| Medical chemistry and physics
(objectives)
The aim of the Biochemistry module (General and Inorganic Chemistry, Introductory Biochemistry and Biochemistry), as a part of the Integrated Course of MEDICAL CHEMISTRY AND PHYSICS, is to provide students with the fundamental knowledge relating to the structure of atoms and chemical elements and of the macromolecules necessary for the functioning and regulation of living organisms and their transformation processes. Put the student in a position to understand the basics of chemistry and cellular metabolism. The teaching also intends to provide the student with the fundamental knowledge relating to the basic concepts of chemistry, the structure of macromolecules underlying the metabolic processes necessary for the functioning and regulation of living organisms: carbohydrates, lipids, nucleic acids. To enable the student to understand the basics of cellular metabolism. The course aims to provide the student with some essential methods used in chemistry and biochemical practice and the theoretical principles on which these methodologies and their field of application are based.
The aim of the Physics module (Applied Physics, Medical Statistics and Informatics), as a part of the Integrated Course of MEDICAL CHEMISTRY AND PHYSICS, is to provide students with knowledge on the fundamentals of applied physics, Statistics and Informatics necessary for their future activity. In particular, the comprehension of physical principles at the base of medical physics and of functioning of medical instrumentation will be addressed. At the end of the course, the students will know the fundamental concepts of application of the Scientific Method to the study of biomedical phenomena (choice and measure of parameters, evaluation of errors), they will be able to describe physical phenomena of complex systems using suitable mathematical tools, they will know the scientific basis of medical procedures and principles of functioning of the equipment commonly used for diagnostics and therapeutics. The student should be able to understand the tools and computer concepts that will be useful for their future profession in the medical field and understand the importance of medical statistics in the research methodology in the medical field; - read a basic biomedical scientific article, understanding its structure and critically evaluating methods and results; handle a simple database, with particular reference to clinical medicine; make a descriptive and inferential analysis.
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Code
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90524 |
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Language
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ENG |
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Type of certificate
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Profit certificate
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| Module: Chemistry
(objectives)
The aim of the Biochemistry module (General and Inorganic Chemistry, Introductory Biochemistry and Biochemistry), as a part of the Integrated Course of MEDICAL CHEMISTRY AND PHYSICS, is to provide students with the fundamental knowledge relating to the structure of atoms and chemical elements and of the macromolecules necessary for the functioning and regulation of living organisms and their transformation processes. Put the student in a position to understand the basics of chemistry and cellular metabolism. The teaching also intends to provide the student with the fundamental knowledge relating to the basic concepts of chemistry, the structure of macromolecules underlying the metabolic processes necessary for the functioning and regulation of living organisms: carbohydrates, lipids, nucleic acids. To enable the student to understand the basics of cellular metabolism. The course aims to provide the student with some essential methods used in chemistry and biochemical practice and the theoretical principles on which these methodologies and their field of application are based.
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Language
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ENG |
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Type of certificate
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Profit certificate
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Credits
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10
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Scientific Disciplinary Sector Code
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BIO/10
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Contact Hours
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100
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Type of Activity
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Basic compulsory activities
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Teacher
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Lazzarino Giacomo
(syllabus)
Hybridization of the carbon atom - sp3, sp2, sp hybridizations and their geometry.
Hydrocarbons - Saturated hydrocarbons: alkanes and cycloalkanes. Nomenclature. Unsaturated hydrocarbons: alkenes and alkynes. Nomenclature. Conformational isomerism and geometric isomerism (cis-trans).
Aromatic compounds - Structure of benzene: the resonance model. Nomenclature of aromatic compounds. Polycyclic aromatic hydrocarbons (outline).
Alcohols, phenols, thiols - Nomenclature. Acidity and basicity of alcohols and phenols. Thiols, analogues of alcohols and phenols.
Aldehydes and ketones - Nomenclature. Preparations of aldehydes and ketones. The carbonyl group. The nucleophilic addition to the carbonyl groups; formation of semiacetals and acetals. The aldol condensation (outline).
