Different metals Essay Example For Students

Different metals Essay Outline1 Introduction2 ELECTROCHEMICAL SERIES3 E ° ( V )4 Ref.5 2H++ 2e?H2 ( g )6 0.00007 ?08 Oxidation / decrease and the electrochemical series9 Reducing agents and oxidizing agents10 REACTIVITY SERIES11 Chemical reaction with H2O and acids12 Single supplanting reactions13 Comparison with standard electrode potencies14 Application of electrochemical series Introduction Different metals get ionised at different rates. For e.g. , metals like Na when exposed to air unite about immediately with the O present therein ( sodium atom gives up an negatron about every bit shortly as it is in contact with O ) . On the other manus, metals like gold if exposed to aerate even for a really long period, do non respond with air. Even if gold is dropped into an acid, it remains unaffected. Based on the easiness with which metals lose their negatrons and organize their ions, the metals are besides arranged in a series called Metal Activity Series. Metallic elements that ionise most easy are placed at the top of the Metal Activity Series, and those that ionise least easy are placed at the lower most terminal. Most of the elements of the periodic tabular array can be arranged in such a manner, which reflects their order of activity. This agreement of elements in order of their increasing rates of ionization i.e. oxidising and cut downing strength, is besides called the activity series or the electrochemical series. ELECTROCHEMICAL SERIES Half-reaction E ° ( V ) Ref. N2 ( g ) + H++e?HN3 ( aq ) ?3.09 Li++e?Li ( s ) ?3.0401 N2 ( g ) + 4H2O + 2e?2NH2OH ( aq ) + 2OH? ?3.04 Cs++e?Cs ( s ) ?3.026 Rb++e?Rb ( s ) ?2.98 K++e?K ( s ) ?2.931 Ba2++ 2e?Ba ( s ) ?2.912 La ( OH ) 3 ( s ) + 3e?La ( s ) + 3OH? ?2.90 Sr2++ 2e?Sr ( s ) ?2.899 Ca2++ 2e?Ca ( s ) ?2.868 Eu2++ 2e?Eu ( s ) ?2.812 Ra2++ 2e?Ra ( s ) ?2.8 Na++e?Na ( s ) ?2.71 La3++ 3e?La ( s ) ?2.379 Y3++ 3e?Y ( s ) ?2.372 Mg2++ 2e?Mg ( s ) ?2.372 ZrO ( OH ) 2 ( s ) + H2O + 4e?Zr ( s ) + 4OH? ?2.36 Al ( OH ) 4?+ 3e?Al ( s ) + 4OH? ?2.33 Al ( OH ) 3 ( s ) + 3e?Al ( s ) + 3OH? ?2.31 H2 ( g ) + 2e?2H? ?2.25 Ac3++ 3e?Ac ( s ) ?2.20 Be2++ 2e?Be ( s ) ?1.85 U3++ 3e?U ( s ) ?1.66 Al3++ 3e?Al ( s ) ?1.66 Ti2++ 2e?Ti ( s ) ?1.63 ZrO2 ( s ) + 4H++ 4e?Zr ( s ) + 2H2O ?1.553 Zr4++ 4e?Zr ( s ) ?1.45 TiO ( s ) + 2H++ 2e?Ti ( s ) + H2O ?1.31 Zn ( OH ) 42?