Binary Compounds w/ Fixed Charge Given The Formula‚ Write The Name Binary Compounds w/ Fixed Charge Given The Name‚ Write The Formula Binary Compounds w/ Variable Charge: Stock System Given The Name‚ Write The Formula Binary Compounds w/ Variable Charge: Stock System Given The Formula‚ Write TheName 1) MgO 2) LiBr 3) Ca3N2 4) Al2S3 5) KI 6) SrCl2 7) Na2S 8) RaBr2 9) MgS 10) AlN 11) Cs2S 12) KCl 13) Sr3P2 14) BaI2 15) NaF 16) CaBr2 17) BeO 18) SrS 19) BF3 20) AlP 21) Rb2O 22) CaI2
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parentheses‚ followed by the name of the element‚ is used for elements that can form more than one positive ion. This is usually seen with metals. You can use a chart to see the possible valences for the elements. Fe2+ Iron (II)Fe3+ Iron (III)Cu+ Copper (I)Cu2+ Copper (II) -ous and -icAlthough Roman numerals are used to denote the ionic charge of cations‚ it is still common to see and use the endings -ous or -ic. These endings are added to the Latin name of the element (e.g.‚stannous/stannic for tin) to
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under kerosene oil because they get tarnished on exposure to air. 2. The general electron configuration of alkali metals is ns1. 3. Alkali metals have largest size and lowest ionization enthalpy in their respective periods. Down the group‚ the size of alkali metals increases whereas ionization enthalpy decreases. 4. Alkali metals have low densities and densities increases from Li to Cs. (Exception: K is lighter than Na‚ due to bigger size of potassium atom). 5. Alkali metals have low
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Chapter Exercise 33 Chapter 34 Importance of redox reactions in modern ways of living Class Practice 36 Chapter Exercise 37 Part Exercise 39 Chapter 35 Energy changes in chemical reactions Class Practice 42 Chapter Exercise 43 Chapter 36 Standard enthalpy change of combustion‚ neutralization‚ solution and formation Class Practice 44 Chapter Exercise 46 Chapter 37 Hess’s Law Class Practice 48 Chapter Exercise 51 Part Exercise 53 Chapter 25 Simple molecular substances with non-octet structures and
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energy are the evidences of a chemical reaction‚ thus‚ of a chemical change. Materials Crucible tongs Evaporating dish Glass rod Test tubes Test tube rack Thermometer Analytical balance Magnesium ribbon pH paper 1M copper (II) sulfate Iron metal 6M hydrochloric acid Procedure Magnesium and oxygen test A small strip of magnesium metal is held on one end with a pair of crucible tongs‚ while the other end is ignited with the flame of Bunsen burner. The burning
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Abstract: The purpose of this experiment was to determine the concentration of an unknown amount of copper sulfate using the spectronic 20. Four solutions of different concentrations of H₂O and CuSO₄ were put into the spectronic 20 to observe their absorption of light. Then‚ a graph was created to plot down the measurements. Using the calibration curve of the graph‚ the concentration of the unknown substance was found out to be .12M. Background/Introduction: Beer’s law (which states that
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complexes will be compared by the color each reflects and by the energy of the waves each absorbs. The purity of the synthesized complex will also be found. Procedure Part I: Preparation of the Complex A sample of copper sulfate pentahydrate (6.285g) was weighed out. The copper sulfate pentahydrate was dissolved in water (11.99mL) in a 250mL beaker. The solution was heated on a hot plate to 90 degrees Celsius. A sample of potassium oxalate monohydrate (10.006g) was dissolved in water (50.0mL).
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separate some light sources in to constituent colors and find out the wavelength of some atomic emissions. We will also try to compare the line spectra found from gas discharge tubes and flame emissions. Finally‚ we will measure the absorbance of Copper sulfate solution as a function of wavelength. Experimental Method: We start our experiment by looking through a Spectroscope at the outside sunlight‚ a regular light bulb (incandescent) and a fluorescent light. This will give us a good observation
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empirical formula for hydrated copper sulfate. In doing this lab‚ one was able to see the gradual change in the composition of a hydrate into an anhydrous salt. The lab was carried out with numerous steps. First‚ one had to safely prepare by putting on goggles. One then had to wash and heat the dish with the flame for about three minutes. After allowing the dish to cool‚ one had to weigh the evaporating dish and record the weight. Two to three grams of copper sulfate hydrate was then added to the
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B. K.‚ R. K. Shukla‚ and V.S Agashe‚ 1972). The Biuret test for protein was used to determine the presence of peptide bonds in proteins. The color of samples before was clear. Both sodium hydroxide and copper sulfate were clear color as well. When you added sodium hydroxide and copper sulfate into the samples‚ protein would turn into purple. The structure of proteins was form by the
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