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Chem chp 12
110
| Question | Answer |
|---|---|
| vibration | movement of particles back and forth around a fixed position; solid, liquid, and gas |
| rotation | movement of particles spinning around their own axis; liquid and gas |
| translation | movement of particles from one location to another to another; liquid and gas |
| solid shape, volume, density, compressibility | definite shape, definite volume, high density, almost impossible to compress |
| liquid shape, volume, density, compressibility | takes shape of container, definite volume, high density but lower than solids, slightly compressible |
| gas shape, volume, density, compressibility | take shape of container, no definite volume, very low density, highly compressible |
| Why are gases easily compressible, whereas liquids are not? | because the particles in gas are far apart with lots of empty space whereas liquid are already packed close together |
| Why do ice cubes float in liquid water? Is this typical behavior? | ice floats because it is less dense than liquid water; this behavior is not typical |
| intermolecular forces | attractive forces b/w separate molecules |
| intramolecular forces | strong forces that hold atoms together within a molecule or compound; covalent bonds, ionic bonds, metallic bonds |
| What type of properties does intermolecular forces give rise to? | boiling point, melting point, vapor pressure, viscosity, surface tension, density, state of matter |
| What does this statement mean? "The relative strength of intermolecular forces and thermal energy affects the physical properties of a substance" | intermolecular forces pull particles together while thermal energy makes them move apart |
| What type of properties does intramolecular forces give rise to? | chemical reactivity, bond strength, molecular structure, stability of compounds, how substances form or break chemical bonds |
| Which two related factors primarily determine the physical state of matter at a given temperature? | intermolecular forces and thermal energy |
| Intermolecular forces are electrostatic attractions that occur __________________ the particles of a in a substance or mixture | between |
| Intermolecular forces are typically __________________ than covalent or ionic bonds | weaker |
| Intermolecular forces affect the __________________ properties of a substance | physical |
| The greater the total magnitude of the intermolecular forces, the __________________ the effect on physical properties | greater |
| dispersion forces | weak intermolecular attractions caused by the temporary movement of electrons, weakest type of intermolecular force |
| How do dispersion forces affect physical properties? | stronger dispersion forces = stronger intermolecular attractions = greater effects on physical properties |
| How does molecular shape affect dispersion forces and physical properties? | molecular shape affects how much surface area molecules have to interact with each other, and stronger dispersion forces generally cause higher boiling point, melting point, viscosity, and lower vapor pressure |
| Does n-pentane or neopentane have the higher boiling point and why? | n-pentane has the higher boiling point because it is long and has more surface contact |
| How does the number of electrons affect the strength of dispersion forces? | the more electrons a particle has, the stronger its dispersion forces are |
| polarizability | how easily an atom or molecules electron cloud can be distorted to create a temporary dipole |
| How does the strength of intermolecular forces compare to the strength of covalent or ionic bonds? | intermolecular forces are much weaker than covalent or ionic bonds |
| How does the magnitude of intermolecular forces affect physical properties? | the greater the magnitude or IMF, the greater their effect on physical properties; stronger attractions = particles are harder to separate |
| Rank the following in order of increasing strength of dispersion forces: Ar, He, Kr, Ne. Explain your reasoning | He < Ne< Ar < Kr; dispersion forces become stronger as the number of electrons increase b/c larger e- clouds are more easily distorted |
| Rank the following molecules in order of increasing strength of dispersion forces: Cl2, H2, I2, N2, O2. Explain your reasoning | H2 < N2 < O2 < Cl2 < I2; all of these molecules are nonpolar, so their main intermolecular force is dispersion forces |
| Which has a lower melting point: butane or isobutane? | isobutane has a lower melting point because it is more compact than butane, giving it less surface area for contact b/w molecules |
| Which has a lower melting point: pentene or cyclopentane? | pentane has a lower melting point because its ring structure allows its molecules to pack more efficiently in the solid |
| dipole-dipole forces | attractive forces between polar molecules that help determine a substances boiling point, melting point, and solubility |
| In general, how do the strengths of dipole-dipole forces and dispersion forces compare for compounds of similar molecular mass? | dipole-dipole forces are generally stronger than dispersion forces |
| How is the strength of a dipole-dipole force affected by polarity? | the more polar a molecule is, the stronger its dipole-dipole forces |
| Do molecules that are more polar than other molecules have stronger or weaker dipole-dipole forces? | they have stronger dipole-dipole forces because they have larger partial positive and negative charges |
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