Class 12 D and F Block Notes PDF

D and F Block Elements NextGen Catalyst By Junaid (Junnu Bhaiya)  D and F Block Elements Group No. 3 4 5 6 7 8 9 10 11 12 3d Sc T...

D and F Block Elements NextGen Catalyst By Junaid (Junnu Bhaiya)  D and F Block Elements Group No. 3 4 5 6 7 8 9 10 11 12 3d Sc Ti V Cr Mn Fe Co Ni Cu Zn 3d14s2 3d24s2 3d34s2 3d54s1 3d54s2 3d64s2 3d74s2 3d84s2 3d104s1 3d104s2 (सुनो) (तुम) (वििाह) (कर लो) (मुझसे) (विर) (कोई) (नह )ीं (कहे गा) (जानू) 4d Y Zr Nb Mo Tc Ru Rh Pd Ag Cd 1 2 2 2 4 1 5 1 6 1 7 1 8 1 10 0 10 1 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d 5s 4d105s2 (Why) (ज़र) (नब) (मूींह) (तक) (ररयू) (रे ह) (पढ़) (एज ) (स ड ) 5d La Hf Ta W Re Os Ir Pt Au Hg 1 2 2 2 3 2 4 2 5 2 6 2 7 2 9 1 10 1 5d 6s 5d 6s 5d 6s 5d 6s 5d 6s 5d 6s 5d 6s 5d 6s 5d 6s 5d106s2 (ला) (हि्) (ता) (डब्ल्यू) (रे ) (उस) (Iron rod से) (वपटाई) (और) (होग ) 6d Ac Rf Db Sg Bh Hs Mt Ds Rg Cn 6d17s2 6d27s2 6d37s2 6d47s2 6d57s2 6d67s2 6d77s2 6d87s2 6d107s1 6d107s2 Important Points 1. D-Block Elements: Comprise Group 3 to 12 of the periodic table. 2. General Electronic Configuration: (n−1)d1−10 ns1−2 For 3d series: 3d1-10 4s1-2 For 4d series: 4d1-10 5s0-2 For 5d series: 5d1-10 6s1-2 For 6d series: 6d1-10 7s1-2 3. Exceptional Electronic Configurations: Some elements exhibit deviations to achieve half-filled or fully-filled stability: Chromium (Cr): [Ar] 4s13d5 (Half-filled 3d subshell) Copper (Cu): [Ar] 4s13d10 (Fully-filled 3d subshell) Similar exceptions: Nb, Mo, Tc, Ru, Rh, Pd, Ag, Pt, Au, Rg. 4. Transition Elements vs. Pseudo-Transition Elements: D-block elements are termed transition elements, except Zn, Cd, Hg, which are called pseudo- transition elements as their d-orbitals are fully filled in the ground state. 6. Transition Elements: For an element to be a transition element, it should have incompletely filled d-orbital either in its ground state or in its most common oxidation state. 7. Pseudo-Transition Elements: Zinc (Zn), Cadmium (Cd), and Mercury (Hg) are termed pseudo-transition elements because their d- orbitals are completely filled [(n-1)d10ns2] in both the ground state and their common oxidation states. Q. Silver atom has completely filled d-orbitals (4d10) in its ground state. How can it be considered a transition element? Ans. In its ground state, silver (Ag) has a completely filled 4d10 orbital with the electronic configuration 4d105s1. However, silver exhibits two oxidation states: +1 and +2: In the +1 oxidation state, an electron is removed from the 5s-orbital, leaving the 4d-orbital fully filled. In the +2 oxidation state, an additional electron is removed from the 4d-orbital, resulting in an incomplete 4d9 configuration. Since the d-orbital becomes incomplete in the +2 oxidation state. That is why it is considered as a transition element. Physical Properties 1. Nearly all transition elements exhibit metallic properties such as high tensile, ductility, malleability, high thermal and electrical conductivity and metallic lustre. Except Zn, Cd, Hg and Mn, other metals have one or more typical metallic structure at normal temperature. With the exception of Zn, Cd, and Hg. The transition metals are very hard, have low volatility, and possess high melting and boiling points due to strong metallic bonding. 2. General Trend: The greater the number of valence electrons in a transition element, the stronger resultant metallic bonding. General Properties of Transition elements Or Trends 1. Atomic and Ionic Sizes The trend in atomic and ionic sizes across the 3d series: Sc > Ti > V > Cr > Mn > Fe ≈ Co ≈ Ni < Cu < Zn The atomic size decreases from Sc to Cr due to increasing effective nuclear charge. Fe, Co, and Ni have nearly the same size due to electron pairing in d-orbitals, causing repulsion. Cu and Zn have slightly larger radii due to weaker nuclear attraction on outer electrons. 