Course Outline For Chemistry
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This course outline provides the details of Chemistry I, a 3-credit course offered in the first semester. The course is designed to give engineering students a fundamental understanding of chemistry. Topics covered include the classification of matter, atomic structure, chemical bonding, stoichiometry, properties of states of matter, and solutions. Evaluation will be based on assignments, attendance, participation, quizzes, a midterm exam, and a final exam. The primary reference book listed is Fundamental of Chemistry.
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This document outlines the lecture schedule and topics, course requirements, and grading scale for General Chemistry I taught by Professor David Rahni at Pace University. The course will cover topics including atomic structure, chemical bonding, stoichiometry, gases, thermochemistry, and periodic properties over 15 weeks. Students will take 3 exams, complete a laboratory component, and homework assignments. The final exam will be cumulative and course grades will be calculated from exams, labs, homework, and other assessments. Biographical information is also provided on Professor Rahni and his academic and professional background.
Chemistry_SrSec_2022-23.pdf
The document provides information on the chemistry curriculum for classes 11 and 12 in India.
Some key points:
1. The curriculum aims to provide students with conceptual knowledge of chemistry to enable them to pursue further academic or professional studies.
2. New areas like synthetic materials, biomolecules, and industrial chemistry have been added to better reflect current topics in chemistry.
3. Greater emphasis is placed on new nomenclature, symbols, fundamental concepts, and applications of chemistry in technology and industry.
4. The class 11 syllabus covers topics like atomic structure, chemical bonding, states of matter, thermodynamics, equilibrium, redox reactions and organic chemistry.
5. Practical work
Chemistry_SrSec_2022-23 (1).pdf
The document provides information on the chemistry curriculum for classes 11 and 12 in India.
Some key points:
1. The curriculum aims to provide students with conceptual knowledge of chemistry to enable them to pursue further academic or professional studies.
2. New areas like synthetic materials, biomolecules, and industrial chemistry have been added to update the syllabus.
3. For class 11, the syllabus covers topics like atomic structure, chemical bonding, states of matter, thermodynamics, equilibrium etc.
4. The class 12 syllabus includes solutions, electrochemistry, kinetics, coordination compounds and various types of organic compounds.
5. Practical work involves volumetric analysis, salt analysis
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Lecture 19&20 For Print
1. Chemical formulas indicate the relative quantities of elements in a compound or ion and imply bonding between atoms. Subscripts indicate the number of atoms present, while coefficients indicate the relative number of molecules or formula units.
2. A chemical equation represents a chemical reaction, showing the reactants on the left and products on the right. Equations must be balanced so that the same number and type of atoms are on both sides. Coefficients are added in front of formulas to balance the equation.
3. There are five main types of chemical reactions: synthesis, decomposition, combustion, single displacement, and double displacement. Synthesis reactions combine reactants to form new compounds. Decomposition reactions break down compounds into simpler substances. Comb
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The document provides information on anomalous electron configurations of some elements, where the actual electron configuration differs from what is expected based on the Aufbau principle. It notes that stable configurations occur for half-filled or completely filled d or f orbitals. Examples are given of elements like Chromium, Copper, Silver, and Gold that have these anomalous configurations due to having superior stability from half-filled or filled d or f orbitals compared to nearly filled orbitals. The exceptions are said to occur more for larger elements where orbital energies are similar.
2 Slide Lecture 13
The document discusses the electron configurations of some elements that deviate from the Aufbau principle, including Cr, Mo, Cu, Ag, and Au having stable configurations with half-filled or filled d subshells. It provides tables comparing the expected and actual electron configurations of these and other elements. The explanation given for these anomalies is that filled or half-filled orbital configurations are more stable than nearly filled or half-filled configurations.
Lecture 5 & 6
This document discusses the early history and development of atomic theory from Democritus to the Bohr model. It begins with Democritus' idea in ancient Greece that matter is made of indivisible "atomos." This idea was later ignored for over 2000 years. In the early 1800s, John Dalton proposed atoms as basic units of matter based on laws of conservation of mass, definite composition, and multiple proportions. However, Dalton's model could not explain experimental findings. Rutherford's gold foil experiment showed atoms have small, dense nuclei and electrons orbiting the outside. But this model failed to explain atomic stability. Finally, Bohr incorporated quantum theory to propose electrons orbiting in discrete energy levels, resolving issues with prior models
Lecture 5 & 6
This document discusses the early history and development of atomic theory from Democritus to the early 20th century. It covers key experiments and models including:
- Democritus' early idea of indivisible atoms (atomos) that was later ignored for over 2000 years.
