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Questions and Answers
What primarily explains the properties of solids and liquids?
What primarily explains the properties of solids and liquids?
Which characteristic is NOT associated with solids?
Which characteristic is NOT associated with solids?
How does temperature affect the kinetic energy of particles?
How does temperature affect the kinetic energy of particles?
What distinguishes intermolecular forces from intramolecular forces?
What distinguishes intermolecular forces from intramolecular forces?
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Which of the following best describes solids in terms of particle arrangement?
Which of the following best describes solids in terms of particle arrangement?
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Which of the following statements about liquids is true?
Which of the following statements about liquids is true?
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Which type of force is responsible for holding molecules together?
Which type of force is responsible for holding molecules together?
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Which property of solids makes them denser than liquids?
Which property of solids makes them denser than liquids?
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What does the graphical representation in phase transitions primarily illustrate?
What does the graphical representation in phase transitions primarily illustrate?
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Where does sublimation or deposition occur on the phase diagram?
Where does sublimation or deposition occur on the phase diagram?
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Which statement correctly defines the critical point on a phase diagram?
Which statement correctly defines the critical point on a phase diagram?
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How are the phases of matter represented on the phase diagram?
How are the phases of matter represented on the phase diagram?
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What phase is illustrated by the upper middle area of the phase diagram?
What phase is illustrated by the upper middle area of the phase diagram?
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Which specific heat change is associated with heating curves?
Which specific heat change is associated with heating curves?
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The phase boundaries on the diagram represent which kind of transitions?
The phase boundaries on the diagram represent which kind of transitions?
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Which statement is true about phase transitions in terms of temperature?
Which statement is true about phase transitions in terms of temperature?
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What is a characteristic of particles in solids?
What is a characteristic of particles in solids?
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Which property is true for liquids?
Which property is true for liquids?
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Which statement about electronegativity is correct?
Which statement about electronegativity is correct?
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What type of interaction results from the attraction of ions?
What type of interaction results from the attraction of ions?
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What defines a nonpolar molecule?
What defines a nonpolar molecule?
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How do particles in liquids behave when heated?
How do particles in liquids behave when heated?
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Which of the following describes the relationship between intramolecular and intermolecular forces?
Which of the following describes the relationship between intramolecular and intermolecular forces?
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What effect does heat have on the density of liquids?
What effect does heat have on the density of liquids?
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What is the electronegativity difference for iodine monobromide?
What is the electronegativity difference for iodine monobromide?
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Which scenario is likely to Result in a polar molecule?
Which scenario is likely to Result in a polar molecule?
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Which of the following statements about London Dispersion Forces (LDF) is accurate?
Which of the following statements about London Dispersion Forces (LDF) is accurate?
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What is a necessary condition for a molecule to exhibit a dipole moment?
What is a necessary condition for a molecule to exhibit a dipole moment?
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Which type of intermolecular force (IMF) is replaced when a stronger IMF is present?
Which type of intermolecular force (IMF) is replaced when a stronger IMF is present?
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What characterizes nonpolar molecules in terms of dipole moments?
What characterizes nonpolar molecules in terms of dipole moments?
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Which molecule is likely to be considered polar?
Which molecule is likely to be considered polar?
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What happens to London Dispersion Forces as molecules become larger?
What happens to London Dispersion Forces as molecules become larger?
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What happens to the viscosity of a liquid as the molecular size increases?
What happens to the viscosity of a liquid as the molecular size increases?
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Which type of intermolecular force is primarily responsible for the higher boiling point of water compared to hexane?
Which type of intermolecular force is primarily responsible for the higher boiling point of water compared to hexane?
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What are the characteristics of capillary action?
What are the characteristics of capillary action?
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At what temperature does water boil under 1 atm pressure?
At what temperature does water boil under 1 atm pressure?
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Which statement best describes vaporization?
Which statement best describes vaporization?
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What is the relationship between intermolecular forces (IMF) and boiling points?
What is the relationship between intermolecular forces (IMF) and boiling points?
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What is an example of capillary attraction?
What is an example of capillary attraction?
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How do longer hydrocarbons affect boiling and melting points?
How do longer hydrocarbons affect boiling and melting points?
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Which of the following describes the process at the boiling point?
Which of the following describes the process at the boiling point?
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Study Notes
Kinetic Molecular Model
- Explains the properties of solids and liquids.
- Explains how intermolecular forces and kinetic energy contribute to the properties of matter.
Intermolecular Forces
- Attractive forces between neighboring particles of one or more substances.
- Pull particles together.
Intramolecular Forces
- Forces inside/within a molecule.
- Ionic bond (metal + nonmetal)
- Covalent bond (Both nonmetals)
- Metallic bond (Both metals)
Kinetic Energy
- Keeps particles at a distance and/or moving around.
- Dependent on the temperature of the substance.
- Higher temperature, higher kinetic energy.
Characteristics of Solids & Liquids
Properties of Solids
- Definite shape and volume.
- Does not flow.
- Incompressible (particles are tightly packed).
- Expand when heated (to a lesser extent than liquids and gasses).
- Denser than liquids.
- Solids assume a crystalline structure when they have a highly ordered packing arrangement.
- Solids that have no definite form, such as rubber and wax, are amorphous solids.
Particles of Solids
- Strongly attracted to each other.
- Vibrate in fixed positions.
- Vibrate faster when heated.
- Intermolecular forces between their particles are stronger than those in liquids, making the solid rigid.
Properties of Liquids
- Definite volume but no definite shape.
- Flow and take the shape of a container.
- Very difficult to compress.
