A) Draw and label five water molecules in a beaker of liquid water and five water molecules a beaker of frozen water. So you have two beakers total. B) Label the oxygens and hydrogens. C) Now, add + and – signs to indicate the charged regions of each molecule. D) Then, indicate the hydrogen bonds. E) Label the covalent bonds. F) Why are the drawings different?

As you can observe in the attached drawing, the water molecule is a polar molecule, which means that it has an irregular distribution of its electron density, and that is why closer to the oxygen atom there is partial negative charge, and closer to the hydrogen atoms there is a partial positive charge.

The hydrogen bonds are the intermolecular forces between the hydrogen atom and the oxygen, which is a very electronegative element, and it is the force that keeps the water molecules together. On the other hand, we have the covalent bonds, which are intramolecular forces that bond the hydrogen atoms to the oxygen atoms, and in this way the water molecule is stabilized.

The drawings between water molecules in liquid water and in frozen water are different simply because the water molecules interact and accommodate differently depending on which is the state of matter. In this case, in the liquid state, the molecules are more scattered, they have more energy, so they tend to form a more "messy" arrangement between them, an arrangement that will depend on the way the hydrogen bonds are formed. On the other hand, in the solid state the molecules have very little space between them, they have less energy because of that, so they tend to form a more organized arrangement between them, just like a crystalline structure, which is also due to the orientation of the hydrogen bonds.