In this experiment, [Co(NH3)5ONO]Cl¬2 was synthesized with a yield of 1.4314 g. It was then used to obtain UV-Vis Spectroscopy data with other prepared cobalt complexes including [Co(NH3)5(H2O)]Cl3, [Co(NH3)5(Cl)]Cl2 , Co(NH3)5(NO2)]Cl2 and [Co(NH3)6]Cl3. Each compound was a different color. Color, by definition, represents the wavelengths of UV light that a particle reflects. UV-Vis spectroscopy measures the amount of UV light absorbed. The easy way to determine wavelength of absorption from the color of the solution was the use of a color wheel like in Figure 1. The wavelengths of the color opposite of the solution’s color in the color wheel were the expected wavelengths of absorption. Co(NH3)5ONO]Cl¬2 was an reddish-orange color so its wavelength …show more content…
Using the d-orbital electron configuration for cobalt in high and low states, the number of unpaired in electrons can be used to calculate the magnet moment for each spin state using the equation, µso¬ = √(4S(S+1)), where S = ½ the number of unpaired electrons. The magnetic moment for the high spin state was calculated to be 8.944 and 0 for the low spin state. The ligand field stabilization energy was also calculated for the high and low spin states using the equation LFSE = Δ_0 (-2/5 x+3/5 y), where x = number of unpaired electrons in the t2g orbital and y = the number of unpaired electrons in the eg orbital. The ligand field stabilization energy was calculated to be 2/5 Δ_0 for the high spin state and 0 for the low spin state. The earliest article to reference “spectrochemical series” on Scifinder was the article, “Relation between the Geometrical Configurations of Inorganic Complexes and Their Absorption Bands. III. General Rule for the First and Second Bands of Co(III) Complexes,” by Yoichi Shimura published in
A spectrum is a group of light wavelengths that are ordered in relation to their wavelength length. The electromagnetic spectrum consists radio waves, microwaves, infrared, visible, ultraviolet, X-rays and gamma rays. (1)Specifically, this lab looks at the visible light part of the spectrum because one of the colors in the visible light spectrum is shine through the sample. The visible light spectrum consists of colors of red, orange, yellow, green, blue, indigo, and violet. The color chosen to be shine through the sample is affected by the color of sample when mixed with the indicator Ammonium Vanadomolybdate (AMV). The color on the color wheel that is opposite of the solution’s color is the color that is shined through the
700 0.03 0.01 0 0 0.028. 720 0.01 0.01 0 0 0.02 0. Figure 2: The absorption spectrum shows how absorbent the photosynthetic pigments are at different wavelengths of light. Note: Green light is between 500 to 570 nm and red light is between 630 to 720 nm.
Oliva-Chatelain, B. L., & Barron, A. R. (2010). Basics of UV-Visible Spectroscopy. Retrieved from openstax cnx: http://cnx.org/content/m34525/latest/
Cobalt can be used for many things such as alloys, laundry detergent, and cobalt can even be found in paint. Cobalt has many different properties that allow it to do many different interesting things. Cobalt is used for electroplating metals. What this means is that Cobalt has the properties to coat other metals and keep them from corroding and keep them shiny and looking brand new. Like I mentioned before, Cobalt can also be used as a magnet. When Co2+ is mixed with Fe2+, the current loss is lowered making it be able to act as a magnet. That is just one of its interesting properties. Cobalt is also found in laundry detergent. That is partly where laundry detergent gets its blue color from. In the ancient times, people noticed that if some cobalt ores were soaked in water, it would cause the water to turn blue. People who washed clothes would make sure not to have cobalt near their clothes, thinking it would also turn their clothes blue, But, if linen or cotton cloth is soaked and washed in water that is stained blue with cobalt, then the cloth or linen would appear whiter. Cobalt compounds have been used in “laundry bluing” since the dawn of times. With these methods of washing clothes, people then came up with ideas such as bleach, but thats a whole other
Nanocrystalline perovskite and spinel magnetic mixed oxides materials have gained immense importance due to their novel properties, which are significantly different from those of their bulk counterparts [1]. Nanocrystals of spinel ferrites, with general formula MFe2O4 (where M = Ni, Cu and Zn) are most interesting class of magnetic materials due to its facinating properties such as low melting point, high spectfic heat, large expansion coefficent and low magnetic transition temperature[2,3]. Because of these properties, ferrite materials are widely used in ferrofluid technology, information storage and magnetic pigments[4-6]. Especially, due to their peculiar magnetic properties and ability to respond at the molecular level, magnetic nanostructures are potential candidates for biomedicine such as targeted drug delivery [7], diagnostics [8], and magnetic separation [9]. These materials are also being explored as contrast agents in magnetic resonance image (MRI) [10], thermo responsive drug carriers [11] as well as in the thermal activation therapy of cancer [12]. The crystal structure of spinel ferrite compounds have a cubic close packing of O2- ions structure linked with two sub-lattice sites namely tetrahedral (A-sites) and octahedral (B-sites) [13]. The magnetic and other properties of spinel ferrite can be varied systematically by changing the identity of the ion, their charges and their distribution among the tetrahedral and octahedral sites [14]. Zinc ferrite (ZnFe2O4) and cobalt ferrite (CoFe2O4) have been most extensively studied system, because they exhibit the typically normal and inverse spinel ferrite respectively [15]. Nickel ferrite (NiFe2O4) is a well known inverse spinel structure ferrite with Ni2+ ions at octahed...
