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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

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 lines 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

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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Answer #1

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

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