Carboxylic acids and their derivatives - Nomenclature of acids. Derivatives of carboxylic acids: esters, amides. Mechanism of esterification; triesters of glycerol.
Amines and other nitrogen compounds - Classification of amines and nomenclature.
Stereoisomery - Chirality. Enantiomers. Polarized light; the polarimeter (outline). Diastereomers.
Carbohydrates - Definitions and classification. The monosaccharides. Chirality in monosaccharides; Fischer's projections. Cyclic structures of monosaccharides. Anomers. Phenomenon of mutarotation. Pyranosic and furanotic structures.
Lipids - Structure, nomenclature, properties.
Nitrogen bases and nucleotides -Structure, nomenclature.
(reference books)
• Chemistry 10th edition, Kenneth W. Whitten/Raymond E. Davis/Larry Peck/George G. Stanley.
• Foundations of College Chemistry, 14 Edition, Hein M, Arena S. John Wiley and Sons Inc.
• Lehninger Principles of Biochemistry, Nelson D. Cox Michael M.
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Dates of beginning and end of teaching activities
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From to |
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Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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Teacher
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Di Venere Almerinda
(syllabus)
General and inorganic chemistry:
Introductory notes - Periodic table of the elements and its meaning: Inorganic nomenclature: acids, bases, salts. Balance of a chemical reaction. Concept of mole, Avogadro number.
Constitution of the atom - Elementary particles: proton, neutron, electron. Isotopes. Electrons and electronic configuration of atoms. Quantum numbers and orbitals. Auf-bau. The chemical bond: covalent, ionic, dative. Hybridization. Weak bonds: ion-dipole, Van der Waals, hydrogen bond. Electronegativity.
States of matter - Gas: equation of state of ideal gases. Absolute temperature and relationship with the average molecular speed. Gaseous mixtures; Dalton's law. Liquids: vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular solids. Metallic solids (outline).
Chemical thermodynamics - Concept of state function. Internal energy of a system. Enthalpy, Hess's law. Entropy. Free energy.
Solutions - Concentration of solutions: % by weight, mole fraction, molarity, molality, normality. Dilutions and mixing of solutions. Vapor pressure of a liquid-liquid solution (Raoult's law). Ideal solutions. Colligative properties: variation of vapor pressure, of melting and boiling temperatures; osmosis and osmotic pressure. Solubility of gases in liquids: Henry's law.
Chemical equilibrium - Equilibrium in the gas phase. Expression of the equilibrium constant. Relationship between Kc and Kp. Factors that influence the balance. Homogeneous and heterogeneous equilibria.
Electrolyte Solutions - Strong and Weak Electrolytes; degree of dissociation. Colligative properties of electrolyte solutions; combination of Van’t Hoff. Acids and bases according to Arrenius, Bronsted and Lowry, Lewis. Strong and weak acids and bases. Ionic dissociation of water. Kw. Equilibrium constant of an acid and a base. Relationship between the equilibrium constant and the degree of dissociation of a weak electrolyte: Oswald's law of dilution. The pH; calculation of pH in solutions of strong and weak acids (and bases). Saline hydrolysis. Buffer solutions. Dissociation of polyprotic acids (outline). Acid-base titrations.
Chemical Kinetics - Introduction to Kinetics; activated complex theory; activation energy. Kinetic equations
Redox reactions and electrochemical potentials - Oxidation number. Redox reactions and their balance.
Biochemistry :
Proteins - Amino acids and their properties.-Peptide bond. Primary structure. Non-protein amino acids. Secondary structure: alpha helix, beta sheet, loops and beta turn. Tertiary and quaternary structure: hydrogen bonds and hydrophobic effect. Misfolding and related pathologies. Generic structure of fibrous and globular proteins. Techniques for the analysis and purification of proteins
Enzymatic kinetics - steady state. The Michaelis-Menten equation. Meaning of Km. Catalytic efficiency: meaning of kcat / Km. Reciprocal Doubles Graph. Classification of enzymes-Inhibitors: competitive and incompetitive inhibition. Mechanisms and graphs of reciprocal doubles. The inhibitors: a-competitive (pure non-competitive) and mixed (non-competitive) inhibition. Irreversible inhibitors and suicide inhibitors. - The transport and storage of oxygen.