V. Amarnath, D. C. Anthony, K. Amarnath, W. M. Valentine, L. A. Wetterau, D. G. J. Org. Chem. 1991, 56, p. 6924-6931.
Figure 1: The hexacyanoferrate iron (III) ion: contains 6 ligands which are bound to the central metal therefore has a coordination number of 6 (n=6¬). (Hussain,2007) [13]
Penicillins have been considered as first-line drug for odontogenic infections. Amoxycillin, a semi synthetic penicillin is the drug of choice in treating dental infections and is the most common antibiotic used by dentists . If a patient with an early stage odontogenic infection does not respond to Amoxycillin , there is a strong probability of the presence of resistant bacteria. Bacterial resistance to the penicillins is a result of the production of beta-lactamase by the bacteria. therefore, beta-lactamase-stable antibiotics should be prescribed to the patient. These include either clindamycin or amoxicillin & clavulanic acid . the American Heart Association considers amoxicillin to be the first choice for prophylaxis against the Endocarditis associated with dental procedures. In long standing infections , gram negative anaerobic organisms may be suspected, therefore metranidazole may be added with amoxicillin. It can cause ‘Antabuse’ reaction such as nausea, vomiting, abdominal cramps in patients who consume alchohol during the medication period. Metronidazole's excellent anaerobic gram negative activity and its low degree of toxicity, make it an excellent drug in the treatment of odontogenic infections.
Classification of IR bands are generally as strong, medium or weak. Strong bands are usually long and covers most of the y-axis. A medium band is of intermediate height. A weak band is short and covers a small portion of the y-axis. This classification of IR bands depends on the relative strength of bond polarity. Strongly polar bonds produce strong bands, medium polarity bonds produce medium bands and weakly polar bond and symmetric bonds produce weak or non – observable bands (Cortes,
Mainly IR spectroscopy has many of importance in the field of organic and inorganic chemistry. The functional group can therefore readily identified by their characteristics frequencies of absorption. This makes the IR spectroscopy the most useful means to obtain the structural information about the organic and inorganic molecules as it measure easily and quickly the atoms vibrations so in this result we are able to indentify the functional group in a molecule. When it is passed through any of organic compounds some of the radiations are absorbed by the molecules and are appeared as absorption bands while the radiations that are not absorbed are given as transmitted energy. As only those frequencies has the ability to absorb that match with the frequencies of vibration bond.
Coordination chemistry came about from the work of Alfred Werner, a Swiss chemist who examined different compounds made up of cobalt (III) Chloride and ammonia. When hydrochloric acid was added, Werner noticed that ammonia could not be removed completely. He then suggested that the ammonia must bind more tightly to the central cobalt ion. However, when aqueous silver nitrate was added, one of the products formed was solid silver chloride. The resulting amount of silver chloride was related to the number of ammonia molecules bounded to the cobalt (III) chloride. For example, when silver nitrate was added to CoCl3•6NH3, all three chlorides were converted to silver chloride. When silver nitrate was added to CoCl3•5NH3, only 2 of the 3 chlorides formed silver chloride. When CoCl3•4NH3 was treated with silver nitrate, only one of the three chlorides precipitated as silver chloride. The resulting observations gave out the formation of complex or coordination compounds. In the inner coordination sphere, which is also referred to as the first sphere, ligands are directly bound to the central metal. In the outer coordination sphere, sometimes called the second sphere, other ions are attached to the complex ion. The following table is a summary of Werner's observations:
Cobalt ferrite nanoparticles are of utmost importance that can be used for biological applications due to their magnetic properties, stability in physiological conditions, low cytotoxicity, as well as biocompatibility [Schwertmann, U., Cornell, R.M. Iron oxides in the laboratory: Preparation and characterization 2nd ed.Willey-VCH, Weinheim: New York, 1991]. Cobalt ferrite is a cubic ferrite with inverse spinel structure, where Co+2 ions are located in B sites and Fe+3 ions are both located at A and B sites. The unit cell is characterized by a length of 8.38 Å and the interaction distances are b = 2.963 Å, u = 0.2714 Å, p = 2.963 Å, q = 0.3106 Å, r =38.336 Å and s = 3.127 Å [A. Goldman, “Modern Ferrite Technology”, New York: Van Nostrand Reinhold, (1990)]. Cobalt ferrite is characterized by high anisotropy values than the normal ferrites such as magnetite and maghemite. The anisotropy constant of bulk cobalt ferrite is in the range 1.8-3.0 x 106 erg/cm3 and the saturation magnetization is 80.8 emu/g at room temperature and 93.9 emu/g at 5 K [L.D. Tung, V. Kolesnichenko, D. Caruntu, N.H. Chou, C. T. O Connor, L. Spinu, “Magnetic properties of ultra fine cobalt ferrite nanoparticles,” J. Appl. Phys., Vol. 93 (2003) 7486-7488]. In cobalt ferrite, as
From the figure it is evident that the value of dielectric constant increased upto x=0.03 there after the dielectric constant decreases. This increase in dielectric constant with increase in concentration of Ce3+ and Dy3+ ions may be due to the fact that the RE3+ ion introduction results in the distortion of cobalt ferrite lattice. It also results in an increase in Fe-O and RE-O bond lengths at octahedral B site resulting in an increase in polarizability with a consequent increase in dielectric constant [17,
behaviour of the Fe-O-P bond angles and tilt angles in the beta-phase. During the transition from
The Fe-Cp stretch occurs at 471 cm-1 and is a single sharp peak, confirming that the iron is equally bonded to all 5 carbons of each ligand.