orbital. Group 11 &12 elements i.e. Cu & Zn have bigger size due to strong shielding of completely filled (n-1)d orbital. The transition elements show variable oxidation state due to small energy difference between (n-1)d &ns orbital as a result both (n-1)d &ns electrons take part in bond formation. The highest oxidation state of an element is equal to number of unpaired electrons present in (n-1)d &ns orbital. Transition elements have high enthalpy of atomization/ sublimation Because
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adding the nitric acid. Place the beaker in fume hood for approximately twenty minutes. If the copper has not completely reacted with the nitric acid; heat the beaker to speed up the reaction. This reaction is represented by the equation: Cu (s) + 4 HNO3 (aq)  Cu(NO3)2+2NO2 (g) +2H2O (l) this reaction resulting in a blue liquid and brown gas that has the odor of chlorine. 2. For step two have a four hundred milliliter beaker filled with three hundred milliliters of ice water. Place the beaker
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Chemistry102 5/7/2013 Lecture Presentation Chapter 17 Additional Aspects of Aqueous Equilibria John D. Bookstaver St. Charles Community College Cottleville‚ MO © 2012 Pearson Education‚ Inc. Common Ion Effect HA(aq) + H2O(l) ⇔ A−(aq) + H3O+(aq) • Adding a salt containing the anion NaA‚ which • is the conjugate base of the acid (the common ion)‚ shifts the position of equilibrium to the left This causes the pH to be higher than the pH of the acid solution 9lowering the H3O+ ion concentration
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external circuit. III. Oxidation takes place at the positive electrode (anode). A. I and II only B. I and III only C. II and III only D. I‚ II and III (2) 3. What happens to the Cr3+(aq) ion when it is converted to CrO (aq)? A. Its oxidation number decreases and it undergoes reduction. B. Its oxidation number decreases and it undergoes oxidation. C. Its oxidation number increases and it undergoes reduction. D. Its oxidation number increases and it undergoes oxidation. (2) 4. The following
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observed that with increasing the dissolved oxygen content of the pulp‚ the pulp pH decreased considerably and the pulp Eh changed from a reducing to more oxidizing value. These changes in pH and Eh of the pulp were found to be favorable for the pyrite oxidation and the oxygen consumption. Therefore‚ Owusu et al. concluded that with increasing aeration time‚ the formation of the iron oxy-hydroxide species and also coating the surface with these species increase. Then‚ however‚ because of the coverage of
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HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers |Chapter 25 Simple molecular substances with non-octet |Page Number | |structures and shapes of simple molecules | | |Class Practice |1 | |Chapter Exercise
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Then the absorbances were recorded from each cuvette and can be seen in table 1. A Beer’s law plot was made from the data that was recorded from the optical absorbance. During the second part of the experiment Fe (NO3)3 was added and diluted with HNO3 . All of the cuvettes were mixed with the same solutions in the second part of the experiment‚ which can be seen in table 2. A dilution calculation was made to determine the initial concentration of Fe3+and SCN-. Then the formula Abs + b/ slope was
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1178 - 181.15 Methyl benzoate 2.00 - 1.088 136.00 Sulfuric Acid 0.60 - 1.840 98.08 Nitric Acid 0.15 - 1.510 63.01 Chemical MP Exp. (°C) MP lit (°C) Methyl-3-nitrobenzoate 72.6-75.7 78.0-80.0 Mmole Calculations: HNO3 (16M)- 0.15 mL* (0.016 mole/mL) = 0.0024 mole* (1000 mmol/mole) = 2.4 mmoles H2SO4 (18M)- 0.60 mL* (0.018 mole/mL) = 0.0108 mole*(1000 mmol/mole) = 10.8 mmoles Limiting Reagent Calculation: methylbenzoate - 2.0 mL*(1.088g/mL)/( 136.00g/mol)= 0
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an iron (II) salt (ammonium iron (II) sulphate) Introduction Oxidation numbers describe the number of electrons the atom will gain or lose during a reaction. Each atom in an equation can be assigned an oxidation number according to certain rules. If the oxidation number of an atom increases as you go from the left side to the right side if an equation‚ oxidation has occurred (electrons have been lost); if the oxidation number decreases‚ reduction has occurred (electrons have been gained)
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Purpose: The purpose of this lab is to develop a deeper understanding of LeChatelier’s Principle by observing several systems at chemical equilibrium and interpreting the effects of varying concentrations and temperature. The principle states that if systems at equilibria are altered or disturbed in any form‚ the equilibria will shift to reduce the disturbing influence ( Catalyst‚ 186). In a 3 part experiment‚ we analyzed the outcome of changes in reactant and product concentrations‚ equilibrium
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