Myoglobin - structure and function.
Hemoglobin - structure and function. The Bohr effect; the effect of 2,3 BPG; the transport of CO2 and NO. Introduction to the theory of protein-ligand interaction: case of only 1 site. Case of n fully cooperative sites. General case. Concerted and sequential model. Effects of point mutations.
Carbohydrates - the different types of classification (structural and functional). Stereoisomerism. Reducing sugars. Main monosaccharides and disaccharides. Sugar derivatives.
Membrane lipids. Cholesterol. Lipids-signal and cofactors: eicosanoids, steroid hormones, fat-soluble vitamins. -Architecture of biological membranes: composition of membranes, common properties of membranes, the bilayer sheet, types of proteins in biological membranes. Dynamics of biological membranes. Transport across biological membranes: simple diffusion and passive transport, glucose transporter, chloride-bicarbonate exchanger, active transport, sodium-glucose symports, aquaporins.
Vitamins - historical introduction. Fat-soluble vitamins structure, function, avitaminosis, hypervitaminosis. Water-soluble vitamins structure, function avitaminosis.
Bioenergetics - free energy in biochemical reactions. Standard free energy and Keq free energy. Examples.
Glycolysis. Pathway of pentose phosphate. Coordinated control of glucose metabolism. Lactic fermentation and alcoholic fermentation. Anaerobic metabolism and caries. The Krebs cycle. Glycogen metabolism and its regulation. Glycogen storage diseases.
Physiological digestion of fats. Lipoproteins - structure and function of chylomicrons, VLDL, LDL and HDL. Glucagon-induced fat mobilization: roles of triacylglycerol lipase and perilipin. Activation of fatty acids and transport across the mitochondrial membrane. Carnitine. Beta-oxidation of saturated fatty acids, even. Examples. Ketogenesis. Beta-oxidation of unsaturated and odd fatty acids.
Protein digestion - role of pH and digestive enzymes. alanine-glucose cycle. Transamination, oxidative demination, non-oxidative demination. glutammine-synthetase: role and its regulation.
Urea cycle.
Notes on the catabolism of the academic year branched and "maple syrup" urine disease. Catabolism of glycine and serine.
Notes on the catabolism of nitrogenous bases - excess uric acid and gout.
The metabolism of heme - introduction to biosynthesis (the glycine pathway, the synthesis of δ-aminolevulinate and the formation of porphobilinogen). The porphyrias. Notes on the catabolism of EME and its degradation to biliverdin and bilirubin.
Chemosmotic coupling - general principles; the change in free energy associated with the flow of electrons and protons; ATP synthase as an energy transducer. Electron transporters (nicotinamide and flavin nucleotides; ubiquinone; cytochromes; iron-sulfur proteins; complexes I, II, III, IV; Q cycle; respirasome. ATP synthase (structure and catalysis; ATP synthase as molecular motor). Inhibitors and uncouplers of respiratory chain.
(reference books)
• Chemistry 10th edition, Kenneth W. Whitten/Raymond E. Davis/Larry Peck/George G. Stanley.
• Foundations of College Chemistry, 14 Edition, Hein M, Arena S. John Wiley and Sons Inc.
• Lehninger Principles of Biochemistry, Nelson D. Cox Michael M.
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Dates of beginning and end of teaching activities
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From to |
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Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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Teacher
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Nicolai Eleonora
(syllabus)
General and inorganic chemistry :
Introductory notes - Periodic table of the elements and its meaning: Inorganic nomenclature: acids, bases, salts. Balance of a chemical reaction. Concept of mole, Avogadro number.
Constitution of the atom - Elementary particles: proton, neutron, electron. Isotopes. Electrons and electronic configuration of atoms. Quantum numbers and orbitals. Auf-bau. The chemical bond: covalent, ionic, dative. Hybridization. Weak bonds: ion-dipole, Van der Waals, hydrogen bond. Electronegativity.
