Answer
See the explanation
Work Step by Step
a. NaBr or $NaBr_{2}$
The more energetically stable compound would be NaBr.
Explanation:
NaBr is a neutral ionic compound, where the sodium (Na) atom has a +1 oxidation state and the bromine (Br) atom has a -1 oxidation state. This results in a stable ionic bond between the two atoms, leading to a lower energy state.
On the other hand, $NaBr_{2}$ would be an unstable compound, as it would have a bromine atom with a -2 oxidation state, which is highly unfavorable. The presence of two bromine atoms bonded to a single sodium atom would create a high-energy, unstable configuration.
b. $ClO_{4}$ or $ClO_{4}^{-}$
The more energetically stable compound would be $ClO_{4}^{-}$ (perchlorate ion).
Explanation:
The perchlorate ion, $ClO_{4}^{-}$, is a stable and well-known anion. The chlorine atom has a +7 oxidation state, and the four oxygen atoms provide a stable, tetrahedral arrangement around the chlorine atom.
In contrast, $ClO_{4}$ would be an unstable neutral species, as the chlorine atom would have a +8 oxidation state, which is highly unfavorable. The neutral $ClO_{4}$ compound would have a higher energy configuration compared to the stable perchlorate ion.
c. $SO_{4}$ or $XeO_{4}$
The more energetically stable compound would be $XeO_{4}$ Explanation:
The Lewis structure cannot be drawn so that it obeys the octet rule for $SO_4$ (30 electrons) unlike $XeO_4$
d. $OF_{4}$ or $SeF_{4}$
The more energetically stable compound would be $SeF_{4}$ (selenium tetrafluoride).
Explanation:
Selenium tetrafluoride, $SeF_{4}$, is a stable and known compound in chemistry. The selenium atom has a +4 oxidation state, and the four fluorine atoms form a stable, square planar arrangement around the selenium atom.
In contrast, $OF_{4}$ (oxygen tetrafluoride) would be an unstable neutral compound. Oxygen typically forms stable compounds with a maximum of two bonds, and the formation of four bonds with fluorine atoms is highly unfavorable. The $OF_{4}$ compound would have a higher energy configuration compared to the stable selenium tetrafluoride.
