redoks
DESCRIPTION
KULIAH MAHASISWA PSIKTRANSCRIPT
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REDOKS
DEPARTMENT OF MEDICAL CHEMISTRYFACULTY OF MEDICINE
LAMBUNG MANGKURAT UNIVERSITY
MASHURI
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PENDAHULUAN
• REAKSI REDOKS ADALAH SEMUA REAKSI/PROSES KIMIA YANG MANA TERJADI PERUBAHAN BILANGAN OKSIDASI (BILOKS)
• OKSIDASI:PENINGKATAN BILOKS/KEHILANGAN ELEKTRON
• REDUKSI:PENURUNAN BILOKS/PENAMBAHAN ELEKTRON
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TERMINOLOGI=ISTILAH
• OKSIDAN=OXIDISER=UNSUR YANG MEMPUNYAI KEMAMPUAN UNTUK MENGOKSIDASI UNSUR LAIN (OXIDIZING AGENTS)
• REDUKTAN=REDUSER=UNSUR YANG MEMPUNYAI KEMAMPUAN UNTUK MEREDUKSI UNSUR LAIN (REDUCING AGENTS)
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BILANGAN OKSIDASI
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• BILANGAN OKSIDASI (BILOKS) ATAU STATUS OKSIDASI MERUPAKAN TOTAL JUMLAH ELEKTRON YANG BERPINDAH DARI SUATU UNSUR ATAU BERTAMBAH PADA SEBUAH UNSUR UNTUK MENCAPAI STATUS OKSIDASINYA
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• V --------------------> V2+ + 2e
STATUS OKSIDASI
VANADIUM +2
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• S + 2e --------------------> S2-
PENAMBAHAN ELEKTRON
STATUS OKSIDASI
SULFUR -2
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• OKSIDASI MERUPAKAN PENINGKATAN BILOKS/STATUS OKSIDASI
• REDUKSI MERUPAKAN PENURUNAN BILOKS/STATUS OKSIDASI
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NO COUNT
YOU LEARN SOME SIMPLE RULES
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RULES
• STATUS OKSIDASI UNSUR/SENYAWA NETRAL ADALAH 0 (NOL) CONTOH N2, Na, P4, H2
• UNTUK ION, STATUS OKSIDASI=MUATANNYA
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PENGGUNAAN BILOKS
• PENAMAAN SEBUAH SENYAWA MISAL: FeSO4 (NAMA DULUBESI (II) SULFAT) DAN FeSO3 (NAMA DULUBESI (II) SULFIT). PENAMAAN MODERN MEREFLEKSIKAN STATUS OKSIDASI SULFUR DALAM SENYAWA TERSEBUT
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• ION SO42-STATUS OKSIDASI
SULFUR ADALAH +6, MAKA ION INI DINAMAKAN ION SULFAT (VI)BESI (II) SULFAT (VI)
• ION SO32-STATUS OKSIDASI
SULFUR ADALAH +4,MAKA ION INI DINAMAKAN ION SULFAT (IV)BESI (II) SULFAT (IV)
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• MENENTUKAN UNSUR YANG DIOKSIDASI ATAU DIREDUKSI DALAM SEBUAH REAKSI
PENGGUNAAN BILOKS
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TIGA KONSEP REDOKS
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I. TRANSFER HIDROGEN*
OXIDATION IS LOSS OF HYDROGEN
REDUCTION IS GAIN OF HYDROGEN
*These are old definition which aren’t used very much nowadays.
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EXAMPLE
CH3CH2OH CH3CHO
oxidation by loss of hydrogen
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EXAMPLE
CH3CH2OH CH3CHO
reduction by gain of hydrogen
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II. TRANSFER OKSIGEN
OXIDATION IS GAIN OF OXYGEN
REDUCTION IS LOSS OF OXYGEN
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EXAMPLE
reduction
Fe2O3+3CO 2Fe+3CO2
oxidation
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EXAMPLE
reduction
Fe2O3+3CO 2Fe+3CO2
oxidation
A Reducing agent=TAKE (REMOVE) oxygen from another
An Oxidising agent=GIVE oxygen to another substance
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III. TRANSFER ELEKTRON
OXIDATION IS LOSS OF ELECTRONS
REDUCTION IS GAIN OF ELECTRONS
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““Oxidation-Reduction Reactions”Oxidation-Reduction Reactions”
LEO says GER
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CONTOH
Cu(s) + 2 Ag+(aq) Cu2+(aq) + 2 Ag(s)
Loss of Electrons =
OXIDATION (LEO) Gain of Electrons =
REDUCTION (GER)
HILANG 2 e- TAMBAH 2 e-
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Cu(s) Cu2+(aq) + 2 e-
Loss of Electrons =
OXIDATION (LEO)
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Ag+(aq) + e- Ag(s)
Gain of Electrons =
REDUCTION (GER)
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CONTOH LAIN
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ATOM NATRIUM KEHILANGAN 1 ELEKTRON
eNaNa10
10 CleCl
ATOM KLOR MENDAPAT 1 ELEKTRON
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eNaNa10
Lose Electrons = Oxidation
NATRIUM DIOKSIDASI
Gain Electrons = Reduction10
CleCl KLOR DIREDUKSI
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Reduction-Oxidation Reactions
oxidation
reduction
Na → Na+ + 1e-
Oxidation: Loss of electrons.
