REDOX OxidationReduction Reactions OxidationReduction Reactions Electrons are transferred
![REDOX Oxidation-Reduction Reactions REDOX Oxidation-Reduction Reactions](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-1.jpg)
![Oxidation-Reduction Reactions • Electrons are transferred from 1 atom to another. • All single-replacement Oxidation-Reduction Reactions • Electrons are transferred from 1 atom to another. • All single-replacement](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-2.jpg)
![Oxidation = loss of electrons. LOSS of ELECTRONS = OXIDATION LEO Oxidation = loss of electrons. LOSS of ELECTRONS = OXIDATION LEO](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-3.jpg)
![Reduction = gain of electrons. GAIN of ELECTRONS = REDUCTION GER Reduction = gain of electrons. GAIN of ELECTRONS = REDUCTION GER](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-4.jpg)
![REDOX • Oxidation & Reduction are complementary. • They occur together & simultaneously or REDOX • Oxidation & Reduction are complementary. • They occur together & simultaneously or](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-5.jpg)
![LEO GOES GER!!! Oxidation of Cu LEO GOES GER!!! Oxidation of Cu](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-6.jpg)
![Oxidation Numbers • In Ionic Compounds: the number of electrons lost or gained by Oxidation Numbers • In Ionic Compounds: the number of electrons lost or gained by](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-7.jpg)
![Assigning Oxidation Numbers Assigning Oxidation Numbers](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-8.jpg)
![8 Rules for Oxidation Numbers 1. of a free, uncombined element = 0. Na 8 Rules for Oxidation Numbers 1. of a free, uncombined element = 0. Na](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-9.jpg)
![8 Rules for Oxidation Numbers 3. Fluorine is always -1. CF 4 4. Hydrogen 8 Rules for Oxidation Numbers 3. Fluorine is always -1. CF 4 4. Hydrogen](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-10.jpg)
![8 Rules for Oxidation Numbers 5. Oxygen is nearly always -2 except when its 8 Rules for Oxidation Numbers 5. Oxygen is nearly always -2 except when its](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-11.jpg)
![8 Rules for Oxidation Numbers 6. The sum of oxidation numbers in a neutral 8 Rules for Oxidation Numbers 6. The sum of oxidation numbers in a neutral](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-12.jpg)
![8 Rules for Oxidation Numbers 8. In covalent compounds, the oxidation number of the 8 Rules for Oxidation Numbers 8. In covalent compounds, the oxidation number of the](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-13.jpg)
![Assign Oxidation Nos • • • K = +1, Cl = -1 KCl Ca. Assign Oxidation Nos • • • K = +1, Cl = -1 KCl Ca.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-14.jpg)
![Electrons are Negative! • Why do we use the word “reduced” when electrons are Electrons are Negative! • Why do we use the word “reduced” when electrons are](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-15.jpg)
![Writing Equations • Even though oxidation & reduction occur together, we can write separate Writing Equations • Even though oxidation & reduction occur together, we can write separate](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-16.jpg)
![Conservation of Mass • # of atoms of each type is the same on Conservation of Mass • # of atoms of each type is the same on](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-17.jpg)
![Conservation of Charge • Total charge on LHS must equal total charge on RHS. Conservation of Charge • Total charge on LHS must equal total charge on RHS.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-18.jpg)
![Reduction Half-Reactions Electrons are gained so • I 2 + 2 e- 2 Ithey Reduction Half-Reactions Electrons are gained so • I 2 + 2 e- 2 Ithey](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-19.jpg)
![Oxidation Half-reactions • K K 1+ + 1 e • Fe 2+ Fe 3+ Oxidation Half-reactions • K K 1+ + 1 e • Fe 2+ Fe 3+](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-20.jpg)
