Question

question 47 of 49
organic chemistry
loudon
roberts & company publishers
presented by macmillan learning
predict the approximate bond angles in each of the molecules.
$^+\ce{ch3}$:
$ce{sicl4}$:

Explanation:

Step1: Analyze $^+CH_3$ electron geometry

The central C atom has 3 bonding pairs, 0 lone pairs. Electron domain geometry is trigonal planar.

Step2: Assign bond angle for $^+CH_3$

Trigonal planar geometry has bond angles of $120^\circ$.

Step3: Analyze $SiCl_4$ electron geometry

Central Si atom has 4 bonding pairs, 0 lone pairs. Electron domain geometry is tetrahedral.

Step4: Assign bond angle for $SiCl_4$

Tetrahedral geometry has bond angles of $109.5^\circ$.

Answer:

$^+CH_3$: $120^\circ$
$SiCl_4$: $109.5^\circ$