Lewis Structures and the Shapes of Molecules Pre-Lab Assignments: To be assigned by your lab instructor. Student Learning Outcomes: Learn how to draw Lewis structures. Learn how to draw Lewis structures for atoms which violate the octet rule. Learn how to use Lewis structures and VSEPR and to predict the shapes of molecules. Learn how to use the shape of a molecule to predict whether or not it is polar. Experimental Goals: The purpose of this lab is to learn how to draw Lewis
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Mohammed and Lambert ( New edition) Chapter 8 pg 123 Anne Tindale Chapter 10 pg 46 The following topics will be covered : 1. Definition of Relative Atomic and Relative Molecular Masses. 2. Calculation of Relative Molecular Masses 3. Converting Moles to Grams / Grams to Moles 4. Calculation from equations Masses of substances /Volumes of gases / Concentration of solutions (Practical :Volumetric Analysis ) 5. % Composition 6. Empirical Formulae
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Final Exam Review Chapter 2 Study Questions 1. Define the following a) element b) compound c) pure substance 2. Classify each of the following as a pure substance or a mixture. For each pure substance‚ indicate whether it is an element or a compound. Which of the mixtures are solutions a) air b) titanium c) oak d) baking soda e) oxygen f) 7-Up g) wine h) carbon monoxide 3. Label each of the following drawings as element‚ compound‚ or mixture (Assume each type of circle
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HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers |Chapter 25 Simple molecular substances with non-octet |Page Number | |structures and shapes of simple molecules | | |Class Practice |1 | |Chapter Exercise
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xam 2 [pic] Summer 2011 Chemistry 1411 EXAM # 2 Activity Series of Metals in Aqueous Solution [pic] CHEM 1411 Exam # 2A Name:________________________________ (Chapters 4‚5‚6‚ and 7) Score: [pic] Part I- ( 3 points each) - Please write your correct answer next to each question number‚ DO NOT CIRCLE. ____ 1. Compare the rates of effusion of CO2 & SO2‚ rCO2/rSO2 A. CO2 will effuse 1.45 times
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Core Module 1: The Chemical Earth Contextual Outline The Earth includes a clearly identifiable biosphere‚ lithosphere‚ hydrosphere and atmosphere. All of these are mixtures of thousands of substances and the use of this pool of resources requires the separation of useful substances. The processes of separation will be determined by the physical and chemical properties of the substances. In order to use the Earth’s resources effectively and efficiently‚ it is necessary to understand the properties
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hydrocarbons are complex. During this process‚ active hydrogen atoms and hydrocarbons fragments are formed. These fragments can combine with each other to form gasses such as Hydrogen (H2)‚ Methane (CH4)‚ Acetylene (C2H2)‚ Ethylene (C2H4)‚ Ethane (C2H6) and many more. The gasses listed are considered combustible. The rate at which each gas are produced depends on the temperature. Therefore‚ the concentration of the individual dissolved gasses found in transformer insulating oil may be used directly
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properties of substances are explained by the arrangement of the atoms‚ ions‚ or molecules of the substances and by the strength of the forces of attraction between the atoms‚ ions‚ or molecules. C4.4: Molecular Polarity The forces between molecules depend on the net polarity of the molecule as determined by shape of the molecule and the polarity of the bonds. C5.4: Phase/Change Diagrams Changes of state require a transfer of energy. Water has unusually high-energy changes associated with its changes of state
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IONIC COMPOUNDS In chemistry‚ an ionic compound is a chemical compound in which ions are held together in a lattice structure by ionic bonds. Usually‚ the positively charged portion consists of metal cations and the negatively charged portion is an anion or polyatomic ion. Ions in ionic compounds are held together by the electrostatic forcesbetween oppositely charged bodies. Ionic compounds have high melting and boiling points‚ and they are hard and very brittle. Ions can be single atoms‚ as the sodium and chlorine in
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Equations of State (EoS) Equations of State • From molecular considerations‚ identify which intermolecular interactions are significant (including estimating relative strengths of dipole moments‚ polarizability‚ etc.) • Apply simple rules for calculating P‚ v‚ or T ◦ Calculate P‚ v‚ or T from non-ideal equations of state (cubic equations‚ the virial equation‚ compressibility charts‚ and ThermoSolver) ◦ Apply the Rackett equation‚ the thermal expansion coefficient‚ and the isothermal compressibility
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