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35 Cards in this Set
- Front
- Back
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What are the five assumptions for the kinetic-molecular theory? |
1. there are many tiny particles that are far apart 2. collisions are elastic 3. there is constant random motion 4. there is no attraction between the particles 5. the temperature depends on the kinetic energy |
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ideal gas |
gas that perfectly fits all the assumptions of the kinetic-molecular theory |
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elastic collision |
no net loss of total kinetic energy, a complete transfer of energy between colliding particles |
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What kind of speed will a small particle have? |
a faster speed |
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what is the formula for kinetic energy? |
kinetic energy= 1/2mv^2 |
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What are the five main physical properties of gasses? |
1. expands 2. fluid 3. low density 4. compressable 5. diffusion and effusion |
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diffusion |
spontaneous mix of particles of multiple substances |
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effusion |
gas particles pass through a tiny opening |
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real gas |
gas that does not completely behave according to the kinetic-molecular theory assumptions |
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Polar molecules are more like which type of gas: real or ideal? Why? |
real as they have strong attractive forces |
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Nonpolar molecules are more like which type of gas: real or ideal? Why? |
Ideal as they have weak attractive forces. |
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Why do liquids have relatively high densities? |
the particles are more tightly packed compared to gasses. this is also why they are not very compressible |
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How do liquids compare to gasses with their rate of diffusion? Why? |
They can diffuse well due to their fluidity, but it is slower than gasses to their stronger attractive forces and closer particles. |
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surface tension |
force that tends to pull adjacent parts of a liquid's surface together; decrease overall surface area |
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capillary action |
attraction of the surface of a liquid to a solid |
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vaporization |
liquid or solid changing to a gas |
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evaporation |
escape from a nonboiling liquid surface to go into a gas state |
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Why does evaporation occur? |
The particles have different kinetic energies, allowing them to pull away from the attractive forces of the liquid into freedom. |
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freezing |
removal of energy as heat to change a liquid to a solid |
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freezing point |
solid and liquid are in equilibrium at 1 atm pressure |
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in crystalline solids, how do melting and freezing points relate? |
they are the same |
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molar enthalpy of fusion |
amount of heat energy needed to melt on mole of a solid at a solid's melting point |
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sublimation |
change of state from a solid directly to a gas |
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deposition |
change of state from a gas to a solid |
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phase diagram |
pressure versus temperature graph that shows when something will be in a certain phase in certain conditions |
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triple point |
when all phases can coexist |
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critical point |
the critical temperature and pressure when it is no longer a liquid |
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critical temperature |
temperature above which a substance cannot be a liquid |
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critical pressure |
lowest pressure where the substance can exist as a liquid while also at critical temperature |
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what is the shape of a water molecule? |
bent |
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what makes water so unique in its physical traits? |
its strong hydrogen bonds |
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why is ice less dense than water? |
as the hydrogen bonds become more organized, empty spaces are left between molecules |
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intermolecular |
forces between molecules and neighboring particles |
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intramolecular |
forces that act within a molecule |
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also some math be ready for that |
good luck i guess |
