The statement is not entirely accurate. In a water molecule (H2O), the electrons are not predominantly attracted to the hydrogen atoms. Instead, the electrons are shared between the oxygen and hydrogen atoms, forming covalent bonds.

The electronegativity of an atom refers to its ability to attract electrons towards itself in a chemical bond. Oxygen is more electronegative than hydrogen, meaning that it has a stronger pull on the electrons in the covalent bonds. This results in a slight polarization of the electron cloud, with the electrons being slightly closer to the oxygen atom.

However, it is important to note that the electron density in a molecule is not static. The electrons are constantly moving and sharing between the atoms, and the exact distribution of electrons can change over time. Therefore, it is not accurate to say that the electrons are attracted more towards the hydrogen atoms in a water molecule.