Chemistry Unit 7 - "Atomic Structure & Periodicity"

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Across
  1. 5. An area of an orbital having zero electron probability
  2. 10. The principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals
  3. 11. The square of the wave function indicating the probability of finding an electron at a particular point in space
  4. 12. A set of orbitals with a given azimuthal quantum number
  5. 13. An inner electron in an atom; one not in the outermost (valence) principal quantum level
  6. 16. The quantum number representing one of the two possible values for the electron spin; either +1/2 or-1/2
  7. 17. The concept that energy can occur only in discrete units called quanta
  8. 19. The electrons in the outermost principal quantum level of an atom
  9. 21. The statement that light exhibits both wave and particulate properties
  10. 22. The energy change associated with the addition of an electron to a gaseous atom
  11. 23. The number of waves (cycles) per second that pass a given point in space
  12. 24. The lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a particular set of degenerate orbitals, with all unpaired electrons having parallel spins
  13. 25. Several series of elements in which inner orbitals (d or f orbitals) are being filled
Down
  1. 1. Elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. The group number gives the sum of the valence s and p electrons
  2. 2. A function of the coordinates of an electron’s position in three-dimensional space that describes the properties of the electron
  3. 3. Half the distance between the nuclei in a molecule consisting of identical atoms.
  4. 4. Radiant energy that exhibits wavelike behavior and travels through space at the speed of light in a vacuum
  5. 6. A group of orbitals with the same energy
  6. 7. Elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties
  7. 8. model for the hydrogen atom in which the electron is assumed to behave as a standing wave
  8. 9. States that in a given atom no two electrons can have the same set of four quantum numbers
  9. 14. An atom with more than one electron
  10. 15. The quantum number relating to the size and energy of an orbital; it can have any positive integer value
  11. 18. A spectrum that exhibits all the wavelengths of visible light
  12. 20. The lowest possible energy state of an atom or molecule