Question

Determine the number of bonding electrons and the number of nonbonding electrons in the structure of of2.

Answer 1

The number of bonding electrons and the number of nonbonding electrons in the structure of OF₂ are 2,8

Further explanation

OF₂ or oxygen difluoride is one of the chemical compound. This molecule adopts a "bent" molecular geometry similar to that of water, but it has very different properties such as being a strong oxidizer.

A bonding electron is an electron involved in chemical bonding. Whereas a non-bonding electron is an electron that not involved in chemical bonding .

Bonding electron or bond pairs are a pair of electrons (one from the central atom and one with the atom which is bonding) and participate in the bonding of the atom.

Non-bonding electron or nshared pair or lone pair refers to a pair of valence electrons that are not shared with another atom in a covalent bond. Lone pairs are found in the outermost electron shell of atoms. They can be identified by using a Lewis structure.

Lewis structure rules are as follows:

1. Pair of bonded electrons is by means of a dash (-) are called a bond
2. Lone pairs or non-bonded electrons are represented by dots
3. Electron represent in the last shell of atoms are called valence electrons.

The lewis structure of OF₂ molecule is as shown as figure below

According to the picture, theare 2 bonding electrons and 8 nonbonding electrons

Learn more

1. Learn more about bonding electrons brainly.com/question/11645803
2. Learn more about nonbonding electrons brainly.com/question/9805874
3. Learn more about the structure of OF2 brainly.com/question/6786947

Answer details

Grade:  9

Subject:  Chemistry

Chapter:  bonding electrons

Keywords: bonding electrons, nonbonding electrons, The structure of OF2,

Answer 2

OF2 - 
O has 6 electrons in outer shell and F has 7 in its outer shell 
Therefore, you have to account for 20 electrons total in the 
structure (7+7+6 = 20) 
therefore draw it linear first. F ---- O-----F 
The two bonds take care of 4 electrons now you have to add another 16. 
Therefore 3 lone pairs on each F and 2 lone pair on O. 
If you check for formal charges, all the atoms are neutral 
F will have 3 lone pairs + 1 bond = 7 electrons (bond = 1/2 electron for formal charge distribution) therefore both the F's are neutral 
Now look at the O: it should have 6.. it has two lone pair and 2 bonds = 4 electrons and 2 bonds = 1 electron each = 2 electrons from bonds = 6 total electrons for formal charge which is exactly the # it should have. There is no need for any double bond in this as there are no charges to be separated. 
Now if u look at the # of domains around O you will see if you include the lone pairs it has a sp3 hybridization (4 domains) therefore a tetrahedron which has 2 lone pairs and 2 bonds.. since there are two lone pairs, the lone pair/bond pair repulsion is so high it is going to repel the two Fluorines and form a bent structure, looks a lot like H2O.