Orbital notation

CHEMICAL SYMBOL ATOMIC NUMBER ORBITAL NOTATION Is 2s 2p ELECTRON CONFIGURATION NOTATION... 

In the spin-orbital notation used above, this state is ... 

PROBLEM 5.12 Give orbital notations for electrons in orbitals with the following quantum numbers ... 

SCHEME 22. MO-Schemee), PES data (eV), and structural parameters of the Group 14-decamethyl-metallocenes X-ray 6gED two independent molecules dtwo conformers in the unit cell in orbital notation for C2v symmetry... 

Fig. 9 presents the general qualitative energy levels and molecular orbital notations for SiH2 (D ), SiH2 (C2 ), SiX2 (C2v) and HSiX (Cs). The notation of Fig. 9 is used throughout. Contributions of X lone pairs have been neglected. 

You will express the arrangements of electrons in atoms through orbital notations, electron configurations, and electron dot structures. 

Write orbital notations and complete electron configurations for atoms of the following elements. 

Orbital notation provides a convenient way to visualize the loss or gain of valence electrons. When zinc metal reacts with sulfuric acid, the zinc forms a Zn + ion with a pseudo-noble gas configuration. 

Figure 8-5 summarizes the formation of an ionic compound from the elements sodium and chlorine using four different methods electron configuration, orbital notation, electron-dot structures, and atomic models. 

Formulating Models Use electron configurations, orbital notation, and electron-dot structures to represent the formation of an ioitic compound from the metal strontium and the nonmetal chlorine. 

Using orbital notation, diagram the formation of an ionic bond between aluminum and fluorine. 

The orbital notation of an element is related to the electron configuration, and both types of notation are often shown at the same time. The real difference in the two types of notation has to do with the level of detail shown. In electron configuration, no details are shown about the actual orbitals. When we see 3p4, we know that there are 4 electrons in the p sublevel, but we don t know in which orbitals the electrons are located. When we do the orbital notation for the element, we get that level of detail for the orbitals. 

The first step for doing the orbital notation is to do the electron configuration. You will then want to remember Hund s Rule, which states that the most stable arrangement of electrons in sublevels is the one with the greatest number of parallel spins. The way that we make use of this rule is to put one electron in each of the orbitals in a particular sublevel, before we double up the electrons in any particular orbital. 

When we write an orbital notation, the orbitals are represented by circles or squares, and the electrons are represented by arrows or slashes. For the sake of clarity, the orbital notation is usually accompanied by the proper electron configuration. 

One last thing In order to do orbital notation, you must be able to do electron configuration. So, if you haven t mastered Lesson 3-4, you should go back and do more practice. 

Write the proper orbital notation for an atom of aluminum. 

The first thing that we need to do is find the electron configuration for aluminum. Because we did this example in the last lesson, I won t go through the steps. Refer back to the last lesson if you don t remember how to do this. We will space the configuration out a bit more this time, so that we have room to write the orbital notation. 

Notice that you will not always fill in all of the circles that you draw. Aluminum only has one electron in the 3p sublevel, so only a single 3p orbital has an electron. For our next example, let s try an orbital notation in which Hund s Rule becomes more important. 

So, if you can do the electron configuration for an element, you should be able to do the orbital notation. Just study the examples from this lesson and make sure you understand them. 

Before we move on to the next lesson, I want to remind you that some books will represent the orbital notation in a slightly different fashion. Your instructor may have a preference for you to use in class, but you should be able to recognize any of the alternate versions that you might see. Figure 3-5a shows the three most common versions for the orbital notation of carbon. 

The following figure shows the orbital notations for six elements. Use these notations to answer questions 3-8. 

Which orbital notation matches up to each of the following elements ... 

Let s look at the Lewis dot notation for an atom of phosphorus. As you recall, the following is the electron configuration and the orbital notation that we found in the last lesson. 

Note that the sides, which represent the p orbitals, received only one dot each, just as the circles representing those same orbitals in the orbital notation for phosphorus received only one dot each. Hund s Rule instructs us to find an empty orbital for each p electron, until we need to double them up. Why, then, do the s electrons double up Because there is only one s orbital, the electrons in the s sublevel have no choice they must share the only s orbital. 

Next, let s compare the electron configuration and orbital notation of the element sulfur to its Lewis dot structure. Sulfur has six electrons in its valence shell, so its dot diagram will show six dots. Does the diagram below make it easier to see how the valence electrons are represented in the Lewis dot structure ... 

For our final example, let s try a chorine (Cl ) ion. We didn t do this example in Lesson 3-4, try it on your own and see if you get the same answer that I show in Figure 3-6c. Remember to go back and do the electron configuration and the orbital notation first, paying careful attention to the charge on the ion. Then construct the Lewis dot notation for the ion, and check it against the answer. 

Perhaps the most interesting thing about the Periodic Table of Elements is how much information is hidden in it. To the untrained eye, the periodic table appears to only show the elemental symbols, elemental names, atomic numbers, and atomic masses. However, someone who knows a bit more chemistry can squeeze much more information out of the same table. You will learn to use the periodic table to check your electron configurations, orbital notations, and Lewis dot notations. You will also learn to use the periodic table to check many relative properties of the elements, such as reactivity, electronegativity, and metallic character. All of this information is there, if you know how to use the table correctly. It is certainly in your best interest to learn as much about the periodic table as possible, because you are allowed to make use of it on many exams and quizzes. If you are able to extract all kinds of information from it, it becomes an incredibly useful cheat sheet, except that you re allowed to use it ... 

C.]—The orbital notation shown in answer C shows 17 arrows, representing the 17 electrons in the chlorine atom. 

D.] —Helium, with an electron configuration of Is2, can be represented by the orbital notation shown in answer D. 

A.]—A neutral atom of fluorine has 9 electrons, as does the orbital notation shown in answer A. 

---