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Questions and Answers
What process occurs when solid ice is heated and changes into liquid water?
What process occurs when solid ice is heated and changes into liquid water?
Which of the following accurately describes the atomic structure where protons and neutrons are found?
Which of the following accurately describes the atomic structure where protons and neutrons are found?
Which property of water is influenced by hydrogen bonding, allowing it to act as a temperature buffer?
Which property of water is influenced by hydrogen bonding, allowing it to act as a temperature buffer?
How does the temperature of water affect the solubility of salts?
How does the temperature of water affect the solubility of salts?
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What type of bond is formed through the sharing of electrons between atoms in a water molecule?
What type of bond is formed through the sharing of electrons between atoms in a water molecule?
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Which of the following best defines the term 'solute'?
Which of the following best defines the term 'solute'?
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What happens to the arrangement of water molecules when it freezes and forms ice?
What happens to the arrangement of water molecules when it freezes and forms ice?
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How does water act as a solvent with ionic and covalent substances?
How does water act as a solvent with ionic and covalent substances?
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Which chemical formula represents sodium chloride?
Which chemical formula represents sodium chloride?
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What term is used for the concentration of dissolved salts in seawater, typically measured in parts per thousand?
What term is used for the concentration of dissolved salts in seawater, typically measured in parts per thousand?
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What characteristic of water results from its polarity, allowing it to form hydrogen bonds?
What characteristic of water results from its polarity, allowing it to form hydrogen bonds?
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What is the role of electrons in the stability of an atom's outer shell?
What is the role of electrons in the stability of an atom's outer shell?
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During the dissolution of sodium chloride in water, what occurs between the sodium ions and water molecules?
During the dissolution of sodium chloride in water, what occurs between the sodium ions and water molecules?
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What is defined as hypersaline water?
What is defined as hypersaline water?
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How does salinity impact the freezing point of water?
How does salinity impact the freezing point of water?
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What effect does precipitation have on seawater salinity?
What effect does precipitation have on seawater salinity?
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At what pH level is water considered neutral?
At what pH level is water considered neutral?
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How does temperature affect the solubility of oxygen in water?
How does temperature affect the solubility of oxygen in water?
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What effect does increasing depth have on the solubility of gases in water?
What effect does increasing depth have on the solubility of gases in water?
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Which factor does NOT impact the density of seawater?
Which factor does NOT impact the density of seawater?
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What is the primary consequence of ice floating on water?
What is the primary consequence of ice floating on water?
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What does the halocline refer to in oceanography?
What does the halocline refer to in oceanography?
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How does atmospheric pressure influence the solubility of gases in water?
How does atmospheric pressure influence the solubility of gases in water?
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What happens to the density of seawater as salinity increases?
What happens to the density of seawater as salinity increases?
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What is the primary reason for the oxygen minimum layer (OML) in the ocean?
What is the primary reason for the oxygen minimum layer (OML) in the ocean?
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Which of the following best describes the photic zone of the ocean?
Which of the following best describes the photic zone of the ocean?
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Study Notes
1.1 Particle Theory and Bonding
- All matter contains particles in constant motion, even if just vibrating.
- The energy of these particles determines their motion and state (solid, liquid, gas).
- Changes in energy lead to changes in state:
- Melting (solid to liquid): Adding energy makes particles vibrate faster, breaking apart from each other and flowing.
- Evaporation (liquid to gas): Heating a liquid gives particles more energy, making them move faster and further apart until they evaporate.
- Boiling: A specific temperature (100°C at 1 atm) where liquid rapidly turns to gas.
- Condensation (gas to liquid): Cooling a gas causes particles to lose energy, slowing down and coming together to form a liquid.
- Freezing (liquid to solid): Cooling a liquid causes particles to lose energy, becoming closer together and forming the structure of a solid.
1.1.2 Atom Structure
- Atoms have a nucleus with protons (positive) and neutrons (neutral).
- Electrons (negative) orbit the nucleus in shells.
- The first shell holds two electrons, and subsequent shells can hold up to eight (octet rule).
- Atoms are most stable when their outermost shell is full.
- Atomic number = number of protons in an atom.
