2. A. The Molecule 1. O—H bond is highly polar 2. Bond angle 105° making it Bent shaped 3. Water Molecule as a whole is polar 4. Attracted to each other by intermolecular hydrogen bonds Greater electronegativity

3. B. Important Properties 1. High surface tension 2. low vapor pressure hydrogen bonds hold molecules to one another, tendency to escape surface is low 3. high specific heat capacity 4.184 J/g×°C 4. high melting and boiling points 0°C and 100°C

4. C. Surface Tension – inward force, or pull, that tends to minimize the surface area of a liquid Surfactant – wetting agent such as soap or detergent that decreases the surface tension by interfering with hydrogen-bonding Responsible for high surface tension

5. I. Water (cont.) D. Atypical Ice 1. As a typical liquid cools, density increases b/c Volume decreases as the mass stays constant 2. As water cools it first behaves like a typical liquid until it reaches 4°C 3. Below 4°C the density of water starts to decrease **Ice is one of only a few solids that float in their own liquid.

6. Atypical Ice Do not need to write. Density of Liquid Water and Ice Temperature (°C)Density (g/cm 3 ) 100° (liquid water)0.9584 500.9881 25°0.9971 10°0.997 4°4°1.000 (most dense) 0° (liquid water)0.9998 0° (ice)0.9168 °

7. Atypical Ice Why does ice behave do differently? Open framework arranged like a honeycomb. Framework collapses, molecules packed closer together, making it more dense