# Emission line spectra for various elements are shown in Table 1 and Table 2 shows the...

Emission line spectra for various elements are shown in Table 1 and Table 2 shows the wavelengths for various colors. Remember, E = h*c/?, where E is energy, h = 6.626*10-34 J*s, c = 3.00*108 m/s, ? is the wavelength, and 1 m = 109 nm.

Table 1. Emission Line Spectra of Various Elements

 Element Emission Lines (nm) H 410.2, 434.1, 486.1, 656.3 He 447.1, 492.1, 501.5, 587.5 Hg 404.7, 435.8, 546.1, 577.0 Na 588.9, 589.5 Mg 487.8, 502.5, 574.1, 710.9

Table 2. Wavelengths of Various Colors

 Color Wavelengths (nm) Violet 380 – 450 Blue 450 – 495 Green 495 – 570 Yellow 570 – 590 Orange 590 – 620 Red 620 – 750
Unknown element A produced line spectra energies of 4.089*10-19 J and 4.579*10-19J. Using Tables 1 and 2 above, calculate the corresponding wavelengths in nm, identify each line's color, and determine the unknown element. Pay attention to significant digits and the colors should be capitalized, e.g. "Orange" with a capital O. Wavelength 1: nm Color 1: Wavelength 2 nm Color 2: Element (use the chemical symbol, i.e., hydrogen would be H):

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