAR CHARGE Al Cl 23 Na +1 He 15 O C C Au +3 U 222 Rn Cu +1 Cu +2 Question: Which of the above atoms are isotopes of one another? Explain how you know this. 11 Copyright 2015 Tim Dolgos

12 Calculate the atomic mass of each of the following isotopes. SHOW ALL WORK. Element Mass Percent Abundance 1) copper amu 69.17% copper amu 30.83% 2) uranium amu 0.72% uranium amu 99.28% 3) hydrogen amu % hydrogen amu 0.015% 4) element Q amu 10.0% element Q amu 20.0% element Q amu 70.0% 12 Copyright 2015 Tim Dolgos

13 Weighted Averages HW (SHOW ALL WORK!) Name *You can round the masses given to you or use them as given just be consistent! 1) Element X exists in three isotopic forms. The isotopic mixture consists of 10.0% 10 X, 20.0% 11 X, and 70.0% 12 X. What is the average atomic mass of this element? 2) Element Y exists in three isotopic forms. The Isotopic mixture consists of 15.0% 21 X, 65.0% 22 X, and 20.0% 23 X. That is the average atomic mass of this element? 3) A mystery element occurs in nature as two isotopes. Isotope A has a mass of amu and its abundance is 19.9%; Isotope B has a mass of amu and its abundance is 80.1%. From this data, calculate the atomic mass of the element and show all work. Lastly, identify the element. 4) A mystery element occurs in nature as two isotopes. Isotope A has a mass of amu and its abundance is 69.17%; Isotope B has a mass of amu and its abundance is 30.83%. From this data, calculate the atomic mass of the element and show all work. Lastly, identify the element. 13 Copyright 2015 Tim Dolgos

14 5) A mystery element occurs in nature as three isotopes. Isotope A has a mass of amu and its abundance is %; Isotope B has a mass of amu and its abundance is %; Isotope C has a mass of amu and its abundance is %. From this data, calculate the atomic mass of the element and show all work. Lastly, identify the element. Isotopes and Average Atomic Mass Example: A sample of cesium is 75% 133 Cs, 20% 132 Cs, and 5% 134 Cs. What is the average atomic mass? Determine the average atomic mass of the following mixtures of isotopes % 127 I, 17% 126 I, 3% 128 I 2. 50% 197 Au, 50% 198 Au 14 Copyright 2015 Tim Dolgos

16 Regents Chemistry Name Principal Energy Level Worksheet Element e-configuration Carbon 1s 2s 2p Helium 1s Neon 1s 2s 2p Oxygen 1s 2s 2p Sulfur 1s 2s 2p 3s 3p 3d Aluminum 1s 2s 2p 3s 3p 3d Sodium 1s 2s 2p 3s 3p 3d Lithium 1s 2s 2p 16 Copyright 2015 Tim Dolgos

17 Calcium 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f Fluorine 1s 2s 2p Chlorine 1s 2s 2p 3s 3p 3d Hydrogen 1s Magnesium 1s 2s 2p 3s 3p 3d Tin 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f Potassium 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 17 Copyright 2015 Tim Dolgos

18 Construct Bohr diagrams for the following: Na electron configuration F electron configuration O electron configuration Li + electron configuration Cl - electron configuration Ne electron configuration 18 Copyright 2015 Tim Dolgos

22 Draw Lewis Dot Diagrams for the following: Charge # Valence e - N Charge # Valence e - C # unpaired valence e - # of bonds # unpaired valence e - # of bonds Charge # Valence e - Li + Charge # Valence e - He # unpaired valence e - # of bonds # unpaired valence e - # of bonds Charge # Valence e - O Charge # Valence e - B # unpaired valence e - # of bonds # unpaired valence e - # of bonds Charge # Valence e - S Charge # Valence e - Kr # unpaired valence e - # of bonds # unpaired valence e - # of bonds Charge # Valence e - Se 2- Charge # Valence e - Ca +2 # unpaired valence e - # of bonds # unpaired valence e - # of bonds 22 Copyright 2015 Tim Dolgos

