Which of the following best represents the two chemical bonds and the molecular geometry of a water (H_2O) molecule?

• A. Two ionic bonds; linear geometry
• B. Two hydrogen bonds; trigonal planar geometry
• C. Two nonpolar covalent bonds; tetrahedral geometry
• D. Two polar covalent bonds; bent geometry

Answer: (D)

Verified step by step guidance

1. Identify the type of bonds in a water (H\_2O) molecule by considering the elements involved: hydrogen and oxygen. Since both are nonmetals, the bonds are covalent rather than ionic.
2. Determine the polarity of the bonds by comparing the electronegativities of hydrogen and oxygen. Oxygen is more electronegative, so the electrons are shared unequally, making the bonds polar covalent.
3. Analyze the molecular geometry by considering the electron pairs around the oxygen atom. Oxygen has two bonding pairs (with hydrogen) and two lone pairs of electrons.
4. Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the shape. The four electron pairs arrange themselves in a roughly tetrahedral electron geometry to minimize repulsion, but the molecular shape considers only the atoms, resulting in a bent geometry.
5. Conclude that the water molecule has two polar covalent bonds and a bent molecular geometry, which matches the correct description.