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Questions and Answers
What type of intermolecular force exists between neutral polar molecules that are very close together?
What type of intermolecular force exists between neutral polar molecules that are very close together?
- London Dispersion Forces
- Ion-Dipole Forces
- Dipole-Dipole Forces (correct)
- Hydrogen Bonding
Which substance is likely to exhibit hydrogen bonding?
Which substance is likely to exhibit hydrogen bonding?
- Sodium Chloride
- Ammonia (correct)
- Carbon Dioxide
- Ethane
What characteristic distinguishes crystalline solids from amorphous solids?
What characteristic distinguishes crystalline solids from amorphous solids?
- Crystalline solids have fixed geometric patterns or lattices. (correct)
- Crystalline solids have a random orientation of particles.
- Crystalline solids tend to melt over a wide range of temperatures.
- Crystalline solids change their physical properties gradually.
Which type of intermolecular force exists between an ion and a dipole?
Which type of intermolecular force exists between an ion and a dipole?
Which of the following is NOT a characteristic of crystalline solids?
Which of the following is NOT a characteristic of crystalline solids?
What is the primary difference in melting behavior between crystalline and amorphous solids?
What is the primary difference in melting behavior between crystalline and amorphous solids?
Which of the following pairs exhibits hydrogen bonding?
Which of the following pairs exhibits hydrogen bonding?
Which structure is characteristic of amorphous solids?
Which structure is characteristic of amorphous solids?
What is the strongest intermolecular force present in ammonia (NH3)?
What is the strongest intermolecular force present in ammonia (NH3)?
Which type of intermolecular force is dominant in methanol (CH3OH)?
Which type of intermolecular force is dominant in methanol (CH3OH)?
What is the dominant intermolecular force in carbon tetrafluoride (CF4)?
What is the dominant intermolecular force in carbon tetrafluoride (CF4)?
Which of the following substances is characterized by ionic bonding?
Which of the following substances is characterized by ionic bonding?
What type of intermolecular force is found in solid potassium bromide (KBr)?
What type of intermolecular force is found in solid potassium bromide (KBr)?
What is the intramolecular bond type in graphite?
What is the intramolecular bond type in graphite?
In which compound do you expect to find dipole-dipole interactions as the dominant intermolecular forces?
In which compound do you expect to find dipole-dipole interactions as the dominant intermolecular forces?
What type of intermolecular force is primarily present in SO2?
What type of intermolecular force is primarily present in SO2?
What is the main reason that water has a higher boiling point than ethyl alcohol?
What is the main reason that water has a higher boiling point than ethyl alcohol?
Why is water referred to as a universal solvent?
Why is water referred to as a universal solvent?
What is the specific heat of water?
What is the specific heat of water?
What does it mean for water to have a high specific heat?
What does it mean for water to have a high specific heat?
Which of the following describes a consequence of water's ability to dissolve gases?
Which of the following describes a consequence of water's ability to dissolve gases?
What characteristic of water allows it to remain a liquid over a wide range of temperatures?
What characteristic of water allows it to remain a liquid over a wide range of temperatures?
How does water's high specific heat benefit the environment?
How does water's high specific heat benefit the environment?
Why is the heat capacity of water significant for plants and animals in aquatic environments?
Why is the heat capacity of water significant for plants and animals in aquatic environments?
What happens to the density of water when it freezes?
What happens to the density of water when it freezes?
Why do small bodies of water like ponds not dry up quickly during summer?
Why do small bodies of water like ponds not dry up quickly during summer?
What occurs due to the ease with which water dissolves pollutants?
What occurs due to the ease with which water dissolves pollutants?
What role does the ice layer on a water body play for aquatic life?
What role does the ice layer on a water body play for aquatic life?
How does the structure of solid water differ from that of liquid water?
How does the structure of solid water differ from that of liquid water?
How does temperature affect the viscosity of a liquid?
How does temperature affect the viscosity of a liquid?
What is the relationship between intermolecular forces of attraction (IMFA) and viscosity?
What is the relationship between intermolecular forces of attraction (IMFA) and viscosity?
In capillary action, what type of intermolecular attraction draws the liquid up the narrow tube?
In capillary action, what type of intermolecular attraction draws the liquid up the narrow tube?
How does vapor pressure change with temperature?
How does vapor pressure change with temperature?
Which statement accurately describes the relationship between IMFA and vapor pressure?
Which statement accurately describes the relationship between IMFA and vapor pressure?
What does molar heat of vaporization measure?
What does molar heat of vaporization measure?
How does the vapor pressure of acetone compare to water at 25°C?
How does the vapor pressure of acetone compare to water at 25°C?
What type of meniscus is formed when a liquid adheres to the walls of a glass tube?
What type of meniscus is formed when a liquid adheres to the walls of a glass tube?
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Study Notes
Intermolecular Forces of Attraction
- London Dispersion Forces: Weak forces present in all molecules, especially significant in nonpolar substances.
- Dipole-Dipole Forces: Occur between neutral polar molecules in close proximity.
- Hydrogen Bonding: A strong type of dipole-dipole interaction involving hydrogen and electronegative atoms (F, N, O).
- Ion-Dipole Forces: Interaction between an ion and the partial charge of a polar molecule.
Types of Solids
- Crystalline Solids: Have fixed geometric patterns or lattices. Melting occurs at specific temperatures, resulting in sharp changes in physical properties.
- Amorphous (Noncrystalline) Solids: Display random orientations of particles and melt over a wide range of temperatures (e.g., charcoal, rubber bands, glass).
Liquids and Intermolecular Forces
- Nonpolar Molecules: Experience London Dispersion Forces.
- Polar Molecules: Can engage in dipole-dipole interactions and hydrogen bonds (H bonded with F, O, N).
- Ion and Polar Molecules: Involve ion-dipole and ionic bonds.
Identifying IMFA in Compounds
- Analyze molecular composition to determine the strongest intermolecular force. Different compounds exhibit varying types of intermolecular forces.
Viscosity
- Defined as the resistance of a liquid to flow, influenced by temperature: higher temperatures typically decrease viscosity.
- Example: Viscosity of water is 1 centipoise, while honey has a much higher viscosity of 10,000 centipoise due to stronger IMFA.
Capillary Action
- The tendency of liquids to rise in narrow tubes, resulting from the interplay of cohesion (attraction between like molecules) and adhesion (attraction between unlike molecules).
Vapor Pressure
- The pressure exerted by a gas in equilibrium with its liquid at a specific temperature, increasing with temperature.
- Independent of liquid amount yet dependent on IMFA: stronger IMFA results in lower vapor pressure.
Molar Heat of Vaporization and Boiling Point
- The energy required to vaporize one mole of a liquid at a given temperature.
- Stronger IMFA correlates with higher boiling points and greater molar heat of vaporization.
Unique Properties of Water
- Universal Solvent: Capable of dissolving a wide variety of ionic and polar covalent compounds.
- High Specific Heat: Water has a specific heat of 1 calorie/g-°C, essential for climate regulation and supporting aquatic life.
- Unusually High Boiling Point: Water remains liquid over a large temperature range due to strong IMFA.
- Lower Density in Solid Form: Ice floats on water, allowing aquatic life to thrive underneath it, insulated by the ice layer.
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