Test 1 and 2

Question 1

Vrms equation

Answer 1

=(3RT/m)^1/2

m is in kg

Question 2

Vanderwaals equation modifications

Answer 2

Brought 2 modifications to the ideal gas equation
1- particles take up space, therefore Vt =V-Vparticles
2-Particles have attraction forces between each other, therefore Pressure decreases because the collisions become less intense

Question 3

Vanderwaals equation

Answer 3

P= nRT/V-nb - a(n/v)^2, where a and b are constants

Question 4

Frequency

Answer 4

Number of waves that pass a point per second in s^-1, represented by v

Question 5

Wavelength

Answer 5

The length of one cycle in nm, represented by lamda

Question 6

Blue light wavelength

Answer 6

400-500 nm

Question 7

Green light wavelength

Answer 7

500-600 nm

Question 8

Red light wavelength

Answer 8

600 - 700 nm

Question 9

Black body radiation

Answer 9

Bodies that are heated emit light

Question 10

Gas comparaison formula

Answer 10

(P2/P1)(V2/V1) = (n2/n1)(T2/T1)

Question 11

What is Vrms

Answer 11

The distribution of particles based on their velocity. V is inversely proportional to T^1/2. The larger the temperature, the larger but lower the curve is

Question 12

Graham’s law of effusion

Answer 12

ta/tb = (ma/mb)^1/2

Question 13

wavelength freqeuncy formula

Answer 13

v x lambda = c

Question 14

Energy of a photon

Answer 14

E = hv

Question 15

photoelectric effect

Answer 15

electrons can be rejected from metals if they meet a certain frequency requirement, called threshold. For example, a metal with a threshold of 600nm could be activated if a light of a smaller wavelength were to strike it.

Question 16

Energy of a state

Answer 16

En = -B/n^2

Question 17

Wavelength mass velocity formula

Answer 17

lambda = h/(m x velocity)

Question 18

Schrodinger’s equations

Answer 18

Wave functions that describe the wave of an electron. Squaring it gives the probability of finding the electron at x.

Question 19

l

Answer 19

l < n

Question 20

naming orbitals

Answer 20

l = 0 -> "s" 
l = 1 -> "p"
l = 2 -> "d"
l = 3 -> "f"

Question 21

m

Answer 21

-l <= m <= l

Question 22

Bohr’s model of the atom

Answer 22

electrons travel in defined circular orbits around the nucleus. The orbits are labeled by an integer, the quantum number n. Electrons can jump from one orbit to another by emitting or absorbing energy.

Question 23

Schrodinger’s model of the atom

Answer 23

Electrons are not in a fixed position, but have a probability of being at a certain position. Described by orbitals

Question 24

Binding energy

Answer 24

the energy it takes to eject electrons from a metal
Calculated using
W(binding energy) = hv(energy of the photon)