Math  /  Geometry

QuestionThe molecular geometry of the SiH4\mathrm{SiH}_{4} molecule is [ Select ] \square , and this molecule is \square [ Select] .

Studdy Solution

STEP 1

What is this asking? We need to figure out the 3D shape of a SiH4\mathrm{SiH}_{4} molecule and whether it's polar or nonpolar. Watch out! Don't mix up electron geometry and molecular geometry!
Also, remember that even if bonds are polar, the *whole* molecule might not be!

STEP 2

1. Determine the central atom.
2. Count the total valence electrons.
3. Draw the Lewis structure.
4. Determine the electron geometry.
5. Determine the molecular geometry.
6. Determine the molecule's polarity.

STEP 3

Silicon (Si) is less electronegative than Hydrogen (H), so Silicon is our **central atom**!

STEP 4

Silicon has **4** valence electrons, and each Hydrogen has **1**.
Since we have **4** Hydrogens, the total number of valence electrons is 4+(41)=84 + (4 \cdot 1) = 8.

STEP 5

Place Silicon in the center and the four Hydrogens around it.
Connect each Hydrogen to the Silicon with a **single bond**.
Each bond uses **2** electrons, so we've used all 42=84 \cdot 2 = 8 of our valence electrons!
Perfect!

STEP 6

The Silicon atom has **four** bonding pairs of electrons and **zero** lone pairs.
This gives us a **tetrahedral** electron geometry.
Think of it like four balloons tied together – they naturally spread out to minimize repulsion, forming a tetrahedron!

STEP 7

Since there are no lone pairs on the central atom, the molecular geometry is the same as the electron geometry: **tetrahedral**!

STEP 8

While the Si-H bonds are slightly polar due to the electronegativity difference between Silicon and Hydrogen, the **tetrahedral** shape of the molecule causes these polarities to *cancel each other out*!
Imagine pulling equally on all four corners of a tetrahedron – it won't budge!
Therefore, the SiH4\mathrm{SiH}_{4} molecule is **nonpolar**.

STEP 9

The molecular geometry of SiH4\mathrm{SiH}_{4} is **tetrahedral**, and the molecule is **nonpolar**.

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