GEN CHEM (CLEAR) - 6.5-6.9 Key Terms

Wave function

uses math to determine precise energy but not exact location

probability density

gives the estimate of an electron's location based on probable regions

electron-density distribution

graphs the likelihood of an electron being in a specific location (often represented by a cloud; usually darker toward the nucleus but lighter further from the nucleus because electrons are naturally pulled toward the nucleus)

Orbitals

the regions in an atom where it is probable to find electrons; different orbitals in different regions of the atom are shaped differently; marked by a number and letter (1s, 2p, 3d, etc)

shell

all orbitals with the same n value (3s, 3p, 3d, 3f)

subshell

all orbitals with the same n and l values (all 3p)

principle quantum number

denotes the shell that the orbital is in; the numbers in electron configurations; only positive integers; represented by the letter n

angular momentum quantum number

denotes the type of orbital/how many orbitals there are in a shell/subshell; the letters in electron configurations; repersented by the letter l     

-S = spherical; innermost; 1 orbital; holds up to 2 electrons    

-P = dumbbell; 2nd; 3 orbitals; holds up to 6 electrons     

-D = clover; 3rd; 5 orbitals; holds up to 10 electrons     

-F = flower-ish; outermost; 7 orbitals; holds up to 4 electrons

magnetic quantum number

represents the 3D orientations of the orbital(s); determines which axis its on (3px, 3py, 3pz)

-s = 0 (so only 1 way it can be oriented)

-p = 1 (so 3 ways it can be oriented)

-d = 3 (so 5 ways it can be oriented)

-f = 5 (so 7 ways it can be oriented)

The radial probability function

uses math to calculate the likelihood of finding an electron x distance from the nucleus (kinda probability density in a spherical area)

Nodes

places where there is no likelihood of finding electrons; empty space between orbitals

Degenerate orbitals

have the same energy and are found in the same subshell (all the 3p or all the 5f, etc)

spin magnetic quantum number

determines the direction that electrons are spinning; always +1/2 or -1/2; in a single orbital

The Pauli exclusion principle

establishes that no electron can have the exact same principle quantum number (n), angular momentum quantum number (l), magnetic quantum number (m_l), and spin magnetic quantum number (m_s); limits electrons per orbital to two, but those two must have different spins.

electron configuration

shorthandedly explains relative locations of electrons (includes n, l, and the # of electrons in each subshell)

    -1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s²5d¹⁰4f¹⁴6p⁶.........etc

orbital diagram

expands an electron configurations with diagrams that show energy change and opposing electron spins (orbitals are represented by boxes, electrons by half arrows)

Hund's rule

states that all orbitals in a subshell must be filled with one electron (all with the same spin) before doubling up with opposite spinning electrons (sit by yourself if you can)

Valence electrons

the electrons on the outermost shell; are easiest to remove; their release or attraction is what causes reactions to happen

Core electrons

the electrons in shells closer to the nucleus (not valence); are harder to remove and aren't really involved with reactions

Representative (main group) elements

have valence electrons in outermost s or p subshells; in the side "blocks" of the periodic table

Transition elements/metals

have valence electrons in an outermost d subshell; in the middle section of the periodic table

f-block metals

the elements in the "ejected" section of the periodic table; have valence electrons in an outermost f subshell

Lanthanide/rare earth elements

have valence electrons in the 4f subshell; the top row of the "ejected" section of the periodic table

Actinide elements

have valence electrons in the 5f subshell; the bottom row of the "ejected" section of the periodic table