Bonding duet rule

Lewis structure Duet rule Octet rule Bonding pair... 

When atoms form covalent bonds, they try to attain a valence-electron configuration similar to that of the nearest noble gas element. Thus hydrogen in a bond would have two electrons (like helium, the duet rule) and others would have eight electrons (like neon and argon, the octet rule). 

In writing Lewis structures for molecules, what is meant by the duet rule To which element does the duet rule apply What do we mean by the octet rule Why is attaining an octet of electrons important for an atom when it forms bonds to other atoms What is a bonding pair of electrons What is a nonbonding (or lone) pair of electrons ... 

However, this is not the only way to pair up the electrons in the molecule. If you were a stavmch adherent of the octet rule, you could have shifted one of the electron pairs of the F O bond in the electron-rich formulation and placed these two electrons on oxygen. Since oxygen gained now an electron, and phosphorus lost one, the FMD bond will become a single bond, but its atoms will be charged, which we can represent as 0 . Now, all the atoms obey the octet rule (and H obeys the duet rule), and we all have peace... 

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). 

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. 

In drawing Lewis structures for covalently bonded molecules, the octet rule is used as a guide (remember that for hydrogen the octet is changed to a duet). Shared electrons count toward the electron total for both atoms in the bond. For example, the Lewis structure for SiH4 looks like this ... 

Arrange the remaining electrons as lone pairs or create double or triple bonds to satisfy the octet rule. Exceptions Hydrogen satisfies the duet (two) rule, and boron and aluminum satisfy the six-electron rule. 

The hydrogen atom duets are satisfied, but we would need two additional electrons to satisfy the octet rule for the carbon atoms. Since these are not available, we can satisfy the octet rule by adding the two remaining electrons as another pair between the carbon atoms to form what is called a double bond ... 

Atoms with eight valence electrons are particularly stable and are said to have an octet. Atoms such as hydrogen, helium, lithium, and beryllium are exceptions to the octet rule as they achieve stability when their outermost shell contains two electrons—a duet. A chemical bond is the sharing or transfer of electrons to attain stable electron configurations among the bonding atoms. 

Rule 3. (The octet rule) Depict all covalent bonds by two shared electrons, giving as many atoms as possible a surrounding electron octet, except for H, which requires a duet. Make sure that the number of electrons nsed is exactly the number counted according to rule 2. Elements at the right in the periodic table may contain pairs of valence electrons not used for bonding, called lone electron pairs or just lone pairs. 

Lewis structures describe bonding by the use of valence electron dots. They are drawn so as to give hydrogen an electron duet and the other atoms electron octets (octet rule). Formal charge separation should be minimized but may be enforced by the octet rule. 

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