+ 2e?Zn ( s ) + 4OH- ?1.199 Ti2O3 ( s ) + 2H++ 2e?2TiO ( s ) + H2O ?1.23 Ti3++ 3e?Ti ( s ) ?1.21 Mn2++ 2e?Mn ( s ) ?1.185 Te ( s ) + 2e?Te2? ?1.143 V2++ 2e?V ( s ) ?1.13 Nb3++ 3e?Nb ( s ) ?1.099 Sn ( s ) + 4H++ 4e?SnH4 ( g ) ?1.07 SiO2 ( s ) + 4H++ 4e?Si ( s ) + 2H2O ?0.91 B ( OH ) 3 ( aq ) + 3H++ 3e?B ( s ) + 3H2O ?0.89 TiO2++ 2H++ 4e?Ti ( s ) + H2O ?0.86 Bi ( s ) + 3H++ 3e?BiH3 ?0.8 2H2O+ 2e?H2 ( g ) + 2OH? ?0.8277 Zn2++ 2e?Zn ( Hg ) ?0.7628 Zn2++ 2e?Zn ( s ) ?0.7618 Ta2O5 ( s ) + 10H++ 10e?2Ta ( s ) + 5H2O ?0.75 Cr3++ 3e?Cr ( s ) ?0.74 ?+e?Au ( s ) + 2CN? ?0.60 Ta3++ 3e?Ta ( s ) ?0.6 PbO ( s ) + H2O + 2e?Pb ( s ) + 2OH? ?0.58 2TiO2 ( s ) + 2H++ 2e?Ti2O3 ( s ) + H2O ?0.56 Ga3++ 3e?Ga ( s ) ?0.53 AgI ( s ) +e?Ag ( s ) + I? ?0.15224 U4++e?U3+ ?0.52 H3PO2 ( aq ) + H++e?P ( white ) + 2H2O ?0.508 H3PO3 ( aq ) + 2H++ 2e?H3PO2 ( aq ) + H2O ?0.499 H3PO3 ( aq ) + 3H++ 3e?P ( ruddy ) + 3H2O ?0.454 Fe2++ 2e?Fe ( s ) ?0.44 2CO2 ( g ) + 2H++ 2e?HOOCCOOH ( aq ) ?0.43 Cr3++e?Cr2+ ?0.42 Cd2++ 2e?Cd ( s ) ?0.40 GeO2 ( s ) + 2H++ 2e?GeO ( s ) + H2O ?0.37 Cu2O ( s ) + H2O + 2e?2Cu ( s ) + 2OH? ?0.360 PbSO4 ( s ) + 2e?Pb ( s ) + SO42? ?0.3588 PbSO4 ( s ) + 2e?Pb ( Hg ) + SO42? ?0.3505 Eu3++e?Eu2+ ?0.35 In3++ 3e?In ( s ) ?0.34 Tl++e?Tl ( s ) ?0.34 Ge ( s ) + 4H++ 4e?GeH4 ( g ) ?0.29 Co2++ 2e?Co ( s ) ?0.28 H3PO4 ( aq ) + 2H++ 2e?H3PO3 ( aq ) + H2O ?0.276 V3++e?V2+ ?0.26 Ni2++ 2e?Ni ( s ) ?0.25 As ( s ) + 3H++ 3e?AsH3 ( g ) ?0.23 MoO2 ( s ) + 4H++ 4e?Mo ( s ) + 2H2O ?0.15 Si ( s ) + 4H++ 4e?SiH4 ( g ) ?0.14 Sn2++ 2e?Sn ( s ) ?0.13 O2 ( g ) + H++e?HO2†¢ ( aq ) ?0.13 Pb2++ 2e?Pb ( s ) ?0.13 WO2 ( s ) + 4H++ 4e?W ( s ) + 2H2O ?0.12 P ( ruddy ) + 3H++ 3e?PH3 ( g ) ?0.111 CO2 ( g ) + 2H++ 2e?HCOOH ( aq ) ?0.11 Se ( s ) + 2H++ 2e?H2Se ( g ) ?0.11 CO2 ( g ) + 2H++ 2e?CO ( g ) + H2O ?0.11 SnO ( s ) + 2H++ 2e?Sn ( s ) + H2O ?0.10 SnO2 ( s ) + 2H++ 2e?SnO ( s ) + H2O ?0.09 WO3 ( aq ) + 6H++ 6e?W ( s ) + 3H2O ?0.09 P ( white ) + 3H++ 3e?PH3 ( g ) ?0.063 HCOOH ( aq ) + 2H++ 2e?HCHO ( aq ) + H2O ?0.03 2H++ 2e?H2 ( g ) 0.0000 ?0 AgBr ( s ) +e?Ag ( s ) + Br? +0.07133 S4O62?+ 2e?2S2O32? +0.08 Fe3O4 ( s ) + 8H++ 8e?3Fe ( s ) + 4H2O +0.085 N2 ( g ) + 2H2O + 6H++ 6e?2NH4OH ( aq ) +0.092 HgO ( s ) + H2O + 2e?Hg ( cubic decimeter ) + 2OH? +0.0977 Cu ( NH3 ) 42++e?Cu ( NH3 ) 2++ 2NH3 +0.10 Ru ( NH3 ) 63++e?Ru ( NH3 ) 62+ +0.10 N2H4 ( aq ) + 4H2O + 2e?2NH4++ 4OH? +0.11 H2MoO4 ( aq ) + 6H++ 6e?Mo ( s ) + 4H2O +0.11 Ge4++ 4e?Ge ( s ) +0.12 C ( s ) + 4H++ 4e?CH4 ( g ) +0.13 HCHO ( aq ) + 2H++ 2e?CH3OH ( aq ) +0.13 S ( s ) + 2H++ 2e?H2S ( g ) +0.14 Sn4++ 2e?Sn2+ +0.15 Cu2++e?Cu+ +0.159 HSO4?+ 3H++ 2e?SO2 ( aq ) + 2H2O +0.16 UO22++e?UO2+ +0.163 SO42?+ 4H++ 2e?SO2 ( aq ) + 2H2O +0.17 TiO2++ 2H++e?Ti3++ H2O +0.19 SbO++ 2H++ 3e?Sb ( s ) + H2O +0.20 AgCl ( s ) +e?Ag ( s ) + Cl? +0.22233 H3AsO3 ( aq ) + 3H++ 3e?As ( s ) + 3H2O +0.24 GeO ( s ) + 2H++ 2e?Ge ( s ) + H2O +0.26 UO2++ 4H++e?U4++ 2H2O +0.273 Re3++ 3e?Re ( s ) +0.300 Bi3++ 3e?Bi ( s ) +0.308 VO2++ 2H++e?V3++ H2O +0.34 Cu2++ 2e?Cu ( s ) +0.340 3?