Chemical Bonding And Molecular Structure

The hydrolysis of XeF is given by the following reaction:

The 'X' in this reaction is XeO .
To determine the structure of XeO , we need to find the number of electron pairs around the central atom Xe.
Xe has 8 valence electrons.
Each oxygen atom forms a double bond with Xe, using 2 electrons each.
So, 3 oxygen atoms use 6 electrons.
The remaining 2 electrons form a lone pair.
Thus, there are 3 bond pairs and 1 lone pair, making a total of 4 electron pairs.
According to VSEPR theory, the arrangement of electron pairs is tetrahedral.
However, due to the presence of a lone pair, the shape of the molecule is pyramidal.

Step 1: Use the Bond Order Formula Bond order is given by:
Step 2: Compute Bond Orders : Electronic configuration in molecular orbitals gives bond order = 2. : Electronic configuration in molecular orbitals also gives bond order = 2. Since both species have the same bond order, they are the correct answer.

Step 1: has no lone pairs on the central atom. has two lone pairs, has one lone pair, and has three lone pairs.

Step 2: Therefore, the correct increasing order of lone pairs is <(SnCl_2\) < <(XeF_2\) .

Step 1: Understanding Lithium Alloys
Lithium forms lightweight alloys that are used in aerospace and defense applications.

Step 2: Choosing the correct metal
Among the given options, lithium forms an alloy with magnesium (Mg), which is used to make armor plates. Thus, the correct answer is Mg.

Step 1: The hybridisation of central atoms in XeF6 and IF7 is sp3d2. Both have six electron pairs around the central atom.

Step 2: The other options have different hybridisations due to the number of bonding pairs and lone pairs on the central atom.