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ATOMIC orbitals!

ATOMIC orbitals!. http://atomictimeline.net//index.php.

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ATOMIC orbitals!

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  1. ATOMIC orbitals!

  2. http://atomictimeline.net//index.php When the a planet moves around the sun, you can plot a definite path for it which is called an orbit. A simple view of the atom looks similar and you may have pictured the electrons as orbiting around the nucleus. The truth is different, and electrons in fact inhabit regions of space known as orbitals. Orbits and orbitals sound similar, but they have quite different meanings. It is essential that you understand the difference between them.

  3. http://atomictimeline.net//index.php To plot a path for something you need to know exactly where the object is and be able to work out exactly where it's going to be an instant later. You can't do this for electrons. The Heisenberg Uncertainty Principle says - loosely - that you can't know with certainty both where an electron is and where it's going next. (What it actually says is that it is impossible to define with absolute precision, at the same time, both the position and the momentum of an electron.) That makes it impossible to plot an orbit for an electron around a nucleus. Is this a big problem? No. If something is impossible, you have to accept it and find a way around it.

  4. Hydrogen's electron - the 1s orbital Suppose you had a single hydrogen atom and at a particular instant plotted the position of the one electron. Soon afterwards, you do the same thing, and find that it is in a new position. You have no idea how it got from the first place to the second. You keep on doing this over and over again, and gradually build up a sort of 3D map of the places that the electron is likely to be found. In the hydrogen case, the electron can be found anywhere within a spherical space surrounding the nucleus. The diagram shows a cross-section through this spherical space.

  5. 95% of the time (or any other percentage you choose), the electron will be found within a fairly easily defined region of space quite close to the nucleus. Such a region of space is called an orbital. You can think of an orbital as being the region of space in which the electron lives. What is the electron doing in the orbital? We don't know, we can't know, and so we just ignore the problem! All you can say is that if an electron is in a particular orbital it will have a particular definable energy.

  6. http://hti.math.uh.edu/curriculum/units/1999/02/07/99.02.07.phphttp://hti.math.uh.edu/curriculum/units/1999/02/07/99.02.07.php

  7. http://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.htmlhttp://chemed.chem.purdue.edu/genchem/topicreview/bp/ch6/quantum.html The three coordinates that come from Schroedinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.

  8. The principal quantum number (n) describes the size of the orbital. Orbitals for which n = 2 are larger than those for which n = 1, for example. Because they have opposite electrical charges, electrons are attracted to the nucleus of the atom. Energy must therefore be absorbed to excite an electron from an orbital in which the electron is close to the nucleus (n = 1) into an orbital in which it is further from the nucleus (n = 2). The principal quantum number therefore indirectly describes the energy of an orbital. The angular quantum number (Azimuthal Quantum Number) (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger There is only one way in which a sphere (l = 0) can be oriented in space. Orbitals that have polar (l = 1) or cloverleaf (l = 2) shapes, however, can point in different directions. We therefore need a third quantum number, known as the magnetic quantum number (m), to describe the orientation in space of a particular orbital. (It is called the magnetic quantum number because the effect of different orientations of orbitals was first observed in the presence of a magnetic field

  9. Na Sodium 23 1s2 2s2 2p6 3s1 (2,8,1) Na 11 1s2 2s22p63s1 angular momentum number principal quantum number

  10. max number of e- type of orbital parts s p d f 1 3 5 7 2 6 10 14

  11. 1s 2s 3s 4s 5s 6s 7s 2p 3p 4p 5p 6p 3d 4d 5d 4f list a sequence here

  12. Scribble by Mr G

  13. http://dbhs.wvusd.k12.ca.us/webdocs/Electrons/QuantumNumbers.htmlhttp://dbhs.wvusd.k12.ca.us/webdocs/Electrons/QuantumNumbers.html • Rules Governing the Allowed Combinations of Quantum Numbers • The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, 2, 3, and so on. • The principal quantum number (n) cannot be zero. The allowed values of n are therefore 1, 2, 3, 4, and so on. • The angular quantum number (l) can be any integer between 0 and n - 1. If n = 3, for example, l can be either 0, 1, or 2. • The magnetic quantum number (m) can be any integer between -l and +l. If l = 2, m can be either -2, -1, 0, +1, or +2.

  14. = nucleus

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