or polyatomic. The simplest compounds to name are binary ionic compounds‚ for example NaCl‚ which is named Sodium Chloride. Na having a positive oxidation number goes first followed by Cl which having a negative oxidation number goes last and is changed from Chlorine to chloride the -ide indicating its negative charge. Of course‚ the
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brass and bronze‚ are very important Has various oxidation states: 0 in elemental copper‚ +1‚ and +2 which is observable in corroded brass/bronze Oxidation states n n n Oxidation state is an indicator of the degree of oxidation of an atom The formal oxidation state is the theoretical charge the atom would have of all bonds were 100% ionic Oxidation is loss of electrons‚ reduction is gain of electrons (OIL RIG) Oxidation States of Copper n n n n n 0
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that all three alcohols should have a different level of reactivity. The hydrogen atom on the hydroxyl functional group can be easily substituted because of its enhanced acidity. This is the basis of a halogenation reaction‚ and controlled oxidation reaction‚ which will be observed through this investigation. Purpose: To observe and compare the reactivity of the isomers of butanol as examples of 1°‚ 2° ‚ and 3° alcohols. Hypothesis: The reactivity of primary alcohol will be lower than
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Module 7 Exam Review ANSWER KEY 1. Define acid. (7.01) An acid is a substance that produces hydrogen ions‚ H+ or hydrodium ionsH3O+ in solution. 2. Compare the three theories of acids. (7.01) An Arrhenius acid is a substance the increases the concentration of hydrogen ion‚ H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion‚ H+ to another substance. A Lewis acid is any substance that accepts a lone pair
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Absorbance of {Fe(SCN)}2+ “Knowns.” Test Tube | Diluted Fe3+ (mL) | Stock 0.50 M KSCN (mL) | Stock of 0.1 M HNO3 (mL) | 1 | 1.0 | 5.0 | 4.0 | 2 | 2.0 | 5.0 | 3.0 | 3 | 3.0 | 5.0 | 2.0 | 4 | 4.0 | 5.0 | 1.0 | 5 | 5.0 | 5.0 | 0.0 | For Part B: Absorbance of {Fe(SCN)}2+ “Unknowns” Test Tube | Stock 0.0025 M Fe(NO3)3 (mL) | Stock of 0.0025 M KSCN (mL) | Stock of 0.1 M HNO3 (mL) | 6 | 1.0 | 1.0 | 5.0 | 7 | 1.0 | 1.5 | 4.5 | 8 | 1.0 | 2.0 | 4.0 | 9 | 1.0 | 2.5 | 3.5 | 10 | 1
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electrolysis‚ or if a voltage is created by a chemical reaction as in a battery‚ it is an electrochemical reaction. In contrast‚ chemical reactions where electrons are transferred between molecules are called oxidation/reduction (redox) reactions. In general‚ electrochemistry deals with situations where oxidation and reduction reactions are separated in space or time‚ connected by an external electric circuit to understand each process. |Contents
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electrode and electrolyte and a salt bridge. In a galvanic cell one metal can undergo reduction and the other oxidation. A typical galvanic cell is based on the spontaneous redox reaction: Net Ionic Equation Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Half Equations Zn(s) → Zn2+(aq) + 2e– Cu2+(aq) + 2e– → Cu(s) The anode will undergo reduction (Zinc) and the cathode will undergo oxidation (Copper) The two half cells must be physically separated so that the solutions do not mix together. A salt
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eukaryotic organelles (mitochondria‚ chloroplasts) CELLULAR RESPIRATION GLUCOSE 1 2 GLYCOLYSIS 1 PYRUVATE OXIDATION2 KREBS CYCLE 3 2 ELECTRON TRANSPORT 4 CHAIN 2 NET ATP PRODUCED = 36 Nelson‚ 2003 Redox Reactions • Reduction-oxidation reactions – Transfer electrons from donor to acceptor atoms • Donor is oxidized as it releases electrons • Acceptor is reduced as it accepts electrons Cellular Respiration Series of chemical reactions and electron exchanges that convert
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Concentration Problem Sets Do the following problems in your lab notebook. Be sure to specify the knowns & unknowns‚ the formulas used‚ show your work with labeled units and round you’re answers to the appropriate significant figures. 15-1 Molarity Problems: (M = moles/ liter ) 1. What is the molar concentration of a 415 ml solution containing 0.745 moles of HCl? (A: 1.80 M HCl) 2. What is the molar concentration of an acetic acid (CH3COOH) solution containing 3.21 moles in 4.50
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CHEMISTRY (Theory) Time allowed : 3 hours General Instructions: (i) All questions are compulsory. Maximum Marks : 70 (ii) Marks for each question are indicated against it. (iii) Question numbers 1 to 8 are very short-answer questions and carry 1 mark each. (iv) Question numbers 9 to 18 are short-answer questions and carry 2 marks each. (v) Question numbers 19 to 27 are also short-answer questions and carry 3 marks each. (vi) Question numbers 28 to 30 are long-answer questions and carry 5 marks
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