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Water is unique as when it freezes, it is less dense that the liquid form. This is unusual as when in the solid form, it is usually more dense than the liquid form. However in the case of water, the hydrogen bonds in water too strong so they aren't broken when water freezes which makes the density of ice to be lighter than liquid water.

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Since water has both positive and negative ends from the oxygen and hydrogen atoms, the bond between the molecules is called a dipole-dipole bond. The covalent bonds between the oxygen atom and the hydrogen atoms form and leave the hydrogen side positive but the oxygen side negative. The specific type of dipole bond in water is a hydrogen bond. Hydrogen is the strongest intermolecular bond as in water, it has no electrons on the inside so it can form stronger bonds with oxygen, the negative side.

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The specific heat of water is 4.184 joules. Water is bounded together by hydrogen bonds, a very strong intermolecular force. When water is heated up, the hydrogen bonds absorb energy and break and when water is cooled, the bonds are reformed. Due to the fact that hydrogen bonds are so strong, it takes a lot of energy or heat to break the bonds, which is what makes the specific heat so high.

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Water is known as a universal solvent due to the polarity of water. The hydrogen molecules have a slightly positive charge but the oxygen has a slightly negative charge. Due to the fact that it has both positive and negative charges, it is able to dissolve more substances than any other liquid.

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A Brønsted-Lowry acid is a solution in which an H+ proton is donated. A Brønsted-Lowry base is a solution that accepts an H+ proton. An amphoteric solution, or in this case, water, is one that can act as a acid or a base.

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In the Penny Lab, we placed drops of water on a "penny" and counted how many drops the penny could hold. The hydrogen bonds hold together the water allowing more drops to stay on the penny portraying the adhesive properties of water and the high surface tension of water.

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In the Heat of Combustion of Paraffin Lab,  we placed a candle under an aluminum can filled with water.  The water has a specific heat of 4.18 J/g °C. By knowing the specific heat of water, it was used to calculate the heat of combustion of paraffin. Water is used as a staple liquid because it has a high specific heat, more energy is needed to raise the temperature, and in this case, the goal was to double the temperature by the energy released from the candle.

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The Heating Curve of Water shows the phases of water by temperature and when they change phases. Along with that, it can also show the density of water. Water becomes less dense as it gets colder, the opposite of normal liquids, making it a unique power. As the temperature of the heating curve decreases, the density of water or ice will decrease. As the temperature of the heating curve increases, the density increases as well.

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In the Solubility of Borax Lab, we had dissolved set amounts of Borax into water, at different temperatures of water till the solution became saturated. We then let it set and crystals formed on the pipe cleaner. This lab shows the example of a universal solvent as borax dissolves in water among many other solutes.

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In the Red Cabbage Lab, we added OH- to the cabbage water to neutralize the solution to an amphoteric solution, or water.

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Specific Heat is the amount of energy needed to raise something by 1 degree. Water has the highest specific heat of any liquid.

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There are 3 intermolecular forces: dipole-dipole, dispersion, and hydrogen bonding. Water is connected by hydrogen bonding which is a type of dipole-dipole force.

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The density of water is unique. When water turns to a solid, ice, the density decreases which is unusual as usually, the more tightly packed the molecules are, the higher the density.

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Water is known as a universal solvent as it dissolves a variety of solutes, more than any other type of solvent.

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Water is amphoteric which means that is can be used as both an acid and base.