Answer: The correct answer is polar, tetrahedral and non-polar.
Explanation:
It is given a compound which is silicon tetrahydride having formula [tex]SiH_4[/tex]
The electronegativities of silicon and hydrogen are 1.9 and 2.1 respectively.
Difference in electronegativity = 2.1 - 1.9 = 0.2
From above, some difference in the electronegativities of the atoms is there. This means that bond polarity of this molecule is polar. If the difference would have been 0, the bond polarity of the molecule is taken as non-polar.
- To determine the molecular shape of the given molecule, we calculate the hybridization of this molecule. The equation used for this is:
[tex]\text{Number of electrons}=\frac{1}{2}[V+N-C+A][/tex]
where,
V = number of valence electrons present in central atom i.e. Silicon = 4
N = number of monovalent atoms bonded to central atom = 4
C = charge of cation = 0
A = charge of anion = 0
Putting values in above equation, we get:
[tex]\text{Number of electron pairs} =\frac{1}{2}[4+4-0+0]=4[/tex]
As, the total number of electron pairs is 4, this means that the hybridization of this molecule will be [tex]sp^3[/tex] and the molecular shape will be tetrahedral.
- The net dipole moment of the molecule is 0 because of the symmetry of the molecule. Thus, the molecule is considered as a non-polar molecule.
Hence, the correct answer is polar, tetrahedral and non-polar.
