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Atomic Structure Review Game

Atomic Structure Review Game. 30 seconds each to complete these questions. 1.Whose model of the atom was that?. Dalton Thomson Rutherford Chadwick. Solid, Indivisible Sphere of Matter. 2. What happened to the cathode ray in the experiment?. It was repelled by a (+) charge.

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Atomic Structure Review Game

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  1. Atomic Structure Review Game

  2. 30seconds each to complete these questions 1.Whose model of the atom was that? • Dalton • Thomson • Rutherford • Chadwick Solid, Indivisible Sphere of Matter

  3. 2. What happened to the cathode ray in the experiment? • It was repelled by a (+) charge. • It bounced back to the cathode. • It was stopped by a magnet. • It was deflected away from a (-) charge. J.J. Thomson & Cathode Ray Response Grid

  4. 3. What particle did Thomson discover through the cathode ray experiment? • a. Electron c. Neutron • b. Proton d. All of the above

  5. 4. What was Millikan able to measure in his oil drop experiment? • Electron’s mass • Electron’s charge • Electron’s radius • Oil’s density Response Grid

  6. 5. What did scientists conclude about the atom when the electron was discovered? • The atom must contain a (+) charge. • The atom was divisible. • Most of the atom’s mass must come from another particle. • All of the above Response Grid

  7. 6. What was the result of the gold foil experiment? • Most alpha particles bounced back. • All alpha particles went straight through. • A few alpha particles bounced back. • None of the above Response Grid

  8. 7. What conclusion did Rutherford come to after the gold foil experiment? • Most of the atom is empty space. • A dense region of (+) charge existed in the atom. • Thomson’s model was incorrect. • All of the above Response Grid

  9. Rutherford’s ExperimentGold Foil

  10. 8. What was Rutherford’s model of the atom? • Planetary model • Neutron model • Gold foil model • Nuclear model Response Grid

  11. 9. Chadwick finished off the atom with the discovery of the ____________. • Electron • Proton • Neutron • Missing link Response Grid

  12. Atomic Structure

  13. 10. The nucleus takes up most of the room in the atom. • True • False • Depends on the element • Depends on the isotope Response Grid

  14. 11. The nucleus accounts for most of the mass of the atom. • True • False • Depends on the element • Depends on the isotope Response Grid

  15. 12. Electrons are about half the size of protons. • True • False • Depends on the isotope • Depends on the atom Response Grid

  16. 13. For an atom to be neutral, it must have the same number of _________. • e- & p+ • e- & no • no & p+ • e- & p+ & no Response Grid

  17. 14. According to the periodic table, what is the number “8” in the picture below? • Atomic mass • Atomic number • Mass number • Isotope number Response Grid

  18. 15. According to the periodic table, what is 15.9994 in the picture? • Molar mass • Mass number • Average Atomic Mass • All of the above Response Grid

  19. 16. What is the number “12” represent in the hyphen notation? • Atomic number • Number of protons • Number of neutrons • Mass number Carbon - 12 Response Grid

  20. 17. The top number is the _______ number while the bottom is the ________ number. • Mass; atomic • Atomic; Mass • Neutron; proton • Proton; neutron Response Grid

  21. 18. Which subatomic particle has to do with isotopes?

  22. 19. What is the mass of a neutron in amu?

  23. 20. List the # of neutrons, # protons, and # electrons for Calcium2+-42.

  24. 21. What is a negative ion called?

  25. 22. Name two isotopes.

  26. 23. Which isotope is all the element’s masses on the periodic table based upon?

  27. 24. If I have 2 isotopes, X-16 and Y-19 and my average atomic mass is 17amu. Which isotope is more abundant?

  28. 25. How many electrons are held in a d orbital?

  29. 26. How many orbitals are in a f sublevel?

  30. 27. How many electrons can be held in the 3rd energy level?

  31. 28. What does Hund’s Rule say? • One electron can be added at a time. • Each orbital must have 1 electron in the same sublevel before a 2nd electron can be placed in that orbital. • Each orbital must contain one electron with an upward spin and one with a downward spin. • There are only 2 electrons in each orbital.

  32. You now have 1 minute for these questions 29. Write the electron configuration for Nitrogen.

  33. 30. How many valence electrons are in Nitrogen?

  34. 31. Write the box orbital notation for Sulfur.

  35. 32. List the 3 types of radiation in order of penetrating strength. (weakest to strongest)

  36. You have 5 minutes to answer this question 33. Phosphorous-32 has a half life of 68 hours. In 340 hours, how much of a 440g sample will have decayed?

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