Atomic Structure

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Anonymous
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205219
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Atomic Structure
Updated:
2013-03-05 19:42:18
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Chem
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atomic structure
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  1. Atomic Radii
    half the distance between adjacent nuclei in a crystal of an element.
  2. Ionization Energy
    energy required to remove an electron from a gaseous atom.
  3. General Atomic Radii trend across the period
    decrease
  4. General Atomic Radii trend down a family
    increase
  5. General Ionization energy trend across the period
    increases
  6. General Ionization Energy trend down a family
    decreases
  7. Electron Affinity
    energy change for the process of adding an electron to a neutral atom in the gaseous state, equivalent to ionization energy for nonmetals.
  8. Electronegativity
    indicates the relative ability of its atoms to attract electrons in a chemical bond. There is a sharing of electrons in a covalent bond, but the atom with the highest electronegativity pulls on the electrons harder.
  9. Electronegativity trends across a period
    increases
  10. Electronegativity trends down a family
    decreases
  11. Similar properties of elements are found in      .and the one major exception is              .
    Families. exception is the lanthanides, inner transition metals (f-block) they have similar properties across a period.
  12. In 1864, an English chemist that noticed when elements were arranged in order of increasing atomic mass, every eighth element had similar properties (law of octaves).
    John Newlands
  13. Russian chemist that arranged the elements by increasing atomic mass and into columns with similar properties. Predicted the existence of undiscovered elements.
    Dmitri Mendeleev
  14. "Father of the Periodic Table"
    Dmitri Mendeleev
  15. In 1913, discovered that atoms of each element contain a unique number of protons and this number was the atomic number of the element.
    Henry Moseley
  16. Arranged the elements by atomic number
    Henry Moseley
  17. Periodic Law
    There is a periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number.
  18. When did Max Planck introduce the quantum theory?
    1901
  19. Bohr applied quantum theory to atoms. What was the essence of Bohr's work?
    The electron in a hydrogen atom moves around in the nucleus only in certain allowable circular movements.
  20. Who published the Uncertainty principle in 1926?
    German physicist, Werner Heisenberg
  21. How does the quantum mechanics or wave mechanics model of the atom differ from the Bohr-Rutherford model of the atom develeped in 1915?
    Bohr said there are distinct or bits of shells, quantum mechanics say probable distance and the orbital size is described for the 1s radius is about 90% of the total electron probability.
  22. Pauli's Exclusion Principle
    No two electrons in the same atom may have the exact same four quantum numbers
  23. DeBroglie's Hypothesis
    Both matter and energy have dual behavior, not only does energy have particle and wave properties but small particles of matter exhibit both particle and wave properties.
  24. Heisenberg's Uncertainty Principle
    We can never know both the position and the momentum of an electron simultaneously;any experiment to measure one will necessarily cause a change in the other
  25. Schrodinger's Wave Equation
    This treats the wave behavior of an electron; it evaluates the energy of an electron by treating it as a wave
  26. The man who did the first theoretical calculations to put electrons in energy levels or shells based upon Planck's Quantum theory was           
    Niels Bohr

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