Question

question 1 (2 points)
consider sulfur dichloride, scl₂. the lewis structure has 2 single bonds and two pairs of nonbonding electrons.
the number of reds is 1.
the bond angles are 2° and the shape is 3.
scl₂ is a 4 symmetrical/asymmetrical molecule.
a. 0 b. 1 c. 2 d. 3 e. 4 f. 180 g. 90 h. 120
i. 109.5 j. diatomic k. linear l. planar trigonal m. bent
n. pyramidal o. tetrahedral p. symmetrical q. asymmetrical

Explanation:

• Number of REDs (Region of Electron Density):
• For \(SCl_2\), the formula for REDs is \( \text{Number of bonding pairs}+\text{Number of non - bonding pairs}\).
• Given 2 single bonds (bonding pairs) and 2 non - bonding pairs. So, \(2 + 2=4\).
• Bond Angles:
• The electron - pair geometry of \(SCl_2\) (with 4 REDs) is tetrahedral. But due to the presence of 2 non - bonding pairs, the molecular geometry is bent.
• The bond angle in a bent molecule with tetrahedral electron - pair geometry (due to repulsion from non - bonding pairs) is less than \(109.5^{\circ}\). But if we consider the ideal case (ignoring some minor effects for the sake of this multiple - choice question), the bond angle is \(109.5^{\circ}\) (approximate value based on electron - pair geometry influence).
• Shape:
• As mentioned above, with 2 bonding pairs and 2 non - bonding pairs around the central \(S\) atom, the shape is bent.
• Symmetry:
• In \(SCl_2\), the two \(S - Cl\) bonds are not in a symmetrical arrangement (because of the non - bonding pairs). So, it is an asymmetrical molecule.

Answer:

E. 4, I. 109.5, M. bent, Q. asymmetrical