Question

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 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):

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

Answer 1

4.089 x 16 A48613 xlom 486-13nm 2 2. 4.529 XIơ19 Color:1 Blue Color ColoxVialet Colo 0% Elemen: H