Chemistry 112
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Chemistry 112. Models of the Atom. Development of Atomic Models. A shortcoming of the discovery of the nucleus and advancements in an atomic model was that it failed to explain chemical behavior A model that focused on the electron was needed

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Chemistry 112

Chemistry 112

Models of the Atom


Development of atomic models
Development of Atomic Models

  • A shortcoming of the discovery of the nucleus and advancements in an atomic model was that it failed to explain chemical behavior

  • A model that focused on the electron was needed

  • Bohr built on Rutherford’s model to include the energy within an atom

    • He suggested that electrons existed within circular paths, called orbitals, outside the nucleus

    • Every electron within an orbital possesses a certain amount of energy

      • They were then called energy levels


The energy of electrons
The Energy of Electrons

  • The e- with the lowest energy are found in the first energy level

  • e- can move from one orbital to another but only if it gains or loses energy

  • The further an e- is away from the nucleus, the more energy it possesses

  • The amount of energy an e- must absorb/release to move from one orbital to another is called a quantum

    • The amount of energy to move from one orbital to the next is not always the same


Bohr s model
Bohr’s Model

  • The model of the atom was better understood but still failed to explain all the properties of atoms with atomic numbers greater than hydrogen

  • Information was being gathered by other scientists on waves and energy that did not correspond with Bohr’s model


Quantum mechanical model
Quantum Mechanical Model

  • Schrodinger used information about electron motion to devise and solve a mathematical equation that described the behavior of the electron

  • The amount of energy an e- possesses is still considered fixed but the pathway is not

  • QMM takes into consideration the amount of energy an e- has and how likely it is to be found in a certain location (probability)

  • e- are most likely to be found close to the nucleus


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