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Electrons in Atoms Unit 11 Review Session

Electrons in Atoms Unit 11 Review Session. Which of the following is a correct atomic orbital designation? 4f 2d. What rule says that within a sublevel (s,p,d,f) we must put 1 electron into each orbital before we put 2 electrons into any one orbital?. Hund’s Rule.

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Electrons in Atoms Unit 11 Review Session

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  1. Electrons in Atoms Unit 11 Review Session Academic Chemistry BRRHS, M. Crowther

  2. Which of the following is a correct atomic orbital designation? 4f 2d Academic Chemistry BRRHS, M. Crowther

  3. What rule says that within a sublevel (s,p,d,f) we must put 1 electron into each orbital before we put 2 electrons into any one orbital? Hund’s Rule Academic Chemistry BRRHS, M. Crowther

  4. Which of the following represents a “p” atomic orbital? Academic Chemistry BRRHS, M. Crowther

  5. What atomic model is depicted below and who developed it? “plum-pudding” J.J. Thomson Academic Chemistry BRRHS, M. Crowther

  6. Which of the following electronconfigurations for Chromium(z=24) is correct?1s22s22p63s23p64s23d4 1s22s22p63s23p64s13d5 Academic Chemistry BRRHS, M. Crowther

  7. How many valence electrons does Aluminum (z=13) have? 1s22s22p63s23p1 3 Academic Chemistry BRRHS, M. Crowther

  8. The Aufbau Principal What principal tells us the order in which to fill atomic orbitals with electrons? Academic Chemistry BRRHS, M. Crowther

  9. Which of the following orbitalnotations for O is correct? 1s 2s 2px 2py 2pz Academic Chemistry BRRHS, M. Crowther

  10. In order for electrons to junp from lower energy sublevels to higher energy sublevels they much absorb an exact amount of energy called a ___________. quantum Academic Chemistry BRRHS, M. Crowther

  11. Which of the following electronconfigurations for Carbon(z=6) is correct? 1s 2s 2px 2py 2pz Academic Chemistry BRRHS, M. Crowther

  12. What atomic model is depicted below and who developed it? Planetary Model N. Bohr Academic Chemistry BRRHS, M. Crowther

  13. State the Pauli Exclusion Principal. Only two electrons, at most, with opposite spin may occupy any one atomic orbital. Academic Chemistry BRRHS, M. Crowther

  14. Which of the following represents a “d” atomic orbital? Academic Chemistry BRRHS, M. Crowther

  15. Which of the following is a correct atomic orbital designation?3f 5s Academic Chemistry BRRHS, M. Crowther

  16. There are 18 electrons in the principal quantum level n=3. True False  Academic Chemistry BRRHS, M. Crowther

  17. How many valence electrons does Germanium (z=32) have? [Ar]3d104s24p2 4 Academic Chemistry BRRHS, M. Crowther

  18. Which of the following orbital notations for Silicon (z=14) is correct? 1s 2s 2px 2py 2pz 3s 3px 3py 3pz Academic Chemistry BRRHS, M. Crowther

  19. Which of the following electron configurations for Ca+2 (z=20) is correct?1s22s22p63s23p63d2 1s22s22p63s23p64s2 Academic Chemistry BRRHS, M. Crowther

  20. What is the volume of probability where an electron may be found? An atomic orbital. Academic Chemistry BRRHS, M. Crowther

  21. Energy __________ in the visible spectrum from red to violet. increases Academic Chemistry BRRHS, M. Crowther

  22. Which of the following electron configurations for Sulfur (z=16) is correct? 1s22s22p63s23p34s1 1s22s22p63s23p4 Academic Chemistry BRRHS, M. Crowther

  23. There are 6 orbitals in the d-sublevel. True False  Academic Chemistry BRRHS, M. Crowther

  24. Which of the following is an electron configuration for *Ar (z=18)?1s22s22p63s23p6 1s22s12p63s23p64s1 Academic Chemistry BRRHS, M. Crowther

  25. Which of the following does not represent a “p” atomic orbital? Academic Chemistry BRRHS, M. Crowther

  26. The name for the electrons in the outer electronic-shell of an atom. (These electrons take part in chemical bonding. The valence electrons. Academic Chemistry BRRHS, M. Crowther

  27. How many valence electrons does the following atom have? Potassium: 1s22s22p63s23p64s1 Silicon: 1s22s22p63s23p2 Academic Chemistry BRRHS, M. Crowther

  28. What noble element would you use to write the shorthand version of the electron configurations for the following elements? Potassium: 1s22s22p63s23p64s1 Silicon: 1s22s22p63s23p2 [Ar] 4s1 [Ne] 3s13p2 Academic Chemistry BRRHS, M. Crowther

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