Although I₃^- is a known ion, F₃^- is not. (b) One of your classmates says that F₃^- does not exist because F is too electronegative to make bonds with another atom. Give an example that proves your classmate is wrong.

Verified step by step guidance

1. Understand the concept of electronegativity: Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Fluorine is the most electronegative element, which means it strongly attracts electrons in a bond.
2. Consider the nature of chemical bonding: Despite its high electronegativity, fluorine can form bonds with other atoms, including other fluorine atoms, as seen in the molecule F2, where two fluorine atoms share a pair of electrons.
3. Explore the concept of polyatomic ions: Polyatomic ions are ions composed of two or more atoms covalently bonded together, carrying a net charge. The I3- ion is an example of a polyatomic ion where iodine atoms are bonded together.
4. Identify a known example of fluorine bonding with another atom: Fluorine can form stable compounds with other elements, such as in the case of HF (hydrogen fluoride), where fluorine is bonded to hydrogen.
5. Conclude with the possibility of fluorine forming bonds: While F3- is not a known ion, the existence of compounds like F2 and HF demonstrates that fluorine can indeed form bonds with other atoms, contradicting the claim that its electronegativity prevents bonding.