Term
|
Definition
| lack an ordered internal structure. Atoms are randomly arranged. |
|
|
Term
|
Definition
| two or more different molecular forms of the same element in the same physical state. |
|
|
Term
|
Definition
| the atoms, ions, or molecules that make up the solid substance are arranged in an orderly, repeating, 3D pattern (crystal lattice). The shape of the crystal reflects the arrangement of the particles within the solid. |
|
|
Term
| Characteristics of solids |
|
Definition
| ordered structure, do not flow, have intermolecular forces of attraction |
|
|
Term
| Characteristics of a liquid |
|
Definition
| lacks ordered structure, flows, has intermolecular forces of attraction |
|
|
Term
| Regarding intermolecular forces: a gas is likely to have... |
|
Definition
|
|
Term
| Regarding intermolecular forces: a solid is likely to have... |
|
Definition
|
|
Term
| Regarding intermolecular forces: a liquid is likely to have... |
|
Definition
|
|
Term
|
Definition
| when a reversable reaction ceases to change its ratio of reactants/products, but substances move between the chemicals at an equal rate. |
|
|
Term
|
Definition
| when the vapor pressure and the atmospheric pressure are equal. |
|
|
Term
| What is energy measured in? |
|
Definition
|
|
Term
| What is mass measured in? |
|
Definition
|
|
Term
|
Definition
> mass = > energy
< mass = < energy |
|
|
Term
| What is specific heat measured in? |
|
Definition
| (joules) over (grams times degrees Celsius) |
|
|
Term
|
Definition
> specific heat = > energy
< specific heat = < energy |
|
|
Term
| What do you measure temperature in? |
|
Definition
|
|
Term
| Condensation is what kind of process? (endothermic or exothermic) |
|
Definition
|
|
Term
| Freezing is what kind of process? (endothermic or exothermic) |
|
Definition
|
|
Term
| What is the relationship between pressure and volume? |
|
Definition
> volume = < pressure
< volume = > pressure |
|
|
Term
|
Definition
| PV=PV (pressure & volume) |
|
|
Term
| What is the relationship between temperature and volume? |
|
Definition
> temperature = > volume
< temperature = < volume |
|
|
Term
|
Definition
| V/T=V/T (volume and temperature) |
|
|
Term
| What is the relationship between temperature and pressure? |
|
Definition
> temperature = > pressure
< temperature = < pressure |
|
|
Term
| What is Gay-Lussac's Law? |
|
Definition
| P/T=P/T (pressure and temperature) |
|
|
Term
| What is the combined gas law? |
|
Definition
| PV/T=PV/T (pressure, volume, and temperature) |
|
|
Term
| What is the ideal gas law? |
|
Definition
| PV/Tn=PV/Tn (pressure, volume, temperature, and MOLES) |
|
|
Term
| When is a reaction spontaneous? |
|
Definition
1. When heat is lost (exothermic) and there is an increase in entropy.
2. When the the amount of heat gained (endothermic) is smaller than the increase in entropy.
3. When the amount of heat lost (exothermic) is bigger than the decrease in entropy. |
|
|
Term
| When is a reaction nonspontaneous? |
|
Definition
1. When heat is gained (endothermic) and entropy decreases.
2. When the amount of heat gained (endothermic) is bigger than the increase in entropy.
3. When the amount of heat lost (exothermic) is smaller than the decrease in entropy. |
|
|
Term
|
Definition
|
|
Term
| What will ALWAYS increase the rate of a reaction? |
|
Definition
| Decreasing the particle size. |
|
|
Term
| What will always increase the rate of which a solution is formed? |
|
Definition
|
|
Term
| What increases the rate at which a solution is formed? |
|
Definition
|
|
