Question at position 17 In a perfectly nonpolar covalent bond, like the bonds found in the diatomic elements, where do the shared electrons spend most of their time? On the “outside” of the nuclei (not between the nuclei). In between the nuclei. Somewhere outside of the molecule. Perpendicular to the bond.

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Question at position 17 asks about where the shared electrons spend most of their time in a perfectly nonpolar covalent bond. 
Option 1: 'On the “outside” of the nuclei (not between the nuclei).' In a covalent bond, electrons are not primarily positioned outside the nuclei; the electron density is concentrated between the two nuclei due to sharing of electrons. This description misplaces the electron density. 
Option 2: 'In between the nuclei.' This matches the fundamental idea of a covalent bond: the two atoms share electrons, and the electron density is greatest in the region between the nuclei, forming a bond region that holds the atoms together. In a perfectly nonpolar bond, the electron distribution is symmetrical about the midpoint between the nuclei, reinforcing that most time is spent between them. 
Option 3: 'Somewhere outside of the molecule.' For a diatomic molecule with a covalent bond, the shared electrons are not predominantly located outside the entire molecule; the bonding region between the nuclei is where they reside. 
Option 4: 'Perpendicular to the bond.' The electron density that forms the bond lies along the bond axis, not perpendicular to it; describing the electrons as being perpendicular would mischaracterize the spatial distribution of the bonding electrons. 
Overall, comparing the options, the description that aligns with the concept of a covalent bond—shared electron density concentrated between the two nuclei—is the statement 'In between the nuclei.'

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