Electron configuration of noble gases

In summary, ionic bonds form when there is a transfer of electrons between atoms of different elements. The result of this transfer produces oppositely charged ions. The ions produced generally obtain the valence electron configuration of noble gases, that is, conform to the octet rule. The oppositely charged ions produced are held together by electrostatic attraction. This attractive force is the ionic bond. 

This rule states that elements will react in order to achieve eight valence electrons. This corresponds with the electronic configuration of noble gases and is the result of the s- and p-orbitals being filled (with the exception of He). Elements try to achieve noble gas configuration due to the stability that having eight valence electrons affords. 

All the isoelectronic species illustrated in the text had the electron configurations of noble gases. Can two ions be isoelectronic without having noble-gas electron configurations Explain. 

Each of these trends can be rationalized in terms of ground state electronic configurations. The noble gases (except for... 

Both the octet rule and the 18-electron rule connect stabihty to noble gas electron configurations. The noble gases in the second and third periods of the periodic table (Ne and Ar) have 8 valence electrons, those in the fourth and fifth (Kr and Xe) have 18. 

When atoms exchange or share electrons, they do so to reach a more stable state. The most stable state of an atom is reached when all of its electron shells are filled—like our old friends the noble gases. Table 4.1 in Chapter 4 gave the electron configurations of the... 

The charge on the nucleus and the number of electrons in the valence shell determine the chemical properties of the atom. The electron configurations of the noble gases (except for that of helium) correspond to a valence shell containing eight electrons—a very stable configuration called an... 

The noble gases, located at the end of each period, have electron configurations of the type ns2np6, where n represents the number of the outermost shell. Also, n is the number of the period in the periodic table in which the element is found. 

It must be emphasized that the octet rule does not describe the electron configuration of all compounds. The very existence of any compounds of the noble gases is evidence that the octet rule does not apply in all cases. Other examples of compounds that do not obey the octet rule are BF,. PF5, and SF6. But the octet rule does summarize, systematize, and explain the bonding in so many compounds that it is well worth learning and understanding. Compounds in which atoms attain the configuration of helium (the duet) are considered to obey the octet rule, despite the fact that they achieve only the duet characteristic of the complete first shell of electrons. 

As mentioned previously, in 1916, Lewis noted that noble gases were particularly stable and did not form compounds. Lewis used these facts to formulate the octet rule. The noble gases have their outer electron shell filled with eight electrons. (Helium is an exception with only two electrons in its outer shell.) The octet rule says that the most stable electron configuration of an atom occurs when that atom acquires the valence electron configuration of a noble gas. That is, when an atom can acquire eight (octet) electrons in its valence shell (or two for hydrogen to become like helium). 

Atoms form bonds in order to obtain a stable electronic configuration, i.e. the electronic configuration of the nearest noble gas. All noble gases are inert, because their atoms have a stable electronic configuration in which they have eight electrons in the outer shell except helium (two electrons). Therefore, they cannot donate or gain electrons. 

Table 9.1 shows the electronic structure of the first three elements of Group I. You will notice in each case that the outer energy level contains only one electron. When these elements react they lose this outer electron, and in doing so become more stable, because they obtain the electron configuration of a noble gas. You will learn more about the stable nature of these gases later in this chapter (p. 143). 

Although helium has an electron configuration of Is2, it is shown in the group of noble gases. Explain. 

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