Question

the diagrams below add a little more detail — they show electrons, represented by dots.
diagram a
diagram b
diagram c
diagram d
which diagram correctly represents the electrons in the bonds of a water molecule?
○ diagram c, because oxygen is more electronegative than hydrogen.
○ diagram a, because hydrogen is more electronegative than oxygen.
○ diagram d, because electrons are randomly distributed when they are shared between atoms.
○ diagram b, because hydrogen and oxygen have about the same electronegativity.
one last review question. are there partial charges on the atoms in a water molecule?
○ yes, because the electrons are shared unequally.
○ yes, because the electrons are shared equally.
○ no, because the electrons are shared equally.
did you fully understand the concept covered in this

Explanation:

• For the first question: In a water molecule (\(H_2O\)), oxygen is more electronegative than hydrogen. This means oxygen has a greater attraction for the shared electrons in the \(O - H\) bonds. In Diagram C, the electrons are shown closer to the oxygen atom, which is consistent with oxygen's higher electronegativity. Diagram A is incorrect because hydrogen is not more electronegative than oxygen. Diagram D is wrong as electrons in a polar - covalent bond (like \(O - H\) in water) are not randomly distributed. Diagram B is incorrect since hydrogen and oxygen do not have the same electronegativity.
• For the second question: Since oxygen is more electronegative than hydrogen in \(H_2O\), the electrons in the \(O - H\) bonds are shared unequally. This unequal sharing leads to partial charges. The oxygen atom has a partial negative charge (\(\delta-\)) and the hydrogen atoms have partial positive charges (\(\delta+\)). So, there are partial charges on the atoms in a water molecule because the electrons are shared unequally.

Answer:

• First question: Diagram C, because oxygen is more electronegative than hydrogen.
• Second question: Yes, because the electrons are shared unequally.