Molecular Shapes of SF4, CF4, and XeF4

Introduction:
Molecular shapes are determined by the arrangement of atoms and bonding pairs around the central atom in a molecule. In this response, we will discuss the molecular shapes of SF4, CF4, and XeF4. These molecules are formed by the combination of sulfur (S), carbon (C), and xenon (Xe) with fluorine (F) atoms.

SF4:
- SF4 consists of one sulfur atom bonded with four fluorine atoms.
- The central sulfur atom has six valence electrons.
- The Lewis structure of SF4 shows that there are four bonding pairs and one lone pair of electrons around the sulfur atom.
- The presence of a lone pair of electrons affects the molecular shape.
- The molecular shape of SF4 is see-saw.
- In the see-saw shape, three fluorine atoms are arranged in a trigonal plane, while the fourth fluorine atom and the lone pair are in a perpendicular position.

CF4:
- CF4 consists of one carbon atom bonded with four fluorine atoms.
- The central carbon atom has four valence electrons.
- The Lewis structure of CF4 shows that there are four bonding pairs around the carbon atom.
- The absence of any lone pair of electrons determines the molecular shape.
- The molecular shape of CF4 is tetrahedral.
- In the tetrahedral shape, the four fluorine atoms are arranged symmetrically around the central carbon atom.

XeF4:
- XeF4 consists of one xenon atom bonded with four fluorine atoms.
- The central xenon atom has eight valence electrons.
- The Lewis structure of XeF4 shows that there are four bonding pairs around the xenon atom.
- The absence of any lone pair of electrons determines the molecular shape.
- The molecular shape of XeF4 is also tetrahedral.
- In the tetrahedral shape, the four fluorine atoms are arranged symmetrically around the central xenon atom.

Conclusion:
The molecular shapes of SF4, CF4, and XeF4 are determined by the arrangement of atoms and bonding pairs around the central atom. SF4 has a see-saw shape due to the presence of a lone pair, while CF4 and XeF4 have a tetrahedral shape as there are no lone pairs. Understanding the molecular shapes of these compounds is crucial in predicting their chemical properties and behavior.