Discuss the shape of the following molecules using the $VSEPR$ model: $BeCl_{2}, BCl_{3}, SiCl_{4}, AsF_{5}, H_{2}S, PH_{3}$

(N/A) The $VSEPR$ theory predicts the shapes based on the number of bonding and non-bonding electron pairs around the central atom:
$1$. $BeCl_{2}$: Central atom $Be$ has $2$ bonding pairs and $0$ lone pairs. Geometry: Linear $(180^{\circ})$.
$2$. $BCl_{3}$: Central atom $B$ has $3$ bonding pairs and $0$ lone pairs. Geometry: Trigonal planar $(120^{\circ})$.
$3$. $SiCl_{4}$: Central atom $Si$ has $4$ bonding pairs and $0$ lone pairs. Geometry: Tetrahedral $(109.5^{\circ})$.
$4$. $AsF_{5}$: Central atom $As$ has $5$ bonding pairs and $0$ lone pairs. Geometry: Trigonal bipyramidal $(90^{\circ}, 120^{\circ})$.
$5$. $H_{2}S$: Central atom $S$ has $2$ bonding pairs and $2$ lone pairs. Geometry: Bent (Angular).
$6$. $PH_{3}$: Central atom $P$ has $3$ bonding pairs and $1$ lone pair. Geometry: Trigonal pyramidal.