+e? 4? +0.36 O2 ( g ) + 2H2O + 4e?4OH? ( aq ) +0.40 H2MoO4+ 6H++ 3e?Mo3++ 2H2O +0.43 CH3OH ( aq ) + 2H++ 2e?CH4 ( g ) + H2O +0.50 SO2 ( aq ) + 4H++ 4e?S ( s ) + 2H2O +0.50 Cu++e?Cu ( s ) +0.520 CO ( g ) + 2H++ 2e?C ( s ) + H2O +0.52 I2 ( s ) + 2e?2I? +0.54 I3?+ 2e?3I? +0.53 ?+ 3e?Au ( s ) + 4I? +0.56 H3AsO4 ( aq ) + 2H++ 2e?H3AsO3 ( aq ) + H2O +0.56 ?+e?Au ( s ) + 2I? +0.58 MnO4?+ 2H2O + 3e?MnO2 ( s ) + 4OH? +0.59 S2O32?+ 6H++ 4e?2S ( s ) + 3H2O +0.60 H2MoO4 ( aq ) + 2H++ 2e?MoO2 ( s ) + 2H2O +0.65 + 2H++ 2e? +0.6992 O2 ( g ) + 2H++ 2e?H2O2 ( aq ) +0.70 Tl3++ 3e?Tl ( s ) +0.72 PtCl62?+ 2e?PtCl42?+ 2Cl? +0.726 H2SeO3 ( aq ) + 4H++ 4e?Se ( s ) + 3H2O +0.74 PtCl42?+ 2e?Pt ( s ) + 4Cl? +0.758 Fe3++e?Fe2+ +0.77 Ag++e?Ag ( s ) +0.7996 Hg22++ 2e?2Hg ( cubic decimeter ) +0.80 NO3? ( aq ) + 2H++e?NO2 ( g ) + H2O +0.80 ?+ 3e?Au ( s ) + 4Br? +0.85 Hg2++ 2e?Hg ( cubic decimeter ) +0.85 MnO4?+ H++e?HMnO4? +0.90 2Hg2++ 2e?Hg22+ +0.91 Pd2++ 2e?Pd ( s ) +0.915 ?+ 3e?Au ( s ) + 4Cl? +0.93 MnO2 ( s ) + 4H++e?Mn3++ 2H2O +0.95 ?+e?Au ( s ) + 2Br? +0.96 Br2 ( cubic decimeter ) + 2e?2Br? +1.066 Br2 ( aq ) + 2e?2Br? +1.0873 IO3?+ 5H++ 4e?HIO ( aq ) + 2H2O +1.13 ?+e?Au ( s ) + 2Cl? +1.15 HSeO4?+ 3H++ 2e?H2SeO3 ( aq ) + H2O +1.15 Ag2O ( s ) + 2H++ 2e?2Ag ( s ) + H2O +1.17 ClO3?+ 2H++e?ClO2 ( g ) + H2O +1.18 Pt2++ 2e?Pt ( s ) +1.188 ClO2 ( g ) + H++e?HClO2 ( aq ) +1.19 2IO3?+ 12H++ 10e?I2 ( s ) + 6H2O +1.20 ClO4?+ 2H++ 2e?ClO3?+ Water +1.20 O2 ( g ) + 4H++ 4e?2H2O +1.23 MnO2 ( s ) + 4H++ 2e?Mn2++ 2H2O +1.23 Tl3++ 2e?Tl+ +1.25 Cl2 ( g ) + 2e?2Cl? +1.36 Cr2O72?+ 14H++ 6e?2Cr3++ 7H2O +1.33 CoO2 ( s ) + 4H++e?Co3++ 2H2O +1.42 2NH3OH++ H++ 2e?N2H5++ 2H2O +1.42 2HIO ( aq ) + 2H++ 2e?I2 ( s ) + 2H2O +1.44 Ce4++e?Ce3+ +1.44 BrO3?+ 5H++ 4e?HBrO ( aq ) + 2H2O +1.45 ?-PbO2 ( s ) + 4H++ 2e?Pb2++ 2H2O +1.460 ?-PbO2 ( s ) + 4H++ 2e?Pb2++ 2H2O +1.468 2BrO3?+ 12H++ 10e?Br2 ( cubic decimeter ) + 6H2O +1.48 2ClO3?+ 12H++ 10e?Cl2 ( g ) + 6H2O +1.49 MnO4?+ 8H++ 5e?Mn2++ 4H2O +1.51 HO2†¢+ H++e?H2O2 ( aq ) +1.51 Au3++ 3e?Au ( s ) +1.52 NiO2 ( s ) + 4H++ 2e?Ni2++ 2OH? +1.59 2HClO ( aq ) + 2H++ 2e?Cl2 ( g ) + 2H2O +1.63 Ag2O3 ( s ) + 6H++ 4e?2Ag++ 3H2O +1.67 HClO2 ( aq ) + 2H++ 2e?HClO ( aq ) + H2O +1.67 Pb4++ 2e?Pb2+ +1.69 MnO4?+ 4H++ 3e?MnO2 ( s ) + 2H2O +1.70 H2O2 ( aq ) + 2H++ 2e?2H2O +1.78 AgO ( s ) + 2H++e?Ag++ Water +1.77 Co3++e?Co2+ +1.82 Au++e?Au ( s ) +1.83 BrO4?+ 2H++ 2e?BrO3?+ Water +1.85 Ag2++e?Ag+ +1.98 S2O82?+ 2e?2SO42? +2.010 O3 ( g ) + 2H++ 2e?O2 ( g ) + H2O +2.075 HMnO4?