...Terminology and Concepts: Matter Matter – anything that occupies space and has mass. Fundamental Particles of Atoms (Historical Point of View) John Dalton (1808) – atomic theory 1. Atoms – small indivisible particles. 2. Atoms – neither created nor destroyed. 3. Atoms – chemical reactions result from combination / separation of atoms. J. J. Thomson (1897) 1. Electrons – negatively-charged particles. 2. Atoms – positively-charged sphere. Ernest Rutherford (1911) 1. Atoms – consists of a positively-charged nucleus with a cloud of electrons surrounding nucleus. 2. Protons – positively-charged particles. Niels Bohr (1913) 1. Electrons – surrounding the nucleus (orbit). James Cadwick (1932) 1. Neutrons – electrically neutral subatomic particles. 2. Neutrons – mass almost the same with a proton. 3. Nucleus of an atom – consists of protons and neutrons. Modern Atomic Model 1. Nucleus of an atom – consists of protons and neutrons. 2. Electrons – moving around the nucleus (orbits / electron shells/ quantum shells) Atoms Atom – smallest particle of an element. Relative atomic mass (Ar) - (an element) average mass of one atom of the element relative to 1/12 times the mass of one atom of carbon-12. = (average mass of one atom of the element) / (1/12 x mass of one atom of C-12) Or = 12 x [(average mass of one atom of the element) / (mass of one atom of C-12)] Cations – positively-charge ions. Example: H+, K+, NH4+ and Mg2+ ...
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...Unit F321: Atoms, Bonds and Groups Definitions to Learn 1. Atoms and Electron Structure Isotopes atoms of an element with different numbers of neutrons and different masses Relative atomic mass average mass of an atom relative to 1/12 of the mass of a carbon-12 atom Relative isotopic mass mass of a particular isotope relative to 1/12 of the mass of a carbon-12 atom Orbital a region that can hold up to 2 electrons with opposite spins 1st ionisation energy energy change when one mole of electrons is removed from one mole of gaseous atoms 2. Equations and acids Acid proton donor (H+ donor) Base proton acceptor (H+ acceptor) Salt produced when the H+ of an acid is replaced by another positive ion 3. Redox Oxidation loss of electrons or increase in oxidation number Reduction gain of electrons or decrease in oxidation number Disproportionation a reaction in which an element is simultaneously oxidised and reduced 4. Moles and Equations Amount of substance the number of moles of substance that you have Mole unit for amount of substance Avogadro constant, NA number of particles present in a mole (6.02 x 1023 mol-1) Empirical formula simplest whole number ratio of the atoms of each element in a compound Molecular formula actual number of atoms of each element in a molecule Concentrated containing a large amount of solute per dm3 (say 10 mol dm-3 or more) Dilute containing...
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...N Area – m2 in Pascals (SI units) Pressure is measured using pressure gauges or diaphragm gauges. Atmospheric Pressure at sea level is 1 atm = 760 mm = 760 torr = 1.01 x 105 Pascals 5.2 The Gas Laws of Boyle, Charles, and Avogadro Boyle’s Law Measured pressure vs. volume. Pressure and Volume are indirectly proportional P = K 1/V At constant temperature, following relationship can be written as P1V1 = P2V2 P1V1 = P2V2 Charle’s Law Measured volume vs. temperature. Volume and temperature are directly proportional. V = K T where temperature is in Kelvin At constant pressure, following relationship can be written as V1 = V2 T1 T2 If you extrapolate the linear relationship between temp and volume down to volume equals to zero, you’ll get T = -273 oC also known as Absolute Zero equivalent to Zero Kelvin. The Effects of Increasing the Temperature of a Sample of Gas at Constant Pressure Avogadro’s Law Equal number of molecules occupy equal volumes at same temperature and pressure. V = K. n where n is number of moles At constant temperature and pressure, following relationship can be written as V1 = V2 n1 n2 These Balloons Each Hold 1.0 L of Gas at 25 Celsius and 1 atm Increased Volume due to Increased Moles of Gas at Constant Temperature and Pressure 5.3 The Ideal Gas Law Combine the three laws into a single gas law, V = K/P V=K x T V = K x n V = nRT P where R is ideal Gas Constant can be rearranged to, PV = nRT R =...
