Noble gas electron

Which of the following ions possess a noble gas electron... 

Transfer of an electron from a sodium atom to a chlorine atom yields a sodium cation and a chloride anion both of which have a noble gas electron configuration... 

Reduction of MCI5 or MCI3 under an atmosphere of CO yields salts of the [M(C06] ions (M = V, Nb, Ta) which have the noble gas electron configuration. Using Na as reductant... 

This is reasonable noble-gas atoms must have an extremely stable electronic structure, because they are so unreactive. Other atoms might be expected to acquire noble-gas electronic structures by losing or gaining electrons. 

As pointed out in Chapter 2, elements close to a noble gas in the periodic table form ions that have the same number of electrons as the noble-gas atom. This means that these ions have noble-gas electron configurations. Thus the three elements preceding neon (N, O, and F) and the three elements following neon (Na, Mg, and Al) all form ions with the neon configuration, is22s22p6. The three nonmetal atoms achieve this structure by gaining electrons to form anions ... 

Cations, anions, and atoms with ground state noble-gas electron cnnfigurations. Atoms and ions shown in the same color are isoelectronic tint. is. they have the same electron configiratiorts. 

These examples illustrate the principle that atoms in covalently bonded species tend to have noble-gas electronic structures. This generalization is often referred to as the octet rule. Nonmetals, except for hydrogen, achieve a noble-gas structure by sharing in an octet of electrons (eight). Hydrogen atoms, in molecules or polyatomic ions, are surrounded by a duet of electrons (two). 

Clearly the explanation of the chemical bond given by Kossel cannot apply to homonuclear molecules such as CI2. Almost simultaneously with the publication of Kossel s theory, Lewis published a theory that could account for such molecules. Like Kossel, Lewis was impressed with the lack of reactivity of the noble gases. But he was also impressed by the observation that the vast majority of molecules have an even number of electrons, which led him to suggest that in molecules, electrons are usually present in pairs. In particular, he proposed that in a molecule such as CI2 the two atoms are held together by sharing a pair of electrons because in this way each atom can obtain a noble gas electron arrangement, as in the following examples ... 

Ions can be isoelectronic without having noble-gas electron configurations. An example is Cu+ and Zn2+, which both have the electron configuration [Ar] 3dw. 

Three of the ions have noble gas electron configurations and thus have no unpaired electrons F is s12s12p6 Ca2+ and S2 are [Ne]3s23/ 6... 

Next, we need to distribute the remaining electrons to achieve a noble gas electron configuration for each atom. Since four electrons were used to form the two covalent single bonds, fourteen electrons remain to be distributed. By convention, the valence shells for the terminal atoms are filled first. If we follow this convention, we can close the valence shells for both the nitrogen and the chlorine atoms with twelve electrons. 

Ti should not display a +6 oxidation state, because in order for Ti to display a +6 oxidation state, two electrons would have to be removed from the noble gas electron configuration of Ar. This is quite unlikely. 

D. The noble gas electron configuration of the singly charged positive ion... 

The tendency of atoms to make the number of their valence electrons eight, like the nobel gases, is known as the octet rule. There are two ways for the elements to gain their octet and obtain a noble gas electron configuration. 

While forming compounds, all atoms tend to acquire noble gas electronic configuration. 

Why do atoms tend to acquire a noble gas electron configuration ... 

Step 3 Subtract the number of shared electrons from the number of valence electrons to get the number of non-bonding electrons. Add these electrons as lone pairs to the atoms surrounding the central atom so that you achieve a noble gas electron configuration for each atom. 

Each atom has achieved a noble gas electron configuration. The positive charge on the ion is included. This is a reasonable Lewis structure for NH4+. 

---