- Slightly expand when heated.
- Denser than gasses.
Particles of Liquids
- Weakly attracted to each other; easily break their interaction.
- Move more freely than those in solids; slide past each other. This makes liquids flow.
- Move faster when heated.
Chemical Bonding
- Any of the interactions that account for the association of atoms into molecules, ions, crystals, and other species.
- Holds together most molecules due to strong attractive forces.
Intermolecular Force
- Force between molecules.
- London dispersion force (LDF)
- Dipole-dipole interaction
- Hydrogen bond
- Ion-dipole interaction
Strength of Bonds
- Intramolecular > Intermolecular
- Intramolecular bonds are stronger than intermolecular bonds.
Attraction
- Results from the interaction of two or more ions forming a bond.
Electronegativity
- Ability of an atom to attract an electron pair shared with another atom in a chemical bond.
- Helps determine polarity.
Polarity
- Comes from the uneven distribution of electrons among the various atoms in a molecule.
Polar
- Uneven distribution of electrons.
Nonpolar
- Electrons are evenly distributed.
- Diatomic atoms.
- Molecules that only contain carbon and hydrogen, such as CH4 (methane) and C2H6 (ethane). The EN difference of carbon and hydrogen is small (< 0.5).
Notes on Polarity
- The arrow always points toward the atom with the stronger electronegativity.
- To find the electronegativity difference, subtract the smaller value from the bigger value. For example:
- Iodine monobromide: I = 2.7; Br = 3.0
- 3.0 - 2.7 = 0.3 (nonpolar).
Types of IMF
-
London Dispersion Forces (LDF)
- Present in all molecules, regardless of their polarity.
- Weakest type of IMF.
- Only IMF present in nonpolar molecules.
- Mas malayo, mas weak (the greater the distance, the weaker the force).
- Exists between all atoms and molecules.
- All molecules have LDF, but since it is weak, it is often replaced by a stronger type of IMF.
- Arise from the continuous movement of electrons in particles.
- LDF is an attraction between a temporary dipole and an induced dipole:
- Nonpolar molecules have zero dipole moment because their electron density is uniform and symmetrical.
-
Dipole-dipole interaction
- Occurs with polar molecules.
- Stronger than LDF.
-
Hydrogen bond
- Strongest type of IMF.
- Only occurs when hydrogen is bonded to a highly electronegative element, like oxygen, nitrogen, or fluorine.
- Leads to high boiling points in molecules like water.
-
Ion-dipole interaction
- Occurs between ions and polar molecules.
Notes on LDF
- Bigger the molecular size, higher viscosity.
- Higher temperature, mas mabilis na flow, lower viscosity (faster flow, lower viscosity).
Temperature
- Concept of boiling point and melting point of a substance.
- The greater the IMF, the higher the boiling and melting point.
- The longer the hydrocarbon, the lower the boiling and melting point temperature.
Boiling Point
- Temperature at which its vapor pressure = external or atmospheric pressure.
- Increasing the temperature of a liquid raises the kinetic energy of its molecules until the energy of the particle movement exceeds the intermolecular forces that hold them together.
- Temperature at which a liquid boils under an atmospheric pressure of 760 mm Hg (1 atm) is referred to as the normal boiling point.
- Normal BP of water = 100°C.
- The greater the IMF, the higher the energy needed to increase the kinetic energy of molecules to break these forces. For example:
- Water has a higher boiling point than hexane because of its strong hydrogen bonds (water), unlike hexane, which only has LDF.
Molar Heat of Vaporization & Condensation
- About absorbing or releasing heat.
- Water escapes to form another state of matter.
Vaporization
- Absorbs heat, liquid to gas.
- When water changes from liquid to gas, enough energy is needed to break the bonds holding the water molecules together in the liquid form.
Condensation
- Releases heat, gas to liquid.
Heating or Cooling
- A graphical representation of the pressure-temperature relationships that apply to the equilibria between the phases of a substance.
- Useful in determining the combination of temperature and pressure at which a substance will exist as a solid, liquid, or gas.
- Focuses on the equilibrium states of matter.
- Does not involve time or heat addition/removal.
- Example of sublimation: dry ice.
- Illustrates the conditions under which a substance exists as a solid, liquid, or gas, including critical points and triple points.
Components of a Heating Curve
Area
- Represents the phases of a matter.
- Single phase of matter exists.
- Solid: leftmost area.
- Liquid: upper middle area.
- Gas: rightmost area.
Line
- Represents the phase changes of a matter.
- Two phases of matter exist.
- The boundary between the different phases:
- First line from the bottom: sublimation or deposition.
- Second line (left): melting or freezing.
- Third line (right): evaporation or condensation.
Points
- Represent a specific set of conditions under which a particular phase or phase change of a substance occurs.
-
Critical point:
- Can't escape the gas state.
- You can't differentiate between liquid and gas.
-
Phase-boundary point:
- The point at which you can go between states.
-
Critical point:
Notes on Heating and Cooling Curves
- Phase changes occur with increased temperature.
- Heating curve: Endothermic.
- Cooling curve: Exothermic.
Capillary Action
- Force that helps liquids to climb against gravity on the surface of something else (adhesive).
- Capillary attraction: Greater adhesion.
- Capillary repulsion: Greater cohesion.
- Strength has a direct relationship with the strength of IMF.
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Description
Explore the principles of the Kinetic Molecular Model as it applies to solids and liquids. This quiz delves into intermolecular and intramolecular forces, the impact of kinetic energy, and the unique properties that define solids and liquids. Test your understanding of how these concepts interact in the realm of matter.
