Term
|
Definition
| a chemical compound composed of only two elements |
|
|
Term
|
Definition
| elements that are present in the gaseous state as molecules composed of two atoms (O2, N2, Cl2, H2, F2, I2, Br2) |
|
|
Term
|
Definition
| a charged ion composed of two or more atoms covalently bonded |
|
|
Term
|
Definition
| a number assigned to an element in chemical combination that represents the number of electrons lost |
|
|
Term
|
Definition
| a compound, typically a crystalline one, in which water molecules are chemically bonded to another compound or an element (a solid with water in it) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| a number equal to the sum of the atomic masses of the atoms in a molecule |
|
|
Term
|
Definition
| a group of atoms bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction |
|
|
Term
|
Definition
| a formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms |
|
|
Term
|
Definition
| a principle stating that mass cannot be created or destroyed |
|
|
Term
| Chemical Equations (States) |
|
Definition
aq - dissolved in water
l - liquid
s - solid
g - gas |
|
|
Term
|
Definition
| a substance that takes part in and undergoes change during a reaction |
|
|
Term
|
Definition
| a substance that is formed as the result of a chemical reaction |
|
|
Term
|
Definition
| a substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change |
|
|
Term
|
Definition
| energy taken in, feels cold to the touch |
|
|
Term
|
Definition
| energy given off, feels warm to the touch |
|
|
Term
|
Definition
| a number placed in front of a molecule in a chemical equation representing the number of atoms needed |
|
|
Term
|
Definition
| a number placed after an atom in a molecule in a chemical equation stating the number of atoms needed to stabalize the charge |
|
|
Term
|
Definition
light a splint of wood
stick it in gas
if you hear a pop then there is hydrogen |
|
|
Term
|
Definition
light a splint of wood
blow it out
stick it in gas
if relights then there is oxygen |
|
|
Term
|
Definition
| the reactant that is used up; once it is all used, the reaction stops |
|
|
Term
|
Definition
| the reactant that is not used up |
|
|
Term
|
Definition
| the temperature at which there is no molecular motion |
|
|
Term
|
Definition
caused by the number of collisions of gas molecules
-standard pressure = 1 atmosphere = 760mmHg = 760torr = 101.3 Kpa |
|
|
Term
|
Definition
| air pressure decreases with altitude |
|
|
Term
|
Definition
|
|
Term
|
Definition
| measure of average kinetic energy of particles |
|
|
Term
|
Definition
Melting
Sublimation
Vaporization
Freezing
Deposition
Condensation |
|
|
Term
|
Definition
| solid to liquid (endothermic) |
|
|
Term
|
Definition
| solid to gas (endothermic) |
|
|
Term
|
Definition
| liquid to gas (endothermic) |
|
|
Term
|
Definition
| liquid to solid (exothermic) |
|
|
Term
|
Definition
| gas to solid (exothermic) |
|
|
Term
|
Definition
| gas to liquid (exothermic) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| when pressure goes up, volume goes down, inversly related (P1V1=P2V2) |
|
|
Term
|
Definition
| when temp goes up volume goes up, directly related (V1/T1=V2/T2) |
|
|
Term
|
Definition
PV=nRT
n = # moles
R = ideal gas law constant |
|
|
Term
| Combustion of a Hydrocarbon |
|
Definition
| the combustion of any hydrocarbon always produces the same products: CO2 and H2O (carbon dioxide and water) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| of water is 0*C (melting point = freezing point) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| when a solid settles out of a solution (the solid is the precipitate) |
|
|
Term
|
Definition
find the amount of product theoretically possible by using the given amount of limiting reactant and stoichiometry
divide the amount of product actually produced in the chemical reaction by the amount of product theoretically possible
Multiply by 100 to make a percent (ideally close to 100) |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
| gas leaking out of opening |
|
|
Term
|
Definition
| the mathematical expression of the relationship between mass of particles and rate of diffusion/effusion |
|
|
Term
|
Definition
| random arrangement, melts over a range of temperatures; examples --> glass and wax |
|
|
Term
|
Definition
| geometric patterns, definite melting point; examples --> sale and water |
|
|
Term
|
Definition
| contains Avogadro's number of atoms |
|
|
Term
|
Definition
| water that has been purified (chemically pure) |
|
|
Term
|
Definition
| energy needed to start a reaction (match for the bunsen burner) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| standard temperature is 273 Kelvin (0*C) |
|
|
Term
|
Definition
| used in compounds just like monatomic ions (Mg2 or N --> one atom), use parenthesis around the polyatomic ion only if more than one is needed, most are negative and end in 'ite' or 'ate' |
|
|
Term
|
Definition
| means standard pressure and temperature, which is 1 atmosphere and 273 Kelvin |
|
|
Term
| Standard Molar Volume of Gas |
|
Definition
| 1 mole of any gas at STP has the same volume as 22.4Liters |
|
|
Term
|
Definition
| when temp goes up pressure goes up (directly related) P1/T1=P2/T2 |
|
|
Term
|
Definition
| P1V1/T1 = P2V2/T2 (always use Kelvin) |
|
|
Term
|
Definition
| at 0 Kelvin would have no volume |
|
|
Term
|
Definition
1st write balanced chemical equation
2nd the given amount, must be converted to moles
3rd use the mole ratio to change given moles into moles of what you are trying to find
4th convert these moles into grams if needed |
|
|
Term
|
Definition
| (M) moles solute/ L solution |
|
|
Term
|
Definition
| (m) moles solute/ kg solvent |
|
|
Term
|
Definition
| no more solute may be dissolved in a solvent |
|
|
Term
|
Definition
| being able to dissolve more solute in a solvent |
|
|
Term
|
Definition
| a solution that contains a higher than saturation concentration of solute |
|
|
Term
|
Definition
| a state of an atom that has had at least one electron removed |
|
|
Term
|
Definition
| when a substance is placed in water, the water molecules pull the other molecules apart |
|
|
Term
|
Definition
| a substance that indicates the degree of acidity or basicity of a solution through color change (litmus paper, pH paper) |
|
|
Term
|
Definition
| measure of hydrogen ion concentration |
|
|
Term
|
Definition
| involves everything in the equation but the spectator ions |
|
|
Term
|
Definition
| an ion that exists in the same form on both the reactant and product sides of the equation |
|
|
Term
|
Definition
| an acid or base solution of known concentration is mixed with and acid or base solution of unknown concentration |
|
|
Term
|
Definition
| reaction between an acid and base which produces a neutral solution (pH 7) |
|
|
Term
|
Definition
made of hydrogen and carbon
ending in 'ane' means only single bonds present
prefix tells number of carbons
meth, eth, prop, but, pent, hex, hept, oct, non, dec
-alkanes are saturated (full of hydrogen) |
|
|
Term
|
Definition
| a cyclopentene with 3 double bonds |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| 5 Types of chemical reactions |
|
Definition
synthesis
decomposition
double displacement
single displacement
combustion |
|
|