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...chapter in the textbook. (The Practice Examples are within the chapter, the problems appear at the end of the chapter.) Students must have their Temple photo ID card during lecture exams. TU-ID Numbers must be correctly and completely filled in on exams to ensure your score is properly recorded. Students are not allowed to have cell phones and other PDA devices on their persons while taking an exam. Cell phones/PDAs are to be placed in bags/backpacks which will be kept at the back of the lecture hall. Students may leave cell phones/PDAs on the front bench of the lecture hall. Students who are caught using cell phones/PDAs during an exam will be ejected from the exam and will receive a score of zero. This violation will be reported to the Dean and the Vice-Provost who will then take the appropriate disciplinary action. Only pens/pencils and scientific calculators (non-programmable and non-graphing) are allowed to be with students during exams. Students are not allowed to take an exam in a lecture section in which they are not registered. Chapter 4 – sections 4.1 – 4.8 Given a balanced chemical equation, you should be able to calculate grams (or moles) of a product (or reactant) given the grams (or moles) of another product (or reactant). Remember: grams A ( moles A ( moles B ( grams B (p. 118). Practice Example 4.1...
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...Study Guide for Exame 2 CHAPTER 3: Stoichiometry * Stoichiometry – study of quantitative aspects of formulas and relations * The mole – SI unit for the amount of a substance. * The amount of matter that contains the same number of atoms as 12.0g of carbon -> 6.022 x 10^23 (Avogadro’s number) * Avogadro’s number – 6.022 x 10^23 * How to determine how many atoms of each element is in a compound: * (moles or grams)(6.022x10^23)(Number of atoms/1molecule) * Molar mass - Molar mass is the weight of one mole (or 6.022 x 1023 molecules) of any chemical compounds. * Mass % of an element in a compound: * ((Number of atoms of element)(atomic weight))/(Formula weight) * Empirical formula – Gives the lowest whole number ratio of atoms of each element in a compound (Grams)/(atomic weight) --- divide by lowest number on all * Molecular formula – gives actual whole number ratio of atoms of each element in each compound. (Molecular formula weight)/(Empirical formula weight) x compound * Formulas from analysis: * Structured formula – a formula that shows the atoms of a compound, their relative positions, and the bonds between them. * Isomers – compounds with the same molecular formula, but different properties and different arrangements of atoms * Writing chemical equations (symbols) : * + adding 2 or more chemicals together * -> Yields (Products) * (arrow forward and backward) reaction...
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...was discovered in 1900 by Max Planck, who had been trying to understand the emission of radiation from heated objects, known as black-body radiation. By assuming that energy can only be absorbed or released in tiny, differential, discrete packets he called "bundles" or "energy elements",[8] Planck accounted for the fact that certain objects change colour when heated.[9] On December 14, 1900, Planck reported his revolutionary findings to the German Physical Society, and introduced the idea of quantization for the first time as a part of his research on black-body radiation.[10] As a result of his experiments, Planck deduced the numerical value of h, known as the Planck constant, and could also report a more precise value for the Avogadro–Loschmidt number,...
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...No. Method of Assessment Attendance for lectures, tutorials and experiments are compulsory for every student. Main Text: Kotz, J. C., Treichel, P. M., & Townsend, J. R. (2012). Chemistry & chemical reactivity (8th ed.). Belmont, CA: Thomson Brooks/Cole. Total 1. Coursework 50% a) Test 1 & 2 (15% each) b) Experiment (20%) 2. Final Examination 50% Grand total 100% Chapter Scopes FHSC1114 PHYSICAL CHEMISTRY CHAPTER 1 Principle of Chemistry Relative Atomic Masses of atoms & molecules Mass number & atomic number Atomic structure (neutrons, protons & electrons) Mole concept & conversion Avogadro’s concept Empirical & molecular formulae Isotopes FHSC1114 Physical Chemistry 1 Centre for Foundation Studies, UTAR Objectives To define relative atomic masses of atoms & molecules To define & determine mass no. & atomic no. To determine no. of neutrons, protons & electrons To understand mole concept & Avogadro’s concept To determine the empirical & molecular formulae Structure of An Atom Atomic Composition 3 subatomic particles made up all atoms: Electrically positive protons Electrically neutral neutrons Electrically negative electrons Table: Properties & Location of Protons, Neutrons & Electrons In Atom Subatomic Symbol Relative Mass Mass Location Particle electrical (g) (amu) charge Proton p+ +1 1.6726 1 In the x 10-24 nucleus...
