Question

what is the molecular geometry of xecl3+? note that you must draw the correct lewis - dot structure to answer this question.
tetrahedral
trigonal pyramidal
trigonal bipyramidal
t - shaped
trigonal planar
question 8
1 pts
what is the approximate bond angle of the o - se - o bond in seo2? indicate whether the angle is <, >, or = to the ideal bond angle. if there is more than one possible set of angles, indicate the smallest angle. do not insert any spaces in your answer, nor should you use the degree sign (°). for example, the h - c - cl bond angle in ch3cl is less than the ideal angle for a tetrahedral geometry (109.5°); you would answer this as \<109.5\ (without the quotes of course).

Explanation:

Step1: Determine valence - electrons of XeCl₃⁺

Xe has 8 valence electrons, Cl has 7 valence electrons. For XeCl₃⁺, the total number of valence electrons is \(8 + 3\times7- 1=28\) (subtract 1 for the positive charge).

Step2: Draw Lewis - dot structure

Place Xe in the center and connect it to 3 Cl atoms with single bonds. Then distribute the remaining electrons as lone - pairs to satisfy the octet rule. Xe has 3 bonding pairs and 2 lone - pairs.

Step3: Use VSEPR theory

According to VSEPR theory, for a central atom with 3 bonding pairs and 2 lone - pairs, the electron - pair geometry is trigonal bipyramidal and the molecular geometry is T - shaped.

Step4: Analyze SeO₂

Se has 6 valence electrons and O has 6 valence electrons. In SeO₂, the total number of valence electrons is \(6 + 2\times6=18\). The Lewis - dot structure of SeO₂ has Se as the central atom double - bonded to 2 O atoms and has 1 lone - pair on Se. The electron - pair geometry around Se is trigonal planar. The ideal bond angle for trigonal planar is 120°. But due to the repulsion of the lone - pair, the O - Se - O bond angle is less than 120°.

Answer:

Question 7: D. T - shaped
Question 8: <120