CM-UY 1004 Lecture Notes - Lecture 5: Pauli Exclusion Principle, Principal Quantum Number, Atomic Orbital

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25 Aug 2016

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Bohr"s model, assumed electrons move in circular orbits a. i. A charged particle should lose energy and spiral into positively charged nucleus: three postulates b. i. Only orbits of certain radii corresponding to certain specific energies are permitted for the electron in a hydrogen atom b. ii. An electron in a permitted orbit is in an allowed energy state. An electron in an allowed energy state does not radiate energy and does not spiral into the nucleus b. iii. Energy is emitted or absorbed by the electron only as the electron changes from one allowed energy state to another. This energy is emitted or absorbed as a photon that has energy. Impossible for us to know the momentum of the electrum and its exact location in space: x, the uncertainty in position and (mv), uncertainty in momentum c. i. As n increases, the orbital becomes larger and the electron spends more time further from the nucleus d. i. 2.

Related Questions

Which of the following statements about the Bohr model of the hydrogen atom is false?

	a.	The energy of each Bohr orbit is quantized.
	b.	An electron in a stationary state does not emit radiation.
	c.	When an electron jumps from one state to another, the electron must gain or lose just the right amount of energy to actually travel the distance between the orbits.
	d.	When an electron jumps to a higher state, energy is absorbed.
	e.	When an electron falls to a lower state, energy is emitted.
	f.	All of the above are correct

CHEM 1430 LIGHT LAB SPRING 2018 A Danish physicist, Neils Bohr, a post-doctoral student in J. J. Thomson's lab and friend of Rutherford, took up the problem of electron arrangement within the atom. Bohr's breakthrough was recognizing Balmer's fixed emission wavelengths, when taken with Planck's Relationship, led to the conclusion the shells, like the radiation emitted, must be quantized (have set, specific energles). Bohr proposed the electrons circulated about the madeus, much like planets cirde surãin seres of concentric shells of increasing size. Each shell stood at a fixed (set) distance from the nucleus with the shell nearest the nucleus taking the m and a shell further away taking the n in the B-R equation. The integral values of m and n taken with the discrete wavelength led Bohr to propose the shells were "quantized," meaning electrons could only exist at the surface of the shells. When an electron moved from a high shell, n, to a low shell, m, light of a foxed wavelength was emitted Bohr reasoned the shells were special due to this quantized nature. An electron in a shell occupied what Bohr described as a "steady state," meaning the electron could circulate about the nucleus without loss or gain of energy. This steady state proposition, which conflicted with classical physics, could not be explained by then available data but was required for Bohr's proposed structure to be stable. Later work revealed the wave-particle duality of the electron which lead to acceptance of the Steady State Proposition. The energy of an electron in any shell, represented by n, can be calculated using an equation derived from combining the Balmer-Rydberg and Planck equations. The energy of an electron in the no shell is given by é¦¯.h RL where hcR,-2.18x10-*) where Ru, is the Rydberg's Constant for the hydrogen atom, h is Planck's Constant and c is the speed of light NOTE: The energy is given a nexative value to refect the stabillting, attractive force between the negatively charged electron and the positively charged nucleus. As the shell number n increases, the attractive force decreases leading to a rising shell energies (E, increases, values less negative). ACTIVITY Calculate the energles for an electron in the first 7 shells of the hydrogen atom using the above relationship, recording the values in the center column of the Hydrogen the right-hand column in the table, convert the shell with the exponent of 10 Improper sclentific notation is typically used to plot data covering several orders of magnitude (powers of ten). Shell Energy Table. For energies to improper scientific notation Hydrogen Shell Energy Table Shell Value, n Calculated Shell Energy.ã Express Shell Energy in improper Scientific Notation, x 10-1 Page 9 of 12

CM-UY 1004 Lecture Notes - Lecture 5: Pauli Exclusion Principle, Principal Quantum Number, Atomic Orbital

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