Bohrs model of the hydrogen atom

In the Bohr model of the hydrogen atom, an electron travels in a circular orbit about the nucleus at approximately 5 x 10 mlles Per hour How many rev°-lutions per second does the electron make if the radius of the orbit is 2 x 10"9 inches ... 

Figure 4.3 The Bohr model of the hydrogen atom. The radii of the electron orbits were determined by the model.

Figure 4.4 A. diagram of the Bohr model of the hydrogen atom as shown by Arnold Sommerfeld in Atomic Structure and Spectral Lines. The radii of the pictured orbits n = 2 and w = 3 are four times and nine times larger than the radius = 1. Orbits forw = 4, 5, 6, and so on are even larger. Spectral lines originate when the atom passes from one energy state, w = 3, to others, n = 2 and n = 1, as pictured.

Why is the Bohr model of the hydrogen atom referred to as the solar system model ... 

The initial enthusiasm for the Bohr model of the atom began to fade soon after its introduction. New discoveries in modern physics indicated that Bohr s ideas needed to be modified. The Bohr model of the hydrogen atom pinpointed both the electron s energy and its distance from the nucleus at exactly the same time. However, the Uncertainty Principle of Heisenberg required that if the energy of the electron is known exactly there must be uncertainty concerning its location. Both could not be known exactly at the same time. 

In the Bohr model of the hydrogen atom, the electron can reside in orbits of known, fixed radius. In the quantum mechanical model, the location of the electron is not known exactly rather, its location is described in terms of the probability of being at a given point about the nucleus. 

Orbital hybridization, like the Bohr model of the hydrogen atom in its ground state, is an effort to dress up a defective classical model by the assumption ad hoc of quantum features. The effort fails in both cases because the quantum-mechanics of angular momentum is applied incorrectly. The Bohr model assumes a unit of quantized angular momentum for the electron which is presumed to orbit the nucleus in a classical sense. Quantum-mechanically however, it has no orbital angular momentum. The hybridization model, in turn, spurns the commutation rules of quantized... 

An atomic orbital is usually described in terms of three integral quantum numbers. We have already encountered the principal quantum number, n, in the Bohr model of the hydrogen atom. The principal quantum number is a positive integer with values lying between the limits 1 < n < oo allowed values arise when the radial part of the wavefunction is solved. 

Figure 3.25 Neils Bohr, who in 1913 postulated the Bohr model of the hydrogen atom, from which derives the notion of electronicshellsthat initiated the modern atomictheory of chemical reactions, as well as the concept of energy levels that underlie the design of lasers. (Published with permission from the Deutsches Museum, Munich.)...

Characterize the Bohr model of the atom. In the Bohr model, what do we mean when we say something is quantized How does the Bohr model of the hydrogen atom explain the hydrogen emission spectrum Why is the Bohr model fundamentally incorrect ... 

The Bohr model of the hydrogen atom postulated that the electron moved in circular orbits corresponding to the various allowed energy levels. Though it worked well for hydrogen, the Bohr model did not work for other atoms. 

BOHR MODEL OF THE HYDROGEN ATOM (SECTION 6.3) Dispersion of radiation into its component wavelengths produces a spectmm. 

The ease with which electrons can be removed from an atom or ion has a major impact on chemical behavior. The ionization energy of an atom or ion is the minimum energy required to remove an electron from the ground state of the isolated gaseous atom or ion. We first encountered ionization in our discussion of the Bohr model of the hydrogen atom. CEO (Section 6.3) If the electron in an H atom is excited from n = 1 (the ground state) to = the electron is completely removed from the atom the atom is ionized. 

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