- John Dalton's atomic theory in the 1800s which was based on the laws of conservation of mass, definite composition, and multiple proportions.
- J.J. Thomson's "plum pudding" model which proposed atoms were made of positive charge with electrons scattered within.
- Ernest Rutherford's gold foil experiment which showed that atoms are mostly empty space with a small, dense positively charged nucleus.
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Lecture 1&2
1. Chemistry is the study of matter and its properties, composition, structure and the changes it undergoes.
2. Matter exists in three physical forms - solid, liquid and gas - depending on conditions like temperature and pressure.
3. Elements and compounds are the two main categories of pure substances, while mixtures can be either homogeneous or heterogeneous.
Lecture 3&4
This lecture discusses scientific measurements and units. It covers the metric system and SI units, dimensional analysis, unit conversions, and significant figures. Key points include:
1. The metric system uses meters, grams, and seconds as fundamental units. There are seven base SI units including the meter for length and gram for mass.
2. Dimensional analysis uses conversion factors to change between units while maintaining the correct dimensions. It is useful for solving chemistry problems.
3. Significant figures indicate the precision of a measurement and how numbers should be rounded. Calculations are rounded according to whether they involve multiplication/division or addition/subtraction.
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This lecture discusses scientific measurements and units. It covers the metric system and SI units, dimensional analysis, unit conversions, and significant figures. Key points include:
1. The metric system uses meters, grams, and seconds as fundamental units. There are seven base SI units including the meter for length and gram for mass.
2. Dimensional analysis uses conversion factors to change between units while maintaining the correct dimensions. It is useful for solving chemistry problems.
3. Significant figures reflect the precision of a measurement and determine how many digits are reported in calculations. Rules for significant figures depend on the operation being used.
Lecture 7
1) The document discusses the electronic configuration of atoms, including the development of wave mechanics and quantum theory to explain the structure of atoms. It introduces concepts like the de Broglie wavelength, quantum numbers, atomic orbitals and shapes, Pauli's exclusion principle, and Hund's rule for electron configuration.
2) Key scientists discussed include de Broglie, Heisenberg, Schrodinger, Pauli, and their contributions to developing models of the atom and allowing prediction of electron configurations.
3) The document provides examples of writing out electron configurations for elements and explaining the rules for filling atomic orbitals in the Aufbau principle.
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Course Outline For Chemistry
- 1. September 15, 2008 EELO AMERICAN UNIVERSITY Chemistry I Course outline 1. Course Code : CHEM 211 2. Credits : 3 3. Instructor : Md. Faysal Ahamed Khan 4. Semester : I 5. Introduction : This course is designed to give a fundamental understanding of Chemistry to Engineers. The topics included: classification of matter, measurement and periodic table of elements, atomic structure, periodicity, chemical bonding, stoichiometry, reactions, the properties of gases, liquids, solids, and solutions, and an introduction to the various types of bonding. The primary reason behind including Chemistry is that it is part of an Engineering program, and Electrical Engineer/Civil Engineer/Computer Engineering should be able to learn (if necessary) any aspect which may relevant to their study program. By taking Chemistry I, you learn about electrons, various types of metals (including things like silicon and germanium, key parts in computers) and the differences between various metals - what oxidizes and what doesn’t and how bonding happened? And about various type of chemical reactions. All of this information prepares you for the challenge of working in industries where might be possible to have encounter various chemical activities. You may not need to care now, but you’ll have the knowledge to build upon if necessary and it’s the potential to understand everything about your chosen field which will help you become an engineer. 6. Contents : 1. What is Chemistry? 8. Stoichiometry 2. Classification of Matter 9. Various chemical bonding 3. Measurement in chemistry 10. Shapes of molecules 4. Atomic structure & Electronic 11. Theories of covalent bonding configuration of the atom 12. Intermolecular forces: Liquids, 5. The periodic table of elements Solids 6. Periodic properties of elements 13. Solutions 7. Chemicals formulas, equations & Various chemical reactions 7. Method of Evaluation: • Assignments/Quizzes 20% • Attendance 5% • Class participation 5% • C. A. T 20% • Final Exam 50% Reference Book: a. “Fundamental of Chemistry”, 3rd Edition by David E. Goldberg b. “Chemistry – The Molecular Nature of Matter and Change”, 3 rd Edition by Martin S. Silberberg Instructor Signature: …………………… Registrar: ……………………