States of matter - Gas: equation of state of ideal gases. Absolute temperature and relationship with the average molecular speed. Gaseous mixtures; Dalton's law. Liquids: vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular solids. Metallic solids (outline).
Chemical thermodynamics - Concept of state function. Internal energy of a system. Enthalpy, Hess's law. Entropy. Free energy.
Solutions - Concentration of solutions: % by weight, mole fraction, molarity, molality, normality. Dilutions and mixing of solutions. Vapor pressure of a liquid-liquid solution (Raoult's law). Ideal solutions. Colligative properties: variation of vapor pressure, of melting and boiling temperatures; osmosis and osmotic pressure. Solubility of gases in liquids: Henry's law.
Chemical equilibrium - Equilibrium in the gas phase. Expression of the equilibrium constant. Relationship between Kc and Kp. Factors that influence the balance. Homogeneous and heterogeneous equilibria.
Electrolyte Solutions - Strong and Weak Electrolytes; degree of dissociation. Colligative properties of electrolyte solutions; combination of Van’t Hoff. Acids and bases according to Arrenius, Bronsted and Lowry, Lewis. Strong and weak acids and bases. Ionic dissociation of water. Kw. Equilibrium constant of an acid and a base. Relationship between the equilibrium constant and the degree of dissociation of a weak electrolyte: Oswald's law of dilution. The pH; calculation of pH in solutions of strong and weak acids (and bases). Saline hydrolysis. Buffer solutions. Dissociation of polyprotic acids (outline). Acid-base titrations.
Chemical Kinetics - Introduction to Kinetics; activated complex theory; activation energy. Kinetic equations
Redox reactions and electrochemical potentials - Oxidation number. Redox reactions and their balance. Standard reduction potentials.
Biochemistry :
Proteins - Amino acids and their properties.-Peptide bond. Primary structure. Non-protein amino acids. Secondary structure: alpha helix, beta sheet, loops and beta turn. Tertiary and quaternary structure: hydrogen bonds and hydrophobic effect. Misfolding and related pathologies. Generic structure of fibrous and globular proteins. Techniques for the analysis and purification of proteins
Enzymatic kinetics - steady state. The Michaelis-Menten equation. Meaning of Km. Catalytic efficiency: meaning of kcat / Km. Reciprocal Doubles Graph. Classification of enzymes-Inhibitors: competitive and incompetitive inhibition. Mechanisms and graphs of reciprocal doubles. The inhibitors: a-competitive (pure non-competitive) and mixed (non-competitive) inhibition. Irreversible inhibitors and suicide inhibitors. - The transport and storage of oxygen.
Myoglobin - structure and function.
Hemoglobin - structure and function. The Bohr effect; the effect of 2,3 BPG; the transport of CO2 and NO. Introduction to the theory of protein-ligand interaction: case of only 1 site. Case of n fully cooperative sites. General case. Concerted and sequential model. Effects of point mutations.
Carbohydrates - the different types of classification (structural and functional). Stereoisomerism. Reducing sugars. Main monosaccharides and disaccharides. Sugar derivatives.
Membrane lipids. Cholesterol. Lipids-signal and cofactors: eicosanoids, steroid hormones, fat-soluble vitamins. -Architecture of biological membranes: composition of membranes, common properties of membranes, the bilayer sheet, types of proteins in biological membranes. Dynamics of biological membranes. Transport across biological membranes: simple diffusion and passive transport, glucose transporter, chloride-bicarbonate exchanger, active transport, sodium-glucose symports, aquaporins.
Vitamins - historical introduction. Fat-soluble vitamins structure, function, avitaminosis, hypervitaminosis. Water-soluble vitamins structure, function avitaminosis.
Bioenergetics - free energy in biochemical reactions. Standard free energy and Keq free energy. Examples.
Glycolysis. Pathway of pentose phosphate. Coordinated control of glucose metabolism. Lactic fermentation and alcoholic fermentation. Anaerobic metabolism and caries. The Krebs cycle. Glycogen metabolism and its regulation. Glycogen storage diseases.
