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1、1,CHM 211 (Organic Chemistry) Summer 2010,Dr. Ned H. Martin Office: Dobo 242E Telephone: 962-3453 (campus) Email: martinnuncw.edu,2,Texts,Organic Chemistry, 7th edition, McMurry Optional Study Guide and Solutions Manual for McMurrys Organic Chemistry, 7th edition Molecular model kit Course Website (
2、Syllabus, Grading Policy): http:/www.uncw.edu/chem/Courses/Martinn/chm211martin/index.htm,3,Grading Policy,Four 40-minute tests, each worth 60 points. The final exam will consist of six sections. The first four are like the four tests; the higher grade counts. Section 5 is new material (since the la
3、st test). Section 6 is comprehensive. You may take (or not) as many of the first four sections as you want. Everyone must take sections 5 and 6. There will be no make up exams. Each of the tests may include at least one problem from the homework assignments. Tests 2- 4 may contain one review questio
4、n from the previous test. 93%=A, 90%=A-, 87%=B+, 84%=B, 80%=B-, etc.,4,Attendance & Homework,Attendance is expected, but not officially monitored for grading purposes. Missing 1 day in the summer is like missing 1 week during a regular semester! Homework problems are assigned, but not collected. Act
5、ively working the homework problems allows you to test whether you understand the material and serves as a review guide for the exams.,5,Keys to Success in CHM 211,Memorization alone is not sufficient. Reasoning alone is not sufficient. Study three times: Before the lecture After the lecture Before
6、the test Actively do problems (Keep a notebook). Cooperate form study groups.,6,What is Organic Chemistry?,The study of carbon-containing compounds Important because: Carbon forms 4 bonds, and can bond to itself in long chains Carbon has three different geometries giving rise to a variety of structu
7、res Carbon bonds strongly to other common elements: O, N, Cl, etc. Organic compounds have many applications and uses: dyes, medicines, fabric, plastics, food (protein, carbohydrates, fats, oils), fuel, pesticides, paint, preservatives, hormones, etc. This PowerPoint covers: Chapter 1. Structure and
8、Bonding,7,C (Carbon),Carbons atomic number = 6, therefore it has 6 protons in its nucleus. A neutral atom of 12C has 6 protons, 6 neutrons and 6 electrons; its amu = 12 ( = 6p + 6n) A neutral atom of 13C has 6 protons, 7 neutrons and 6 electrons; its amu = 13 ( = 6p + 7n) A neutral atom of 14C has ?
9、 protons, ? neutrons and ? electrons; its amu = ? ( = ?p + ?n) Carbons atomic weight = 12.011; this is a weighted average of the three isotopes: 12C, 13C, and 14C.,8,Parts of an Atom,Protons (+ charge) and neutrons (0 charge) are in the center or nucleus of the atom Electrons (- charge) are consider
10、ed to be a cloud of charge around the nucleus. Orbitals describe where the electrons are. Electrons have very little mass compared to protons and neutrons. Electrons are found in s orbitals (spherical), p orbitals (dumbbell), or d orbitals (various shapes) Electrons are grouped in different layers o
11、r shells.,9,1.1 Atomic Structure,Structure of an atom Positively charged nucleus (very dense, protons and neutrons) and small (10-15 m) Negatively charged electrons are in a cloud (10-10 m) around nucleus Diameter is about 2 10-10 m (200 picometers (pm) the unit Angstrom () is 10-10 m = 100 pm,10,1.
12、2 Atomic Structure: Orbitals,Quantum mechanics: describes electron energies and locations by a wave function, A plot of 2 describes the region where electrons are most likely to be An electron cloud has no specific boundary so we represent its shape by the region of highest probability of finding an
13、 electron. Solutions of the wave equation give rise to regions of electron density on each atom of specific shapes (atomic orbitals),11,Shapes of Atomic Orbitals,Four different kinds of orbitals occupied by electrons Denoted s, p, d, and f (listed in increasing energy) s and p orbitals are most impo
14、rtant in organic chemistry s orbitals: spherical, with the nucleus at center p orbitals: dumbbell-shaped, with the nucleus at the center,12,p-Orbitals,There are three perpendicular p orbitals, px, py, and pz, of equal energy Lobes of a p orbital are separated by region of zero electron density, call
15、ed a node.,13,1.3 Atomic Structure: e- Configuration,The lowest energy electron configuration of an atom of any element can be predicted by following three rules: The aufbau principle: Electrons are filled into the lowest energy orbitals first (1s, then 2s, then 2p, then 3s, then 3p, then 4s, then 3
16、d) The Pauli exclusion principle: Only two electrons may occupy an orbital; they must have opposite spin orientations. Hunds rule: If there are two or more equal energy (degenerate) orbitals available, the electrons will spread out among the orbitals with parallel spins, only pairing up after the orbitals are half-filled.,14,Examples of Electron Configuration,15,1.4 The Nature of the Chemical Bond,Atoms form bonds because the compound that results is more stab
