("Electron density" is another way of talking about how likely you are to find an electron at a particular place.)Ģs (and 3s, 4s, etc) electrons spend some of their time closer to the nucleus than you might expect. If you look carefully, you will notice that there is another region of slightly higher electron density (where the dots are thicker) nearer the nucleus. This is similar to a 1s orbital except that the region where there is the greatest chance of finding the electron is further from the nucleus - this is an orbital at the second energy level. s orbitals are spherically symmetric around the nucleus - in each case, like a hollow ball made of rather chunky material with the nucleus at its centre. The "s" tells you about the shape of the orbital. The "1" represents the fact that the orbital is in the energy level closest to the nucleus. The orbital occupied by the hydrogen electron is called a 1s orbital. 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. Note: If you wanted to be absolutely 100% sure of where the electron is, you would have to draw an orbital the size of the Universe! You can think of an orbital as being the region of space in which the electron lives. Such a region of space is called an orbital. The diagram shows a cross-section through this spherical space.ĩ5% 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. In the hydrogen case, the electron can be found anywhere within a spherical space surrounding the nucleus. 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. You have no idea how it got from the first place to the second. Soon afterwards, you do the same thing, and find that it is in a new position. Suppose you had a single hydrogen atom and at a particular instant plotted the position of the one electron. Note: In this diagram (and the orbital diagrams that follow), the nucleus is shown very much larger than it really is. Note: Over the years I have had a steady drip of questions from students in which it is obvious that they still think of electrons as orbiting around a nucleus - which is completely wrong! I have added a page about why the idea of orbits is wrong to try to avoid having to say the same thing over and over again! If something is impossible, you have to accept it and find a way around it. That makes it impossible to plot an orbit for an electron around a nucleus.
(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.) The Heisenberg Uncertainty Principle says - loosely - that you can't know with certainty both where an electron is and where it's going next. 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. The impossibility of drawing orbits for electrons It is essential that you understand the difference between them. Orbits and orbitals sound similar, but they have quite different meanings.
The truth is different, and electrons in fact inhabit regions of space known as orbitals.
A simple view of the atom looks similar and you may have pictured the electrons as orbiting around the nucleus. When a planet moves around the sun, you can plot a definite path for it which is called an orbit. d orbitals are described only in terms of their energy, and f orbitals only get a passing mention. It explores s and p orbitals in some detail, including their shapes and energies. This page explains what atomic orbitals are in a way that makes them understandable for introductory courses such as UK A level and its equivalents.
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