1.1.3 Mixtures and Compounds
- Seawater is a mixture of different elements and compounds.
- Nearly every element is found in the ocean, usually combined as compounds.
1.1.4 Covalent Bonding
- Covalent bonds involve sharing of electron pairs between non-metal atoms.
- These bonds are strong because they complete the outermost electron shells of the atoms involved.
- Water molecules form a covalent bond through sharing.
1.1.5 Covalent Molecules
- Water (H₂O): Needed for photosynthesis.
- Oxygen (O₂): Needed for respiration.
- Carbon Dioxide (CO₂): Needed by plants for photosynthesis.
- Sulfur Dioxide (SO₂): Needed by bacteria for chemosynthesis.
- Glucose (C₆H₁₂O₆): Produced by photosynthesis.
1.1.6 Ionic Bonding
- Ionic bonds occur when atoms gain or lose electrons to create charged ions.
- Opposites attract: Positive ions (cations) bond with negative ions (anions).
- Salts are formed from ionic bonds (e.g., sodium chloride).
1.1.7 and 1.1.8 Ionic Substances and Salts in Seawater
- Ionic substances include sodium chloride (NaCl), magnesium sulfate (MgSO₄) and calcium carbonate (CaCO₃).
- These are common salts found in seawater.
1.1.9 and 1.1.10 Hydrogen Bonding in Water
- Hydrogen bonds form between polar molecules (like water) due to uneven electron sharing.
- Water's polarity allows it to dissolve many ionic and polar substances.
- Water has high specific heat capacity, meaning it absorbs or releases a lot of heat without a significant temperature change.
- Water's density properties help regulate temperature in the environment by the low density of ice.
- Hydrogen bonding is crucial for water's properties (high boiling point, solubility, and ice floating).
1.2 Solubility in Water
- Solvent: A substance capable of dissolving other substances.
- Solute: A substance that can be dissolved.
- Solution: A mixture of solute and solvent.
- Dissolution: The process of dissolving.
- Solubility: How much solute can dissolve in a given amount of solvent.
- Salinity: Concentration of dissolved salts in seawater (measured in parts per thousand, ppt).
- Salinity affects the freezing point of water.
- Temperature and pressure affect the solubility of salts and gases in water.
1.2.6 Surface Runoff, Precipitation, and Evaporation
- Precipitation (rain, snow) lowers salinity by adding water.
- Evaporation increases salinity by removing water.
- Surface runoff can affect salinity with fresh water (dilution) or salts (increase)
1.2.7 pH Scale
- pH measures the concentration of hydrogen ions (H⁺) in a solution.
- The pH scale ranges from 0 to 14.
- Acidic solutions have a pH less than 7.
- Neutral solutions have a pH of 7.
- Alkaline (basic) solutions have a pH greater than 7.
1.2.8 Measuring pH
- Litmus paper, universal indicator, and pH probes can be used to measure pH.
1.2.9 Oxygen Solubility in Water
- Temperature and salinity affect oxygen solubility.
- Warmer temperatures and higher salinity reduce oxygen solubility.
- Increased depth increases pressure which increases oxygen concentration
- The solubility of CO2 is high.
1.2.10 Factors Affecting Gas Solubility in Water
- Factors like temperature, pressure, atmospheric pressure and salinity all play a role in impacting gas solubility.
1.3 Density and Pressure in Water
- Water temperature affects density (warmer water is less dense).
- Salinity affects density (higher salinity increases density).
- Pressure increases density.
- Density differences create water layers (e.g., thermocline, halocline).
- Ice floats because it is less dense than liquid water; this prevents the entire water body from freezing.
1.3.4 Importance of Floating Ice
- Ice acts as a thermal insulator.
- This prevents the entire body of water from freezing.
- Allows marine organisms to live.
1.3.5 Temperature and Salinity Gradients in Water
- Gradients in temperature and salinity create distinct water layers (e.g., surface layer, thermocline, halocline).
- These layers influence mixing and circulation.
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Description
This quiz covers the fundamental concepts of particle theory and atom structure. You'll explore how energy changes affect states of matter such as melting, boiling, and freezing. Through this quiz, understand the behavior of particles in solids, liquids, and gases.