23 Bohr and Lewis Dot Diagrams Element Electron Configuration # Valence e - Bohr Diagram Lewis Dot # Kernel e - Diagram Carbon Valence e - = p = n = e = Kernel e - = Oxygen Valence e - = p = n = e = Kernel e - = Sodium p = n = e = Valence e - = Kernel e - = Neon Valence e - = p = n = e = Kernel e - = 23 Copyright 2015 Tim Dolgos

24 Bohr and Lewis Dot Diagrams (continued) Element Electron Configuration # Valence e - Bohr Diagram Lewis Dot # Kernel e - Diagram Fluorine Valence e - = p = n = e = Kernel e - = Argon Valence e - = p = n = e = Kernel e - = Nitrogen p = n = e = Valence e - = Kernel e - = Lead Valence e - = p = n = e = Kernel e - = 24 Copyright 2015 Tim Dolgos

30 Regents Chemistry Electron Configuration Worksheet Name Period For the questions 1-10, assume all atoms are neutral. Use the electron configurations to determine the identity of the element and whether it is in the ground or excited state. Electron Configuration Identity Ground/Excited Give an electron configuration for the following: 11. Sulfur in its ground state. 12. Helium in an excited state. 13. Give the ground state electron configuration for calcium. 14. Give the correct electron configuration for the Ca +2 ion. 15. How many valence electrons are there in atom of bromine? 16. How many valence electrons are there in a Cl - ion? 17. How many kernel electrons are there in a phosphorus atom? 18. How many valence electrons are there in a neon atom? 19. How many principal energy levels are there in a iron atom? 30 Copyright 2015 Tim Dolgos

31 20. When atoms of an element are emitting a certain wavelength (or color) of light, it means that a) the atoms have gained energy and electrons have jumped to an excited state. b) the atoms have gained energy and electrons have fallen back to the ground state. c) the atoms have lost energy and electrons have fallen back to the ground state. d) the atoms have lost energy and electrons have jumped to an excited state. Use the emissions spectra results below to answer questions 14 and 15: Gas A Gas B Gas C Gas D Unknown Gas 21. According to these experimental spectra results, the unknown gas is a mixture of which gases? 22. The lines on the visible light spectrum for the gases above represent a) electrons jumping to the same excited state or energy level. b) electrons falling back down to their ground state from the same energy level. c) electrons jumping to multiple excited states or energy levels. d) electrons falling back down to their ground state from multiple energy levels. 23. How do the energy and the most probable location of an electron in the third shell of an atom compare to the energy and the most probable location of an electron in the first shell of the same atom? a) In the third shell, an electron has more energy and is closer to the nucleus. b) In the third shell, an electron has more energy and is farther from the nucleus. c) In the third shell, an electron has less energy and is closer to the nucleus. d) In the third shell, an electron has less energy and is farther from the nucleus. 24. An atom of oxygen is in an excited state. When an electron in this atom moves from the third shell to the second shell, energy is 31 Copyright 2015 Tim Dolgos

32 a) emitted by the nucleus b) absorbed by the nucleus c) emitted by the electron d) absorbed by the electron 25. Which electron configuration could represent a strontium atom in an excited state? a) b) c) d) Imagine an emission spectrum produced by a container of hydrogen gas. Changing the amount of hydrogen in the container will change the colors of the lines in the spectrum. a) True b) False 27. In the previous question, changing the gas in the container from hydrogen to helium will change the colors of the lines occurring in the spectrum. a) True b) False 28. An absorption spectrum appears as a continuous spectrum interrupted by a series of dark lines. a) True b) False 29. Emission spectra are characterized by narrow bright lines of different colors. a) True b) False 32 Copyright 2015 Tim Dolgos

History, Atomic Theory, and Atoms Review Packet HW: Due Wednesday, November 22 nd

History, Atomic Theory, and Atoms Review Packet HW: Due Wednesday, November 22 nd Name Date Period Atomic Theory Fill in the missing information in the chart below: Name of Researcher Equipment/ Experiment