Chapter 10 Modern Atomic Theory And The Periodic Table

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Across
  1. 1. small packets of energy in streams of light
  2. 2. 2nd sublevel
  3. 5. all the Group IIIB to Group IIB (3-12) elements
  4. 7. lowest energy level
  5. 8. columns in the periodic table
  6. 10. in a given atom, no 2 electrons may have the same set of 4 quantum numbers therefore an orbital must have electrons with opposite spins ↓↑
  7. 12. the energy level expressed by the principal quantum number n
  8. 15. Every principle energy level is divided into _____
  9. 16. When a gas emits light shown through a prism, the beaming colored lines are part of a _____
  10. 19. distance between two peaks or trough inside a wave
  11. 21. this method of arranging electrons uses numbers, letters, and superscripts
  12. 25. energy is emitted in tiny distinct packets called _____
  13. 26. 4th sublevel
  14. 27. this atom's orbital configuration is 1s² 2s²2p⁶ 3s²3p⁶ 4s²3d¹⁰
  15. 28. 1st sublevel
Down
  1. 1. as stated by this principle, an orbital cannot contain more than 2 electrons
  2. 3. this atom's orbital configuration is 1s² 2s²2p⁶ 3s²3p⁶ 4s²
  3. 4. this method of arranging electrons uses arrows and boxes
  4. 6. what is white light?
  5. 9. neon’s orbital configuration
  6. 10. rows in the periodic table
  7. 11. all the Group A’s elements in the Periodic Table
  8. 13. outermost electron shell
  9. 14. Who said this: “electrons revolve in specific regions at various distances from the nucleus called energy levels”
  10. 17. Group VIIA Elements
  11. 18. electrons on the outermost energy level
  12. 20. Which rule is this: electrons will occupy separate orbitals of the same energy before pairing of electrons occur
  13. 22. region in space around a nucleus with a high probability of finding an electron
  14. 23. 3rd sublevel
  15. 24. this atom's orbital configuration is 1s² 2s²2p⁶ 3s²3p⁶