Question

electronegativity
all of the following molecules
are polar covalent. because the
electrons are unequally shared,
one element will have a slightly
positive charge and another will
have a slightly negative charge.
sort the specified
atom as carrying a
slight positive charge
or a slight negative
charge.
item bank
slight positive
charge
slight negative
charge
o in h2o
c in c - o
f in h - f
h in h - cl

Explanation:

In a polar covalent bond, the more electronegative atom attracts the shared electrons more strongly, resulting in a slight negative charge on it and a slight positive charge on the less electronegative atom.

• For \(O\) in \(H_2O\): Oxygen (\(O\)) is more electronegative than hydrogen (\(H\)). So, \(O\) has a slight negative charge.
• For \(C\) in \(C - O\): Oxygen (\(O\)) is more electronegative than carbon (\(C\)). So, \(C\) has a slight positive charge.
• For \(F\) in \(H - F\): Fluorine (\(F\)) is more electronegative than hydrogen (\(H\)). So, \(F\) has a slight negative charge.
• For \(H\) in \(H - Cl\): Chlorine (\(Cl\)) is more electronegative than hydrogen (\(H\)). So, \(H\) has a slight positive charge.

Answer:

Slight Positive Charge: \(C\) in \(C - O\), \(H\) in \(H - Cl\)
Slight Negative Charge: \(O\) in \(H_2O\), \(F\) in \(H - F\)