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...Aristotle (384—322 B.C.E.) Aristotle is a towering figure in ancient Greek philosophy, making contributions to logic, metaphysics, mathematics, physics, biology, botany, ethics, politics, agriculture, medicine, dance and theatre. He was a student of Plato who in turn studied under Socrates. He was more empirically-minded than Plato or Socrates and is famous for rejecting Plato's theory of forms. As a prolific writer and polymath, Aristotle radically transformed most, if not all, areas of knowledge he touched. It is no wonder that Aquinas referred to him simply as "The Philosopher." In his lifetime, Aristotle wrote as many as 200 treatises, of which only 31 survive. Unfortunately for us, these works are in the form of lecture notes and draft manuscripts never intended for general readership, so they do not demonstrate his reputed polished prose style which attracted many great followers, including the Roman Cicero. Aristotle was the first to classify areas of human knowledge into distinct disciplines such as mathematics, biology, and ethics. Some of these classifications are still used today. As the father of the field of logic, he was the first to develop a formalized system for reasoning. Aristotle observed that the validity of any argument can be determined by its structure rather than its content. A classic example of a valid argument is his syllogism: All men are mortal; Socrates is a man; therefore, Socrates is mortal. Given the structure of this argument, as long as the...
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...solution. The Kb for N2H4 is 4.0x10-6M. (2%) 6. An aqueous solution of aniline of concentration 0.24M is prepared. What concentration of sodium hydroxide is needed in this solution so that anilinium ion concentration remains 1x10-3M? (Ka for C6H5NH3+ =2.4x10-5M) (10-2M) 7. An aqueous solution contains 10% ammonia by mass and has a density of 0.99g cm-3. Calculate hydroxyl and hydrogen ion concentration in this solution.(Ka for NH4=5.0x10-10M) (9.28x10-13 mol L-1) CALCULATION OF pH 8. Calculate pH value of (a) .00001M HCl solution, and (b) 0.04M HNO3 solution assuming complete dissociation in each case. (4)(1.398) 9. Calculate the hydrogen ion concentration in moles/liter of a solution whose pH is 5.4 (3.98x10-6mole/liter) 10. Will the pH of water be same at 4oc and 25oC? Explain? 11. Saccharin...
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...University of Phoenix Material What Is Life? Read each statement. Write a 100-word summary explaining how that media piece supports that statement and include reference citations. 1. Find a media piece—article, video, presentation, song, or other—related to the scientific method, creating hypotheses, or designing experiments. Include the link or reference citation for the piece and describe how it helped you better understand how the scientific method is used to create hypotheses and experiments. [pic] 2. Find a media piece—article, video, presentation, song, or other—that recognizes the fundamental concepts of chemistry in biology. Include the link or reference citation for the piece and describe how it helped you better understand how fundamental concepts of chemistry affect biology. [pic] 3. Find a media piece—article, video, presentation, song, or other—that describes the energy metabolism of cells. Include the link or reference citation for the piece and describe how it helped you better understand the energy metabolism of cells. [pic] 4. Find a media piece—article, video, presentation, song, or other—that compares structures and functions of different cell types. Include the link or reference citation for the piece and describe how it helped you better compare structures and functions of different cell types...
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...Abstract: This paper describes the ideal gas law, and the difference between non-ideal and ideal gases. The ideal gas law describes the state of a gas’ condition at a given time, shown by its pressure, volume, temperature and number of moles. Knowledge of three of these properties is sufficient to complete the equation. This paper also includes other gas laws that either have been the foundation for the ideal gas law, or have been derived from it. An ideal gas is a gas which follows the ideal gas law, which in fact no gas does, but at high temperatures and low pressure non-ideal gases approach ideal behavior. Since the ideal gas law cannot release precise results on non-ideal gases, an equation has been derived which proves to be more useful when dealing with non-ideal gases. The Van der Waals equation takes account of the intermolecular attraction- and repulsive forces, and describes the behavior of non-ideal gases. In the conclusion of this paper it is shown that gases at low pressure and high temperature will show the behavior of an ideal gas, and fulfill the ideal gas law, but no gases are in fact ideal gases. Indhold Abstract: 1 Indledning: 1 Gaslovene og idealgas: 2 Real Gas: 4 Forsøg: ”Bestemmelse af molarmassen for lightergas” 6 Konklusion: 8 Litteraturliste: 8 Indledning: Gas er en tilstandsform, som alle stoffer kan antage. Derudover findes der tilstands former for flydende og fast stof. Tilstandsformerne kendetegnes på hvor stærke deres brownske...