Physiological digestion of fats. Lipoproteins - structure and function of chylomicrons, VLDL, LDL and HDL. Glucagon-induced fat mobilization: roles of triacylglycerol lipase and perilipin. Activation of fatty acids and transport across the mitochondrial membrane. Carnitine. Beta-oxidation of saturated fatty acids, even. Examples. Ketogenesis. Beta-oxidation of unsaturated and odd fatty acids.
Protein digestion - role of pH and digestive enzymes. alanine-glucose cycle. Transamination, oxidative demination, non-oxidative demination. glutammine-synthetase: role and its regulation.
Urea cycle.
Notes on the catabolism of the academic year branched and "maple syrup" urine disease. Catabolism of glycine and serine.
Notes on the catabolism of nitrogenous bases - excess uric acid and gout.
The metabolism of heme - introduction to biosynthesis (the glycine pathway, the synthesis of δ-aminolevulinate and the formation of porphobilinogen). The porphyrias. Notes on the catabolism of EME and its degradation to biliverdin and bilirubin.
Chemosmotic coupling - general principles; the change in free energy associated with the flow of electrons and protons; ATP synthase as an energy transducer. Electron transporters (nicotinamide and flavin nucleotides; ubiquinone; cytochromes; iron-sulfur proteins; complexes I, II, III, IV; Q cycle; respirasome. ATP synthase (structure and catalysis; ATP synthase as molecular motor). Inhibitors and uncouplers of respiratory chain.
(reference books)
• Chemistry 10th edition, Kenneth W. Whitten/Raymond E. Davis/Larry Peck/George G. Stanley.
• Foundations of College Chemistry, 14 Edition, Hein M, Arena S. John Wiley and Sons Inc.
• Lehninger Principles of Biochemistry, Nelson D. Cox Michael M.
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Dates of beginning and end of teaching activities
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From to |
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Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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| Module: Physics
(objectives)
Aim of the integrated course of Physics and Statistics (Applied Physics, Medical Statistics and Informatics) is to provide students with knowledge on the fundamentals of applied physics, Statistics and Intormatics necessary for their future activity. In particular, the comprehension of physical principles at the base of medical physics and of functioning of medical instrumentation will be addressed.
At the end of the course, the students will know the fundamental concepts of application of the Scientific Method to the study of biomedical phenomena (choice and measure of parameters, evaluation of errors), they will be able to describe physical phenomena of complex systems using suitable mathematical tools, they will know the scientific basis of medical procedures and principles of functioning of the equipment commonly used for diagnostics and therapeutics.
The student should be able to understand the tools and computer concepts that will be useful for their future profession in the medical field and understand the importance of medical statistics in the research methodology in the medical field; - read a basic biomedical scientific article, understanding its structure and critically evaluating methods and results; handle a simple database, with particular reference to clinical medicine; make a descriptive and inferential analysis.
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Language
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ENG |
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Type of certificate
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Profit certificate
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Credits
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7
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Scientific Disciplinary Sector Code
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FIS/07
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Contact Hours
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70
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Type of Activity