2. Ionisation Enthalpies Trends in the ionisation enthalpies (IE1, IE2, IE3): First Ionisation Enthalpy (IE1): Sc < V < Cr < Ti < Mn < Ni < Cu < Co < Fe < Zn  Second Ionisation Enthalpy (IE2): Sc < Ti < V < Mn < Fe < Cr < Co < Zn < Ni 3d > 4d 3. Density The trend in densities of the 3d series: Sc < Ti < V < Zn < Cr < Mn < Fe < Co < Ni < Cu Density increases across the series as atomic mass increases while atomic size decreases, leading to higher packing efficiency. Zn has lower density due to its larger atomic size and fully filled d-orbitals. 4. Melting Points The melting points trend in the 3d series: Sc < Ti < V < Cr > Fe > Co > Ni > Mn > Cu > Zn Simplified trend: Zn < Cu < Mn < Ni < Co < Fe < Sc < Ti < V < Cr Reason: o Melting points depend on metallic bonding strength, which is influenced by the number of unpaired d-electrons. o Cr has the highest melting point due to its half-filled 3d5 configuration, maximizing metallic bonding. o Zn has the lowest melting point due to its fully filled 3d10 configuration, leading to weaker bonding. 5. Heat of atomisation: The heat of atomisation is the amount of energy required to convert one mole of a substance in its standard state (solid, liquid, or gas) into its individual gaseous atoms under standard conditions. Trends in Heat of Atomisation Across the 3d Series: Zn < Mn < Sc < Cu < Cr < Fe < Co < Ni < Ti < V Zinc (Zn) has the lowest Heat of atomisation: The enthalpy of atomisation is influenced by the stability of the crystal lattice and the strength of metallic bonds. Zinc (3d104s2) has a fully filled 3d-orbital, and no d-electrons participate in the formation of metallic bonds. In contrast, other elements in the 3d series involve one or more unpaired d-electrons in metallic bonding, resulting in stronger metallic bonds. Since zinc's metallic bonds are weaker due to the lack of d-orbital involvement, it has the lowest enthalpy of atomisation among the 3d-series elements. 6. Oxidation states: Transition elements exhibit variable oxidation states because of their unique electronic configurations and the ability to involve both their ns and (n−1)d orbitals in bonding. ▪ Important Points: o Mn (Z=25), 3d54s2 Mn has the maximum number of unpaired electrons present in the d-subshell (5 electrons). Hence, Mn exhibits the largest number of oxidation states, ranging from +2 to +7. o Scandium (Z=21) does not exhibit variable oxidation states. Sc shows only +3 oxidation states. o In Group 6, Mo (VI) and W (VI) are more stable compared to Cr (VI). As a result, Cr (VI), in the form of dichromate in acidic medium, acts as a strong oxidizing agent, while MoO3 and WO3 are not as strong oxidizing agents. (Cr (VI) ki stability kam hoti hai, isliye woh asani se electron le leta hai aur ek strong oxidising agent ban jaata hai. Lekin Mo aur W zyada stable hain, is wajah se unmein yeh tendency kam hoti hai.) o Lower oxidation states are observed in complex compounds with ligands showing π-acceptor behaviour along with σ-bonding. For example, in Ni(CO)4 and Fe(CO)5, the oxidation states of Nickel and Iron are zero. (Jab kisi complex compound mein ligands σ-bonding ke saath π-acceptor ki tarah bhi behave karte hain, toh unmein lower oxidation states hoti hain. For example: Ni(CO)4 mein nickel ka oxidation state zero hota hai. Fe(CO)5 mein iron ka oxidation state bhi zero hota hai. Yeh is wajah se hota hai kyunki CO ligands π-acceptor ki tarah act karte hain aur electrons share karke metal ki oxidation state ko kam karte hain.) 7. Magnetic Property: Property Diamagnetism Para-magnetism