Lecture - Bohr Model, Line Spectra Intro

What type of spectrum is shown at the top of Figure 6.7?

• Continuous spectrum

• Line emission spectrum

• Absorption spectrum

• None of the above

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NGSS.HS-PS4-3

Which element is represented by the third spectrum from the top in Figure 6.7?

• Sodium (Na)

• Hydrogen (H)

• Helium (He)

• Mercury (Hg)

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NGSS.HS-PS4-3

What implies that photons making up atomic spectra can have only discrete energies?

• The continuous nature of light

• The discrete wavelengths of atomic spectra

• The infinite energy levels within the atom

• The uniform distribution of energy in photons

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NGSS.HS-PS4-3

What is the equation that relates the energy of a photon to its frequency and wavelength?

• E = mc^2

• E = hλ

• E = hv = hc/λ

• E = h/mλ

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

When are photons produced within an atom?

• When an electron moves to a higher energy level

• When an electron remains in the same energy level

• When an electron moves from one energy level to another within the atom

• When an electron is removed from the atom

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NGSS.HS-PS4-3

How are electronic energies within an atom characterized?

• As continuous and unlimited

• As quantized and limited to specific values

• As variable and dependent on temperature

• As infinite and random

How many electrons does a hydrogen atom have, giving it a simple atomic spectrum?

• Two electrons

• A single electron

• Three electrons

• Four electrons

What happens when hydrogen is energized by high voltage?

• Atoms absorb radiation

• Atoms emit radiation

• Atoms become stable

• Atoms split into ions

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NGSS.HS-PS4-3

What is the wavelength of the Balmer series line for hydrogen when the electron transition is from n=3 to n=2?

• 656 nm

• 486 nm

• 434 nm

• 410 nm

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

Which wavelength corresponds to the transition of an electron from n=4 to n=2 in the Balmer series for hydrogen?

• 656 nm

• 486 nm

• 434 nm

• 410 nm

Tags

NGSS.HS-PS4-1