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Basic compulsory activities
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Teacher
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FILABOZZI ALESSANDRA
(syllabus)
Mechanics
Chapter 1: Introduction, Measurement, Estimating
1.4: Measurement and Uncertainty; Significant Figures
1.5: Units, Standards, and SI Units
1.6: Converting Units
1.8: Dimensions and Dimensional Analysis
Chapter 2: Describing Motion: Kinematics in One Dimension
2.1: References Frames and Displacement
2.2: Average Velocity
2.3: Instantaneous Velocity
2.4: Acceleration
2.5: Motion at Constant Acceleration
Chapter 3: Kinematics in Two Dimensions; Vectors
3.1: Vectors and Scalars
3.2: Addition of Vectors-Graphical Methods
3.3: Subtraction of Vectors and Multiplication of a Vector By a Scalar
3.4: Adding Vectors by Components
Chapter 4: Dynamics: Newton's Laws of Motion
4.1: Force
4.2: Newton's First Law of Motion
4.3: Mass
4.4: Newton's Second Law of Motion
4.5: Newton's Third Law of Motion
4.6: Weight-The Force of Gravity; and the Normal Force
4.7: Solving Problems with Newton's Laws: Free-Body Diagrams
4.8: Problems Involving Friction, Inclines
4.9: Problem Solving-A General Approach
Chapter 5: Circular Motion; Gravitation
5.1: Kinematics of Uniform Circular Motion
5.2: Dynamics of Uniform Circular Motion
5.6: Newton's Law of Universal Gravitation
Chapter 6: Work and Energy
6.1: Work Done by a Constant Force
6.3: Kinetic Energy and the Work-Energy Principle
6.4: Potential Energy
6.5: Conservative and Nonconservative Forces
6.6: Mechanical Energy and its Conservation
6.7: Problem Solving Using Conservation of Mechanical Energy
6.8: Other Forms of Energy: Energy Transformations and the Law of Conservation of Energy
6.10: Power
Chapter 7: Linear Momentum
7.1: Momentum and Its Relation to Force
7.2: Conservation of Momentum
7.8: Center of Mass (CM)
7.10: Center of Mass and Translational Motion
Chapter 8: Rotational Motion
8.1: Angular Quantities
8.2: Constant Angular Acceleration
8.4: Torque
8.5: Rotational Dynamics; Torque and Rotational Inertia
8.6: Solving Problems in Rotational Dynamics
8.7: Rotational Kinetic Energy
Chapter 9: Static Equilibrium; Elasticity and Fracture
9.1: The Conditions for Equilibrium
9.2: Solving Statics Problems
9.3: Applications to Muscles and Joints
9.4: Stability and Balance
9.5: Elasticity; Stress and Strain
9.6: Fracture
Fluids
Chapter 10: Fluids
10.1: Phases of Matter
10.2: Density and Specific Gravity
10.3: Pressure in Fluids
10.4: Atmospheric Pressure Gauge Pressure
10.5: Pascal's Principle
10.6: Measurement of Pressure; Gauges and the Barometer
10.7: Buoyancy and Archimedes' Principle
10.8: Fluids in Motion; Flow Rate and the Equation of Continuity
10.9: Bernoulli's Principle
10.10: Applications of Bernoulli's Principle: from Torricelli to Airplanes, Baseballs, and TIA
10.11: Viscosity
10.12: Flow in Tubes: Poiseuille's Equation, Blood Flow
Electricity and Magnetism
Chapter 16: Electric Charge and Electric Field
16.1: Static Electricity; Electric Charge and its Conservation
16.2: Electric Charge in the Atom
16.3: Insulators and Conductors
16.4: Induced Charge; the Electroscope
16.5: Coulomb's Law
16.6: Solving Problems Involving Coulomb's Law and Vectors
16.7: The Electric Field
16.8: Field Lines
16.9: Electric Fields and Conductors
Chapter 17: Electric Potential
17.1: Electric Potential Energy and Potential Differences
17.2: Relation Between Electric Potential and Electric Field
17.3: Equipotential Lines
17.4: The Electron Volt, a Unit of Energy
17.5: Electric Potential Due to Point Charges
17.7: Capacitance
17.8: Dielectrics
17.9: Storage of Electric Energy
Chapter 18: Electric Currents
18.1: The Electric Battery
18.2: The Electric Current
18.3: Ohm's Law: Resistance and Resistors
18.4: Resistivity
18.5: Electric Power
18.8: Microscopic View of Electric Current
Chapter 19: DC Circuits
19.1: EMF and Terminal Voltage
19.2: Resistors in Series and in Parallel
19.3: Kirchhoff's Rules
19.4: EMFs in Series and in Parallel; Charging a Battery
19.5: Circuits Containing Capacitors in Series and in Parallel
