Question

A tetrahedral molecule,$X{Y_4}$ , would be formed if X were used in which of the following orbital hybridization.
A.${p^2}$
B.${s^2}$
C.$sp$
D.$s{p^2}$
E.$s{p^3}$

Answer 1

Tetrahedral-Tetra signifies four, and hedral relates to a face of a solid tetrahedral literally means having four faces. This shape is found when there are four bonds all on one central atom, with no lone electron pairs. In accordance with the VSEPR theory, the bond angles between the electron bonds are ${109.5^ \circ }$

Complete step by step answer:
In a tetrahedral molecular geometry, a central atom is located at the center with four substituents that are located at the corners of a tetrahedron. When all four substituents are the same, as in methane as well as its heavier analogues. Methane and other perfectly symmetrical tetrahedral molecules belong to the point group, but most tetrahedral molecules have lower symmetry. Tetrahedral molecules can be chiral. Some examples of tetrahedral molecules include the ammonium ion, methane ion, and phosphate ion.

A tetrahedral molecule, $X{Y_4}$ , would be formed if X were used in $s{p^3}$ orbital hybridization.
The central atom X will have four bond pairs and zero lone pairs of electrons. These will occupy four $s{p^3}$ hybrid orbitals. This results in tetrahedral geometry.

So, the correct answer is (E) $s{p^3}$

Note:
The bond angle for a symmetric tetrahedral molecule such as methane may be calculated using the dot product of two vectors. The molecule can be inscribed in a cube with the tetravalent atom at the cube centre which is the origin of coordinates, O. The four monovalent atoms are at four corners of the cube chosen so that no two atoms are at adjacent corners linked by only one cube edge.