Chemistry for Engineers Mastery Activity #18 PDF

 Republic of the Philippines **Sorsogon State University** **COLLEGE OF ENGINEERING AND ARCHITECTURE** **Sorsogon City Campus** *Magsaysay Street, Salog (Pob.), Sorsogon City, Sorsogon* Tel. No.; 056 211-0103 loc 136; Email Address: coea\@sorsu.edu.ph **Chemistry for Engin...

 Republic of the Philippines **Sorsogon State University** **COLLEGE OF ENGINEERING AND ARCHITECTURE** **Sorsogon City Campus** *Magsaysay Street, Salog (Pob.), Sorsogon City, Sorsogon* Tel. No.; 056 211-0103 loc 136; Email Address: coea\@sorsu.edu.ph **Chemistry for Engineers (CHE)** Mastery Activity \#18 Name: \_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_\_ Course and Year: \_\_\_\_\_\_\_\_\_\_\_ Score: \_\_\_\_\_\_\_ Term: [1^st^ Semester, 2024-2025] Instructor: [Engr. Noel G. Benavides, PhD] [Oxidation Number Rules:] 1. The oxidation number of any pure element is 0. 2. The oxidation number of a monatomic ion equals that charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in a compound is always -1. 5. Oxygen has an oxidation number of -2 unless it is combined with F, in which it is +1 or +2, or it is in peroxide (such as H~2~O~2~ or Na~2~O~2~), in which it is -1. 6. Hydrogen is +1, unless combined with a metal, and then it is -1. 7. In compounds, Group 1 is +1, Group 2 is +2, and Aluminum is +3. 8. The sum of the oxidation numbers of all atoms in a neutral compound is 0. 9. The sum of the oxidation numbers in a polyatomic ion equals the charge of the ion. **Part A:** In the following questions, give the oxidation number of the indicated atoms/ion: +-----------------------------------+-----------------------------------+ | 1\. N in N~2~O~3~ | 16\. C in CH~4~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 2\. S in H~2~SO~4~ | 17\. Mn in MnO~2~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 3\. C | 18\. S in SO~3~^2-^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 4\. C in CO | 19\. Mg^2+^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 5\. Na in NaCl | 20\. Cl^-^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 6\. H in H~2~O | 21\. O~2~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 7\. Ba in BaCl~2~ | 22\. P~4~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 8\. N in NO~2~^-^ | 23\. Na in Na~2~S | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 9\. S in Al~2~S~3~ | 24\. S in H~2~S | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 10\. S in HSO~4~^-^ | 25\. Ca^2+^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 11\. Cl in Fe(ClO~2~)~3~ | 26\. C in CN^-^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 12\. Fe in Fe(ClO~2~)~3~ | 27\. H in OH^-^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 13\. N in NO~3~^-^ | 28\. Mn in KMnO~4~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 14\. Cu^2+^ | 29\. I in Mg(IO~3~)~2~ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | | | | | 15\. Zn^2+^ | 30\. C in C~2~O~4~^2-^ | | **­­­­\_\_\_\_\_\_\_\_\_\_** | **­­­­\_\_\_\_\_\_\_\_\_\_** | +-----------------------------------+-----------------------------------+ **Part B:** Identify the species being oxidized and reduced in each of the following reactions and write their half reactions: 1. 2 Cr^+^ + Sn^4+^ → 2 Cr^3+^ + Sn^2+^ 2. 3 Hg^2+^ + 2 Fe (s) → 3 Hg~2~ + 2 Fe^3+^ Half-reactions: 3. 2 As (s) + 3 Cl~2~ (g) → 2 AsCl~3.~ Half-reactions: 4. Zn + Cu^2+^ Zn^2+^ + Cu 5. C + H~2~SO~4~ → CO~2~ + SO~2~ + H~2~O Half-reactions: 6. HNO~3~ + HI → NO + I~2~ + H~2~O Half-reactions: 7. KMnO~4~ + HCl → MnCl~2~ + Cl~2~ + H~2~O + KCl 8. Sb + HNO~3~ → Sb~2~O~3~ + NO + H~2~O Half-reactions: