Test 6 & 7

Question 1

what is hund’s rule?

Answer 1

e⁻ fill up all orbitals before they start pairing in them

Question 2

eqn for lightspeed, c

Answer 2

λ * ν = c

Question 3

symbol for wavelength

Answer 3

λ, lambda

Question 4

symbol for frequency

Answer 4

ν, nu

Question 5

units of frequency

Answer 5

cycles/second → 1/s → s⁻¹ → Hertz (Hz)

Question 6

eqn for E w/ Planck’s constant h and what it means

Answer 6

E = hν or Energy = Planck’s Constant * frequency to find E in J of 1 photon

Question 7

what did einstein discover about light, x 2

Answer 7

confirmed Planck’s theory and discovered dual wave/particle nature of light

Question 8

what is de Broccoli’s eqn for matter wave lengths?

Answer 8

λ = h/(momentum * velocity), where units are in meters

Question 9

elec config for Cu

Answer 9

[Ar]4s¹ 3d¹⁰

Question 10

elec config for Cr

Answer 10

[Ar]4s¹ 3d⁵

Question 11

10⁻⁶

Answer 11

micro

Question 12

10⁻⁹

Answer 12

nano

Question 13

10⁻¹²

Answer 13

pico

Question 14

acronym to remember order of electromagnetic spectrum

Answer 14

Red Meat Is Very Unhealthy, Xspecially Grilled

Radio, Microwave, Infrared, Visible, UV, Xray, Gamma

Question 15

when d-block elements form ions, which orbital loses e⁻ first?

Answer 15

the s orbital

Question 16

what is the aufbau principle

Answer 16

The statement that an electron occupies the lowest available energy orbital

Question 17

what is the Pauli Exclusion Principle

Answer 17

No 2 electrons in the same atom can have the same 4 quantum numbers

Question 18

decrease in ionization energy is due to an increase in what?

Answer 18

electron shielding

Question 19

e⁻ affinity trend

Answer 19

Increases towards top and right of PT, except for at (½) filled orbitals

Question 20

ionization E trend

Answer 20

Increases towards top and right of PT, except for at (½) filled orbitals

Question 21

atom radius size trend

Answer 21

Increases towards bottom and left of PT

Question 22

define diamagnetism

Answer 22

all e⁻ are paired, only very slightly repelled

Question 23

define paramagnatism

Answer 23

some unpaired e⁻ leads to a strong attraction to magnetic field

Question 24

the number of valence electrons is equal to what

Answer 24

the atom’s main group number

Question 25

how to solve for Zₑբբ charge of an electron when determining e⁻ shielding

Answer 25

Zₑբբ = nuclear charge - # e⁻ below

For P on level 3: +15 - (2 + 2 + 6) = +5 for e⁻ on level 3

Question 26

define excited state

Answer 26

e⁻ hops to higher orbit

Question 27

define ground state

Answer 27

e⁻ goes to lowest E level possible

Question 28

define degenerate orbitals

Answer 28

orbitals w/ same E

Question 29

how does λ change from L→R on EMS

Answer 29

long → short

Question 30

how does ν change from L→R on EMS

Answer 30

low → high

Question 31

how does E change from L→R on EMS

Answer 31

low → high

Question 32

who found the H spectrum to compare against a prism rainbow’s continuous spectrum

Answer 32

Balmer

Question 33

what did Bohr do, and how did he support the Balmer series

Answer 33

made e⁻ E levels; n = 1, UV; n = 2, visible (which Balmer’s spectrum is on); n = 3, infrared

Question 34

what did de Broccoli come up with?

Answer 34

matter has a dual particle/wave nature

Question 35

define Heisenberg’s uncertainty principal

Answer 35

can’t know both e⁻ location and momentum, only probability of both

Question 36

Schrodinger’s wave equation

Answer 36

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

Question 37

occurrence and shape of s orbital

Answer 37

1 @ each E level

spherical

Question 38

occurrence and shape of p orbital

Answer 38

3 @ each E level when n ≥ 2

dumbbell shaped

Question 39

occurrence and shape of d orbital

Answer 39

5 @ each E level when n ≥ 3

multi-lobed (like petals)

Question 40

occurrence and shape of f orbital

Answer 40

7 @ each E level when n ≥ 4

weird shapes bro

Question 41

3 things about quantum # n

Answer 41

principal quantum number
E level of e⁻
goes from 1, 2, 3, 4 … on to infinity

Question 42

3 things about quantum # l

Answer 42

angular momentum quantum number
orbital type s, p, d, or f
goes from 0, 1, 2, 3 … on to n - 1

Question 43

3 things about quantum # mₗ

Answer 43

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

Question 44

3 things about quantum # mₛ

Answer 44

spin quantum number
spin direction of the e⁻ in the orbital
±½

Question 45

how to write mₛ and mₗ on test

Answer 45

write like “m sub s/l”, DO NOT write it as a subscript T-T