![]() ![]() Electrons are no longer thought of as being randomly distributed around a nucleus or restricted to certain orbits (in that regard, Bohr was wrong). Quantum mechanics predicts two major things: quantized energies for electrons of all atoms (not just hydrogen) and an organization of electrons within atoms. However, later researchers generalized Bohr’s ideas into a new theory called quantum mechanics The theory of electrons that treats them as a wave., which explains the behavior of electrons as if they were acting as a wave, not as particles. Figure 8.5 "Bohr’s Model of the Hydrogen Atom" shows a model of the hydrogen atom based on Bohr’s ideas.įigure 8.5 Bohr’s Model of the Hydrogen Atomīohr’s description of the hydrogen atom had specific orbits for the electron, which had quantized energies.īohr’s ideas were useful but were applied only to the hydrogen atom. This means that only certain frequencies (and thus, certain wavelengths) of light are emitted. Finally, Bohr suggested that the energy of light emitted from electrified hydrogen gas was equal to the energy difference of the electron’s energy states: E light = h ν = Δ E electron Because the energies of the electron can have only certain values, the changes in energies can have only certain values (somewhat similar to a staircase: not only are the stair steps set at specific heights but the height between steps is fixed). Bohr suggested that the energy of the electron in hydrogen was quantized because it was in a specific orbit. Quantities that have certain specific values are called quantized When a quantity is restricted to having only certain values. ![]() He suggested that the electron in a hydrogen atom could not have any random energy, having only certain fixed values of energy that were indexed by the number n (the same n in the equation above and now called a quantum number An index that corresponds to a property of an electron, like its energy.). In 1913, the Danish scientist Niels Bohr suggested a reason why the hydrogen atom spectrum looked this way. The spectrum of hydrogen was particularly simple and could be predicted by a simple mathematical expression. It turns out that every element has its own unique, characteristic line spectrum. This image is called a line spectrum An image that contains only certain colors of light. However, when electricity is passed through a gas and light is emitted and this light is passed though a prism, we see only certain lines of light in the image (part (b) in Figure 8.3 "Prisms and Light"). This image is known as a continuous spectrum An image that contains all colors of light. We notice this when the visible portion of the electromagnetic spectrum is passed through a prism: the prism separates light into its constituent colors, and all colors are present in a continuous rainbow (part (a) in Figure 8.3 "Prisms and Light"). ![]() Incandescent lights and fluorescent lights generate light via these two methods, respectively.Ī hot object gives off a continuum of light. There are two fundamental ways of generating light: either heat an object up so hot it glows or pass an electrical current through a sample of matter (usually a gas). Learn the quantum numbers that are assigned to electrons.zip file containing this book to use offline, simply click here. You can browse or download additional books there. More information is available on this project's attribution page.įor more information on the source of this book, or why it is available for free, please see the project's home page. Additionally, per the publisher's request, their name has been removed in some passages. However, the publisher has asked for the customary Creative Commons attribution to the original publisher, authors, title, and book URI to be removed. Normally, the author and publisher would be credited here. ![]() This content was accessible as of December 29, 2012, and it was downloaded then by Andy Schmitz in an effort to preserve the availability of this book. See the license for more details, but that basically means you can share this book as long as you credit the author (but see below), don't make money from it, and do make it available to everyone else under the same terms. This book is licensed under a Creative Commons by-nc-sa 3.0 license. ![]()
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