19.6: RC Circuits-Resistor and Capacitor in Series
Chapter 20: Magnetism
20.1: Magnets and Magnetic Fields
20.2: Electric Current Produce Magnetic Fields
20.3: Force on an Electric Current in a Magnetic Field: Definition of B
20.4: Force on an Electric Charge Moving in a Magnetic Field
20.5: Magnetic Field Due to a Long Straight Wire
20.8: Ampere's Law
Chapter 21: Electromagnetic Induction and Faraday's Law
21.1: Induced EMF
21.2: Faraday's Law of Induction; Lenz's Law
21.3: EMF Induced in a Moving Conductor
21.4: Changing Magnetic Flux Produces an Electric Field
(reference books)
Douglas C. Giancoli "FISICA: Principi con applicazioni" Terza edizione o successive, casa Editrice Ambrosiana
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Dates of beginning and end of teaching activities
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Delivery mode
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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Teacher
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Napolitano Antonio
(syllabus)
Vibrations and Waves
Chapter 11: Vibrations and Waves
11.7: Wave Motion
11.8: Types of Waves: Transverse and Longitudinal
11.9: Energy Transported by Waves
11.10: Intensity Related to Amplitude and Frequency
11.11: Reflection and Transmission of Waves
11.12: Interference; Principle of Superposition
11.13: Standing Waves; Resonance
Chapter 12: Sound
12-1 Characteristics of Sound
12-2 Intensity of Sound: Decibels
12-4 Sources of Sound: Vibrating Strings and
Air Columns
12-6 Interference of Sound Waves; Beats
12-7 Doppler Effect
Chapter 22: Electromagnetic Waves
22.1: Changing Electric Fields Produce Magnetic Fields; Maxwell's Equations
22.2: Production of Electromagnetic Waves
22.3: Light as an Electromagnetic Wave and the Electromagnetic Spectrum
22.5: Energy in EM Waves
Chapter 24: The Wave Nature of Light
24.4: The Visible Spectrum and Dispersion
Chapter 25: Optical Instruments
25-11: X-Rays and X-Ray Diffraction
25-12: X-Ray Imaging and Computed Tomography (CT Scan)
Nuclear Physics and Radioactivity
Chapter 27: Early Quantum Theory and Models of the Atom
27.10: Early Models of the Atom
27.12: The Bohr Model
Chapter 30: Nuclear Physics and Radioactivity
30.1: Structure and Properties of the Nucleus
30.2: Binding Energy and Nuclear Forces
30.3: Radioactivity
30.4: Alpha Decay
30.5: Beta Decay
30.6: Gamma Decay
30.7: Conservation of Nucleon Number and Other Conservation Laws
30.8: Half-Life and Rate of Decay
30.9: Calculations Involving Decay Rates and Half-life
Chapter 31: Nuclear Energy; Effects and Uses of Radiation
31.1: Nuclear Reaction and the Transmutation of Elements
31.5: Measurement of Radiation-Dosimetry
31.9: Nuclear Magnetic Resonance (NMR) and Magnetic Resonance Imaging (MRI)
Thermodynamics
Chapter 13: Temperature and Kinetic Theory
13.1: Atomic Theory of Matter
13.2: Temperature and Thermometers
13.3: Thermal Equilibrium and the Zeroth Law of Thermodynamics
13.4: Thermal Expansion
13.6: The Gas Laws and Absolute Temperature
13.7: The Ideal Gas Law
13.8: Problem Solving with the Ideal Gas Law
13.9: Ideal Gas Law in Terms of Molecules: Avogadro's Number
13.10: Kinetic Theory and the Molecular Interpretation of Temperature
Chapter 14: Heat
14.1 Heat as Energy Transfer
14.2 Internal Energy
14.3: Specific Heat
14.4: Calorimetry
14.5: Latent Heat
14.6: Heat Transfer: Conduction
14.7: Heat Transfer: Convection
14.8: Heat Transfer: Radiation
Chapter 15: The Laws of Thermodynamics
15.1: The First Law of Thermodynamics
15.2: Thermodynamic Processes and the First Law
15.4: Second Law of Thermodynamics-Introduction
(reference books)
Douglas C. Giancoli “PHYSICS: Principles with Applications” Seventh edition or subsequent, Pearson Education. Inc
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Traditional
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Attendance
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Mandatory
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Evaluation methods
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Written test
Oral exam
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