![Identifying Half-Reactions • Reduction: electron term is on reactant side. • Oxidation: electron term Identifying Half-Reactions • Reduction: electron term is on reactant side. • Oxidation: electron term](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-21.jpg)
![Vocabulary Interlude • Oxidizing Agent: Is itself reduced. Accepts electrons from something else – Vocabulary Interlude • Oxidizing Agent: Is itself reduced. Accepts electrons from something else –](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-22.jpg)
![Figuring out what is what! • Given an unbalanced equation. • Goal: Balance it. Figuring out what is what! • Given an unbalanced equation. • Goal: Balance it.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-23.jpg)
![What’s oxidized & what’s reduced? USE OIL RIG What’s oxidized & what’s reduced? USE OIL RIG](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-24.jpg)
![4 3 2 1 0 -1 -2 -3 -4 2) And if you’re lucky 4 3 2 1 0 -1 -2 -3 -4 2) And if you’re lucky](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-25.jpg)
![Oxidizing & Reducing Agents • They are both ALWAYS on the reactant side. • Oxidizing & Reducing Agents • They are both ALWAYS on the reactant side. •](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-26.jpg)
![Oxidizing & Reducing Agents • What’s oxidized & what’s reduced: 0 +2, -1 0 Oxidizing & Reducing Agents • What’s oxidized & what’s reduced: 0 +2, -1 0](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-27.jpg)
![Oxidizing & Reducing Agents 3, -1 2, -1 4, -1 2 Fe. Br 3 Oxidizing & Reducing Agents 3, -1 2, -1 4, -1 2 Fe. Br 3](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-28.jpg)
- Slides: 28
![REDOX OxidationReduction Reactions REDOX Oxidation-Reduction Reactions](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-1.jpg)
REDOX Oxidation-Reduction Reactions
![OxidationReduction Reactions Electrons are transferred from 1 atom to another All singlereplacement Oxidation-Reduction Reactions • Electrons are transferred from 1 atom to another. • All single-replacement](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-2.jpg)
Oxidation-Reduction Reactions • Electrons are transferred from 1 atom to another. • All single-replacement & combustion rxns are redox rxns.
![Oxidation loss of electrons LOSS of ELECTRONS OXIDATION LEO Oxidation = loss of electrons. LOSS of ELECTRONS = OXIDATION LEO](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-3.jpg)
Oxidation = loss of electrons. LOSS of ELECTRONS = OXIDATION LEO
![Reduction gain of electrons GAIN of ELECTRONS REDUCTION GER Reduction = gain of electrons. GAIN of ELECTRONS = REDUCTION GER](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-4.jpg)
Reduction = gain of electrons. GAIN of ELECTRONS = REDUCTION GER
![REDOX Oxidation Reduction are complementary They occur together simultaneously or REDOX • Oxidation & Reduction are complementary. • They occur together & simultaneously or](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-5.jpg)
REDOX • Oxidation & Reduction are complementary. • They occur together & simultaneously or not at all.
![LEO GOES GER Oxidation of Cu LEO GOES GER!!! Oxidation of Cu](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-6.jpg)
LEO GOES GER!!! Oxidation of Cu
![Oxidation Numbers In Ionic Compounds the number of electrons lost or gained by Oxidation Numbers • In Ionic Compounds: the number of electrons lost or gained by](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-7.jpg)
Oxidation Numbers • In Ionic Compounds: the number of electrons lost or gained by an atom when it forms ions. Oxidation states of Vanadium
![Assigning Oxidation Numbers Assigning Oxidation Numbers](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-8.jpg)
Assigning Oxidation Numbers
![8 Rules for Oxidation Numbers 1 of a free uncombined element 0 Na 8 Rules for Oxidation Numbers 1. of a free, uncombined element = 0. Na](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-9.jpg)
8 Rules for Oxidation Numbers 1. of a free, uncombined element = 0. Na He O 2 N 2 S 8 Cl 2 2. of a monatomic ion = charge on ion. +2 -1 +3 P Ca = +2. Cl = -1. Al = +3. Remember: Ions occur in ionic compounds: Ca. Cl 2, Al(NO 3)3, etc.
