Use Lewis structures to explain why Br3- and I3- are stable, while F3- is not.

Valence electrons are the electrons contained in the outermost shell of an atom that can potentially be involved in chemical bonding. In the context of the Lewis structure exercise, understanding valence electrons is crucial because they determine how atoms bond and form compounds.

For instance, bromine (Br) and iodine (I) atoms, mentioned in the exercise, have seven valence electrons each, placed in their outermost shell. Fluorine (F) also has seven valence electrons, but despite this similarity, F does not behave the same way in compounds as Br and I do. The number and arrangement of valence electrons influence an atom's ability to engage in chemical bonds, aiming to achieve a stable electronic configuration, typically by following the octet rule.

The octet rule states that atoms are generally most stable when they have eight electrons in their valence shell, resembling the electron configuration of a noble gas. In the exercise, Br₃^- and I₃^- adhere to the octet rule, which means that through bonding, the atoms adjust their electrons to either share, lose, or gain electrons in order to complete their octet.

Specifically, the central bromine or iodine in Br₃^- and I₃^- carries two lone pairs and bonds with two other halogen atoms to fulfill this requirement. However, for F₃^-, the situation is different. Due to the small size of fluorine and its high electronegativity, having multiple fluorine atoms around a central F atom leads to significant electron-electron repulsion, which violates the octet rule's provision for stability.

Electron-electron repulsion is a principle where negatively charged electrons repel each other due to their like charges. This repulsion affects molecular shape and stability, and is a key factor in the Lewis structures exercise.

The smaller size and high electronegativity of F cause the electrons to be closer together, increasing the repulsion between them. This repulsion can prevent the formation of a stable octet and leads to the instability of F₃^-. Conversely, Br and I have larger atomic radii which means their valence electrons are more spread out, reducing the electron-electron repulsion. This allows Br₃^- and I₃^- to form stable linear structures, adhering to the octet rule and minimizing repulsion between the valence electrons.