The total number of lone pair present in XeF4 ?

Question

Answer

Valency of Xe is 8 in XeF4 it make 4 bond with F so 4 valency used and remaining 4 it will remain as 2 lone pair... 2 valency = 1 lone pair

Answer

. According to Lewis Dot structure, Xe has 8 electrons in outermost shell and it is capable of expanding its octet due to the presence of a d-orbital. Each atom of F consists of 7 electrons in outermost shell and share 1 electron with Xe, hence completing their octet and so, 4 electrons are left in Xe outermost shell forming 2 lone pairs.

Answer

Total Number of Lone Pairs in XeF4

Background Information

Xenon tetrafluoride (XeF4) is a chemical compound that consists of one xenon atom and four fluorine atoms. It is a colorless solid with a melting point of 116.3°C and a boiling point of 207.3°C. The structure of XeF4 is square planar, with the xenon atom in the center and the four fluorine atoms positioned in a plane around it.

Bonding in XeF4

The bonding in XeF4 is covalent. Each of the four fluorine atoms shares one electron with the xenon atom, forming four single bonds. The xenon atom also has two lone pairs of electrons.

Determination of Lone Pairs

To determine the number of lone pairs in XeF4, we need to look at the electron configuration of the xenon atom. Xenon has eight valence electrons, which are distributed as follows:

1s2 2s2 2p6 3s2 3p6

In XeF4, the xenon atom forms four single covalent bonds with the fluorine atoms. This means that it uses up four of its valence electrons, leaving four electrons unpaired. These four unpaired electrons are arranged in two lone pairs around the xenon atom.

Total Number of Lone Pairs

Therefore, the total number of lone pairs in XeF4 is two. The two lone pairs are arranged in a plane perpendicular to the plane of the four fluorine atoms.

Conclusion

In summary, XeF4 has a square planar structure with four single covalent bonds between the xenon atom and the fluorine atoms. The xenon atom has two lone pairs of electrons, giving a total of two lone pairs in the molecule.

Answer

Xe is a noble gas (group 18 element). It has 8 electrons in its outermost orbit/ shell. Fluorine is a halogen (group 17 element). It has 7 electrons in its outermost shell.

Each fluorine atom requires an electron to complete its octet. Thus 4 fluorine atoms require 4 electrons to form four covalent bonds. Xe has 8 electrons in its outermost shell. It shares 4 electrons with 4 F atoms. This way 4 electrons of Xe are used up in bond formation with F whereas its 4 electrons do not participate in bonding, that is, it has 2 lone pairs.

Lone pair means the electron pair which is not used in bond formation.

Answer

2 lone pair of electrons

Answer

Lone pair = 6-4=2
Hybrid orbital of XeF4= 6
Monovalent (Fluorine)=4

Answer

2 lone pairs.

Answer

2 lone pairs.

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