Electrons No unpaired electrons One or more unpaired electrons Magnetic Behaviour Repelled by a magnet Attracted by a magnet Spin only moment or Spin only magnetic moment (µ): µ = √𝒏(𝒏 + 𝟐) BM Where, μ: Magnetic moment in Bohr Magnetons (BM) n: Number of unpaired electrons Q. Calculate the spin-only magnetic moment of a divalent ion in aq. solution if its atomic number is 25. Ans: Electronic configuration of Mn2+: [Ar]4s03d5 Number of unpaired electrons = 5 µ = √𝑛(𝑛 + 2) BM µ = √5(5 + 2) BM µ = √𝟑𝟓 BM 8. Formation of Coloured ions: When an electron from a lower energy d orbital is excited to higher energy d orbital, the energy of excitation corresponds to the frequency of light absorbed. This frequency absorbed generally lies in the visible region. The colour observed corresponds to the complementary colour of light absorbed. The frequency of light that is absorbed is determined by Nature of ligand Size of metal ion Oxidation state of metal  In addition to d-d transitions, the colour of compounds may also arise from: Charge Transfer Spectra: o Compounds with d0 or d10 configurations, where no d-d transitions are expected, can still be intensely coloured due to charge transfer transitions. o Example: In MnO4−, the pink colour arises from charge transfer from ligand to metal. o In Fe4[Fe(CN)6]3, the blue colour results from charge transfer between metal atoms (metal- to metal charge transfer). Polarization: o The colour of compounds like AgBr and AgI is due to polarization effects rather than electronic transitions. Thus, both charge transfer and polarization phenomena play significant roles in the coloration of compounds lacking d-d transitions. 9. Formation of Complex compounds: Due to smaller size of metal ions high ionic charges and the availability of d orbitals for bond formation transition elements form a number of complex compounds. Examples of some complex compounds/ions are [Fe(CN)6]3−, [Fe(CN)6]4-, [Cu(NH3)4]2+, [Pt(Cl)4]2-, [Cu(Cl4]2- 10. Catalytic Properties: Transition metals and their compounds are well-known for their catalytic activity. This is primarily due to their ability to: To adopt multiple oxidation states To form complexes Transition metal ions are effective catalysts due to their ability to change oxidation states. For example, Fe(III) catalyzes the reaction between iodide (I−) and persulfate (S2O82−) as follows: Reaction: 2I− + S2O82− → I2 + 2SO42− ▪ Mechanism: 1. Step 1: 2Fe3+ + 2I− → 2Fe2+ + I2 Here, Fe3+ oxidizes I− to I2 2. Step 2: 2Fe2+ + S2O82− → 2Fe3+ + 2SO42− S2O82− oxidizes Fe2+ back to Fe3+, regenerating the catalyst. Transition Metal / Compound Catalyst Process V2O5 Contact Process (for SO2 → SO3) Ni (Nickel) Hydrogenation Fe (Iron) Haber Process (N2+H2 → NH3) MnO2 Decomposition of KClO3 → KCl+O2 PdCl2 Wacker Process (Oxidation of ethylene to acetaldehyde) Pt / PtO2 Adam’s Catalyst TiCl4+(C2H5)3Al Ziegler-Natta Catalyst (Production of Polythene) 11. Formation of Interstitial compounds: Interstitial Compounds are formed when small atoms like hydrogen (H), carbon (C), or nitrogen (N) are trapped within the crystal lattice of metals. These compounds are generally non-stoichiometric and do not strictly follow ionic or covalent bonding. Example: TiC, Mn4N, Fe3H, VH0.56 and TiH1.7 etc. The principal physical and chemical characteristics of these compounds are: High Melting Point: Interstitial compounds have a higher melting point than pure metals. Hardness: These compounds are very hard. Retention of Metallic Properties: Despite the presence of small atoms, interstitial compounds often retain metallic characteristics. Chemical Inertness: Interstitial compounds are usually chemically inert and do not react easily. 