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...CH 111: General Chemistry Dr. Ananda M The University of Dodoma, Tanzania Teaching Compendium on General Chemistry (CH 111) by Dr. AnandaMurthyM.Sc., M.Phil., Ph.D. Department of Chemistry, School of Physical Sciences, College of Natural &Mathematical Sciences, The University of Dodoma. UDOM- Study Material 2013-14 Page 1 CH 111: General Chemistry Dr. Ananda M Preface The importance of learning chemistry cannot be overemphasized. In this regard, all branches of chemistry contribute to the overall role that chemistry plays in daily life. The course content of CH 111 is designed to bridge the gap between the high school and the undergraduate chemistry, with respect to some fundamental topics in chemistry for first year chemistry students. This compendium will be helpful to the students, due to its relevance to the course content and will promote better understanding of the subject matter. It is intended to enable students to achieve the learning objectives and learning outcomes of CH 111 by being a quick reference to learners. The author of the compendium has presented the contents in a simplified manner by using various illustrations, including structures, tables, figures, and other relevant information to help the learner understand easily. This compendium will, to greater extent, help in understanding the basic concepts in chemistry. Dr. J.J. Makangara Senior Lecturer, Department of Chemistry, Former Dean, School of Physical Sciences, College...
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...CHM 1101 Introductory Chemistry Dawn Fox Medeba Uzzi August, 2007 Compiled and edited by Medeba Uzzi Authors’ Note This document is an initiative by the authors in an attempt to deal with what they think may be one of the reasons contributing to the relatively high failure rate in the introductory Chemistry course (CHM 1101) at the University of Guyana. It was brought to our attention that many first year students taking CHM 1101 are unable to efficiently cope with the frenetic pace of the Semester system and even less able to deal comprehensively with the large content in CHM 1101. It is hoped that by providing this paper, students will not need to make lots of notes in lectures and so they can focus on grasping the concepts taught. The document is meant to be a guide to the topics covered in CHM 1101 and is by no means exhaustive. Students are still required to attend classes regularly and punctually and to engage meaningfully in lectures and tutorials. Further, supplemental reading of these topics in any good General Chemistry text is expected. Dawn Fox Medeba Uzzi 2 SECTION 1 – Modules A – D: section deals with the foundation for chemistry. It introduces students to matter & its classification, Atom & its structure, Periodic table and chemical rxns. Introduction to Science and Measurement What is Chemistry? – Chemistry is the study of matter and its transformations Natural sciences refer to the systematic study of the natural world (our...
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...Introduction to Chemistry I (MAE1106) Chapter 1: Properties, Measurement and Units Matter: All things we can see, or touch, whether books, pencils, telephones, or people as they have some thing in common. They are all composed of matter which is defined as anything that takes up space and has mass. Matter is generally considered to be a substance (often a particle) that has rest mass and (usually) also volume. Mass and weight are not really the same. The mass of a body is a measure of its resistance to a change in its velocity. Weight refers to the force with which an object of a certain mass is attracted by gravity to the earth or other body that may be near such as moon. The volume is determined by the three-dimensional space it occupies, while the mass is defined by the usual ways that mass is measured. Matter is also a general term for the substance of which all observable physical objects consist Properties of Substances Physical (Properties and Changes) A physical property is one that is displayed without any change in composition. (Intensive or Extensive) 1. Intensive: A physical property that will be the same regardless of the amount of matter. density: m/v • color: The pigment or shade • conductivity: electricity to flow through the substance • malleability: if a substance can be flattened • luster: how shiny the substance looks 2. Extensive: A physical property that will change if the amount of matter changes. • mass: how much...
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...Atoms, Molecules and Ions. AN ATOM is the smallest particle of an element. They cannot be split into smaller particles in chemical reactions. Iron is made of iron atoms (Fe). Sulphur is made of sulphur atoms (S) A MOLECULE is a small group of atoms joined together. The atoms may be the same (e.g. O2) or different (e.g. H2O). The chemical formula shows the number and type of atoms present. Non-metal compounds are made of molecules: Carbon dioxide contains CO2 molecules Methane (natural gas) contains CH4 molecules AN ION is an atom or group of atoms with an electrical charge (+ or -). Metal compounds such as sodium chloride or copper sulphate contain ions. Sodium chloride is made of Na+ and Cl- ions Copper Sulphate is made of Cu2+ and SO42- ions Note that metals form positive ions while non-metals form negative ions. A solid is represented by (s). e.g. H2O(s) is ice. A liquid is represented by (l) e.g. Fe(l) is molten iron. A gas is represented by (g) e.g. H2O(g) is steam. A solution in water is represented by (aq). Salt dissolved in water is NaCl(aq). You should remember that the common gases are diatomic (have 2 atoms in each molecule). These are Oxygen O2; Hydrogen H2; Nitrogen N2; and Chlorine Cl2. Elementary Particles Atoms are made up of smaller particles called protons, neutrons and electrons. The protons and neutrons cluster together in a small nucleus at the centre of the atom while the electrons orbit the nucleus. The main properties...
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