AP Chemistry Ultimate Guide

attraction between opposite charges and the strength can vary depending on how far the charges are from each other.

shape of the space an electron can be found in

the energy an atom must absorb to eject an electron

electrons must fill up orbitals, subshells, and shells in order of increasing energy.

electrons can jump to higher energy levels when absorbing this energy

demonstrates the electron organization of an atom

number of atoms in a single mole of any given element

have an overall negative charge

have an overall positive charge

how much an element attracts electrons to it’s nucleus

expresses the concentration of a solution in terms of volume

the closer an electron is to the nucleus, the stronger the attraction and the less potential energy there is

electrons in the outermost shell

graph of the ionization energies for all electrons when ejected from the nucleus.

have significantly less mass than protons and neutrons and do not contribute to the mass.

atoms of an element with different numbers of neutrons, but same amount of protons.

percent by mass of each element in a compound.

a molecule with a similar radius replaces a metal atom

stored, motionless energy

energy in motion

between two nonmetals

between two metals

between a metal and nonmetal

an atom with a smaller radii fills the space between metal atoms with larger radii

strongest bond, held together in lattice structure

electron organization for metallic bonds

different yet equally likely forms of a molecule’s structure f

the most likely version of a lewis dot structure to form

three-dimensional structure of a molecules arrangement

IMF between all molecules, very weak attraction, caused by random electron movements

oppositely charged ends of a molcule

the rate at which a gas will escape a pin-sized hole from high to low pressure

an unequal share of electrons

equally shared electrons

IMF that occurs when a positive dipole of a molecule is attracted to the negative dipole of another molecule

IMF between hydrogen and oxygen, nitrogen, or fluorine

a compound that can donate a proton

compound capable of accepting a proton

a compound that can behave as both an acid or a base

a substance that speeds up a reaction rate

a substance created in one elementary step and used up in another

how long it takes for half of a substance to decompose

energy required for a reaction to start/occur

when energy is transferred from system to surroundings (beaker feels hot)

heat transfers from surroundings to system (beaker feels cold)

releasedw

absorbed

enthalpy change

total heat content of a system (H)

amount of energy released when one mole of a compound is produced from pure substances

the relative amount of products and reactants at any point in time

equilibrium constant

when a stress is added to a reaction, the equation will change to adjust for the stress and return to equilibrium

when an element is added to a solution with a salt, the salt equilibrium will change if the element is similar to the salt

reaction is reversible and constantly occurring with no change in concentrations of product or reactants

temperature

acid and base react, producing water and a salt

dissolves completely in water

1.0 x 10^-14

can resist pH change when small amounts of strong acid or base added

can give up more than one proton

just enough acid/base added to base/acid to neutralize

G, determines thermodynamic favorability based on the entropy, enthalpy, and temperature

S, the disorder of a system, “chaos”

25 celsius, 1 atm, 1M

determine the average mass for different isotopes of a specific element

when two electrons fill up an orbital, they must spin in opposite directions: clockwise and counterclockwise.

when electrons are filling the orbitals of the subshell, they will only have two in one orbital when it is not possible to have each electron in its own orbital.

has all shells completely full of electrons

two electron pairs

three electron pairs

four electron pairs

five electron pairs

six electron pairs

gases are composed of a large number of particles that behave like hard, spherical objects in a state of constant, random motion.

low

high

the amount of light that does not get through (gets absorbed) by a colored solution

used to determine an unknown element in a precipitate reaction

carbon + hydrogen (and sometimes oxygen) is ignited and produces CO2 and waters

when elements or simple compounds are combined to form a single, more complex compound.

electrons are swapped between reactants and the oxidation states of the reactants are changed.

opposite of synthesis- occurs usually in the presence of heat

two aqueous solutions mixing to create a solid precipitate.

when an acid (H+) reacts with a base (OH)- to form water and a salt.

alkali metals, ammonium, nitrate

zero

most common charge

total charge

+1

-1

based on the activation energy for a reaction and the temperature

log[A]=-kt+ln[A]₀

rate = k

reactions only occur when chemicals collide with each other with sufficient energy (activation energy)

1/[A] = kt+ 1/[A]₀

t= .693/k

not evenly mixed, not all parts are equal

evenly mixed, all parts are equal

the steps that occur in a reaction