![8 Rules for Oxidation Numbers 3 Fluorine is always 1 CF 4 4 Hydrogen 8 Rules for Oxidation Numbers 3. Fluorine is always -1. CF 4 4. Hydrogen](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-10.jpg)
8 Rules for Oxidation Numbers 3. Fluorine is always -1. CF 4 4. Hydrogen is nearly always +1, except when it’s bonded to a metal. Then it’s -1. H 2 O, HNO 3, H 2 SO 4 Li. H Ca. H 2 Na. H
![8 Rules for Oxidation Numbers 5 Oxygen is nearly always 2 except when its 8 Rules for Oxidation Numbers 5. Oxygen is nearly always -2 except when its](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-11.jpg)
8 Rules for Oxidation Numbers 5. Oxygen is nearly always -2 except when its -Bonded to fluorine, where O is +2 OF 2 -In the peroxide ion, where O is -1. O 22 -
![8 Rules for Oxidation Numbers 6 The sum of oxidation numbers in a neutral 8 Rules for Oxidation Numbers 6. The sum of oxidation numbers in a neutral](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-12.jpg)
8 Rules for Oxidation Numbers 6. The sum of oxidation numbers in a neutral compound is 0. H 2 O CO 2 NO SO 3 7. The sum of oxidation numbers in a polyatomic ion = charge of the ion. Sum in SO 42 - = -2. Sum in NO 3 - = -1.
![8 Rules for Oxidation Numbers 8 In covalent compounds the oxidation number of the 8 Rules for Oxidation Numbers 8. In covalent compounds, the oxidation number of the](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-13.jpg)
8 Rules for Oxidation Numbers 8. In covalent compounds, the oxidation number of the more electronegative atom is the negative charge it would have if it was an ion. *NH 3: N = -3, H = +1. Si. Cl 4: Si = +4, Cl = -1.
![Assign Oxidation Nos K 1 Cl 1 KCl Ca Assign Oxidation Nos • • • K = +1, Cl = -1 KCl Ca.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-14.jpg)
Assign Oxidation Nos • • • K = +1, Cl = -1 KCl Ca. Br 2 Ca = +2, Br = -1 CO C = +2, O = -2 C = +4, O = -2 CO 2 Al(NO 3)3 Al = +3, O = -2, N = +5 Na 3 PO 4 Na = +1, O = -2, P = +5 H 2 S H = +1, S = -2 NH 4+1 N = -3, H = +1 SO 3 -2 S = +4, O = -2
![Electrons are Negative Why do we use the word reduced when electrons are Electrons are Negative! • Why do we use the word “reduced” when electrons are](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-15.jpg)
Electrons are Negative! • Why do we use the word “reduced” when electrons are gained? Look at how the oxidation number changes. For example, if Cl gains an electron it becomes Cl-1. The oxidation number decreased from 0 to -1. The oxidation number was reduced.
![Writing Equations Even though oxidation reduction occur together we can write separate Writing Equations • Even though oxidation & reduction occur together, we can write separate](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-16.jpg)
Writing Equations • Even though oxidation & reduction occur together, we can write separate equations for each process. • Called Half-Reactions. • In order to balance a redox equation, we have to split the full equaton into halfreactions.
![Conservation of Mass of atoms of each type is the same on Conservation of Mass • # of atoms of each type is the same on](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-17.jpg)
Conservation of Mass • # of atoms of each type is the same on both sides of the equation. • Still holds for half-reactions. • Do this step first.
![Conservation of Charge Total charge on LHS must equal total charge on RHS Conservation of Charge • Total charge on LHS must equal total charge on RHS.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-18.jpg)
Conservation of Charge • Total charge on LHS must equal total charge on RHS. • In the past, we usually had both sides neutral. (0 = 0. ) • Note: Total charge can be nonzero. Just has to be equal on the 2 sides. • If not balanced, add electrons to whichever side is too positive.