12. Alloy Formation: Brass: (Cu-Zn) Bronze: (Cu-Sn) German Silver: 25-30% Copper (Cu), 40-50% Nickel (Ni), 25-30% Zinc (Zn) Bell Metal: 80% Copper (Cu), 20% Tin (Sn) Gun Metal: 80% Copper (Cu), 10% Tin (Sn), 2% Zinc (Zn) Brass: 60% Copper (Cu), 40% Zinc (Zn) These alloys are used in various applications based on their unique properties like strength, durability, and corrosion resistance. 13. Trends in the M2+/M standard electrode Potential / Trends in the M2+/M standard electrode potential / Trends in stability of higher oxidation states / Chemical reactivity and E0 values All Cu2+ halides are stable except iodide Cu2+ + I- → Cu2I2 + I2 Many Cu+ compound are unstable in aqueous solution Cu+ → Cu2+ + Cu Stability Cu2+ > Cu+ due to more negative ΔH which greater than second Ionisation energy of Cu. Highest fluoride of Mn is MnF4 while oxides is Mn2O7. Oxidising Power: VO2+ < Cr2O72- < MnO4- Mn3+ & Co3+ are strong oxidising agent while Ti2+, V2+, Cr2+ are strong Reducing agent. Higher oxidation number oxides are acidic in nature. Mn+7 halide does not exist, MnO3F exist. CrO basic, Cr2O3 is amphoteric. Cr+6 is less stable than Mo+6 and W+6 Cr+6 is strong oxidising agent while MoO3 and WO3 are not. In stability of VF2 is due to lower oxidation number VX2 (X= Cl, Br, I) Beyond Mn, no metal has trihalide except FeX3 & CoF3 (X= F, Cl, Br) Halides of V5+ exist as VF5 Halides of Cr+6 exist as CrF6 Other halides of V 𝐻𝑦𝑑𝑟𝑜𝑙𝑦𝑠𝑖𝑠 V → VOX3 V2O3 is basic, V2O4 less basic and V2O5 is amphoteric H+ V2O4 → VO2+ salt H+ V2O5 → VO2+ salt OH− V2O5 → VO34- salt  Some Important Compounds of Transition elements Oxide and Oxo anions of Metals 1. Formation of Oxides: o Transition metals react with oxygen at high temperatures to form oxides. o Except for scandium (Sc), most metal oxides are ionic in nature. 2. Ionic and Covalent Nature: o The ionic character of oxides decreases as the oxidation number of the metal increases. o Example: Mn2O7 (a green oily covalent compound), CrO3, and V2O5 have low melting points and exhibit predominantly acidic character. 3. Acidic Character of Higher Oxides: o Mn2O7 forms HMnO4 (permanganic acid). o CrO3 forms H2CrO4 and H2Cr2O7 (chromic and dichromic acids). 4. Amphoteric Nature: o V2O5 is mainly acidic but amphoteric, forming VO43− (from alkalis) and VO2+ (from acids). o Cr2O3 is amphoteric, while CrO is purely basic. These oxides exhibit a variety of chemical behaviours based on their oxidation states and metal centres, ranging from basic and amphoteric to highly acidic. Potassium Permanganate KMnO4 ▪ Methods of Preparation: Commercial Methods: Potassium permanganate is prepared by fusing manganese dioxide (MnO2, pyrolusite) with an alkali metal hydroxide (like KOH) and an oxidizing agent (such as KNO3). Reaction: 2MnO2 + 4KOH + O2 → K2MnO4 + 2H2O This produces a dark green compound, Potassium manganate (K2MnO4). In Acidic Medium: Disproportionation: K2MnO4 undergoes disproportionation in neutral or acidic solutions to form potassium permanganate (KMnO4): 3MnO42- + 4H+ 2MnO4- + MnO2 + H2O This process results in the formation of the purple-coloured KMnO4, a strong oxidizing agent. In Basic Medium: Electrolytic Oxidation: The green potassium manganate (K2MnO4) is subjected to electrolytic oxidation to convert it into Potassium permanganate (KMnO4): 𝐸𝑙𝑒𝑐𝑡𝑟𝑜𝑙𝑦𝑡𝑖𝑐 𝑜𝑥𝑖𝑑𝑎𝑡𝑖𝑜𝑛 MnO42- → MnO4- 𝑖𝑛 𝑎𝑙𝑘𝑎𝑙𝑖𝑛𝑒 𝑚𝑒𝑑𝑖𝑢𝑚 This two-step process results in the formation of deep purple KMnO4 a strong oxidizing agent widely used in various chemical reactions. Laboratory Method: In the laboratory, Mn2+ salts can be oxidized to permanganate (MnO4−) using peroxodisulphate (S2O82−) as the oxidizing agent in an acidic medium. Reaction: 2Mn2+ + 5S2O82− + 8H2O → 2MnO4− + 10SO42− + 