chemistry chapter 5

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Across
  1. 2. A fundamental property of all submicroscopic systems described as the impossibility of knowing both the energy, or momentum, and the exact position of a particle.
  2. 3. A charged atom or group of atoms with a net negative charge due to the gain of electrons.
  3. 7. A principle that states that the two electrons in an orbital must have opposite spins.
  4. 9. The lowest energy level of an electron in the Bohr model.
  5. 10. A model of atoms proposed by Niels Bohr in which electrons move around the nucleus in well defined orbits.
  6. 13. A principle that states that electrons will fill the lowest available energy sublevels before any can occupy higher-energy sublevels.
  7. 14. A charged atom or group of atoms with a net positive charge due to the loss of electrons.
  8. 16. The orbits or energy levels in atomic models.
  9. 19. The quantum number that identifies the principal or main energy level of an electron.
  10. 20. A three-dimensional region representing the most probable position for an electron according to the quantum-mechanical model.
  11. 22. The current model of the atom in which protons and neutrons are located in the nucleus with electrons in orbitals around the nucleus.
  12. 23. Any energy state, other than the ground state, resulting from an electron absorbing energy.
  13. 24. A massless particle of light consisting of a bundle of wave energy.
Down
  1. 1. The current description of both light and matter as having characteristics of waves and particles simultaneously.
  2. 4. Divisions of principal energy levels within an atom that are further divided into orbitals.
  3. 5. The electrons in the outermost energy level of an atom that are the ones most likely to be involved in chemical bonding.
  4. 6. A measure of the angular moment of an electron in an orbital.
  5. 8. The arrangement of electrons in an atom of an atom in its ground state.
  6. 11. The rule stating that electrons fill a sublevel by a single electron occupying each orbital before a second electron can occupy any orbital.
  7. 12. A notation or diagram used to illustrate the electron configuration of an atom, consisting of horizontal lines , representing the orbitals and labeled by sublevels, and arrows, representing the electrons in that orbital.
  8. 15. A shorthand method of representing atoms and their valence electrons, consisting of the atom’s chemical symbol with surrounding dots representing its valence electrons.
  9. 17. A charged atom or group of atoms due to the gain or loss of electrons.
  10. 18. An abbreviated form of electron configuration consisting of the last noble gasses in the configuration in brackets followed by any additional electron configuration for that element.
  11. 21. An incomplete spectrum, in the form of a series of coloured lines, that is unique for each element.