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Determine the number of bonding electrons and the number of nonbonding electrons in the structure of OF2. Enter the number of bonding electrons followed by the number of nonbonding electrons in the dot structure of this molecule separated by a comma (e.g., 1,2).

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Answer:

(4,20)

Explanation:

Oxygen di-fluoride or OF2 is a polar molecule, formed through the covalent bonding between one Oxygen and two Fluorine atoms.

Oxygen has atomic no. 8 and its electronic configuration is as below:

  • 1s^2, 2s^2, 2p^4

Oxygen has 4 electrons in the valence shell. It has the ability to share two electrons with other atoms through covalent bond and get stable.

The atomic number of Fluorine is 7, and its electronic configuration is as:

  • 1s^2, 2s^2, 2p^5

So, Fluorine atom  has the capacity to accept 1 electron to form 1 covalent bond or in the formation of the F- ion.  

The structure of OF2 is a bent structure with O atom sandwiched by two fluorine atoms like F-O-F. So there are two electrons on oxygen atom that are taking part in the formation of covalent bond with each Fluorine atom (Please dot structure in figure).

Now we can easily calculate no of bonding and non-bonding electrons.

  • No. of bonding electrons = 4 (two from oxygen and two from fluorine atoms each)
  • No. of non-bonding electrons= 20 (6+6 from two Fluorine atoms and 6 from Oxygen atom)

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OF2-

O has 6 electrons in its outer shell and F has 7 electrons in its outer shell

Further Explanation

Therefore, you want to account for a complete of 20 electrons in

structure (7 + 7 + 6 = 20)

therefore draw linear first. F ---- O ----- F

Two bonds make sure of 4 electrons now you have got to feature 16 others.

Therefore 3 free pairs on each F and a pair of free pairs on O.

If you check the formal charges, all atoms are neutral

F will have 3 electron pairs + 1 bond = 7 electrons (bond = 1/2 electron for the formal charge distribution) therefore both F's are neutral

Now look O: it must have 6. it's two negatron pairs and a pair of bonds = 4 electrons and a pair of bonds = 1 electron each = 2 electrons from the bond = 6 total electrons for the precise formal charge # should have. there's no need for double bonds during this case because there aren't any costs to separate.

Now if you observe # domains around O you'll see if you enter a free pair that has sp3 hybridization (4 domains) therefore a tetrahedron that has 2 electron pairs and a pair of bonds .. because there are two electron pairs, repulse single pairs/pairs the bond is so high that it expels both fluorine and forms a bent structure, noticeably like H2O.

Learn More

Electrons Bond  https://brainly.com/question/11486787

Outer Shell  https://brainly.com/question/11486787

Details

Grade: College

Subject: Chemistry

Keyword: electron, bond, shell