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The molecular shape of the SiH2Cl2 molecule is approximately __________ and its dipole moment is ______ .
A. Tetrahedral, zero
B. Tetrahedral, greater than zero
C. trigonal planar, zero
D. trigonal planar, greater than zero

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Answer:

A

Explanation:

The molecule would not have a net dipole moment because the dipole moments cancel out. Being a vector quantity, dipole moment is affected by the direction of the dipole. If the dipoles are such that they are oriented opposite each other, theory simply cancel out. Polarity of individual bonds in a molecule does not automatically imply that the molecule must poses a net dipolev moment. The polarity of the Si-H and Si-Cl bonds cancel out cause they are oriented opposite each other hence the molecule is non polar.

samueladesida43

The molecular shape of the SiH2Cl2 molecule is approximately tetrahedral and its dipole moment is zero.

MOLECULAR SHAPE:

  • Molecular shape of a molecule refers to the three-dimensional arrangement of the atoms that make up that molecule.

  • In SiH2Cl2 molecule, silicon is a central atom that bonds to 2 atoms of hydrogen and chlorine atoms respectively. Hence, making it a tetrahedral molecule.

  • The polarity of the Si-H and Si-Cl bonds cancel out in the SiH2Cl2 molecule because they are opposite charges, hence the molecule is non polar and have no dipole moment.

Learn more about molecular geometry at: https://brainly.com/question/7558603?referrer=searchResultsional

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