of interactions between molecules. We have to draw Lewis structures during this lab. Describe single‚ double and triple bonds. We also must predict the structure of a molecule using the VSEPR theory. Materials: Balloons Colored Pencils Molecular Model Kit Procedures: Part 1 1. Blow up all of the balloons in the lab kit and tie them. 2. Blow the three blue ones up slightly larger than you do the five red balloons. 3. The blue balloons will represent the repulsive field
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Topic 10 Rate of Reaction Part A Unit-based exercise Unit 36 An introduction to rate of reaction Fill in the blanks 1 concentration; time 2 instantaneous 3 a) the gaseous product / carbon dioxide evolved b) loss in mass 4 a) colorimeter b) standard alkali c) the gaseous product / carbon dioxide evolved 1 time to reach the opaque stage 5 transmittance; 6 hydroxide; titrimetric True or false 7 T In the oxidation of methanoic acid by bromine‚ the intensity of the orange colour of bromine
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How do ionic compounds form? How do electrons change the shape of a molecule? These are just a couple of the questions that this paper will answer. How do ionic compounds form? Ionic compounds are formed by positive and negative ions. An ionic bond means that there are valence electrons being shared between the two molecules. This can cause the molecule to become negative or positively charged. An ionic compound is formed by the complete transfer of electrons from a metal to a nonmetal and the
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Gases Chapter 5 1 Elements that exist as gases at 250C and 1 atmosphere 2 3 Physical Characteristics of Gases • • • • Gases assume the volume and shape of their containers. Gases are the most compressible state of matter. Gases will mix evenly and completely when confined to the same container. Gases have much lower densities than liquids and solids. NO2 gas 4 Force Pressure = Area (force = mass x acceleration) Units of Pressure 1 pascal (Pa) = 1 N/m2 1 atm = 760
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HKDSE CHEMISTRY – A Modern View (Chemistry) Coursebook 3 Suggested answers Chapter 25 Simple molecular substances with non-octet structures and shapes of simple molecules Page Number Class Practice 1 Chapter Exercise 2 Chapter 26 Bond polarity Class Practice 4 Chapter Exercise 5 Chapter 27 Intermolecular forces Class Practice 7 Chapter Exercise 9 Chapter 28 Structures and properties of molecular crystals Class Practice 11 Chapter Exercise 12 Part Exercise 14 Chapter 29 Chemical cells in daily life
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ONE-SCHOOL.NET Short Notes: Form 5 Chemistry Rate or Reaction Calculation Rate of Reaction (Average Rate) Rates of reaction = Quantity change of reactants/products Total time for the reaction If the quantity change is immeasurable Rates of reaction = 1 Total time for the reaction Find the Rate From a Graph Average Rate Rates At an Instant The rate of reaction is equal to the slope of the graph The rate of reaction at an instant‚ t‚ is equal to the of quantity against
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Molecular Structure or "The Shape Molecules are In" Directions: Make a copy of this document and change the file name to “your last name‚ VSEPR Lab.” Place the document in the Google folder with your name on it. Follow each instruction to build molecular models and answer the following questions. Make sure your notes‚ comments‚ and answers are in a different text color. When you have finished with the lab questions attach a 12 page conclusion that summarizes and explains the main points of the lab
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Molecular Geometry A. Natural Orientation of Volumes about a Central Point. You will need 20 round balloons for this experiment. Join them together as indicated in the Balloon Arrangement column and then describe the shape in the space provided. Balloon Arrangement Description of the Shape Two-Balloon Set Linear Three-Balloon Set Trigonal Planar Four-Balloon Set Tetrahedral Five-Balloon Set Trigonal Bipyramidal Six-Balloon Set Octahedral B. Valence Shell Pairs: Single
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Electron pair geometry: This geometry includes all the electron pairs (bp + lp) around the central atom. Molecular geometry: This includes only placement of atoms (bp) in the molecule. When there is no lone pair in molecules the two geometries are same. PART C VSEPR Theory (Valence Shared Electron Pair Repulsion Theory) Syllabus: Various rules under VSEPR theory to explain molecular geometry (following examples may be taken to explain various rules- BeCl2‚ BF3‚ CH4 ‚ NH4+ ‚ PCl5 ‚ SF6‚
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Name Period Date Molecular Geometry – Ch. 9 For each of the following molecules‚ draw the Lewis Diagram and tally up the electron pairs. Then‚ identify the correct the molecular shape and bond angle. molecule lewis diagram e- tally shape bond angle 1. SeO3 2. AsH3 3. NO2 - 4. BeF2 molecule lewis diagram e- tally shape bond angle 5. SiH4 6. SeH2 7. PF5 8. SCl6 Name:
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