Inorganic Chemistry II

Paper Code: 
CHY 211
Credits: 
3
Contact Hours: 
45.00
Max. Marks: 
100.00
Objective: 

Course Objectives:

This course will enable the students to –

  1. acquaint the students with physical and chemical properties of s and p block elements.
  2.  make students learn the concepts of various diagrammatic presentations i.e. Latimer, Frost, Pourbaix and Ellingham diagrams of potential data along with metallurgy and volumetric analysis.

Course Outcomes (COs):

Course

Learning outcomes

(at course level)

Learning and teaching strategies

Assessment

Strategies

Paper Code

Paper Title

 

CHY-211

 

 

 

 

 

 

 

Inorganic Chemistry II

 

 

 

 

 

 

The students will be able to:

 

CO29: describe the general characteristics of the alkali and alkaline earth metals and also explain the flame colour and spectra of these metals and their compounds

CO 30: utilize half-reactions to calculate cell potentials and determine spontaneity of reactions and nernst equation to determine effects of concentrations on cell potentials

CO 31: distinguish between equivalence and end point and carry out redox titration, complexometric titrations. acid base titrations, experiments and associated calculations

CO 32: identify some common acid-base and metal ion indicators and be able to specify which ones to use for various titrations

CO 33: draw structures of various xenon compounds and relate behavior of halogens and noble gases

Class lectures

 

Tutorials

 

Group discussions

 

Peer teaching and learning

 

Question preparation

Subjective type

  • Long answer
  • Short answer

Objective type

  • Multiple choice questions
  • One answer/two answer type questions
  • Assertion and reasoning

Class test

 

Semester end examinations 

 

Quiz

 

Solving problems in tutorials

 

Assignmentnts

 

Presentations 

 

8.00
Unit I: 
Chemistry of s-block Elements

Introduction, electronic configuration, diagonal relationships, comparative study of properties of alkali and alkaline earth metals : size of atoms and ions, density, ionization energy, electronegativity, MP & BP, flame colour and spectra, solutions in liquid ammonia, salient features of hydrides and their classification (ionic, covalent and interstitial), solvation and complexation tendencies, Crown ethers and cryptands, biological importance, , anamolousbehaviour of Li and Be, basic Beryllium acetate and nitrate.

13.00
Unit II: 
Chemistry of p-block Elements
Periodicity in properties of p-block elements with special reference to electronic configuration, atomic and ionic radii, ionization energies, electron-affinity, electronegativity, allotropy, inert pair effect, catenation including diagonal relationship. 
Structure and bonding, preparation, properties and uses: Boric acid and borates, boron nitrides, boronhydrides (diborane)and borazinecarboranes,carbidesand its classification, fluorocarbons and graphitic compounds, silicatesand silanes, structural aspects of oxides and oxy acids of phosphorus,nitrogen and sulphur, fullerenes.
 
8.00
Unit III: 
Halogens and Noble Gases
General properties of halogens like atomic radius, density, electronegativity, ionization energy, nonmetallic character, color, electron affinity, oxidation states, oxidizing power and reactivity. Unique position of Fluorine, basic nature of halogen, preparation and properties of interhalogen compounds, polyhalides, pseudohalogens. 
Noble gases- introduction,isolation, chemical properties of noble gases, chemistry of xenon, structure and bonding in xenon compounds.
 
7.00
Unit IV: 
Oxidation and Reduction

Reduction potentials – redox half reactions, concept of over potential; diagrammatic presentation of potential data (Latimer, Frost and Pourbaix diagrams); redox stability in water, disproportionation, oxidation by atmospheric oxygen; elements extracted by reduction – Ellingham diagrams.

9.00
Unit V: 
Basic Principles of Volumetric Analysis
Simple theoretical background of following types of titrations:
Acid base titrations:Basicprinciples and its applications
Iodometric &iodimetric titrations: Basic principle, application in standardization ofiodineby CuSO4-hypo and H3AsO3.
Redox titrations : Standard potential, SHE, electrochemical series, emf calculations, internal & external indicators, applications in K2Cr2O7   oxidation reaction.
Complexometric titrations: Types of EDTA titrations, masking and de-masking agents, metal ion indicator, application in estimation of total hardness.
Precipitation titrations: Basic principle, application in Volhard’s method.
 
References: 
  • Concise Inorganic Chemistry; Fifth Edition; J.D. Lee; Wiley India(P) Ltd, New Delhi, 2008. 
  • Inorganic Chemistry; Seventh International Edition; M. Weller, T. Overton, J. Rourke, F. Armstrong; Oxford University Press, New York, 2018.
  • Vogel’s Textbook of Quantitative Chemical Analysis; Sixth Edition; M. Thomas, B. Sivasankar, J. Mendham, R.C. Denney, J. D. Barnes; Pearson Education, New Delhi, 2009.
 
Academic Year: 
2020-2021
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