Test 6 & 7 Flashcards
what is hund’s rule?
e⁻ fill up all orbitals before they start pairing in them
eqn for lightspeed, c
λ * ν = c
symbol for wavelength
λ, lambda
symbol for frequency
ν, nu
units of frequency
cycles/second → 1/s → s⁻¹ → Hertz (Hz)
eqn for E w/ Planck’s constant h and what it means
E = hν or Energy = Planck’s Constant * frequency to find E in J of 1 photon
what did einstein discover about light, x 2
confirmed Planck’s theory and discovered dual wave/particle nature of light
what is de Broccoli’s eqn for matter wave lengths?
λ = h/(momentum * velocity), where units are in meters
elec config for Cu
[Ar]4s¹ 3d¹⁰
elec config for Cr
[Ar]4s¹ 3d⁵
10⁻⁶
micro
10⁻⁹
nano
10⁻¹²
pico
acronym to remember order of electromagnetic spectrum
Red Meat Is Very Unhealthy, Xspecially Grilled
Radio, Microwave, Infrared, Visible, UV, Xray, Gamma
when d-block elements form ions, which orbital loses e⁻ first?
the s orbital
what is the aufbau principle
The statement that an electron occupies the lowest available energy orbital
what is the Pauli Exclusion Principle
No 2 electrons in the same atom can have the same 4 quantum numbers
decrease in ionization energy is due to an increase in what?
electron shielding
e⁻ affinity trend
Increases towards top and right of PT, except for at (½) filled orbitals
ionization E trend
Increases towards top and right of PT, except for at (½) filled orbitals
atom radius size trend
Increases towards bottom and left of PT
define diamagnetism
all e⁻ are paired, only very slightly repelled
define paramagnatism
some unpaired e⁻ leads to a strong attraction to magnetic field
the number of valence electrons is equal to what
the atom’s main group number
how to solve for Zₑբբ charge of an electron when determining e⁻ shielding
Zₑբբ = nuclear charge - # e⁻ below
For P on level 3: +15 - (2 + 2 + 6) = +5 for e⁻ on level 3
define excited state
e⁻ hops to higher orbit
define ground state
e⁻ goes to lowest E level possible
define degenerate orbitals
orbitals w/ same E
how does λ change from L→R on EMS
long → short
how does ν change from L→R on EMS
low → high
how does E change from L→R on EMS
low → high
who found the H spectrum to compare against a prism rainbow’s continuous spectrum
Balmer
what did Bohr do, and how did he support the Balmer series
made e⁻ E levels; n = 1, UV; n = 2, visible (which Balmer’s spectrum is on); n = 3, infrared
what did de Broccoli come up with?
matter has a dual particle/wave nature
define Heisenberg’s uncertainty principal
can’t know both e⁻ location and momentum, only probability of both
Schrodinger’s wave equation
ψ(x, y, z)² = probability density of e⁻ = orbitals; x, y, and z = e⁻ coordinates and a function of quantum #s: n, l, mₗ, mₛ
occurrence and shape of s orbital
1 @ each E level
spherical
occurrence and shape of p orbital
3 @ each E level when n ≥ 2
dumbbell shaped
occurrence and shape of d orbital
5 @ each E level when n ≥ 3
multi-lobed (like petals)
occurrence and shape of f orbital
7 @ each E level when n ≥ 4
weird shapes bro
3 things about quantum # n
principal quantum number
E level of e⁻
goes from 1, 2, 3, 4 … on to infinity
3 things about quantum # l
angular momentum quantum number
orbital type s, p, d, or f
goes from 0, 1, 2, 3 … on to n - 1
3 things about quantum # mₗ
magnetic quantum number
3D coordinates of orbital; or the shape
from -l…0…l (so, if l = 2, then mₗ could be -2, -1, 0, 1, 2
3 things about quantum # mₛ
spin quantum number
spin direction of the e⁻ in the orbital
±½
how to write mₛ and mₗ on test
write like “m sub s/l”, DO NOT write it as a subscript T-T
