Test 10/8/14

Question 1

What did Planck do?

Answer 1

Quantization, “this not that”

Question 2

What did Einstein do?

Answer 2

Photoelectric effect

Question 3

What did Balmer do?

Answer 3

He created a wavelength equation but, couldn’t explain it.

Question 4

What did Bohr do?

Answer 4

Energy levels in hydrogen

Question 5

What did Heisenberg do?

Answer 5

Uncertainty principle

Question 6

What did Schrodinger do?

Answer 6

Quantum mechanics

Question 7

What did Pauli do?

Answer 7

Exclusive principle

Question 8

Which among the following are not quantized: a) shoelaces b) cars passing through a toll plaza every day c) birds in an aviary d) flow of a river in ml/hr e) percentage of salt in a solution

Answer 8

D

Question 9

Which of the following are quantized: a) canned soup from a grocery store b) weight of jelly beans c) elevation of a person on a ramp

Answer 9

A

Question 10

In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. In one transition between energy states, an electron moves from n= 1 to n= 2. Is energy absorbed or emitted in the process? Does the electron move closer to or further from the nucleus?

Answer 10

Absorbed, further

Question 11

What must be done to an atom, or what must happen to an atom, before it can emit light?

Answer 11

It must get excited.

Question 12

What experimental evidence leads us to believe that electron energy levels are quantized?

Answer 12

Because atoms emit certain colors.

Question 13

Which atom is more apt to emit light, one in the ground state or one in the excited state? Why?

Answer 13

Excited because it means the atom can fall.

Question 14

According to Bohr, what happened when an electron absorbs a photon?

Answer 14

It would get excited.

Question 15

What does E= hf stand for?

Answer 15

E= energy (J) h= Planck’s constant, (6.63 x 10^-34) (J) f= frequency (Hz)

Question 16

What does c= (lambda)f stand for?

Answer 16

c= speed of light (3 x 10^8) (m/s) lambda= wavelength (m or nm) f= frequency (Hz)

Question 17

How many eV’s in one Joule?

Answer 17

1.6 x 10^-19

Question 18

1s has __ e-? 3p? 5d? 7f?

Answer 18

2, 6, 10, 14

Question 19

When you do a question that asks for a transition between energy levels use which equation?

Answer 19

1/ lambda = 1.097 x 10^7 ( 1/hf^2 - 1/hi^2)

Question 20

A visible wavelength is between ____ and ____?

Answer 20

400 and 700

Question 21

A UV wavelength is shorter than ____?

Answer 21

400

Question 22

An infrared (IR) is bigger than ____?

Answer 22

700

Question 23

Ei = hf + Ef, what are the 4 steps? (10 Point Bonus on Test)

Answer 23

(1) hf = Ei - Ef (2) hc/lambda = -Rh/ni^2 - -Rh/nf^2 (3) hc/lambda = Rh ( 1/nf^2 - 1/ ni^2) (4) 1/lambda = Rh/hc (1/nf^2 - 1/ni^2)

Question 24

What does E = -Rh/n^2 stand for?

Answer 24

E= energy (J) -Rh = -13.6 (eV) n= energy level (1, 2, 3, 4, etc)