xef2o lewis structure

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xef2o Lewis structure is a polyatomic molecule. Its chemical name is xenon oxydifluoride. It consists of one xenon atom ,two fluorine atom and one oxygen atom. In xef2o Lewis structure the xenon is present in a central of an atom. Xenon having 8 electrons around it ,must have  extra electrons in the structure.

 Xef2O Lewis structure basis on the periodic table we determined that , it has 28 valence electrons. 8 for Xenon, 7 for Fluorine and 6 for oxygen. By adding them,  there are 8 + 7 *2 +6= 28. There are 28 valence electron in the XeF2O Lewis structure.

Put Xe at the center, which is the least electronegative atom ant  put fluorine on either side of it , than the oxygen above it. Put each electron on each bond than six electron around Xe. so it obey the octet rule.

To know the all details of xef2o Lewis structure :

How to draw Lewis structure of xef2o:

 xef2o lewis structure contain one xenon , two fluorine and one oxygen atom in it.  It is much heavy and extremely rare in nature. Xenon is present in group 18. It has 8 valence electron. It was the first Noble Gas found in the chemical compounds. Fluorine is present in group 17 of the periodic table. It is the most reactive chemical element in all of the halogens. This is much lighter than other which has 7 electrons .

Oxygen is present in group 16, 6 valence electron is present here. It is also called chalcogens first of all let’s count valence electron of xef2o by adding from 8 + 7*2 +6= 28 electrons. xef2o lewis structure has 28 total Valence Electrons.  By putting xenon in the middle of it , because it is less electronegativity in nature .Fe is present two side of the Lewis structure of xef2o and oxygen on the top of it.

Let’s add electron between atoms , so we get an chemical bond. So that we get 6 in that way. Then complete the octet of the fluorine atom than the oxygen and xenon, we get only 26 electron by that. Another more two electron will give to the xenon. Xenon can have more than 8 Valence Electrons, which extend the octet. So it was ok with more than 8 in the xenon atom but we are not sure this is the reasonable structure of xef2o. There is another probability to make the Lewis structure in best approach . similarly if we get another xef2o Lewis structure where,  Xe present on central. F is present on each side of it and oxygen present above it.

Here the oxygen which is present it gives two extra  electrons to the xenon atom. Now Xe contain more than 8 electrons that is 12 electron. Oxygen have two lone pairs right now . which can be form double bond  between oxygen and xenon atom. This bonding with each other by double bond  is also stable form. This is approaching the best Lewis structure, because all the formal charges are zero here.

xef2o lewis structure
Image credit of xenon by istock

xef2o Lewis structure shape :

 xef2o Lewis structure shape can be determined by its structure. The shape of this is trigonal bipyramidal. By VSEPR arrangement the xenon atom present in Central and an oxygen is present above it. It give rise to T shape geometry. This contain two free valence electrons ion pair. Here xenon -oxygen bond domain occupied the trigonal plane. Xenon-fluorine bond, which is present here are trans to one another. This Xe-F bond also perpendicular to the trigonal plane .

We know by the VSEPR arrangements , that gives rise to T shape. The xenon atom is present in the exact center . Two Fluorine atom is present at the side of the Xe  and Oxygen the above or below. so it looks like T-shape, If we ignore 2 lone pairs here. 2 lone pairs are ignored , by determining the shape. The two electrons which is present above the xenon are free or lone pairs. This is not in count while determining the shape of the molecule. Here xenon -oxygen bond domain occupied the trigonal plane. Xenon-fluorine bond, which is present here are trans to one another. This Xe-F bond also perpendicular to the trigonal plane .

xef2o lewis structure formal charges :

Let’s see the formal charges of xef20. Here Xenon, have 8 pairs of electron in periodic table. Here 4 electrons which are not in bonding or in non bonding in xef20 lewis structure. There are six valance electron ,which are involved in chemical bond. Which divided by 2. So it gives 8 – 4 – 6 / 2 = 1. So the charges plus one (+1). The formal charge calculated by the formula,

formal charge = valence electron – non-bonding valence electron – bonding electron / 2.

Oxygen have six valence electron So if we have to find the formal charge of oxygen six non-bonding electrons are present . Two bonding electrons are present here,  Which is divided by 2.  So we get Formal charge is 6 – 6 – 2/2 = -1.

 Finally for Fluorine have seven valence electron. We have six electrons are non-bonding. We have two bonds which involve in chemical bond . So we get by the formula , that for formal charge of  fluorine is 7 – 6 – 2 /2 = 0 , Which is same formal charge for both fluorine atom.  All the formal charges are not 0,  so we are not considered, this is the best Lewis structure . The formal charges are different here.

 If  considered another probability by Moving electron pair from oxygen. We have same number of electrons here What’s changing only the two electrons position of oxygen . Due to  the internal setting that is double bond in between xenon and Oxygen . Oxygen of Xef20 lewis structure having two lone pairs. Doubly bonded oxygen bonded with  xenon ,which having more than eight electrons outside it . So if we consider the formal charge of Xenon By the second lewis structure the valence electron is 8 here There is two pairs of non-bonding electrons. Bonding electrons are present here Which is  8 divided by 2 So we get the formal charge of Xe is  8-4 -8 /2 =0 .

