A water molecule is held together by two single polar covalent bonds true or false?

True. A water molecule (H2O) is held together by two single polar covalent bonds. To understand why, let's break down the structure of a water molecule.

First, we have oxygen (O) at the center, surrounded by two hydrogen (H) atoms. Oxygen has six valence electrons, and it needs two more electrons to complete its outer shell and achieve stability.

Each hydrogen atom has one valence electron, and it needs one more electron to achieve stability.

To form a water molecule, each hydrogen atom shares one electron with the oxygen atom through a covalent bond. This results in a total of two polar covalent bonds in a water molecule.

The oxygen atom attracts the shared electrons more strongly than the hydrogen atoms, causing an uneven distribution of electrons. As a result, the oxygen atom becomes partially negative (δ-) because of the electron density, while the hydrogen atoms become partially positive (δ+).

Thus, each covalent bond in a water molecule is polar, meaning there is a partial separation of charge across the bond.