When sodium is excited in a flame, two ultraviolet spectral lines at lambda - 372.1 nm and lambda = 376.4 nm respectively are emitted. which wavelength represented photons?

a) higher energy?

b) longer wavelengths?

c) higher frequences?

Question

Chemistry

Sebastian Pollard

30 November, 08:21

When sodium is excited in a flame, two ultraviolet spectral lines at lambda - 372.1 nm and lambda = 376.4 nm respectively are emitted. which wavelength represented photons?

a) higher energy?

b) longer wavelengths?

c) higher frequences?

+3

Answers (1)

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Meyers · Answer 1

The wavelength that represented photons is at lambda = 376.4 nm.

The wavelength with the higher energy is at lambda - 372.1 nm.

The longer wavelength is, of course, at lambda 376.4 nm.

The wavelength with the higher frequency is 376.4 nm.

When sodium is excited in a flame, two ultraviolet spectral lines at lambda - 372.1 nm and lambda = 376.4 nm respectively are emitted. which wavelength represented photons?a) higher energy?b) longer wavelengths?c) higher frequences?

When sodium is excited in a flame, two ultraviolet spectral lines at lambda - 372.1 nm and lambda = 376.4 nm respectively are emitted. which wavelength represented photons?

a) higher energy?

b) longer wavelengths?

c) higher frequences?