Question

note: to answer some of the questions, it may help to reference a periodic t

examine the image of a molecule of iodine trichloride (icl3).

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how does the molecule break the octet rule?

Explanation:

Step1: Recall the octet rule

The octet rule states that atoms tend to gain, lose, or share electrons so that they have eight electrons in their valence shell.

Step2: Analyze the central atom (I) in \(ICl_3\)

Iodine (I) is the central atom. Iodine has 7 valence electrons. In \(ICl_3\), it forms 3 single bonds with chlorine (Cl) atoms (each bond contributes 1 electron to iodine's valence shell). So, from the bonds, iodine gets 3 electrons. Additionally, iodine has 2 lone pairs (each lone pair has 2 electrons). The total number of valence electrons around iodine is \(3\times1 + 2\times2= 3 + 4=10\) electrons.

Answer:

The central iodine atom has 10 valence electrons (3 bonding pairs and 2 lone pairs) instead of 8, thus breaking the octet rule.