Quantum

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Author:
jfindley
ID:
266217
Filename:
Quantum
Updated:
2014-03-12 18:30:43
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Chemistry
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  1. Where are lower energy levels?
    closer to the nucleus
  2. Where are high energy levels?
    farther from nucleus
  3. What is quantum?
    energy needed for an electron to jump from ground to excited state
  4. What is ground state?
    electrons in lowest energy level possible
  5. What is an excited atom?
    • electrons move to higher energy levels when an atom gains energy
    • unstable
    • atom soon emits the same amount of energy absorbed which is seen as visible light
  6. What is the speed of light?
    3.0 x 108   
  7. What is the equation for c?
    c=wavelength x frequency
  8. what is the energy equation?
    e= h x f
  9. What is Plank's constant?
    h= 6.626 x 10-34
  10. What is electromagnetic radiation?
    • form of energy that exhibits wavelike behaviors as it travels through space
  11. What is the electromagnetic spectrum?
    encompasses all forms of electromagnetic radiation
  12. What is photoelectric effect?
    photo electrons emitted from metal's surface when light of specific frequency strikes it
  13. What is a photon?
    particle of electromagnetic radiation with no mass that carries a quantum of energy
  14. What is atomic emission spectrum?
    set of frequencies of the electromagnetic waves emitted by atoms of an element
  15. Who proposed the quantum model?
    Neils Bohr
  16. What did Louis deBroglie propose?
    • electron wave-particle duality
    • all moving particles exhibit wavelike characteristics
  17. What did Heisenburg's uncertaincy principle say?
    it is impossible to know both the velocity and position of a particle at the same time
  18. What did Edwin Schodinger do?
    • developed quantum mechanical model of the atom
    • predicts probable location of an electron
    • electrons treated as waves and not in circular orbits
  19. What does a s look like?
    sphere
  20. What does p look like?
    dumbell
  21. What does d look like?
    double dumbell
  22. What is Aufabau principle?
    each electron occupies the lowest energy level possible
  23. What is Pauli eclusion priciple?
    • only two electrons with oppposite spins can occupy an orbital¬†
    • no 2 electrons within the same element habe the same 4 quantum numbers
  24. What is Hund's Rule?
    single electrons with the same spin must occupy each equal energy orbital before electrons can be paired
  25. What are Valence electrons?
    electron in atom's highest energy levels
  26. what is n?
    principle quantum number
  27. what is l?
    • describes the orbital shape within an energy level
    • sublevel
  28. How many electorons can an orbital hold?
    2
  29. How many orbitals does s have?
    2
  30. How many orbitals does p have?
    3
  31. How many orbitals does d have?
    5
  32. How many orbitals does f have?
    7
  33. What is m?
    describes the orentation of orbital in space
  34. What is s (quantum number)?
    describes spin of electron orbital

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