HOMEWORK # 6 Spectral Lines WS

Aim # 6: How can we identify an unknown element?

http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/pem1s3_1.swf

1 Ultra Violet 2 Visible range 3

1. When electron falls to: n = 1 level gives UV Range (Lyman Series) n = 2 level gives Visible Range (Balmer Series) n = 3,4 or 5 levels gives IR Range (Paschen Series)

2. Electromagnetic Spectrum

The electromagnetic spectrum includes all the wavelengths of radiant energy from short gamma rays to long radio waves.

3. The Visible Spectrum The visible spectrum is that part of the electromagnetic spectrum that is visible to the eye, generally with wavelengths ranging between about 400 and 700 nm.

4. Spectroscope An instrument that breaks light into colored bands

Line Spectra for Hydrogen

Line Spectra for Mercury, and Neon Hg Ne

5. Bright-Line Spectra or Fingerprints of Elements: Each element has its own distinct line spectra. Helium line spectra

Excited State unstable and drops back down Spectrum Excited State n=4 UV Excited State Paschen Series n=3 Excited State unstable and drops back down Excited State Vi s ible But only as far as n = 2 this time Balmer Series n=2 Energy released as a photon Frequency proportional to energy drop IR Lyman Series n=1 Ground State

Absorption or dark line spectrum. 6. Type of Spectrum Type of Spectrum A. Continuous Spectrum B. Bright line spectrum Absorption or dark line spectrum.

A. Continuous Spectrum: We see all the colors Solids, liquids, and dense gases emit light of all wavelengths, without any gaps.

B. Bright line spectrum: selected colors

If there is a source of light behind it, a thin gas will absorb light of the same wavelengths it emits. We call this an absorption or dark line spectrum.

Origin of Continuum, Emission, and Absorption Spectra The origins of these three types of spectra are illustrated in the following figure.

7. Flame Test Every element absorbs and emits different amounts of energy (different colors).

Lithium Potassium Copper Calcium

"Flame spectrum" of Na Scale: wavelength in nm

"Flame spectrum" of Calcium (Ca). Scale: wavelength in nm.

Colors of Various Gases

End of the show

Practice ,practice , practice makes you perfect!!

1. The characteristic bright-line spectrum of sodium is produced when its electrons (1) return to lower energy levels (2) jump to higher energy levels (3)  are lost by the neutral atoms (4)  are gained by the neutral atoms

2. Draw four vertical lines showing the wavelengths of the spectral lines for the Balmer Series of hydrogen: 410.2, 434.4, 486.1, and 656.3 nm.

The diagram shows the characteristic spectral line patterns of four elements. Also shown are spectral lines produced by an unknown substance. Which pair of elements is present in the unknown? 1. lithium and sodium 3. lithium and helium 2. sodium and hydrogen 4. helium and hydrogen

August 2008

Base your answers to questions 66 through 69 on the information below. In a laboratory, a glass tube is filled with hydrogen gas at a very low pressure. When a scientist applies a high voltage between metal electrodes in the tube, light is emitted. The scientist analyzes the light with a spectroscope and observes four distinct spectral lines. The table below gives the color, frequency, and energy for each of the four spectral lines. The unit for frequency is hertz, Hz.

66. On the grid in your answer booklet, plot the data from the data table for frequency and energy. Circle and connect the points, including the point (0,0) that has already been plotted and circled for you. [1]

67. A spectral line in the infrared region of the spectrum of hydrogen has a frequency of 2.3 × 1014 hertz. Using your graph, estimate the energy associated with this spectral line. [1]

68. Explain, in terms of subatomic particles and energy states, why light is emitted by the hydrogen gas. [1]

69. Identify one condition not mentioned in the passage, under which hydrogen gas behaves most like an ideal gas. [1]

June 2008

31. The wave-mechanical model of the atom is required to explain the (1) mass number and atomic number of an atom (2) organization of atoms in a crystal (3) radioactive nature of some atoms (4) spectra of elements with multielectron atoms

The Balmer series refers to the visible bright lines in the spectrum produced by hydrogen atoms. The color and wavelength of each line in this series are given in the table below.

72. On the diagram in your answer booklet, draw four vertical lines to represent the Balmer series. [1]

72. Allow 1 credit for all four lines drawn correctly ± 0. 3 division 72 . Allow 1 credit for all four lines drawn correctly ± 0.3 division. The lines can be drawn above, through, or below the scale.

73. Explain, in terms of both subatomic particles and energy states, how the Balmer series is produced. [1]

73 [1] Allow 1 credit. Acceptable responses include, but are not limited to: When the electron in an excited hydrogen atom returns from a higher energy state to a lower energy state, a specific amount of energy is emitted. Light is emitted when the excited electron drops from a higher electron shell to a lower electron shell.