+ 3H++ 2e?MnO2 ( s ) + 2H2O +2.09 F2 ( g ) + 2e?2F? +2.87 F2 ( g ) + 2H++ 2e?2HF ( aq ) +3.05 The Great Gatsby and Browning’s Poetry EssayThe places oflithiumandsodiumare changed on such a series: gold and Pt are besides inverted, although this has small practical significance as both metals are extremely unreactive. Standard electrode potencies offer a quantitative step of the power of a reduction agent, instead than the qualitative considerations of other responsiveness series. However, they are merely valid forstandardconditions: in peculiar, they merely apply to reactions in aqueous solution. Even with this provision, the electrode potencies of Li and Na and hence their places in the electrochemical series appear anomalous. The order of responsiveness, as shown by the energy of the reaction with H2O or the velocity at which the metal surface tarnishes in air, appears to be K gt ; Na gt ; Li gt ; alkalic Earth metals, the same as the contrary order of the ( gas-phase ) ionization energies. This is borne out by the extraction of metallic Li by the electrolysis of aeutecticmixture oflithium chlorideandpotassium chloride: Li metal is formed at the cathode, non K. Asaltis a chemical incorporating ametal ionand anegative ionbonded together. The metal ions might dwell of Cu, Na or Zn etc. The negative ions could be sulphate, chloride or oxide etc. Some metals are stronger than others. If a strong metal is assorted with a salt from a weaker metal, the strong metal grabs the negative ion from the weaker 1. Here is an illustration: Lead is stronger than Gold, so if Lead is heated with Gold chloride, it reacts to give Lead chloride and Gold Calcium is stronger than Zinc, so if Calcium is heated with Zinc chloride, it reacts to give Calcium chloride and Zinc Iron is stronger than Silver, so if Iron is heated with Silver sulfide, it reacts to give Iron sulfide and Silver Zinc is stronger than Lead, so if Zinc is heated with Lead phosphate, it reacts to give Zinc phosphate and Lead Sodium is stronger than Iron, so if Sodium is heated with Iron bromide, it reacts to give Sodium bromide and Iron Features of the electrochemical series ( Activity series ) In the electrochemical series the elements that are lower in the series get discharged ( lose their charge to go impersonal ) more easy than the 1s above them. Hydrogen is besides included as a mention point in the series. The positively charged power and the cut downing power of the elements on a regular basis decrease downwards while the negatively charged power and the oxidising power of the elements