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Intermol. Force **
Part 3
| Question | Answer |
|---|---|
| How is kinetic energy and vapor pressure related? | kinetic energy allow molecules to overcome the attractive force between the molecules; the weaker the force, more molecules escape, the more molecules escape the greater the vapor P. |
| why does vapor P increases with T? | at higher T, more molecules have the KE to escape the attractive force of the liquid phase. The more molecules in the vapor phase, the higher the vapor pressure |
| What will the interior bubble do if the external P is greater than the vapor P? | it will collapse |
| If the external P is equal to or lower than the vapor P, then the bubble will... | remain or expand and the liquid boils |
| At 100 C the vapor P of water is what? | 760 torr (1 atm), water boils. |
| "triple point" | condition of T and P where are 3 physical states are in equilibrium |
| gases are most likely under... | high T |
| solids are most likely under... | high P |
| which is denser, liquid water or ice? | liquid, the liquid state is more compacted than the solid state for water |
| what T will water boild? | 100 C if the water is at 1 atm of pressure |
| at pressure below 4.58 torr, water will be... | a gas or solid, there can be no liquid phase. |
| give examples of crystalline solids | diamonds, and quartz crystals, |
| crystalline solids | atoms/molecules/ions pack together in an ordered arrangement. Have flat surfaces w/unique angles between faces and unique 3-dimensional shape |
| amorphous solids | no ordered structure, no well defined faces/angles/or shape. Often are mixtures of molecules which do not stack together well, or large flexible molecules. |
| examples of amorphous solids | glass and rubber |
| crystal lattice | identical points on each unit cell of the crystal. |
| cubic | shape of unit cell. all sides are equal length, all angles are 90 degrees |
| does a unit cell have to be cubic? | no |
| what are the 2 arrangement that sphere can be pack in 3 dimensions | hexagonal close packing and cubic close packing |
| hexagonal close packing | layer 3 sits in depressions of layer 2 and is directly above positions in layer 1 |
| cubic close packing | layer 3 sits in depressions of layer 2 but is not directly above positions in layer 1 |
| coordination number | number of particles surrounding a particle in the crystal structure |
| what intermolecular forces hold molecular solids together? | dipole-dipole, dispersion, and hydrogen bonds |
| Why are molecular solids soft and have low melting T? | because their intermolecular forces are weaker than chemical (covalent) bonds |
| dispersion bond energy (kJ/mol) | about 1.0 |
| hydrogen bond (strongest dipole-dipole) bond energy (kJ/mol) | about 12 - 16 |
| ionic bond energy (kJ/mol) | about 50 - 100 |
| covalent bond energy (kJ/mol) | about 100 - 1000 |
| what are the force that holds covalent solids together? | covalent bonds |
| what is the force that holds ionic solids together? | ionic bonds |
| What does the strength of the ionic interaction dependent on? | the strength of the charge of the ions |
| the bonding of metallic solids increases with what? | the #s of electrons available for bonding |
| why can metals carry electrical current? | because of the delocalization of electrons (electrons are free to move about the metal structure) |
| what are the 3 kinds of cubic unit cells? | primitive cubic, body-centered cubic, and face-centered cubic |
| which solids are hard and brittle and have high melting point? | ionic solids |
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