Question 19 Which of the following is true about emission spectra? emission of energy from elements occurs when electrons move from lower energy levels to higher energy levels individual elements emit continuous spectra the emission of individual elements are unique and can be used to identify the element a spectroscope uses diffraction or dispersion to separate continuous spectra into line spectra

If an atom has an emission line at a given shade of color (e.g., hydrogen at 656 nm), then does that atom have an absorption line at that same shade of color? Use the slider button under the label km/s to change the speed of the glowing object: negative speeds for objects approaching us, and positive speeds for objects recessing from us.  Describe changes to each of the continuous spectrum, emission line spectrum, and absorption line spectrum as the speed changes.  This change is called the Doppler effect, and is essential for measuring the speeds of objects located at a distance. Suppose you were given a spectrum of a planet.  The spectrum has a collection of absorption lines.  Describe how you would use this simulation to identify what lines were present (or absent) in the spectrum, and therefore what atoms were present (or absent) on the planet.

In Einstein's photoelectric effect, electrons are ejected from metal atoms when exposed to light of a specific energy, called the work function. If the work function for gold is 492.1 kJ/mol, what wavelength of light can eject electrons from gold? Group of answer choices 2.43 x 10-7 nm 276 nm 243 nm 3.63 x 106 nm

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The diagram below shows the wavelengths of four emission lines of the H atom. Using the Bohr model, four of the six transitions listed below each correspond to one of these lines in the spectrum. Which transition is responsible for the line at 410 nm? 410 nm 434 nm Light A85 nm Hatoms Prism 657 nm Emission Spectrum On = 2 to n = 3 On= 3 to n = 2 On-4 to n =2 On= 5 to n = 2 On- 6 to n = 2 On=1 to n = 5

Which of the following scientists first populated the sharp lines in the emission spectra of elements were caused by electrons going from high energy levels to low energy levels?

Which of the following colors from the visible range has the greatest frequency yellow red orange green O blue Which of the following colors from the visible range has the shortest wavelength green red orange O blue O yellow

Using the Bohr model, pick which electronic transition will emit a photon with the shortest wavelength. Group of answer choices n = 1 → n = 3 n = 2 → n = 1 n = 6 → n = 4 n = 3 → n = 2

The minimum frequency of light needed to eject electrons from a metal is called the threshold frequency, ?0. Find the minimum energy needed to eject electrons from a metal with a threshold frequency of 3.20×1014 s−1. With what maximum kinetic energy will electrons be ejected when this metal is exposed to light with a wavelength of 285 nm?

Data for the photoelectric effect of silver are given in the table. Frequency of incident radiation (1015 s−1) Kinetic energy of ejected electrons (10−19 J) 2.00 5.90 2.50 9.21 3.00 12.52 3.50 15.84 4.00 19.15 Using these data, find the experimentally determined value of Planck's constant, h , and the threshold frequency, ν0 , for silver.