What is the total number of bonds in the molecule? A) 0 B) 1/2 C) 1 D) 2 E) More information is needed. 3. What is the hybridization of I in the molecule ICl3? A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3 4. What is the hybridization of S in the molecule H2S? A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3 5. What is the hybridization of C in the ion CN-? A) sp B) sp2 C) sp3 D) dsp3 E) d2sp3 6. Atoms that are sp3 hybridized form ____ pi bond(s). A) 0 B) 1 C) 2 D) 3 E) 4 7. What
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It would have 6 neutrons and is a stable isotope. 7. Iconic bonds give or take an electron which make a very strong bond and are normally polar. Two elements when put together that make an iconic bond would be NaCi. 8. Covalent bonds are two elements that share their electrons they are also a very strong bond. Two elements that make a covalent bond would be H2O. 9. Electronegativity is when one of the atoms takes more of its share of electrons; this
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Draw an arrow-pushing mechanism for the following reaction. [pic] [pic] The methanol attacks from the back side of the cyclic bromonium ion, since the Br is blocking the front side from attack. b. This is two additions of H-Cl to a pi-bond, one after the other. [pic] [pic] [pic] 4. Give IUPAC names for the following structures |a. |[pic] |b. |[pic] | |
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University of Phoenix Material Week 4 Exercises Prepare written answers to the following exercises: 1. Imagine that you are an environmental scientist. Working in collaboration with a university chemist, you were able to determine from mass spectrometry that four elements exist in your soil samples. They are Se, Sn, Pb, and Cd. You need to determine which elements will most likely combine with oxygen to produce oxides that are present in your sample. To do so, refer to the periodic
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Written Assignment 1: Intermolecular Forces and Liquids and Solids Answer all assigned questions and problems, and show all work. 1. Explain and give an example for each type of intermolecular force. A: a. Dipole-dipole interaction: a dipole-dipole interaction is the electrostatic attraction between the positive end of one polar molecule and the negative end of the other. Dipole-dipole attraction occurs between molecules which are permanent dipoles (polar covalent molecules). An example
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SCI Ch.1 – Ch.10 Outline Ch. 1 The scientific law describes an important relationship that is observed in nature to occur consistently time after time. A model is a description of a theory or idea that accounts for all known properties. The steps in the scientific method includes 1. Observation 2. Question 3. Background research 4. Hypothesis 5. Methods 6. Equipment 7. Experiment; collect data 8. Results; analyze results 9. Conclusions 10. New hypothesis. A hypothesis should start with
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chapter and the next, we examine chemical bonding in detail. We examined ionic bonding briefly in Chapter 2 and will do so in more detail in Chapter 11. We will also examine intermolecular forces in detail in Chapter 11. Here we will apply what you have learned about atomic structure (Chapter 6), electron configurations, and periodic trends (Chapter 7) to the chemical bonds formed between atoms and ions and the shapes of molecules and ions that contain covalent bonds. • 8-1 Biology: Molecular shape
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CHEMISTRY CHEMISTRY (CLASSES XI–XII) Rationale Higher Secondary Stage is the most crucial stage of school education because at this stage specialised discipline based, content oriented courses are introduced. Students reach this stage after 10 years of general education and opt for Chemistry with a purpose of mostly for pursuing their career in basic sciences or professional courses like medicines, engineering, technology and studying courses in applied areas of science and technology at tertiary
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Kevion Young General Chemistry II Lab Zakita Jones February 25, 2014 –March 25, 2014 Labs # 3 and 4 Title: Chemical Bonding Lewis Structures and Shapes of Molecules and Ions References/Tools: 1. Chapter 9: Models of Chemical Bonding 2. Chapter 10: The Shapes of Molecules 3. The Modern Periodic Table 4. Electron Configuration (SPDF notation, Orbital diagram), Lewis Symbols, Lewis Structures, Molecular
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Single Bonds The atoms share a pair of electrons, and that pair is referred to as a bonding pair. The pairs of electrons which do not participate in the bond have traditionally been called "lone pairs". A single bond can be represented by the two dots of the bonding pair, or by a single line which represents that pair. The single line representation for a bond is commonly used in drawing Lewis structures for molecules. · Hydrogen atoms form one bond. · Carbon atoms four bonds. ·
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