Electrons in Atoms

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Across
  1. 2. The shape of an “s” type orbital
  2. 3. The shape of a “p” type orbital
  3. 5. The maximum number of electrons that can be held in an “s” type sublevel
  4. 6. The transition metal section of the Periodic Table makes up this sublevel section
  5. 7. This sublevel section appears as two long rows typically found belowthe periodic table
  6. 9. Hund’s rule states that the first electrons placed into equal energy orbitals must be ______________.
  7. 11. The abbreviated way of writing electron configurations begins with this kind of element
  8. 15. The symbol placed around the element used at the beginning of an abbreviated electron configuration.
  9. 17. The term used to describe orbitals that have equivalent energy
  10. 19. The maximum number of electrons that can be held in a “p” type sublevel
  11. 20. The maximum number of electrons that can be held in an “f” type sublevel
  12. 21. The Pauli Exclusion Principle states that electrons that occupy the same orbital must have opposite _______.
  13. 22. The number of orbitals in a “d” type sublevel
Down
  1. 1. The physical area of space occupied by 2 electrons
  2. 2. Groups 1 & 2 make up this sublevel section on the Periodic Table
  3. 4. Principle that states electrons will fill in an atom in order of increasing orbital energy
  4. 8. The number of orbitals in an “s” type sublevel
  5. 9. Groups 13-18 make up this sublevel section on the Periodic Table
  6. 10. Has the abbreviated configuration [Ne]3s²3p⁵
  7. 12. Has the electron configuration 1s²2s¹
  8. 13. The number of orbitals in an “f” type sublevel
  9. 14. Rule that states that electrons will fill in one to an equivalent energy orbital first before pairing up
  10. 16. The number of orbitals in a“p” type sublevel
  11. 18. The maximum number of electrons that can be held in an “d” type sublevel