Imagine that in another universe, atoms and elements are identical to ours, except that atoms with six valence electrons have particular stability (in contrast to our universe where atoms with eight valence electrons have particular stability). Give an example of an element in the alternative universe that corresponds to: a. a noble gas b. a reactive nonmetal c. a reactive metal

Valence electrons are the outermost electrons of an atom and are crucial in determining how an element reacts chemically. They are the electrons involved in forming bonds with other atoms to create chemical compounds. In our universe, atoms typically strive to have eight valence electrons to reach a stable configuration—a principle known as the octet rule. However, in the alternative universe we're imagining, the rules shift to prioritize six valence electrons for stability.

To put it in context, envision a ring toss game where everyone wants to grab six rings to win a prize, instead of the eight rings they'd normally snatch in our own universe. Elements will 'toss' or 'grab' electrons until they reach that magic number—six—in this alternate realm.

Noble gases in our universe are known for their lack of reactivity, due to having a complete set of valence electrons satisfying the octet rule. This makes them highly stable and seldom engaging in chemical reactions. In the alternative universe, an element like oxygen—typically a reactive nonmetal with six valence electrons in our cosmos—would take the place of noble gases.

Think of them as the aloof royalty in the periodic table kingdom of this other universe; they have everything they need and typically keep to themselves, avoiding the 'social' chemical reactions that other elements participate in.

Reactive nonmetals in our universe are elements that readily gain or share electrons to complete their valence shell. In this alternative scenario, an element with either five or seven valence electrons would be unstable and, therefore, reactive, as they are close to the desired six-electron stable state. It's as if they are playing a game of musical chairs, always looking for the chance to gain or share electrons to fill the seats around their table.

Using the playbook from this new universe, nitrogen, which has five valence electrons, is the element that is a seat short and, therefore, eager to react with other elements to reach the full table of six.

In contrast to nonmetals, reactive metals are elements that tend to lose their valence electrons to attain a stable electron configuration. In our universe, metals react by losing one, two, or more electrons to achieve the octet. However, in the alternative universe, a metal would aim to lose electrons to reach the six-electron rule.

Boron becomes an example of a reactive metal in this other reality. It starts off with three valence electrons and would likely lose them to reach the stable state, akin to unloading extra cargo to sail smoothly. Such metals are akin to generous donors in a game of electron exchange, always willing to give up their valence electrons to stabilize themselves and in the process, engage in the formation of compounds.