Final answer:
The question "Is I₄⁻ consistent?" from 1.3. is equivalent to asking whether the given ion, I₄⁻, follows the octet rule and has a stable electronic configuration.
Step-by-step explanation:
In the context of chemistry and molecular structures, consistency often refers to adherence to certain principles, such as the octet rule. The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable configuration with eight electrons in their outermost shell. In the question "Is I₄⁻ consistent?" from section 1.3., the focus is on the ion I₄⁻, which means a central iodine atom surrounded by four additional iodine atoms, resulting in a negative charge.
To determine the consistency of I₄⁻, one needs to assess whether the ion satisfies the octet rule for each iodine atom. Iodine typically forms negative ions by gaining one electron to achieve a stable configuration. In I₄⁻, the central iodine atom must adhere to the octet rule by having eight electrons in its outermost shell, including those gained from the surrounding iodine atoms.
Further analysis involves confirming that each surrounding iodine atom also adheres to the octet rule. If all atoms in I₄⁻ follow the octet rule, the ion is considered consistent. However, if any iodine atom deviates from the octet rule, the consistency is compromised, indicating a less stable electronic configuration.
In summary, the question "Is I₄⁻ consistent?" is equivalent to assessing whether the I₄⁻ ion conforms to the octet rule, ensuring a stable electronic arrangement for each iodine atom in the structure.