the beginning of the end
protons and neutrons
subatomic particles in the nucleus
electrons
subatomic particles in the outer shells of the atom
1 amu
mass of protons and neutrons
mass number
protons + neutrons
atomic number
number of protons / nuclear charge
number of neutrons
mass number - atomic number
number of electrons
equals the number of protons
Isotopes
atoms of the same element and same atomic number but different mass numbers
atomic mass
average mass of isotopes by abundance
mass spectrometer
identifies isotopes; each peak represents a different isotope and height = relative abundance
photoelectron spectroscopy
each peak represents a subshell, and the height of the peak represents the number of electrons; peaks further to the left have an increased binding energy and are part of a lower energy level.
binding energy
energy required to remove an electron from the corresponding shell
core electrons
inner electrons
valence electrons
outer electrons
s sublevel
2 e-
p sublevel
6 e-
d sublevel
10 e-
f sublevel
14 e-
aufbau principle
to “build up” electrons are added to the lowest subshell first
Mg electron configuration
Sulfur electron configuration
S^(2-) electron configuration
Gallium electron configuration
Phosphorus electron configuration
Neon electron configuration
Rhodium electron configuration
Coulomb’s Law
Coulombic force = (charge on particle 1 * charge on particle 2) / distance between particles²
charge increases, distance decreases
Coulombic force increases when
Effective Nuclear Charge
approximate nuclear charge felt by the outer electron due to shielding by the core electrons
Electron affinity
energy released when an electron is added to an atom
Cation
positively charged ion (Ca2+)
Anion
negatively charged ion (Cl-)
empirical formula
mole ratio of elements in a compound in simplest form
molecular formula
(molar mass / mass of empirical formula) * empirical formula
% composition
(mass of X / molar mass of compound) * 100
Pb
element?
S2O
How to find empirical formula