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15: Water

Last updated

Mar 21, 2025
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- 14.15: Diffusion and Effusion and Graham's Law
- 15.1: Structure of Water

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Topic hierarchy

15.1: Structure of Water
This page explores the molecular characteristics and importance of water, highlighting its composition of one oxygen and two hydrogen atoms, its bent shape due to polar covalent bonding, and its ability to form strong hydrogen bonds. The tetrahedral geometry around the oxygen atom allows for multiple hydrogen bonds, significantly contributing to water's unique properties and its essential roles in biological processes.
15.2: Structure of Ice
This page explains that ice is less dense than liquid water because of hydrogen bonding and its hexagonal structure, allowing it to float. While ice has beneficial uses, such as cooling and recreation, it can also cause damage. As water cools, it reaches maximum density at 4°C before becoming less dense at freezing, which helps aquatic life survive under the ice during winter, preventing complete freezing of lakes.
15.3: Physical Properties of Water
This page discusses the global challenge of water loss due to evaporation, prompting farmers to consider measurement tools like evaporation pans. It highlights water's unique physical properties, including high melting and boiling points due to hydrogen bonding, as well as high surface tension. The page also explains that water has a low vapor pressure that increases with temperature, affecting the rate of molecules transitioning to the vapor phase.
15.4: Solute and Solvent
This page discusses how freezing temperatures in winter can harm car radiators, potentially causing issues like broken hoses and cracked engine blocks. It explains the concept of solutions, highlighting how a solute dissolves in a solvent to create a homogeneous mixture. Water is noted as a versatile solvent, forming stable aqueous solutions with various substances, and a true solution is defined as having dissolved particles smaller than 1 nm that do not settle or change when filtered.
15.5: Dissolving Process
This page explains the process of making coffee by extracting material from coffee beans using hot water. It details how substances like sugar and milk can enhance the drink through dissolution, where water's polar nature allows it to mix with and stabilize various compounds, such as salt and sugar, through solvation and hydration. The page highlights the interactions between water and both ionic and covalent substances, resulting in a homogeneous mixture.
15.6: Liquid-Liquid Solutions
This page discusses the 2010 Gulf of Mexico oil spill, highlighting how the nonpolar nature of crude oil prevents it from mixing with water. It explains the concept of miscibility, noting that nonpolar compounds like oil do not dissolve in polar solvents, emphasizing the principle "like dissolves like" and the necessity of polarity for solubility in water through hydrogen bonding.
15.7: Electrolytes and Nonelectrolytes
This page discusses the benefits and risks of jogging, particularly in hot conditions. It emphasizes the importance of electrolytes, which are crucial for bodily functions, and notes that loss of these during exercise can lead to nausea and fatigue. Key electrolytes include calcium, sodium, potassium, and magnesium. The page recommends sports drinks as a means to replenish electrolytes and avoid health issues during exercise.
15.8: Dissociation
This page discusses the hazards of winter ice on roads and sidewalks and the use of deicing salts like sodium chloride and calcium chloride to melt ice. It explains the dissociation of these ionic compounds into individual ions when dissolved in water, contrasting this with nonionic compounds, such as sucrose, which do not dissociate. The importance of understanding these processes for effective winter road maintenance is also highlighted.
15.9: Strong and Weak Electrolytes
This page explains the role of sulfuric acid in car batteries as a key electrolyte that ionizes to provide power. It highlights the sealing of modern batteries to prevent acid leakage, and distinguishes between strong electrolytes, which fully ionize and conduct electricity well, and weak electrolytes that only partially ionize, resulting in a mixture of ions and intact molecules.
15.10: Suspensions
This page discusses the impact of storms on the clarity of the Caribbean Sea, explaining how they create a turbid suspension. It defines suspensions as heterogeneous mixtures where larger particles settle, contrasting them with solutions. Examples like milk and water-based paint are provided, highlighting the need for stirring to keep suspended particles evenly distributed.
15.11: Colloids
This page explains colloids as heterogeneous mixtures with particle sizes between solutions and suspensions, highlighting the Tyndall effect, which involves light scattering. Unlike suspensions, colloidal particles do not settle or separate by filtration. It also describes emulsions, a type of colloid that requires an emulsifying agent for stability, with examples like mayonnaise and soap that help mix nonpolar and polar substances.

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