Chemistry: A Molecular Approach (Tro) Chapter 10 Chemical Bonding II: Molecular Shapes‚ Valance Bond Theory‚ and Molecular Orbital Theory 1) Determine the electron geometry (eg) and molecular geometry(mg) of BCl3. A) eg=trigonal planar‚ mg=trigonal planar B) eg=tetrahedral‚ mg=trigonal planar C) eg=tetrahedral‚ mg=trigonal pyramidal D) eg=trigonal planar‚ mg=bent E) eg=trigonal bipyramidal‚ mg= trigonal bipyramidal Answer: A 2) Determine
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Reactions • Oxidation number: The charge that an atom in a molecule would develop if the most electronegative atoms in the molecule took the shared electrons from the less electronegative atoms. • Oxidation numbers are not real; they are only based on assumptions. They are useful bookkeeping tools though‚ and can help us keep track of electrons during a reaction. • The sum of all oxidation numbers in a molecule must equal the charge of that molecule. • Rules 1-4 about oxidation numbers: what’s nice about
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objective of this experiment is to conduct a free radical reaction and measure the ratio of products through a GC analysis. Free radical reactions are important to understand because they allow chemists to design synthesis of complex molecules from very simple organic molecules. The reagents used were 2‚3-dimethylbutane as the carbon chain‚ t-butyl peroxybenzoate as the initiator‚ and sulfuryl chloride as the source of chloride radicals. The predicted products are 1-chloro-2‚3-dimethylbutane and 2-chloro-2
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Copy the following questions into your assessment document. You may copy and paste the table‚ or create a similar table in the document.) After completing the molecular models‚ fill in the table below: (18 points) Molecule What is the central atom of this molecule? Number of lone pairs on the central atom Number of atoms bonded to the central atom Molecular geometry Bond angle (based on VSEPR theory) CCl2F2 C Zero 4 Tetrahedral 109 degrees HCN C Zero 2 Linear 180 degrees
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distribution is affected based on the individual’s age‚ sex‚ muscle/adipose tissue ratio‚ state of hydration‚ genetic heritage‚ and health (Doweiko‚ 2009). Once the drug molecules are distributed they reach circulation and can be carried to the site of action. However‚ the drug molecule acts as a foreign substance to the body so the way the molecule transports varies depending on how the body
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? Heat of formation of potassium chloride K(s) + ½ Cl2(g) → KCl(s) -437 a) -1537 kJ b) -663 kJ e) -717 kJ c) -157 kJ d) -839 kJ 8. Choose the bond below that is most polar. c) H-F d) H-Cl b) H-Br a) H-I e) C-H 9. Which molecule or compound below contains a polar covalent bond? a) C2H4 d) NCl3 b) ZnS c)
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Chapter 2 Extra Credit 1. The diffirence between atoms and molecules is that atoms are the smallest units of matter and can not be divided by chemical means. Molecules are made up of atoms of the same kind that are together in a group. The difference between covalent bonds and ionic bonds are that covalent bonds have 2 atoms sharing the same electron. Ionic bonds occur when an atom takes one electron away from another atom. 2. Adhesion and Cohesion differ because adhesion is when 2 substance
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circumstances under which each forms. Ch 3.3 “Ion Formation” “Covalent Bonding” “Polarity in Water Molecules and Hydrogen Bonding” How Atoms Bond; Examples of Hydrogen Bonds http://www.youtube.com/watch?v=QqjcCvzWwww&list=PL3FE5B87E56E7A849&index=3 10 Describe the atomic components and their bonding in water molecules as an example of a compound having polar covalent bonds. Ch 3.3 “Polarity in Water Molecules and Hydrogen Bonding”
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Cohesion is the bond between two of the same substances. A hydrogen bond is a type of cohesion in water in which the hydrogen atoms of one water molecule being attracted to the oxygen atom of another water molecule. In water‚ each molecule in the middle is pulled equally in every direction by neighboring molecules. The cohesion forces between water molecules at the surface of water is surface tension. The cohesion forms a “film like” layer on the surface of water. Some substances may reduce the cohesion
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which the molecules merge as an outcome of their spontaneous movement or randomized motion of kinetic energy. It is when two chemical species react together at every encounter (combining or merging of the two species for a number of subsequent collisions in solution) and chemical change take place as fast as the reactants can diffuse together (Reichardt‚ 1988). It may occur in solids‚ liquids‚ or gasses. It depends on many factors like temperature‚ molecular weight‚ concentration of molecules in the
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