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Exceptions to the Octet Rule 1. odd number of electrons ex. NO 2. central atom has less than an octet ex. BF 3 Exceptions to the Octet Rule 3. central atom has more than an octet of e–’s expanded valence possible for larger central atoms in the 3rd period and below ex. PCl 5 XeF 4

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For example, I knew that the first covalent compound needed an expanded octet. After doing the Lewis diagram, I realized that bromine had twelve electrons in its valence shell, so it needed an expanded octet. I knew that the seventh covalent compound needed a resonance structure.

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Octet deficient Expanded octet Online Classes : [email protected] www.youtube.com/megalecture www.megalecture.com 5) An example is the reaction between ammonia and hydrogen chloride.

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Oxygen belongs to the 2 group, and thus doesn't have an empty d - orbital, so it can't have more than an octet of electrons. Same goes for Nitrogen. Bromine belongs to group 4, thus has empty d - orbitals, and can expand further than Sulfur can - it can have more than an octet of electrons. Solution = { Carbon, Oxygen, Nitrogen }

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Explanation: 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.

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Each chlorine atom has completed its octet of electrons, but the central phosphorus atom has a share in 10 valence electrons which is 2 more than an octet of electrons. The valence shell of the phosphorus atom is said to have expanded in order to accommodate all 5 bonding pairs of electrons.

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Argon compounds have been synthesised and have expanded octets. Some researchers argue that the expanded-octet structures of the oxides, oxoacids and oxoanions of the 3p–5p non-metals (e.g. P, As, S, Se, Te, Cl, Br, I and Xe) are more consistent with experimental bond lengths than structures that obey the octet rule.

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Currently, she is studying law in University of Mumbai. The noble gases are unreactive because of their electron configurations. [3] This completes the explanation of the octet rule in this case. [2] Thus sodium will, in most cases, form a compound in which it has lost a single electron and have a full outer shell of eight electrons, or octet.

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Following on from discussing octet expansion in species such as SeMe 6, ClMe 3 and ClMe 5, I felt impelled to return to SF 6, often used as an icon for hypervalence.. With this molecule we have twelve electrons to partition, six from sulfur and one each from six fluorines (the other six electrons on each F are presumed to form three sets of lone pairs).

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