The number of lone pair of electrons present on Xe in \(\mathrm{XeF}_{2}\) is ........ (a) 1 (b) 2 (c) 3 (d) 4

Understanding the valence electrons of an atom is a fundamental aspect of chemistry which plays a critical role in predicting how an element will react and bond with other elements. In the case of Xenon (Xe), which is a noble gas, it has 8 valence electrons. Noble gases are typically unreactive due to their complete valence electron shells, which makes Xenon unique because it can form compounds like \textbf{XeF}\(_2\).

When determining the number of lone pairs in a compound like \textbf{XeF}\(_2\), the valence electrons of Xenon contribute to both the bonds formed with other atoms and any remaining electrons, which exist as lone pairs. This is a key concept when predicting the structure and reactivity of molecules containing Xenon. The 8 valence electrons around Xenon need to be accounted for, with some participating in bonding and others remaining as non-bonding lone pairs.

Molecular geometry is the three-dimensional arrangement of atoms within a molecule. It's important for predicting the physical and chemical properties of a compound, including reactivity, polarity, and phase of matter at room temperature. For \textbf{XeF}\(_2\), the molecular geometry can be predicted using the Valence Shell Electron Pair Repulsion (VSEPR) theory, which states that electron pairs around a central atom will arrange themselves as far apart as possible to minimize repulsion.

In the example of \textbf{XeF}\(_2\), Xenon is the central atom with three lone pairs and two bonding pairs of electrons. The three lone pairs will repel each other to occupy equatorial positions, resulting in a linear structure for the molecule. This adjustment to minimize repulsion affects the molecular geometry, and thus the overall shape and properties of the molecule.

Chemical bonding is the process by which atoms combine to form compounds. There are several types of chemical bonds, including ionic, covalent, and metallic bonds. In the context of \textbf{XeF}\(_2\), we observe covalent bonding, where electrons are shared between Xenon and Fluorine atoms to achieve stable electron configurations.

In a covalent bond, each atom contributes one or more electrons to the bond to fill their valence shells. For Xenon in \textbf{XeF}\(_2\), it shares one electron with each Fluorine atom, forming two single covalent bonds. After these bonds are formed, the remaining electrons on Xenon that are not involved in bonding are organized into lone pairs. These aspects of bonding and lone pair arrangements are fundamental to understanding how molecules form and behave.