regularly addition upwards. Significance of the electrochemical series ( Activity series ) This series is an of import tool that helps in foretelling many electrochemical reactions. All metals placed above H will displace H from acids while those below it do non displace H from acids. Elementss with high electropositive or negatively charged power are extremely reactive elements. Each component in the series will displace any other component below it from a solution of its salt. For e.g. , when we add zinc turnings in Cu sulfate solution, Cu is replaced by Zn because Zn is in higher place as compared to Cu. In the replacing of one metal ion from its solution by another metal, the component that gives up negatrons most easy to go an ion will be in the solution. This is because it will accept the negatrons back with greatest trouble. Application of electrochemical series Higher the SRP, greater is the inclination to accept e- , higher is the inclination to acquire reduced and greater is the oxidising power. Fluorine system ( F2/F ) -has the highest SRP and hence it possesses highest oxidizing power and this increases down the group. Lower the SRP, lesser is the inclination to accept e- , higher is the inclination to donate negatrons, higher is the inclination to acquire oxidized and greater is the cut downing power. In the ECS, Lithium has the lowest SRP. Hence, it has the highest cut downing power and this goes on diminishing down the series. Higher the SRP, greater is the inclination to accept e-to signifier anions, higher is the electro negative nature. In the ECS, Fluorine system has the highest SRP and hence it is most electro negative and this goes on increasing down the series. Lower the SRP, lesser is the inclination to accept the negatrons, greater is the inclination to donate the e-to signifier cations and higher is the electro positive nature. In the ECS, Li system has the lowest SRP and is extremely electro positive which goes on diminishing down the series. A metal system happening above H2, displaces H2from dilute acids, from H2O steam depending on its place and gets tarnished. A metal system happening below H2does non displace H2from dilute acids, H2O or steam does non acquire tarnished. In general, a metal system with highest SRP, has highest oxidising power, more electro negative, gets displaced by all other system above it and ever Acts of the Apostless as positive electrode. A metal system with lowest SRP has highest cut downing power, more electro positive, displaces all other systems below it and ever Acts of the Apostless as negative electrode.