Final answer:
An atom with the electron configuration 2-6 (like oxygen) would most likely form a bond with an atom that has 1 or 2 valence electrons to share or transfer. The best match among the provided options is the atom with the electron configuration 2-2 as they can share electrons to achieve a full valence shell.
Step-by-step explanation:
To determine which atom would most likely form a bond with an atom having the electron configuration 2-6, we need to look for an atom that could either share or transfer electrons to achieve a stable electron configuration, generally depicted by having a full valence shell similar to that of a noble gas. The electron configuration 2-6 suggests an oxygen atom, which has 6 valence electrons and needs 2 more to complete its valence shell. The ideal bonding partner would be an atom with an electron configuration that has 1 or 2 electrons in its outermost shell that it can share or transfer.
Option 1) Configuration 2, likely represents a hydrogen atom with only 1 electron to share, which isn't enough. Option 2) Configuration 2-2, likely represents a beryllium atom which can share its 2 valence electrons. Option 3) Configuration 2-8, represents a neon atom, which already has a full valence shell and is not likely to bond. Finally, option 4) Configuration 2-8-8, represents an argon atom, another noble gas with a complete valence shell, making it chemically inert.
The most likely atom to form a bond with an atom having electron configuration 2-6 is the one with configuration 2-2, as the two atoms can share their valence electrons to achieve stable configurations analogous to the noble gases.