Monday, May 3, 2021

Expanded Octets Resources | Wyzant Resources

zack May 03, 2021 No comments

The Octet Rule is a general rule that is used to describe chemical bonding and draw Lewis Structures. The rule states that Main Group elements form There are numerous other exceptions including expanded octets which can have up to twelve valence electrons. Even with the exceptions, the...Which elements cannot have expanded octets? Question.Which elements can exhibit expanded octet and have more than eight electrons around them? How is this rationalized?(Redirected from Expanded octet). A hypervalent molecule (the phenomenon is sometimes colloquially known as expanded octet) is a molecule that contains one or more main group elements apparently bearing more than eight electrons in their valence shells.-Elements In The Fourth Row Of The Periodic Table And Beyond Often Exhibit Expanded Octets. -Elements in the third row of the periodic table and beyond often exhibit expanded octets.

Which elements can have expanded octets? Which elements...

The Expanded Octet. In addition to the 3s and 3p orbitals, elements in and beyond the third period of the periodic table also have 3d orbitals available for bonding. There are more than eight valence electrons around the central atom in a number of compounds of those elements.The octet rule can be 'expanded' by some elements by utilizing the d-orbitals found in the third principal energy level and beyond. Deviations from the Octet Rule. A hypervalent molecule is a molecule that contains one or more main group elements that bear more than eight electrons in their...Elements which have d-orbitals (i. e. n=3 or higher) can form compounds with an expanded octet. Some examples are;Phosphorous Pentachloride PCl5Sulfur Hexafluoride SF6Dichloro Heptoxide Cl2O7. So are elements in row three and beyond which can have expanded octet structures.In expanded octets, the central atom can have ten electrons, or even twelve. Hence, the third period elements occasionally exceed the octet rule by using their empty d orbitals to accommodate additional electrons.

OneClass: Which elements can exhibit expanded octet and have...

In the Lewis model, a bond is a shared electron. Please explain which molecule could have an expanded octet?Some of the elements of the third-period and periods below can have expanded octet because they have d- sub-level. We have 2 possible answers. A and B. Because lodine and chlorine. Sulfur and phosphorous are in the 3d or lower periods. In the compound P2S5, where P forms 5 bonds.Expanded octet. Sections. Directory. References. Expanded octet. chemistry. Share. …of, without having to invoke octet expansion, by the distributed bonding effect of delocalized electrons. Consider SF 6 , which according to Lewis's theory needs to use two of its 3 d orbitals in addition to its four 3 s...Expanded octet occurs when an atom is able to have more than 8 valence electrons. For example, in SO₃, the sulfur atom forms 6 covalent bonds, hence it has 12 valence electrons. Expansion of octet is possible only from Period 3 elements onwards, d...In order to have an expanded octet, and atom has to have a d sublevel. (This allows paired electrons to split into two single electrons by using an additional orbital.) n=3 is the first energy level with a d-sublevel. So any element in periods 1 and 2 are automatically excluded, which in your list would be C...

Re: An rationalization of expanded octets?

Postby Irvin Xu 4I » Wed Oct 29, 2014 5:44 pm

Rarely, if ever, will you see a steel in the 3rd duration or upper be the central atom in a Lewis structure, because metals form ionic bonds, now not covalent ones (occassionally you'll see a smaller metalloid, like Boron, be the central atom and form covalent bonds). Since metals are "giving away" electrons, they will by no means have expanded octets because they wont have enough electrons to even use the d subshell. You can't in point of fact lower the formal rate of an entire structure, you can only disperse it such that it falls at the most electronegative atom(s) within the structure. Again, massive metals won't ever be the central atom, and won't use their d subshell.Hope this is helping.