Water Properties Quiz

A water molecule (H2O) consists of two hydrogen atoms covalently bonded to one oxygen atom. The oxygen atom has a partial negative charge, while the hydrogen atoms have partial positive charges, making it a polar molecule.

Hydrogen bonds occur when the slightly positive hydrogen atom of one water molecule is attracted to the slightly negative oxygen atom of another water molecule. This creates a strong, interconnected network between water molecules.

Water's unique properties, such as high surface tension, its ability to dissolve substances, and its unusual density behavior, are all directly influenced by the polarity of water molecules and their ability to form hydrogen bonds.

Surface tension is the force that holds water molecules together at the surface, creating a thin skin-like layer. This is because of the strong hydrogen bonds between water molecules.

High surface tension allows insects to walk on water and supports energy transfer between the atmosphere and the ocean.

Water's polarity allows it to dissolve a wide range of ionic and polar compounds by forming hydration shells around them. This makes it an excellent solvent.

Water is less dense in its solid state (ice) than in its liquid state. This is because water molecules form a structured lattice in ice, which makes them less tightly packed.

The fact that ice is less dense than water is crucial for aquatic life, as it prevents lakes and oceans from freezing solid, allowing marine organisms to survive in cold environments.

Water's ability to resist temperature changes. It requires a lot of energy to raise or lower its temperature.

Water's strong hydrogen bonds make it resistant to temperature changes, acting as a stabilizing force for Earth's climate.

Oceans act like massive heat movers, carrying warm water from the equator towards the poles and vice versa, regulating global temperatures.

When water evaporates, it absorbs heat from the environment and stores it. This heat is released during condensation, driving weather patterns.

The relative proportions of major dissolved ions (like chloride and sodium) in seawater remain constant, regardless of the overall salinity.

This principle implies that the ocean's chemical composition is remarkably stable over time, even though the salinity can vary.

The total amount of dissolved salts in seawater.

The six major ions that make up the majority of dissolved salts in seawater.

The process that occurs near the surface of the ocean where phytoplankton use sunlight to convert carbon dioxide, nitrogen, and phosphorus into organic matter, releasing oxygen as a byproduct.

The consumption of oxygen and release of carbon dioxide by marine organisms, including phytoplankton, zooplankton, and fish, as they break down organic matter for energy.

The breakdown of dead organic matter by bacteria, releasing carbon dioxide, nitrogen, and phosphorus back into the water. It occurs throughout the water column.

The process by which nitrogen and phosphorus released from decomposition are brought back to the surface through upwelling, fueling new phytoplankton growth.

The movement of carbon from the atmosphere to the deep ocean, driven by phytoplankton photosynthesis and the sinking of their organic matter after they die.

The process by which seawater becomes salty. Evaporation removes freshwater, leaving behind salts, while chloride and sodium, with long residence times, accumulate.

Nitrogen, phosphorus, carbon dioxide, and oxygen are interconnected through biological processes such as photosynthesis, respiration, decomposition, and nutrient recycling, influencing global nutrient and carbon dynamics.

The average salt content of seawater, typically around 35 parts per thousand (ppt).

The CCD is the depth in the ocean where the rate of calcium carbonate (CaCO3) dissolution equals the rate of CaCO3 supply, preventing its accumulation.

Factors that affect the dissolution of calcium carbonate include:

1. CO2 Concentration: Higher CO2 makes water more acidic, increasing dissolution.
2. Pressure: Increased pressure at depth enhances CaCO3 solubility.
3. Temperature: Cold water dissolves more CaCO3.
4. Water Chemistry: Deep water is often undersaturated with CaCO3, promoting dissolution.

Even though calcium carbonate is dissolving below the CCD, calcareous sediments can still accumulate because:

1. Above the CCD: Conditions are less favorable for CaCO3 dissolution.
2. High Supply: A large amount of carbonate material from surface waters can exceed the rate of dissolution.

The change in salinity with depth, marked by a rapid decrease in salinity.

The change in temperature with depth, characterized by a rapid decrease in temperature.

Regions where respiration significantly exceeds oxygen replenishment, often found in areas with limited circulation and high organic matter decomposition.

Areas with high nutrient concentrations and high levels of dissolved CO2, typically due to cold temperatures and upwelling.

Higher salinity in the subtropics is driven by high evaporation rates, while lower salinity at the equator and poles is attributed to higher precipitation rates and melting ice.

Warmer temperatures at the equator due to direct solar radiation, with temperatures declining towards the poles.

Evaporation and precipitation influence salinity and SST vertically, while mixing and surface currents play a role in distributing these properties horizontally.

The movement of water masses driven by density differences, resulting in a continuous circulation throughout the ocean.

Waves travel in water depths greater than half their wavelength (Depth > λ/2). The longer the wavelength, the faster the wave travels.

Waves traveling in water depths between half and one-twentieth of their wavelength (λ/20 < Depth < λ/2). Wave speed is affected by both wavelength and water depth, with shallower depths slowing the waves down.

Waves traveling in water depths less than one-twentieth of their wavelength (Depth < λ/20). Wave speed is controlled by water depth, with shallower water leading to slower wave movement.

As waves move from deep to shallow water, they slow down, their wavelength shortens, and their height increases.

When a wave becomes too steep (height to wavelength ratio greater than 1:7) near the shoreline, it breaks.

Waves bend towards areas of shallower water, aligning more parallel to the shoreline.

The elliptical motion of water particles in shallow water, which reaches the seafloor, contributes to sediment movement, causing coastal erosion and deposition.

Two waves interacting with each other, combining through a process that can be either constructive (amplifying the wave) or destructive (canceling the wave).