Na has been oxidized: Reducing agent.
Cl + 1e- → Cl-
Reduction: Gain of electrons.
Cl has been reduced: Oxidizing agent.
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Oxidising agents (OXIDAN)
• Oxygen, O2
• Ozone, O3
• Chlorine, Cl2
• Bromine, Br2
• Nitric acid, HNO3
• Conc sulphuric acid, H2SO4
• Potassium manganate (VII), KMnO4
• Potassium dichromate (VI), K2Cr2O7
• H2O2 in acid medium
Reducing agents (REDUKTAN)
• Hydrogen, H2
• Sulphur dioxide, SO2
• Hydrogen sulphide, H2S
• Carbon monoxide, CO
• Carbon, C
• Metals, Fe & Zn
• H2O2 in alkali medium
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How do you go about balancing an Oxidation-Reduction equation?
BAGAIMANA MENYEIMBANGKAN SEBUAH
PERSAMAAN REDOKS?
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WRITING IONIC EQUATIONS FOR REDOX REACTIONS: Electron-half-equations
(SETENGAH REAKSI SUASANA ASAM)
• Step 1:PISAHKAN PERSAMAAN MENJADI SETENGAH REAKSI.• Step 2:SEIMBANGKAN ATOM KECUALI O & H.• Step 3:SEIMBANGKAN O DENGAN PENAMBAHAN H2O.• Step 4:SEIMBANGKAN H DENGAN PENAMBAHAN ION H+
(SUASANA ASAM)• Step 5:SEIMBANGKAN MUATAN DENGAN PENAMBAHAN e-.• Step 6:SEIMBANGKAN KOEFISIEN KEDUA PERSAMAAN
TERSEBUT DENGAN MENGALIKANNYA DENGAN SUATU BILANGAN SEHINGGA KEDUA REAKSI TERSEBUT SEIMBANGKAN
• Step 7:JUMLAHKAN KEDUA SETENGAH REAKSI TERSEBUT, HILANGKAN SPESIES YANG MUNCUL PADA KEDUA SISI DARI REAKSI BERSIH
• Step 8:CEK ATOM DAN MUATAN APAKAH TELAH SEIMBANG
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WRITING IONIC EQUATIONS FOR REDOX REACTIONS:
Electron-half-equations (SETENGAH REAKSI PADA SUASANA BASA)
• Step 9:IDENTIFIKASI JUMLAH PROTON (H+), LALU TAMBAHKAN DENGAN JUMLAH YANG SAMA ION OH- PADA KEDUA SISI PERSAMAAN
• Step 10:JIKA H+ DAN OH- TAMPAK PADA SISI YANG SAMA PERSAMAAN, DENGAN PERBANDINAGN 1:1 MEMBENTUK H2O.
• Step 11:HILANGKAN MOLEKUL AIR YANG TAMPAK PADA KEDUA SISI PERSAMAAN
• Step 12:CEK MUATAN DAN ATOM
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TAKE HOME EXERCISE
1. Reaksi antara chlorine and iron (II): Cl2+Fe2+Cl-+Fe3+
2. Reaksi antara hydrogen peroxide and manganate (VII):
MnO4-+H2O2Mn2++O2
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3. Oksidasi Etanol oleh Natrium dikromat (VI):
CH3CH2OH+Cr2O72-CH3COOH+Cr3+
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WRITING IONIC EQUATIONS FOR REDOX REACTIONS:
Oxidation states (oxidation numbers)
• Assign oxidation numbers to all atoms• Identify oxidized and reduced species• Compute electrons lost (oxidation) and gained (reduction)• For reactions in acidic or basic solution, add H+/H2O (acidic)
or OH-/H2O (basic) to balance the charges.• Multiply these by appropriate factors make electrons lost =
electrons gained• Complete the equation by final inspection.
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REDOX IN BIOLOGICAL SYSTEM
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Cellular Respiration
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Photosynthesis
6 CO2 + 6 H2O + light → C6H12O6 + 6 O2
Carbon Dioxide + Water + Light energy → Glucose + Oxygen
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REDOX ON LIVE
SOURCE:
(http://www.google.co.id)
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Refining Metals