Lyman Balmer Paschen

Which electron transition between the energy

levels of hydrogen causes the emission of a photon of

visible light?

• 𝑛 = 6 to 𝑛 = 5

• 𝑛 = 5 to 𝑛 = 6

• 𝑛 = 5 to 𝑛 = 2

• 𝑛 = 2 to 𝑛 = 5

Tags

NGSS.HS-PS4-3

Which of the following transitions is the result of

the atom absorbing a photon of the shortest

wavelength?

• A

• B

• C

• D

Tags

NGSS.HS-PS4-1

The diagram below shows the Balmer series electron

transitions in a hydrogen atom. Which spectrum will have the highest energy?

• A. 𝐸2 𝑡𝑜 𝐸5

• 𝐸3 𝑡𝑜 𝐸6

• 𝐸3 𝑡𝑜 𝐸2

• 𝐸6 𝑡𝑜 𝐸2

Tags

NGSS.HS-PS4-3

What is the wavelength and color of the emitted

photon, due to a transition in a hydrogen atom from

the 𝑛 = 3 state to the 𝑛 = 2 state?

• 486 nm Green

• 656 nm Red

• 486 nm Blue

• 434 nm Violet

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-3

Which of the transitions below for a hydrogen

atom involves the least energy?

• 𝑛= 5 𝑡𝑜 𝑛 = 3

• 𝑛 = 5 𝑡𝑜 𝑛 = 4

• 𝑛 = 2 𝑡𝑜 𝑛 = 5

• 𝑛I= 4 𝑡𝑜 𝑛 = 7

A photon having an energy of 9.40 electron volts

strikes a hydrogen atom in the ground state. Why is

the photon not absorbed by the hydrogen atom?

• The atom’s orbital electron is moving too

  fast

• The photon striking the atom is moving

  too fast

• The photon’s energy is too small

• The photon is being repelled by

  electrostatic force

What is the minimum energy required to ionize a

hydrogen atom in the n=3 state?

• 0.66 eV

• 1.51 eV

• 12.09 eV

• 13.6 eV

The energy level diagram for a hypothetical atom

is shown in the figure below. Which of the labeled

transitions in the diagram would produce a photon

with the shortest wavelength?

• A

• B

• C

• D

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-3

Which type of photon is emitted when an electron

in a hydrogen atom drops from the n=2 to the n=1

energy level?

• Ultraviolet

• Visible light

• Infrared

• Radio wave

Tags

NGSS.HS-PS4-3

The visible lines from hydrogen are all members

of the ____.

• Lyman series

• Balmer series

• Paschen series

• Lyman and Paschen series

Tags

NGSS.HS-PS4-3