Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound ICl_5?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
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Which of the following compounds has a Lewis dot structure that obeys the octet rule for all atoms in a neutral molecule?
A
CCl4
B
CO2
C
NO2
D
BF3
Verified step by step guidance1
Step 1: Recall the octet rule, which states that atoms tend to form bonds until they are surrounded by eight electrons in their valence shell, achieving a noble gas configuration. This rule mainly applies to second-period elements like C, N, O, and F.
Step 2: Analyze the Lewis structure of each compound to check if all atoms satisfy the octet rule. For example, draw the Lewis structure of CCl4: Carbon (C) is the central atom bonded to four chlorine (Cl) atoms. Each Cl has three lone pairs, and C shares four pairs of electrons, completing the octet for all atoms.
Step 3: For CO2, draw the Lewis structure with carbon in the center double bonded to two oxygen atoms. Each oxygen has two lone pairs. Check if all atoms have eight electrons around them, which they do in this structure.
Step 4: For NO2, consider that nitrogen is bonded to two oxygen atoms and has an unpaired electron (making it a radical). This means nitrogen does not have a complete octet, so NO2 does not obey the octet rule for all atoms.
Step 5: For BF3, boron is bonded to three fluorine atoms but only has six electrons around it, not eight. Boron is an exception to the octet rule here, so BF3 does not obey the octet rule for all atoms.
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