4. Metal lons with Variable Oxidation Numbers Some metals have variable oxidation numbers like: Oxidation Metal states Classical System Stock System ion Cu +1 Cuprous Сopper I +2 Cupric Сopper l Fe +2 Ferrous Iron II +3 Ferric Iron III Pb +2 Plumbous Lead II +4 Plumbic Lead IV Au +1 Aurous Gold I +3 Auric Gold III Hg +1 Mercurous Mercury I +2 Mercuric Mercury II Со +2 Cobaltous Cobalt II +3 cobaltic Cobalt III Fill up the table below: Formula Classical name Stock Nomenclature Ex: Cuo Cupric oxide Copper Il oxide 1. CuSO4 2. Pbo 3. РЫ(СОз)2 4. 5. FeSO4 8

4. Metal lons with Variable Oxidation Numbers Some metals have variable oxidation numbers like: Oxidation Metal states Classical System Stock System ion Cu +1 Cuprous Сopper I +2 Cupric Сopper l Fe +2 Ferrous Iron II +3 Ferric Iron III Pb +2 Plumbous Lead II +4 Plumbic Lead IV Au +1 Aurous Gold I +3 Auric Gold III Hg +1 Mercurous Mercury I +2 Mercuric Mercury II Со +2 Cobaltous Cobalt II +3 cobaltic Cobalt III Fill up the table below: Formula Classical name Stock Nomenclature Ex: Cuo Cupric oxide Copper Il oxide 1. CuSO4 2. Pbo 3. РЫ(СОз)2 4. 5. FeSO4 8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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4. Balance the reactions in the following. H₂ + N₂ → NH3 CaCl2 + AgNO3 → Ca (NO3)2 + AgCl SnO₂ + H₂ →→→ H₂O + Sn Na2CO3 + HCl → NaCl + H₂O + CO2 Fe2(SO4)3 + KOH → K2SO4 + Fe (OH)3 C₂H6O2 + O2 CO2 + H2O Fe(OH)2 → Fe3O4+H₂ + H₂O Balanced equation lu comes from carbohydrates, which are broken down into
regarding redox, in the following reaction, copper loses 2 electrons and zinc gains 2. Cu(s) + ZnSO4(aq)-------->CuSO4(aq)+ Zn(s) true or false?
80°F Sunny The oxidation number of an element can vary. O True Search F8 6725 F9 O False - « Οι F10
What is the net ionic equation for the following reaction: 2AgNO3 + Cu(s)→→ Cu(NO3)2 + 2Ag (s) Oa) 2NO3 + Cu(s) → 2NO3 + 2Ag (s) Ob) 2Ag* (aq) + Cu(s) → 2 Ag(s) + Cu²+ (aq) c) same as the balanced equation d) None of the above
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Identify the oxidation number of each element in each given compound.
By the half-reaction method the balanced equation of the following redox reaction is Fe+3 Fe(s) + Mg (aq) +2 (aq)+ Mg(s) O a. Fe*3(aq)+ 3 e -Fe(s) O b. Fe*3(aq)+ Mg(s) - Fe(s) + Mg*2 (aq) Oc 3 Fe*3(aq)+ 2Mg(s) - 3Fe(s) + 2Mg*2 (aq) O d. 2Fe*3 (ag) + 3Mg - 2FEG) + 3Mg*2 (aq) page ourse Syllabus Jump to
how do you find the oxidation numbers for the underlined element in each of the following molecules or ions?
1. What is the concentration of a 1.0 M solution of K+(aq) ions in equivalents/liter? 2. A solution having initial concentration of 0.445 M and initial volume of 45.0 mL is diluted to 100.0 mL. What is its final concentration?
2. Specify which of the following are oxidation-reduction reactions and identify the substance being oxidized and the substance being reduced, when appropriate. a. Cu (s) + 2 Ag (aq) + 2 Ag (s) + Cu²+ (aq) b. HCl (g) + NH, (g) → NH,Cl (s) c. SiCl, (l) + 2 H₂O (1)→ 4 HCl (aq) + SiO₂ (s) d. SiCl, (l) +2 Mg (s) 2 MgCl, (s) + Si (s) e. Al(OH), (aq) → AlO, (aq) + 2 H₂O (1) f. CH, (g) +H,O (g) + CO (g) + 3H, (g) g. Zn (s) + 2 HCl (aq) → ZnCl, (aq) + H₂(g) h. 2H* (aq) + 2 CrO, (aq) + Cr₂O," + H₂O (1)
Consider the reaction below: 2 MnO4– + 5 C2O42– + 16 H+ ➜ 2 Mn2+ + 8 H2O + 10 CO2 A 30.0 mL sample of an oxalate solution is found to react completely with 14.5 mL of a 0.1725 M solution of MnO4–. What is the oxalate ion concentration in the sample? Select one: a.0.141 M b.0.033 M c.0.208 M d.0.083 M
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