16H+ Mechanism: Oxidation: The S2O82− ions oxidize Mn2+ to MnO4− ▪ Characteristics Properties of KMnO₄: Heating Effect: KMnO₄ decomposes at 513 K. 2KMnO₄ → K2MnO₄ + MnO2 + O2 Appearance: KMnO₄ forms dark purple (almost black) crystals, which are isostructural with KClO₄. The salt has low solubility in water. Colour and Magnetism: It exhibits an intense colour and weak, temperature-dependent paramagnetism. Magnetic Properties: The green manganate ion (MnO₄²⁻) is paramagnetic, while the permanganate ion (MnO₄⁻) is diamagnetic. Bonding: π-bonding occurs through the overlap of the p-orbital of oxygen with the d-orbital of manganese. MnO₄²⁻ MnO₄⁻ Geometry: Tetrahedral Tetrahedral Ion Colour: Green ion Purple ion Colour due to: d-d transition LMCT Spectra Hybridization: sp3 d3s Magnetism: Paramagnetic Diamagnetic ▪ KMnO4 is a good oxidizing agent in acidic, basic or neutral medium. 𝐵𝑎𝑠𝑖𝑐 MnO₄⁻ → MnO₄²⁻ N-factor= 1 𝑁𝑒𝑢𝑡𝑟𝑎𝑙 𝑜𝑟 𝐴𝑙𝑘𝑎𝑙𝑖𝑛𝑒 MnO₄⁻ → MnO2 N-factor= 3 𝐴𝑐𝑖𝑑𝑖𝑐 + MnO₄⁻ → Mn² N-factor= 5 Important Oxidising reaction of KMnO4 In Acidic Medium: In Neutral or faintly alkaline solution: Potassium Dichromate K2Cr2O7 ▪ Methods of Preparation: It is an important chemical used in leather industry and an oxidant for preparation of many azo compounds. It is prepared from Chromite ore (FeCr2O4) Firstly, Chromite ore (FeCr2O4) is fused with Na2CO3 or K2CO3 in excess air: 4FeCr2O4 + 8Na2CO3 + 7O2 → 8Na2CrO4 + Fe2O3 + 8CO2 (Yellow) Yellow solution of Na2CrO4 is filtered and acidified with sulphuric acid to give a solution from which Orange Sodium dichromate Na2Cr2O7.2H2O is crystallised. Na2Cr2O7.2H2O is more soluble than K2Cr2O7. Sodium dichromate is treated with Potassium chloride Na2Cr2O7 + 2KCl → K2Cr2O7 + 2NaCl ▪ Chemical Properties: Heating effect: ∆ K2Cr2O7 → K2CrO4 + Cr2O3 + O2 (Orange) (Yellow) (Green) (Colourless) PH: OH− On increasing PH: Cr2O72- → CrO42- (Basic) H+ On increasing PH: CrO42- → Cr2O72- (Acidic) Structures: K2CrO4 K2Cr2O7 All Cr-O bond have same length 6(Cr-O) bond have same length 2(Cr-O) bond have same length Tetrahedral Tetrahedral Sp3 Sp3 Colour: Yellow Colour: Orange Due to LMCT Due to LMCT Sodium and Potassium dichromate are good oxidising agent. But Potassium dichromate is used as primary standard in volumetric analysis. Chemical Reactions:  Chromyl Chloride Test: HELP US TO BRING MORE QUALITY CONTENT FOR YOU GUYS SCAN QR CODE TO DONATE You can Donate from any UPI App Even a small bit of help will be appreciable  The Lanthanoids La Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu लेकर स ने पर नविया प्रेम क समाई यूूँ ह गिगि तब विल हुआ और तुम लाजिाब लगते हो 57 58 59 60 61 62 63 64 65 66 67 68 69 70 71 4f 0 1 3 4 5 6 7 7 9 10 11 12 13 14 14 5d 1 1 0 0 0 0 0 1 0 0 0 0 0 0 1 6s 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 1. The Lanthanoids Elements (Ln) : Comprise Period 6, Atomic Number 57-71 of the periodic table. 2. General Electronic Configuration: (n−2)f1−14 (n−1)d0−1 ns2 3. Oxidation State: Most common oxidation state is +3 Some exist in +2 and +4 and have more tendency to gain oxidation state is +3. Eu2+ & Yb2+ tries to get +3 so it acts as reducing agent. Ce4+ tries to get +3 so it acts as oxidizing agent. Pr+4, Nd+4, Tb+4, Dy+4 in MO2. Samarium (Sm) is very like Europium (Eu) both +2 and +3. Ce4+/Ce3+ → +1.74 V Ce4+ is good analytic reagent. 4. Ionic Radius (Ln+3) Left to right Ionic radii decreases due to increase Effective nuclear charge (Zeff) due to poor shielding effect. La3+ > Ce3+ > Pm3+ > Sm3+ …………………………….. 