Physics Experiment : Spectroscopy, Hydrogen, Mercury, Other Gases And Light Sources Using Spectroscopy

The purpose of this experiment is to determine the maximum absorbance of fast green, and the chlorophylls, also in the case of fast green create a concentration curve to determine an unknown substance. Each test will use the spectrophotometer.

I. Introduction: The reason we are able to observe different colors of light during the flame test is because the electrons move from their normal stable configuration, or ground state, to a different orbital and an excited state. When electrons are in an unstable state they need to get rid of energy in order to get back to their ground state. They do this through giving off light energy as photons. Depending on the element the photon will give off a certain color and move from its unstable, excited state back to a stable, ground state as they give off their energy through light.

The best technology available today for studying the chemical composition of stars and planets is spectroscopy, a scientific tool that dissects light into its component colours (Astronomy mag. P.31). “A planet within 100 light-years of Earth is close enough to provide sufficient light for scientists to dissect light into its component colors” (Ray Villard, Astronomy ). Spectrographs are used by astronomers to observe discrete spectra. Discrete spectra are produced by gases, such as … when specific wavelengths of light are absorbed or emitted by the gases. This causes dark bands to appear on the spectrum where the specific wavelengths of light are absent. A scientist can

Experiments 2-1 and 2-2 study the production of hydrogen gas by different chemical reactions. By using a hydrogen gas collection apparatus and the principles of chemistry, we were able to evaluate the data and reach our goal. Experiment 2-1 uses zinc, magnesium and aluminum and how much hydrogen gas they produce to predict the volume of hydrogen gas produced for different masses of each metal. In this experiment we see that each metal has an increasing amount of hydrogen gas as mass goes up, however each metal had different amount of hydrogen gas for the same mass. Zinc produced the least amount of hydrogen gas, then increasing with magnesium, and aluminum produced the highest amount. The

Then, by measuring and calculating the emission lines in the hydrogen line spectrum, the data on table 1.3 was collected. The calculated wavelength (Calc λ) was determined by the Balmer-Rydberg formula.

Please complete the entire experiment as instructed in the lab manual except for any modifications noted below. Fill out the

Usually an excited state can take the form of the electron bouncing from its start energy level or annual also called the ground state. The excited states that are found in the atoms which are in molecules are really crucial for some chemical reactions. The excited electron does not stay in the excited state for a long time, in a while it goes down back to the ground state. When an electron goes down from the excited state, its energy decreases in the form of light, this process is called emission (What is an Excited

By looking at the different wavelengths or the spectrum of light from a celestial object, you can tell many of its properties and features. To do this, the Hubble Telescope is equipped with various scientific instruments. Each instrument used

Dehydration and moderate fever are the casual enormities a person faces throughout his/her life. Similarly, in my teenage years, I also overcame such a condition and carelessly disregarded it as another week of some light nausea and fever. However, the stomach sickness and continuant abdominal cramps left me thinking upon other possibilities. But my undying habit or love for unhealthy and processed foods made me overlook my stomach pains. I rather intentionally disregarded the fact in face of fear and remained content with several pain killers.

In 1913 Niels Bohr proposed a hydrogen-atom model that linked the atom’s electron to the photon emission. According to his model, electrons circle the nucleus only in allowed circuits. When the electron is in one of these orbits, the atom has a definite, fixed energy. The electron has the lowest energy state when it is in the orbit closest to the nucleus. The energy of the electron is higher as the electron is in orbits that are successively farther from the nucleus. He also discovered that an electron can be one orbit or another but not in between.

Comparing the hydrogen to lithium, hydrogen is an element with little orbitals compared to lithium. Hydrogen has little amounts of energy levels, so its energy is diagram will

n = 3 to n = 2 is called Balmer-alpha or H-alpha, and is visible in the red part of the electromagnetic spectrum. This is the easiest way for astronomers to trace the ionized hydrogen content of gas clouds. Since it takes nearly as much energy to excite the hydrogen atoms electron from n = 1 to n = 3 as it does to ionize the hydrogen atom, the probability of the electron being excited to n = 3 without being removed from the atom is very small. Instead, after being ionized, the electron and proton recombine to form a new hydrogen atom. In the new atom, the electron may begin in any energy level,

In this model, electrons move in fixed orbits at fixed distances from the nucleus. Each of these orbits represents a certain quantity of energy. The outer orbits have more energy than the inner orbits. Atoms do not emit radiation, such as light, when the electrons are in the fixed orbit, but an electron can move to a different orbit. If an electron moves down to an orbit with less energy, energy is released in the form of radiation – a light quantum. If the electron moves from an orbit closer to the nucleus to one farther from the nucleus, energy is absorbed. The frequencies and wavelengths of the light quanta are unique for each atom. In addition to creating a model, Bohr’s formula and associated calculations correlated the spectral lines observed for the hydrogen atom with electron energy levels for electrons in the Bohr hydrogen atom model. This indicated that the emission spectrum resulted from emission of small amounts of energy when electrons moved between

Kelvin begins at 0 degrees which gives an exact estimation of the determined absolute temperature, yet Celsius only shows how much the temperature has increased.

Spectroscopy is used as a collective term for all the analytical techniques based on the interaction of light and matter. Spectrophotometry is one of the branches of spectroscopy where we measure the absorption of light by molecules that are in a gas or vapour state or dissolved molecules/ions (Tombs, et.al, 1959). Spectroscopy is the use of electromagnetic radiation by a sample in order to identify components of the sample (qualitative analysis) or to measure the amount of material in that sample (quantitative analysis) (Tombs, et.al, 1959). Absorption is a process in which