alkali metals
1st group 1+ charge
alkaline earth metals
2nd group 2+ charge
transition metals
3rd -12th group varying charges, including Sn and Pb, excluding Ag and Cd and Zn
Ag charge
1+
Cd and Zn charge
2+
halogens
17th group 1- charge
noble gases
18th group no/neutral charge
metalloids
along the staircase, excluding Al some of the characteristics of metals
metals
left to the staircase generally solid, shiny, lustrous, ductility, malleable, conductive
nonmetals
right to the staircase opposite/no characteristics of metals
wavelength
distance between 2 identical points on consecutive waves λ
frequency
the number of waves that pass a fixed point in unit time ν
energy
energy of a specific quantum of energy E=hν frequency times planck's constant
energy and frequency relationship
directly related
energy and wavelength relationship
inversely related
wavelength and frequency relationship
inversely related
speed of light equation
c=λν
Bohr's Model
circular rings electrons follow a fixed path energy levels n=1 to n=7
Quantum Mechanical Model (QMM)
different shaped areas with a 90% chance of finding an electron electrons do not follow fixed path energy levels n=1 to n=7
Orbit
Heisenberg Uncertainty Principle
we cannot know both the position and speed of a particle with perfect accuracy, the more we know about the position the less we know about the momentum and vise versa
Orbital
an area where there is a 90% chance of finding a given electron different shapes = s, p, d, f energy levels n=1 to n=7
S Orbital
spherical starts at 1st energy level (n=1)
node
an area with no electrons/low probability of electrons being found
P Orbital
dumbbell/lobe starts at 2nd energy level (n=2) each level contains 3 degenerate orbitals
degenerate orbitals
orbitals having the same energy levels but they are positioned differently
D Orbital
clover leaf starts at 3rd energy level (n=3) each level contains 5 degenerate orbitals
F Orbital
starbursts starts at 4th energy level (n=4) each level contains 7 degenerate orbitals
energy levels
the fixed amount of energy that a system described by quantum mechanics
valence electrons
outer electrons in an atom
core electrons
inner electrons in an atom
orbital diagram
a type of notation which illustrates an atom's electron distribution and electron spin within orbitals.
Hund's rule
electrons must be unpaired before they are paired in a sublevel
Pauli Exclusion
no more than two electrons can occupy the same orbital and two electrons in the same orbital must have opposite spins
Aufba Principle
electrons fill from lowest to highest energy
period similarities
same number of core electrons
group similarities
same number of valence electrons
Trends with atomic radius
decreases as you go the the left and increases as you go down
Trends with ionization energy
increases as you go the the left and decreases as you go down
atomic radius and IE relationship
inversely related
atomic radius and reactivity relationship
directly related
reactivity and IE relationship
inversely related