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CHEMISTRY for TECHNOLOGISTS L T P C 3 0 2 4 Common to I Sem. B.Tech CHEMISTRY FOR TECHNOLOGISTS L T P C 3 0 2 4 Common to I sem. B.Tech. – BIO. TECH, CHEMICAL and FOOD TECHNOLOGY OBJECTIVES To acquire molecular level understanding of matter To understand the basics of surface chemistry and nanomaterials To attain knowledge on natural products and polymers UNIT I - CHEMICAL BONDING 9 Types of chemical bonds - electronegativity - bond polarity and dipole moments, partial ionic character of covalent bonds - VB theory - concept of hybridization. Molecular orbital theory - LCAO - bonding in homonuclear and heteronuclear diatomic molecules. Intermolecular forces - types - hydrogen bonding - importance of hydrogen bonding in biomolecules - van der Waals forces – consequences. UNIT II - SURFACE CHEMISTRYAND CATALYSIS 9 Adsorption-difference between adsorption and absorption-types-factors influencing adsorption- adsorption from solutions- types of isotherms-Freundlich adsorption isotherm -Langmuir adsorption isotherm -industrial applications of adsorption - applications of surface active agents - detergency-wetting - water repellency- emulsifiers - CMC and defoamers. Catalysis - general characteristics -types of catalysis -acid -base catalysis - enzyme catalysis - characteristics-Michaelis - Menton equation -effect of temperature on enzyme catalysis - Langmuir- Hinshelwood mechanism for heterogeneous catalysis. UNIT III - NANO MATERIALS 9 Basics-distinction between nanoparticles and bulk materials - size-dependent properties - nanoparticles - nanocluster – nanorod - nanotube and nanowire - synthesis of nanoparticles - chemical methods -metal nanocrystals by reduction ,solvothermal synthesis, photochemical synthesis, sonochemical synthesisandchemical vapor deposition -physical methods - ball milling ,electrodeposition - biogenic synthesis - properties and applications. UNIT IV - HETEROCYCLIC COMPOUNDS AND NATURAL PRODUCTS 9 Heterocyclic compounds-synthesis and reactions of pyrrole -furan - thiophene- pyridine- quinoline-isoquinoline. Terpenoids- Isolation - Isoprene rule-structural elucidation of citral and menthol. UNIT V - POLYMERS 9 Polymers-definition - polymerization - types - addition and condensation polymerization - free radical polymerization mechanism - effect of structure on the properties of polymers - strength, plastic deformation, elasticity and crystallinity - plastics - preparation - properties and uses of PVC, teflon, polycarbonate, polyurethane, nylon-6,6, PET,KEVLAR-Green polymers- Introduction –poly lactic acid (PLA) TEXT BOOKS 1. P. C. Jain and Monika Jain, “Engineering Chemistry”, DhanpatRai Publishing Company (P) LTD, New Delhi, 2015 2. Bahl B. S., and Arun Bahl, “A Text Book of Organic Chemistry”, S. Chand, New Delhi, 2016. REFERENCES 1. R.D. Madan, “Modern Inorganic Chemistry”, S. Chand, New Delhi, 2012 2. I L Finar “Organic Chemistry” ELBS (1994) 3. Gowarikar V. R., Viswanathan N.V. and Jayadev Sreedhar, ―Polymer Science‖, New Age International (P) Ltd., New Delhi, 2011 4. B.S. Murthy, P.Shankarand others,“Text book of Nano-science and nanotechnology”, University Press, IIM. Syllabus for Chemistry Laboratory 30 (Any 10 experiments tobe conducted) 1. Estimation of mixture of acids by conductometry 2. Estimation of copper / ferrous ions by spectrophotometry 3. Estimation of acid by pH metry. 4. Estimation of alkalinity by indicator method. 5. Estimation of chloride by argentometric method 6. Determination of total, temporary and permanent hardness by EDTA method. 7. Estimation of DO by winkler’s method 8. Estimation of sodium and potassium in water by flame photometry 9. Determination of corrosion rate on mild steel by weight loss method 10. Determination of molecular weight of a polymer by viscometry method. 11. Verification of adsorption isotherms ( acetic acid on charcoal) 12. Phase change in a solid. 13. Preparation of simple drug 14. Determination of rate constant of a reaction 15. Determination of distribution coefficient 16. Preparation of Thiokol rubber. TOTAL PERIODS 75 OUTCOMES On completion of the course students will be able to Be conversant with basics of molecule formation and interactions measure molecular/bulk properties like absorbance, molecular weight, DO and chloride Apply the knowledge of surface chemistry in practical and industrial applications Be familiar with structure and properties of natural products Be assertive on various types of polymers and their properties including green polymers UNIT I CHEMICAL BONDING 1.1 TYPES OF CHEMICAL BONDS The chemical bonds can be classified based on the nature of the interaction between the bonded atoms. Two major types of chemical bonds are covalent bonds and ionic bonds. Generally metals reacts with non-metals to form ionic compounds, and the covalent bonds are