Question at position 20 Which of the listed compounds is part of the tetrahedral electron group arrangement? SO2 AsF3 CO2 ICl4–

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BlackTom AI · Accepted Answer

First, let's restate the problem to focus on the core concept: identifying which compound has a tetrahedral arrangement of electron groups around the central atom.
Option 1: SO2. In sulfur dioxide, the sulfur atom has two sigma bonds to oxygens and one lone pair, giving three regions of electron density. That corresponds to a trigonal planar electron geometry, not tetrahedral.
Option 2: AsF3. Arsenic trifluoride has three As–F bonds and one lone pair on arsenic, totaling four regions of electron density around the central atom. Four regions lead to a tetrahedral electron geometry, so this option matches the tetrahedral arrangement.
Option 3: CO2. Carbon dioxide has two double bonds with the carbon center, which results in two regions of electron density. That yields a linear electron geometry, not tetrahedral.
Option 4: ICl4–. The iodide center in iodide tetrachloride has four bonds to chlorine and two lone pairs, totaling six electron regions. This creates an octahedral electron geometry, not tetrahedral.
In summary, to identify a tetrahedral electron group arrangement, look for a central atom with four regions of electron density (typically 4 bonding pairs, 0 or 1 lone pairs, depending on the specific case). Among the options, only AsF3 satisfies this criterion because it has four electron groups around the arsenic center (three bonds plus one lone pair), giving a tetrahedral electron geometry.

Question at position 20 Which of the listed compounds is part of the tetrahedral electron group arrangement? SO2 AsF3 CO2 ICl4–

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