Methanol, CH3OH, contains a C-O bond. In this bond, which of the following best describes the charge on the carbon atom.

a.) -1
b.) +1
c.) uncharged
d.)slightly negative
e.) slightly positive

the answer key says slightly positive but isn't it uncharged? what makes something "slightly" charged?

c

In a C-O bond, the oxygen atom is more electronegative than the carbon atom. This means that the oxygen atom has a stronger attraction for electrons, resulting in a partial negative charge (denoted as δ-) on the oxygen atom. Conversely, the carbon atom has a partial positive charge (denoted as δ+), as it has a weaker attraction for electrons. This partial charge separation is due to the unequal sharing of electrons in the bond.

While the carbon atom in methanol doesn't carry a full positive charge (+1), it does have a partial positive charge, which is denoted as "slightly positive" in the answer choices.

In the molecule methanol (CH3OH), the C-O bond is a polar covalent bond. A polar covalent bond is a type of bond in which the electrons are unequally shared between the atoms involved.

In this case, oxygen has a higher electronegativity value compared to carbon. Electronegativity is a measure of an atom's tendency to attract electrons towards itself. Oxygen is more electronegative than carbon, so it attracts the bonded electrons more strongly, resulting in a partial negative charge (δ-) on the oxygen atom. Conversely, the carbon atom, which is less electronegative than oxygen, experiences a partial positive charge (δ+).

It is important to note that the carbon atom is not fully positive as in the case of ionic bonds. The term "slightly positive" is used to describe this partial positive charge. It indicates that although the carbon atom has a slight deficiency of electrons due to the unequal sharing, it is not fully charged since it still retains some of its electrons.

In summary, the correct answer is "e.) slightly positive" because of the partial positive charge on the carbon atom in the C-O bond of methanol.