Question

How many lone pairs are there in KrF4​

Answer 1

Answer:

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Explanation:

According to VSEPR theory, the shape of the given compound is octahedral. The given compound has 36 valence electrons in total.

Answer 2

The number of lone pairs in KrF$_{4}$ is 2.

• The number of lone pairs in a compound can be determined by using the formula: ( Number of free electrons after bonding)/2.
• The given compound is KrF4.

• Kr (krypton ) is an element of group 18. The elements of group 18 have 8 electrons on the outermost shell. Hence Kr can share up to a value of 8 electrons. ( 8 bonds).
• Fluorine belongs to the group VIIA. The elements of the group VIIA require only 1 electron for completing the stable octet configuration. Hence Fluorine requires an electron for bonding.
• In the given compound KrF$_{4}$, Krypton is being bonded with 4 Fluorine atoms, As each Fluorine atom requires one electron to complete its octet configuration. 4 Fluorine atoms require a total of 4 electrons for completing octet of all the 4 Fluorine atoms.
• After sharing 4 electrons, Krypton has 4 more electrons in the outermost shell. Since 2 electrons together are considered as a lone pair, The total number of lone pairs if there are 4 free electrons is 2. Hence, the total number of lone pairs in KrF4 is 2.

Therefore, KrF4 has a total of 2 lone pairs.