Definitions

the weighted mean mass of an atom of an element relative to 1/12 of the mass of an atom of 12C

the mass of an atom of an isotope compared to 1/12 the mass of an atom of 12C

the energy required to remove 1 electron from each atom in 1 mole of a gaseous element to form 1 mole of gaseous 1+ ions

the attractive force that the outer shell of electrons experiences from the nucleus

the repulsion between electrons in inner shells

a region within an atom that can hold up to 2 electrons with opposite spin

a group of the same type of atomic orbitals within a shell

the ability of an atom to attract the bonding pair of electrons in a covalent bond

the attraction between the d+ H atom on 1 molecule and the lone pair of electrons on the d- Fluorine, Nitrogen or Oxygen on a different molecule

number of particles = ( mass (g) / molar mass (g/mol) ) x 6.02x10^23 (number of particles = moles x 6.02x10^23)

atom economy = ( sum of molar masses of desired products / sum of molar masses of all products ) x 100

percentage yield = (actual yield / theoretical yield ) x100

pV = nRT pressure(Pa) x volume(m^3) = number of moles x gas constant x temperature(K)

8.314 J/mol/K

add 273 degrees

6.02 x10^23

the exact number of atoms of each element present in a molecule

the simplest whole number ratio of atoms in a molecule

a series of compounds with the same functional group, with each successive member differing by a CH2 group, and having the same general formula

when a covalent bond breaks and one electron from the bonding pair is given to each atom previously involved in the bond to create 2 free radicals

an atom with a single unpaired electron that is very reactive

when a covalent bond breaks and one atom takes both of the bonding pair of electrons to become a negative ion, leaving the other atom as a positive ion

the overlapping of 2 orbitals directly in the plane of the 2 atoms

using water to break chemical bonds opposite of condensation