5. Basic Strength of Hydroxides: Left to right, Basic strength decreases Ce(OH)3 > Gd(OH)3 6. Chemical Reactions: 7. General Properties: All Ln are silvery white soft metal & tarnish rapidly in air. Sm is steel hard due to strong metallic bonding and good conductor of Heat and electricity. Except La3+ and Lu3+ all are coloured. Except f0 type (La3+ & Ce4+) and f14 (Yb2+ & Lu3+) all are paramagnetic. They easily form alloys with other metals mainly Iron Mischmetal: (La ≈ 95%, Iron ≈ 5% & traces Ca, S, C, Al) Mischmetal is used in Mg-based alloys to produce bullets shell and lighter flint. Hardness is directly proportional to atomic numbers.  The Actinoids Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr थोडा पापड यूूँ नापो पुराने आम कम वबकेंगे कैफे में ऐसे िरमाओ मैडम नूडल्स लाओ 89 90 91 92 93 94 95 96 97 98 99 100 101 102 103 5f 0 0 2 3 4 6 7 7 9 10 11 12 13 14 14 6d 1 2 1 1 1 0 0 1 0 0 0 0 0 0 1 7s 2 2 2 2 2 2 2 2 2 2 2 2 2 2 2 1. The Actinoids Elements (Ac) : Comprise Period 7, Atomic Number (89 – 103)`of the periodic table. 2. General Electronic Configuration: (n−2)f1−14 (n−1)d0−1 ns2 3. Oxidation State: Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 3 --- 3 3 3 3 3 3 3 3 3 3 3 3 3 4 4 4 4 4 4 4 4 5 5 5 5 5 6 6 6 6 7 7 Short Trick for Oxidation States in Actinides: Ac to Lr: Common oxidation state is +3, except for Th. Th to Bk: Common oxidation state is +4. Pa to Am: Common oxidation state is +5. U to Am: Common oxidation state is +6. Np to Pu: Common oxidation state is +7. 4. Ionic Sizes: Left to right size decreases due to increase Effective nuclear charge (Zeff) due to poor screening of 5f electrons or Actinoid contraction. 5. General Characteristics or Properties: All are Paramagnetic. All are silvery white in appearance but display a variety of structure. This is due to irregularity in metallic radii. They get tarnished on exposure to alkali All are radioactive (Atomic no. 92 onwards all elements are called transuranic elements). All are reacted with Non-metal at moderate temperature All are reacted with HCl but effect with HNO3 is small due to the formation of Oxide layer. Magnetic properties of the actinoids are more complex than those of lanthanoid. Actinoids compound or their ions are coloured most probably due to charge transfer of f-f transition. They react with boiling water to form mixture of oxides and hydrides. 6. Some Applications of D & F Block Elements TiO for the Pigment industry, MnO2 for use in dry cell along with use of Zn. Group 11 are still worthy called Coinage metals. Special light-sensitive properties of AgBr. AgBr is an important chemical used in Photography. Along with AgBr, Ag and AgI can also be used. Many of the elements or compounds of this block elements are important catalyst. The silver UK coins are a Cu/Ni alloy. Some compounds like MnO4-, CrO42- are good oxidising agents. Iron and steels are the most important construction material. Their production is based on reduction of iron oxides, the removal of impurities and the addition of carbon and alloying metals like Cr, Mn, Ni. 6. Differences: Lanthanides Actinides 1. In addition to +3 oxidation state, they exhibit +2 In addition to +3 oxidation state, they show +4, +5, and +4 oxidation states only. +6 and +7 oxidation state. 2. Most of their ions are colourless. Most of their ions are coloured. 3. They do no form complexes easily. They have much greater tendency to form complexes. 4. They do no form oxocations. They form oxocations such as UO22+, PuO22+ and UO+. 5. Their compounds are less basic Their compounds are most basic. 6. Except Promethium (Pm), they are They are radioactive. non-radioactive. 7. Their magnetic properties can be easily Their magnetic properties cannot be easily explained. explained. HELP US TO BRING MORE QUALITY CONTENT FOR YOU GUYS SCAN QR CODE TO DONATE You can Donate from any UPI App Even a small bit of help will be appreciable