H CHEM SPRING SEMESTER VOCAB

1 mole = …

6.02 x 10^23 particles

empirical formula

simplest ratio

molecular formula

actual ratio

hydrate

contains water molecules (water loosely bonded, compound still solid)

anhydrous

without water

stoichiometry

amount of reactants + products = chemical reaction

theoretical yield

maximum of product that you can make from reaction

limiting reactant

limit of reaction, chooses how many product there will be

excess reactant

left over (shown by smallest yield)

percent yield

actual yield/theoretical yield x 100

kinetic molecular theory

1. gas particles = so fast + far part = do not influence each other

2. move in straight lines (collisions are elastic)

3. energy depends on mass & velocity

effusion

movement of gas through a TINY OPENING

diffusion

mixing one gas into another

pressure

P = F/A

Dalton's Law of Partial Pressure

Ptotal = P1 + P2 + P3…

Combined Gas Law

P1 V1 / T1 = P2 V2 / T2

absolute zero

-273 C

Avogadro's Principle

equal VOLUMES of a gas at the same PRESSURE + TEMP have the same # of MOLES

STP

standard temperature (O C or 273 K) and pressure (1 atm)

ideal gas law

PV = nRT

first law of thermodynamics

energy can be transferred and transformed, but it cannot be created or destroyed.

Calorie

1000 calories

Joule

SI unit for energy, 4.184 J = 1 cal

specific heat

q = mcΔT (raises temp of 1g of ANY substance 1 C)

enthalpy

energy at constant pressure

endothermic

ABSORBED (+) ; needs MORE ENERGY to make products

exothermic

RELEASED (-) ; has too much energy to form products

calorimeter

determines SPECIFIC HEAT of an unknown substance; cylinder

Hess's Law

total enthalpy changes is same regardless how many steps in reaction

spontaneous process

without outside intervention; energy is already present

entropy (S)

of ways energy can be distributed (more distributed, more used)

Second Law of Thermodynamics

entropy of universe is always increasing

Gibbs Free Energy

determines if spontaneous; energy available to do work

solution

solute in a solvent (salt water)

solute

being dissolved (salt)

solvent

does the dissolving (water)

molarity

M = mol/L

percent by mass

mass of solute / mass of solution x 100%

solvation

surrounding a solute w/ a solvent to form a solution

saturated solution

max amount dissolved

supersaturated

oversaturated at elevated temp & slowly cooled down (can lead to crystalization)

Henry's Law

at given temp, solubility of gases = proportional to their pressure (S1 / P1 = S2 / P2

colligative particles

depend on AMOUNT OF PARTICLES & not type of substance

Equilibrium expression

Keq stuff

le chatelier's principle

reactions can take place to relieve applied stress to make reactant or product (stressors: pressure, temp, volumes, moles)

arrhenius model

when dissolved in water… acids release hydrogen; bases release hydroxide

bronsted lowry model

ACIDS = proton donors ; BASES = proton acceptors

strong acid/base

completely dissociated/ionized

weak acid/base

don't completely dissociate, less free ions more molecules

pH

potential hydrogen, measurement of hydrogen in concentration in aqueous solution

neutralization

amounts equal (pH + pOH + 7, 7)

titration

determines concentration by reacting known volume with known concentration

equivalence point

point when color changes

organic compound

carbon bonded to hydrogen

hydrocarbon

simplest organic compounds, hydrogen + carbon

saturated hydrocarbon

single bond

unsaturated hydrocarbon

double / triple bond

line angle notation

each line segment is a carbon; hydrogen implied

substituent group

branches attached to longest chain

parent chain

longest chain

cyclic hydrocarbon

compounds with a hydrocarbon ring

benzene

a cycloalkENE with formula C6H6; double bonds are delocalized = more stable

isomer

same molecular formula, different structures

structural isomer

same chemical formula, different arrangements

stereoisomer

same order, oriented differently in space

cis

(Z); same side

trans

(E); across from

chirality

MIRROR IMAGE but don't function the same

functional group

halocarbon, alcohol, ether, amine, aldehyde, ketone, carboxylic acid, amide, ester