#Atomic spectra line spectra series#

This energy is equal the difference between the excited and the original level. To the electron fall back, it emits an amount of energy in form of light (photon) with a specific wavelength. That way, the electron returns to its original state. However, the electron tends to be in the lowest unoccupied energy level available. When an electron is excited, by heart or electrical discharge, it jumps to a higher energy level. By the quantum mechanical theory, a bounded electron can only occupy a set of states centered on the nucleus, and each state corresponds to a specific energy level. The electrons of an atom are bounded to the nucleus by the electromagnetic force. As well known, the atom is compounded by a nucleus with positive (protons) and neutral (neutrons) charges surrounded by a cloud of negative charges (electrons). The specific wavelengths emitted by the gas are related to their atomic structure. This is a technique very important in astronomy where scientists use to analyze the properties of distant objects, like their chemical elements. That way, it is possible to use the spectrum analyze to identify the composition of material. Scientist found that each element of periodic table has a unique set of spectral lines, as a signature of the element. This means that a heated gas emits light in just some specific wavelength. The spectrum of the heated gas was discrete lines or spectra lines. In 1850s, Anders Jonas Angstrom observed that the light emitted by a high heated gas did not have a continuum spectrum, like white light, when it passes through a prism. This was the beginning of the Spectrum Analyze Technique. In the 19 th century, scientist discovered that they could use the light emitted by heated or electrical discharged materials to analyze their properties. The table below shows the range of wavelength for each of seven colors of the rainbow. The result is that red light bends less sharply than violet as it passes through the prism, creating a spectrum of colors. The decomposition of the white light in different colors results from different wavelengths, as a consequence, they move at different speeds in the prism, with red light moving faster than violet. This means that the white light is formed by the combination all visible colors. In sequence of this experiment, Newton combined those colored beams in another prism which resulted in another white light beam. Newton classified this spectrum in a range of seven different colors (Red, Orange, Yellow, Green, Bleu, Indigo and Violet). The answer is choice 1.In the 1670s, Isaac Newton, during optical experiments observed that a beam of white light was decomposed in a continuum spectrum of all visible colors, like a rainbow, when it pass through a prism. If the lines are not present, that element is not part of the mixture. Line up the lines to identify the unknown elements. Is can be used to identify an element in mixtures. Since each element has different numbers of protons, neutrons and most importantly electrons, the emission spectrum for each element is different.

#Atomic spectra line spectra series#

This series is referred to as the Lyman Series.įurther the electron falls, the more energy it releases. This series is called the Balmer series.Įlectron falls to the 1st energy level, the light given off is t=in the Is in the visible region of the spectrum and spectral line of color are Series of electron transitions is referred to as the Paschen series.Įlectron falls to the 2nd energy principal energy level, the light given off Level, the light given off is in the infrared region of the spectrum. Hydrogen atom, if the electron falls to the 3rd energy principal energy It is when they return to the ground state energy is given off.īut electrons don't have to go directly there. Ground state (lowest energy configuration)Įxcited State (higher energy configuration)Ģ-6-1 **Note the # of electrons are the same This is not the cause of the spectral lines.

'Excite electrons fall back to lower energy levels releasing energy in the form of light.'Įxciting an electron promotes it to a higher sublevel of energy level. Lines Spectra and Excited Electron States