present in the compounds formed by nonmetals. Octet rule-Duet role: When the electronegativity difference between the two combining atoms is large, the least electronegative atom completely transfers one or more of its valence electrons to the other combining atom so that both atoms can attain the nearest inert gas electronic configuration. The complete transfer of electron leads to the formation of a cation and an anion. Both these ions are held together by the electrostatic attractive force which is known as ionic bond. While undergoing a chemical reaction, atoms of group 1A-7A elements tend to gain, lose, or share sufficient electrons to achieve an electron configuration having eight valance electrons. After gaining, losing, or sharing, ions/atoms will have the electron configuration like that of the noble gases nearest to them in atomic number. Cation : loses one, two or three electrons and in losing electrons, the atom becomes a positively charged ion called a cation (Na+, Ca2+, Mg2+) (usually metals). Cation has an electron configuration like that of the noble gas nearest to it in atomic number. Anion :gains one, two or three electrons and in gaining electrons, the atom becomes a negatively charged ion called an anion (Cl-, O2-, S2-) (usually nonmetals). Anion has an electron configuration like that of the noble gas nearest to it in atomic number. 1.1.1 Ionic bonds: ionic bonds usually form between a metal and a nonmetal. In ionic bonding, electrons are completely transferred from one atom to another. In the process of either losing or gaining negatively charged electrons, the reacting atoms form ions. The oppositely charged ions are attracted to each other by electrostatic forces, which are the basis of the ionic bond. There are enormous differences between the chemical and physical properties of an atom and those of its ion(s). For example sodium is a soft metal and it reacts violently with water. Chlorine is a gas and it is very unstable and reactive. Both sodium and chlorine are poisonous. However, NaCl (common table salt made up of Na+ and Cl-) is quite stable and unreactive. Na (1s2 2s2 2p6 3s1) + Cl (1s2 2s2 2p6 3s1 3p5) → Na+ (1s2 2s2 2p6) + Cl- (1s2 2s2 2p6 3s1 3p6) 1.1.2 Covalent bonds: Covalent bonds usually form between two nonmetals or a metalloid and a nonmetal. In covalent bonds, the atoms share one or more pairs of electrons (by using their valence electrons) between each other to obtain a filled valence level. This type of mutual sharing of one or more pairs of electrons between two combining atoms results in the formation of a chemical bond called a covalent bond. The valence electrons which are shared between two atoms are called “shared pair of electrons” or “bonding pair of electrons”. The valance electrons which are not shared are called “unshared pair of electrons” or “lone pairs”. These electrons are not involved in bonding. If two atoms share just one pair of electron a single covalent bond is formed as in the case of hydrogen molecule. If two or three electron pairs are shared between the two combining atoms, then the covalent bond is called a double bond or a triple bond, respectively. 1.2 ELECTRONEGATIVITY: Electronegativity is measure of an atom’s attraction for the electrons it shares in a chemical bond with another atom. The electronegativity shows, how tightly an atom holds the electrons that it shares with another atom. When the electronegativity increases, the ionisation energy also increases. Note: 1.Electronegativity generally increases from left to right across a row of the Periodic Table. 2.Electronegativity generally increases from bottom to top within a column of the Periodic Table. 1.3 POLARITY OF BONDS Polarity: A molecule will be polar if it has two properties at the same time: 1. It has polar bonds. 2. Its centers of partial positive charge and partial negative charge lie at different places within the molecule. In order to find the polarity of a molecule, we should: 1. Draw the Lewis Structure. 2. Determine the bond angle and the shape of the molecule. 3. Predict the electronegativity of which atom is higher than others. 4. Indicate partial positive charge and partial negative charge for each atom and draw the dipole signs. 5. If the centers of partial positive charge and partial negative charge lie at the different places within the molecule, molecule would be polar. Otherwise, molecule is nonpolar. 1.4 DIPOLE MOMENT: The molecule possesses the dipole moment can be defined as the product of the magnitude of the charge and the distance between the centres of positive and negative charge as a result of polarisation.The polarity of a covalent bond can be measured in terms of dipole moment which is defined as Dipole moment (µ) = charge (Q) × distance of separation (r) [μ = Q × 2d] Where μ is the
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