Chemical Reactions REDOX

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1 Chemical Reactions REDOX There are two types of Chemical Changes: 1. Reactions in which ions are being rearranged with no change in their oxidation states. METATHESIS. Reactions in which electrons are being transferred from atom(s) to atom(s). REDOX Metathesis Reaction Types Redox Double Neutralization Precipitation Single Combustion Synthesis Decomposit Displacement Displacement Ion Exchange Ions are combined to form new compounds Electron Transfer Electrons are lost from one atom, or group of atoms, and gained by another atom, or group of atoms, resulting in new atomic interactions forming new compounds Metathesis reactions occur when two ionic aqueous solutions are mixed and the ions switch partners. AX + BY AY + BX Metathesis reactions remove ions from solution in two ways: 1. form an insoluble solid.. form predominantly unionized molecules like H O (l) and CO (g). Ion removal is the driving force of metathesis reactions. 1. Precipitation reactions are metathesis reactions in which an insoluble compound is formed from two aqueous solutions. The solid precipitates out of the solution much like rain or snow precipitates out of the air.. Acid-Base (neutralization) Reactions Formation of the nonelectrolyte H O acid + base salt + water A salt is another name for an ionic compound formed from the cation of a base and an anion from an acid 1

2 3. Double Displacement reactions Are reactions where two aqueous solutions result in the formation of nonelectrolyte compounds other than water. Example: HCl + Na SO NaCl + H O SO (aq) 3(aq) (aq) g Redox Reactions Reactions in which one or more electrons are transferred Na (s) + Cl (g) NaCl (s) Species loosing electrons is said to be oxidized and the species gaining electrons is said to be reduced Types of Redox Rxn s Synthesis Decomposition Single Replacement Combustion Electrons are transferred in most cases Combustion of Methane CH 4 + O CO + H O Carbon looses electrons and oxygen gains electrons Notice that in the reaction, there are no ions present as either reactants or products, however, electrons are still transferred An understanding of oxidation states will show the transfer of electrons Oxidation Numbers In order to keep track of what loses electrons and what gains them, we assign oxidation numbers. Oxidation States (Oxidation Numbers) A system of book-keeping for electrons in molecules or ions The imaginary charges atoms would have in molecules and real charges in ionic compounds

3 Oxidation states provide a way to track electrons in chemical reactions Especially useful for reactions containing covalent compounds which have no charges * Note Charges are written: Fe +, Cl 1- Oxidation states are written: Fe +, Cl -1 Assigning Oxidation Numbers 1. The oxidation state of an atom in an element is zero Na (s), O (s), Hg (l). The oxidation state of a monatomic ion is the same as its charge Na +, Cl -, N -3, Ca + Alkali metals, alkaline earth metals, Al, Ga, Ge. 3. Fluorine is always -1 in its compounds HF, PF 3 H +1 F -1, P +3 F -1 Notice the oxidation states are written +1, whereas a charge would be written Oxygen is always - in its compounds H O, CO Exceptions: Peroxides (containing O - ) in which oxygen is -1 5.Hydrogen is +1 when bonded to a non-metal and -1 when bonded to a metal H O, HCl, H 3 N 3

4 6. Other oxidation states are calculated from algebraic sum of known states Transitions, metalloids, and usually carbon, silicon, and boron. The sum of the oxidation numbers in a neutral compound is 0; The sum of the oxidation numbers in a polyatomic ion is the charge on the ion. 7. For non-described atoms in compounds, the atom with the greatest electronegativity is assigned a negative oxidation state equal to its imaginary charge in an ionic compound CN, CN - 1. Identify the oxidation states for each atom in each of the following compounds/ions: SF 6 PbS Al 3+ N HClO NaNO CO AsH CaCO 3 HNO K Cr O 7 P 4 S NO 3 - NH 4 + Identify the oxidation state for each of the following compounds in the reaction: CH 4 + O CO + H O Notice, carbon has changed from a 4 to a + 4 oxidation state and oxygen has changed from 0 to and Carbon was oxidized and oxygen was reduced Recognizing a Redox Reaction Oxidation and Reduction Reaction Type Oxidation Reduction In terms of oxygen gain loss In terms of hydrogen loss gain In terms of electrons loss gain A species is oxidized when it loses electrons. Here, zinc loses two electrons to go from neutral zinc metal to the Zn + ion. 4

5 Oxidation and Reduction Oxidation and Reduction A species is reduced when it gains electrons. Here, each of the H + gains an electron and they combine to form H. What is reduced is the oxidizing agent. H + oxidizes Zn by taking electrons from it. What is oxidized is the reducing agent. Zn reduces H + by giving it electrons. Common Oxidizing and Reducing Agents Metals (Cu) are reducing agents HNO 3 is an oxidizing agent Cu + HNO 3 --> Cu + + NO K + H O --> KOH + H Metals (Na, K, Mg, Fe) are reducing agents. Identify the species being reduced and oxidized in each of the following reactions. Then label the oxidizing agent and the reducing agent in the reaction: a. C (s) + 3F (g) CF 3(s) b. S 8 (s) + 8O (g) 8SO (s) c. H O H (g) + O (g) d. Mg (s) + O (g) MgO (s) e. KClO 3 (s) KCl (s) + 3O (g) f. Ca (s) + O (g) CaO (s) g. Cu (s) + AgNO 3(aq) Cu(NO 3 ) (aq) + Ag (s) h. Na (s) + H S (aq) Na S (aq) + H (g) 5

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