Lecture 10

Question 1

Mass energy equivalence

Answer 1

E = mc^2

Question 2

deBroglie wavelength

Answer 2

λ = (h)/(mn) = h/p
m - mass in kg
n - velocity (m/s)
h - Planck constant (Js)
p- momentum

Question 3

Quantum mechanical model

Answer 3

Used orbitals instead of orbits.
Better model than Bohr because it accurately explains and predicts what we currently know about electron and atom behavior and characteristics

Question 4

Electron energy

Answer 4

Proportional to Ψ and had the same energies for H atoms as Bohr model

Question 5

Spatial distribution

Answer 5

Proportional to Ψ^2

Question 6

Schrödinger wave equation

Answer 6

Allows us to solve for the energy stages associated with a particular atomic orbital
H Ψ = E Ψ

Ψ - wave function
E - energy of atom
H - Hamiltonian

Question 7

Ψ

Answer 7

Wave function

Question 8

Atomic orbital

Answer 8

Wave function associated with energy state of atom

Question 9

Probability distribution

Answer 9

Spatial distribution

Question 10

Probability density

Question 11

n

Answer 11

• Principal quantum number
• SIZE of orbital/distance from nucleus ENERGY LEVEL

Question 12

ℓ

Answer 12

• Angular momentum quantum number
• from 0 to n-1
• SHAPE of orbital or SUBLEVELS
  s p d f g

Question 13

m ℓ

Answer 13

• magnetic quantum number
• -ℓ to ℓ
• spatial ORIENTATION if the orbital

Question 14

Orbital

Answer 14

An area where the probability of finding an electron is high

Question 15

What do energy levels if the H atom depend on?

Answer 15

Only the n value

Question 16

Number of nodes

Answer 16

(n - 1)

Question 17

ms

Answer 17

Specifying the direction of spin if an electron around its own axis
- -1/2 to 1/2