Hydrogen spectrum

Which series of the hydrogen spectrum is visible to the human eye?

• A. Lyman series

• B. Balmer series

• C. Paschen series

• D. Brackett series

What is the principal quantum number (n) for the first line of the Lyman series?

• A. 1

• B. 2

• C. 3

• D. 4

Which of the following transitions will result in the emission of a photon in the Balmer series?

• A. n = 3 to n = 2

• B. n = 4 to n = 1

• C. n = 5 to n = 3

• D. n = 6 to n = 4

Tags

NGSS.HS-PS4-3

The Rydberg constant (R_H) for hydrogen is approximately:

• A. 1.097×10⁵m⁻¹

• B. 1.097×10⁷ m⁻¹

• C. 1.097×10⁹m⁻¹

• D. 1.097×10¹¹m⁻¹

Tags

NGSS.HS-PS4-1

Which of the following series corresponds to transitions ending at the n=3 level?

• A. Lyman series

• B. Balmer series

• C. Paschen series

• D. Pfund series

What is the series of spectral lines in the hydrogen spectrum that falls in the ultraviolet region?

• a. Lyman series
  

• b. Balmer series

• c. Paschen series

• d. Brackett series

Tags

NGSS.HS-PS4-1

NGSS.HS-PS1-2

Who was the scientist who first experimentally determined the equation for the spectral lines of the hydrogen atom?

• a. Niels Bohr

• b. Erwin SchrÃdinger

• c. Werner Heisenberg

• d. Max Planck

Calculate the wavelength of the photon emitted when an electron in a hydrogen atom transitions from n=3 to n=2.

• a. 699 nm

• b. 600 nm

• c. 500 nm

• d. 656 nm

Tags

NGSS.HS-PS4-1

If the energy difference between two levels in a hydrogen atom is 2.55 eV, determine the wavelength of the emitted photon. (Use the formula E=hc / λ ; hc=1240 eV⋅nm)

• a. 400 nm

• b. 420 nm

• c. 486 nm

• d. 500 nm

Tags

NGSS.HS-PS4-1