Discuss the shape of the following molecules using the VSEPR model: $BeCl _{2}, BCl _{3}, S i C l _{4}, AsF _{5}, H _{2} S , PH _{3}$

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Discuss the shape of the following molecules using the VSEPR model: $BeCl _{2}, BCl _{3}, S i C l _{4}, AsF _{5}, H _{2} S , PH _{3}$

Solution:

$BeCl_2$

The central atom does not have a lone pair, but it does have two bond pairs. As a result, its shape is AB2, or linear.

$BCl_3$

The central atom has three bond pairs but no lone pairs. As a result, it has the shape AB3 or trigonal planar.

$SiCl_4$

There are no lone pairs on the central atom, but it does have four bond pairs. As a result, its shape is AB4 or Tetrahedral.

$AsF_5$

There are no lone pairs on the central atom, but it does have 5 bond pairs. As a result, it has the shape AB5 or trigonal bipyramidal.

$H_2S$

The central atom has one lone pair and two bond pairs. As a result, its shape is AB2E or bent.

$PH_3$

The central atom has one lone pair and three bond pairs. As a result, its shape is AB3E, which stands for Trigonalbipyramidal.

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