What is the lewis structure for RnF2 [Solved]

see the pic for extra element

Reply 6

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Reply 6

Reply : (1) The variety of valence electrons current within the compound is, 20 (2) The variety of bonded electrons current within the compound is, 4 (3) The variety of lone pair electrons current within the compound is, 16 (4) The variety of single bonds current within the compound is, 2 Clarification : Lewis-dot construction : It reveals the bonding between the atoms of a molecule and it additionally reveals the unpaired electrons current within the molecule. Within the Lewis-dot construction the valance electrons are proven by dot. The given molecule is, As we all know that oxygen has 6 valence electrons and fluorine has 7 valence electrons. Due to this fact, the full variety of valence electrons in = 6 2(7) = 20 In line with Lewis-dot construction, there are 4 variety of bonding electrons and 16 variety of non-bonding electrons or lone pair of electrons. The Lewis-dot construction of is proven under.

see the pic for extra element

Clarification: Under is an attachment containing the answer.

See hooked up image. Clarification: Good day. As youll be able to see on the hooked up image, this Lewis construction requires all the weather to achieve eight electrons after bonding, thats the reason the phosphorous is bonded with the 2 carbon atoms through a single bond with the carbon having the three fluorine atoms and a double bond with the carbon having the 2 carbon atoms. Such association is because of the truth that: P will get eight electrons by acquiring three from the 2 sided carbon atoms. The primary carbon will get eight electrons from its preliminary 4, three supplied by every surrounding fluorine and one from the central phosphorous. Every fluorine will get eight valence electrons from their preliminary seven and one from the out there carbon atoms. Finest regards.

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Reply 7

Sulfur and Fluorine are nonmetals so they may kind covalent bonds to achieve stability. To take action, they may observe the octet rule: they may share sufficient electrons in order to have their valence shell full with 8 electrons. Sulfur is within the Group 16 within the Periodic Desk and has 6 valence electrons. Thus it should share 2 pairs of electrons to achieve the octet. Fluorine is within the Group 17 within the Periodic Desk so every F has 7 valence electrons. Thus, every F must share 1 pair of electrons to achieve the octet. As a consequence, they are going to be bonded within the order F S F, with a single bond between every pair of atoms.

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