Question

determine the idealized bond angles for each molecule.
drag the items into the appropriate bins.
pcl₃ scl₂ ch₃f cs₂
90 degrees 120 degrees 180 degrees 109.5 degrees

Explanation:

Step1: Analyze \( \text{PCl}_3 \)

\( \text{PCl}_3 \) has a trigonal pyramidal geometry (central \( \text{P} \), 3 bonding pairs, 1 lone pair). The ideal bond angle for trigonal pyramidal (derived from tetrahedral) is \( 109.5^\circ \) (slightly less due to lone pair, but idealized is \( 109.5^\circ \)).

Step2: Analyze \( \text{SCl}_2 \)

\( \text{SCl}_2 \) has a bent geometry (central \( \text{S} \), 2 bonding pairs, 2 lone pairs). Derived from tetrahedral, idealized bond angle is \( 109.5^\circ \) (actual is less, but idealized is tetrahedral - based \( 109.5^\circ \)).

Step3: Analyze \( \text{CH}_3\text{F} \)

\( \text{CH}_3\text{F} \) is a tetrahedral - like molecule (central \( \text{C} \), 4 bonding pairs). The ideal bond angle for tetrahedral is \( 109.5^\circ \).

Step4: Analyze \( \text{CS}_2 \)

\( \text{CS}_2 \) has a linear geometry (central \( \text{C} \), 2 bonding pairs, 0 lone pairs). The ideal bond angle for linear is \( 180^\circ \).

Now, categorize:

• \( 90^\circ \): None of the molecules have idealized \( 90^\circ \) (unless octahedral, which these aren't).
• \( 120^\circ \): None of the molecules have trigonal planar geometry (which has \( 120^\circ \)) here.
• \( 180^\circ \): \( \text{CS}_2 \) (linear geometry).
• \( 109.5^\circ \): \( \text{PCl}_3 \), \( \text{SCl}_2 \), \( \text{CH}_3\text{F} \) (all derived from tetrahedral electron - pair geometry).

Answer:

• \( 90 \) degrees: (No molecules)
• \( 120 \) degrees: (No molecules)
• \( 180 \) degrees: \( \text{CS}_2 \)
• \( 109.5 \) degrees: \( \text{PCl}_3 \), \( \text{SCl}_2 \), \( \text{CH}_3\text{F} \)