Answer:
In some cases, they could bond to form covalent compounds. However, in most instances they will not interact.
Explanation:
Remember that elements desire to have a full octet (8 valence electrons). The configuration given represents an element with 8 valence electrons. I know this because the outermost shell (denoted by the 2 coefficient) has 8 electrons (2s²2p⁶ = 2 + 6 = 8). Therefore, this element is stable.
The other atom has 7 valence electrons. Since it is 1 electron away from having a full octet, it really wants 1 more electron. The original element is unlikely to give up an electron because that would prevent it from having a full octet. As such, when the atoms are close to one another, they will most likely not interact. The element with the full octet is most likely a noble gas, and these elements rarely form bonds. Noble gases can form bonds with halogens (elements with 7 valence electrons) but only if there are excess halogens and particular noble gases in the system.
