Bohr Theory, Page 2

Frequency

Frequency is the measure of the number of waves that pass of given point in space in a defined period of time. It is a variable used to describe light that has its origins in treating light as if it were a wave.

Ground State

The Ground State according to Bohr Theory is the position on an energy level diagram that the electron is located in under normal conditions, such as room temperature. When located at Ground State, the electron is in the orbit that is closest to the nucleus and has the least allowed quantity of energy. It is the position of maximum stability for an electron on an atom. An electron that is not located in the Ground State, or position of greatest stability, will be located in the Excited State.

Heisenberg Uncertainty Principle

The Heisenberg Uncertainty Principle is a concept that was originally based on a mathematical equation. The equation was developed by Werner Heisenberg. The introduction of this concept caused scientists to rethink the behavior of all matter. In essence, it places limitations on what information can be know about a specific block of matter. More on Heisenberg

The Heisenberg Uncertainty Principle is a mathematical concept. It states that it is impossible to know both the position and momentum of an object precisely at any given instant in time. The mathematical relationship between these two ideas is inverse, or indirect. The more that is known about one of the two terms, the less that is known about the other. Amongst its many interpretations is the idea that in measuring either location or momentum for an object, the concept being measured will actually be changed. Bohr Theory ran into trouble with this principle because Bohr tried to predict the movement of the electron too precisely. By restricting the electron to certain locations on the atom and having it move in paths called orbits, he violated the Heisenberg Uncertainty Principle. The Modern Theory of Atomic Structure, created by Schrodinger, eventually solved the problem of Bohr's conflict with the Heisenberg Uncertainty Principle.

Orbit

According to Bohr Theory an orbit is the path that an electron follows as it moves around the nucleus.

The orbits appear as a series of concentric circles with their centers located at the nucleus. This idea will eventually be replaced with the concept of the orbital in the Modern Theory of Atomic Structure. The concept of the orbit should not be confused with the term known as the orbital. This term was introduced in the Modern Theory of Atomic Structure and represents a much different idea.

Photon

A photon is a packet of energy. A series of photons, or energy packets, passing through space is considered as one of two common models used for describing light. The idea of the photon arises from work down by Max Planck. Planck claimed that light could be described as energy packets. The distance between these energy packets corresponds to the light variable known as wavelength. The number of photons passing a point in space in a defined period of time corresponds to the light variable known as frequency.

Max Planck

Max Planck developed the Particulate Theory of Light. This theory says that light can be treated as a series of energy packets called photons. The size of the energy packets, measured as energy content, can vary and, as they do so, they change the color of the light.

This idea restricts the electron to having certain very specific quantities of energy. In other words, the electron was not allowed to have any random value of energy. The energy is said to be quantized, meaning limited to specific quantities. This idea was initially controversial, when first introduced. Eventually, it became widely accepted, and it provided Bohr with the final piece of information needed to complete his theory of basic electronic behavior.

Quantum Jump

A Quantum Jump is also an electron transition. It occurs when an electron moves from one energy level to another. It does so by gaining or losing energy in continuously changing amounts. In essence, at one instant the electron has a specific quantity of energy and then suddenly has a larger or smaller quantity without having any level of energy content between those two amounts. This radical idea was first developed by Max Planck. Once Bohr applied this concept to his description of the electron's behavior, he was able to move forward with his theory.

Wavelength

Wavelength is the distance between correspond points on adjacent waves. It is a variable used to describe light that has its origins in treating light as if it were a wave.

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