Similarly if we consider the formal charge of oxygen , here oxygen have six valence electrons, 4 Non bonding electrons are here. Bonding electrons is present here is 4. Four electrons are present here, which is  divided by 2 We get 6 – 4 – 4/2 = 0 . Now we have to find out  the formal charge of fluorine atom.

Fluorine  has seven valence electrons,6 Non bonding electrons. Two bonding electrons are present here . So by determining the formal charge of F is 7 – 6 – 2 / 2 = 0 So here we can see that the formal charge of xenon, Oxygen and Fluorine has 0 charges on each.  Because the formal charges are  zero here it is the best lewis structure for xef20.

xef2o lewis structure lone pairs:

Basis on the best lewis Structure of xef2o. There is only two electrons present on the xenon atom and  on oxygen atom. Because of the two lone pair the geometry should be trigonal bipyramidal. To calculate the shape of the molecule the lone pair will not be counted. so only the molecule is considered in  T-shape molecule.

Xef2O hybridization :

Here in xef2o 3 Sigma Bond and two lone pairs are present .By adding three sigma and two lone pair there is whole 5 . So the hybridization is sp3d . This means 1s, 3p and 1d is present here. xef2o is present having 3 Sigma bonds Which is bonding with two fluorine and one oxygen atoms. There are two lone pairs are present above the xenon atom. So counting the whole is five. So the hybridization must be sp3d. Hybridization sp3d means trigonal bipyramidal. Here xenon -oxygen bond domain occupied the trigonal plane. Xenon-fluorine bond, which is present here are trans to one another. This Xe-F bond also perpendicular to the trigonal plane .

xef2o lewis structure resonance

Resonance are the sets of Lewis structure that describe the delocalization of electrons. The  delocalization of electron mostly in atoms of a polyatomic molecule. In many cases there is several structure , so the best structure can be determined the shape and  hybridization of the molecules. So we need best resonance structure for it. In most cases we couldn’t determined the exact structure of any molecule because the structure is complex in nature. Presence of fractional bonds and partial charges present in it .We need more resonate structure to determine the best lewis in a complex molecule. Here in xef20 is the best lewis structure, one of these is approaches more stable because there is  formal charges present in it.

If  considered xef2o  by Moving electron pair from oxygen. We have same number of electrons here Which changing only the two electrons position of oxygen . Due to  the internal setting that is double bond in between xenon and Oxygen . Oxygen of Xef20 lewis structure having two lone pairs. Doubly bonded oxygen bonded with  xenon ,which having more than eight electrons outside it . So if we consider the formal charge of Xenon by this lewis structure, the valence electron is 8 here There is two pairs of non-bonding electrons. Bonding electrons are present here Which is  8 divided by 2 So we get the formal charge of Xe is  8 – 4 – 8 / 2 = 0 .

Similarly if we consider the formal charge of oxygen , here oxygen have six valence electrons, 4 Non bonding electrons are here. Bonding electrons is present here is 4. Four electrons are present here, which is  divided by 2 We get 6 – 4 – 4/2 = 0 . Now we have to find out  the formal charge of fluorine atom.

Fluorine  has seven valence electrons,6 Non bonding  electrons. Two bonding electrons are present here . So by determining the formal charge of F is 7 – 6 – 2 / 2 = 0 So here we can see that the formal charge of xenon, Oxygen and Fluorine has 0 charges on each.  Because the formal charges are  zero here it is the best resonate lewis structure.

xef2o Lewis structure octet rule :

 The octet rule is very important while doing resonate structure . If the molecule is more complex we need octet rule because after arrangements , we have to check each atoms are contained 8 electrons. So we have to remember that where the atom loses gains or shared a pair of electrons , than it must be obey the octet rule. we have to know that all the atoms contain 8 electrons on each of the atom. In xef2o, each of the atom obey octet rule.

 If  consider electron pair from oxygen. We have same number of electrons here What’s changing only the two electrons position of oxygen . Due to  the internal setting that is double bond in between xenon and Oxygen . Oxygen of Xef20 lewis structure having two lone pairs. Doubly bonded oxygen bonded with  xenon ,which having more than eight electrons outside it . So if we consider the formal charge of Xenon By the second lewis structure The valence electron is 8 here There is two pairs of non-bonding electrons.

Bonding electrons are present here Which is  8 divided by 2 So we get the formal charge of Xe is  8 – 4 – 8 / 2 = 0 .Similarly if we consider the formal charge of oxygen , here oxygen have six valence electrons, 4 Non bonding electrons are here. Bonding electrons is present here is 4. Four electrons are present here, which is  divided by 2 We get 6 – 4 – 4/2 = 0 . Now we have to find out  the formal charge of fluorine atom.

Fluorine  has seven valence electrons,6 Non bonding electrons. Two bonding electrons are present here . So by determining the formal charge of F is 7 – 6 – 2 / 2 = 0 So here we can see that the formal charge of xenon, Oxygen and Fluorine has 0 charges on each.  Because the formal charges are  zero here it is the best lewis structure for xef2o. Here oxygen, fluorine all obey octet rule.

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