Exam 2 Flashcards
principle quantum number
n = energy level of electron/orbital
positive integer
angular momentum quantum number
l = shape of orbital
l = 0, 1, 2, …, n-1
magnetic quantum number
mₗ = orbital orientation
mₗ = -l, …, 0, …, l
spin quantum number
mₛ = spin of specific electron
mₛ = ±1/2
letter names associated with l values
l = 0, 1, 2, 3, 4
l = s, p, d, f, g
sketch orbital:
n=1
l=0
1s
0 nodes - nucleus doesn’t count
sphere
sketch orbital:
n=2
l=0
2s
1 node - radial
hollow sphere
sketch orbital:
n=2
l=1
2p
1 node - planar
dumbbell shape
sketch orbital:
n=3
l=1
3p
2 nodes - 1 planar, 1 radial
dumbbell with 2 hats
sketch orbital:
n=3
l=2
3d
2 nodes - planar
4 leaf clover or dumbbell with donut
sketch orbital:
n=4
l=2
4d
3 nodes - 2 planar, 1 radial
4 leaf clover or dumbbell with 4 hats
Hund’s Rule
Electrons should be placed evenly across degenerate orbitals before doubling up.
Pauli’s Exclusion Principle
Every electron within an atom has a unique identity, as determined by its n, l, mₗ, and mₛ values.
Aufbau Principle
When determining which electrons are in which orbitals, start from the lowest energy possibilities (orbitals).
paramagnetic
there are unpaired electrons in the atom
net spin non-zero
affected by magnetic fields
diamagnetic
all electrons are paired within the atom
net spin = 0
atomic radius
(definition and periodic trends)
half of the distance between 2 bonded of an element
decreases across periods
increases down groups
effective nuclear charge
(definition and periodic trends)
strength of the pull of the nucleus on electrons
increases across periods
decreases down groups
ionization energy
(definition, periodic trends, and first vs. second ionization energy)
the energy required to move a valence electron
increases across periods
decreases down groups
first vs. second….
ionic bonds nomenclature
e.g. NaCl
e.g. MgSO₄
e.g. FeCl₃
- metal (cation), then nonmetal (anion)
- cation element name + anion with “-ide” ending
- add roman numeral after cation if needed
e.g. sodium chloride
e.g. magnesium sulfate
e.g. iron (III) chloride
cation nomenclature
e.g. Al⁺
e.g. Fe³⁺
add “ion”
add roman numeral after element name if transition metal
e.g. aluminum ion
e.g. iron (III) ion
monoatomic anion nomenclature
e.g. Cl⁻
e.g. O²⁻
add suffix -ide
e.g. chloride
e.g. oxide
molecular compound nomenclature PREFIXES
1-10
1 = mono-
2 = di-
3 = tri-
4 = tetra-
5 = penta-
6 = hexa-
7 = hepta-
8 = octa-
9 = nona-
10 = deca-
molecular compound nomenclature
e.g N₂O
e.g. ICl₃
- less electronegative element first
- add prefixes except for mono- on first element
- add “-ide” suffix to last element
e.g. dinitrogen monoxide
e.g. iodine trichloride