![Reduction HalfReactions Electrons are gained so I 2 2 e 2 Ithey Reduction Half-Reactions Electrons are gained so • I 2 + 2 e- 2 Ithey](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-19.jpg)
Reduction Half-Reactions Electrons are gained so • I 2 + 2 e- 2 Ithey are like a reactant ! • O 2 + 4 e- 2 O-2 • Half-reactions must demonstrate conservation of mass & conservation of charge. • # of atoms of each element on LHS equals “ “ “ “ RHS. • Total charge on LHS = Total charge on RHS
![Oxidation Halfreactions K K 1 1 e Fe 2 Fe 3 Oxidation Half-reactions • K K 1+ + 1 e • Fe 2+ Fe 3+](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-20.jpg)
Oxidation Half-reactions • K K 1+ + 1 e • Fe 2+ Fe 3+ + 1 e • Cu 2+ + 2 e- Electrons are lost so they appear on the product side! • Total Charge on LHS = Total Charge on RHS • # atoms LHS = # atoms RHS
![Identifying HalfReactions Reduction electron term is on reactant side Oxidation electron term Identifying Half-Reactions • Reduction: electron term is on reactant side. • Oxidation: electron term](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-21.jpg)
Identifying Half-Reactions • Reduction: electron term is on reactant side. • Oxidation: electron term is on product side.
![Vocabulary Interlude Oxidizing Agent Is itself reduced Accepts electrons from something else Vocabulary Interlude • Oxidizing Agent: Is itself reduced. Accepts electrons from something else –](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-22.jpg)
Vocabulary Interlude • Oxidizing Agent: Is itself reduced. Accepts electrons from something else – aids oxidation for another species. • Reducing Agent: Is itself oxidized. • Loses electrons to something else – aids reduction for another species.
![Figuring out what is what Given an unbalanced equation Goal Balance it Figuring out what is what! • Given an unbalanced equation. • Goal: Balance it.](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-23.jpg)
Figuring out what is what! • Given an unbalanced equation. • Goal: Balance it. • Procedure: – Assign oxidation numbers to everything – Split into half-reactions – Balance them separately – “Match” the electrons – Add them together
![Whats oxidized whats reduced USE OIL RIG What’s oxidized & what’s reduced? USE OIL RIG](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-24.jpg)
What’s oxidized & what’s reduced? USE OIL RIG
![4 3 2 1 0 1 2 3 4 2 And if youre lucky 4 3 2 1 0 -1 -2 -3 -4 2) And if you’re lucky](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-25.jpg)
4 3 2 1 0 -1 -2 -3 -4 2) And if you’re lucky you strike oil & it shoots up 1) You dig down with an oil rig
![Oxidizing Reducing Agents They are both ALWAYS on the reactant side Oxidizing & Reducing Agents • They are both ALWAYS on the reactant side. •](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-26.jpg)
Oxidizing & Reducing Agents • They are both ALWAYS on the reactant side. • Identify them by seeing how the oxidation 4 numbers change. 3 0 +2 +2 0 Mg + Cu 2+ Mg 2+ + Cu Mg is oxidized, so Mg is the reducing agent! 2 1 0 -1 -2 -3 -4
![Oxidizing Reducing Agents Whats oxidized whats reduced 0 2 1 0 Oxidizing & Reducing Agents • What’s oxidized & what’s reduced: 0 +2, -1 0](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-27.jpg)
Oxidizing & Reducing Agents • What’s oxidized & what’s reduced: 0 +2, -1 0 Ca + Fe. Cl 2 Ca. Cl 2 + Fe • Assign oxidation numbers • Figure out what increases & what decreases. Ca is oxidized; Fe 2+ is reduced. Ca = reducing agent; Fe. Cl 2 = oxidizing agnt. 4 3 2 1 0 -1 -2 -3 -4
![Oxidizing Reducing Agents 3 1 2 1 4 1 2 Fe Br 3 Oxidizing & Reducing Agents 3, -1 2, -1 4, -1 2 Fe. Br 3](https://slidetodoc.com/presentation_image/fb74bc4001bea397bf91fe2d51247ba8/image-28.jpg)
Oxidizing & Reducing Agents 3, -1 2, -1 4, -1 2 Fe. Br 3 + Sn. Br 2 2 Fe. Br 2 + Sn. Br 4 Fe 3+ is reduced to Fe 2+ Sn 2+ is oxidized to Sn 4+ Fe. Br 3 is the oxidizing agent. Sn. Br 2 is the reducing agent.
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