6.1 Intro to Chemical Bonding Name:
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1 6.1 Intro to Chemical Bonding Name: A. Chemical bond Favored by nature because: 3 main types of bonds B. Ionic Bonds C. Covalent Bonds D. Metallic Bond E. Bond Determination RECALL: Electronegativity Electronegativity Difference Bond Type 1
2 Polar covalent bond Nonpolar covalent bond Sample Problem A Use electronegativity values listed below to classify bonding between sulfur, S, and the following elements: hydrogen, H; cesium, Cs; and chlorine, Cl. In each pair, which atom will be more negative? S: 2.5 H: 2.1 Cs: 0.7 Cl: 3.0 Bonding between S and: Electronegativity difference Bond type More negative atom H Cs Cl 2
3 6.2.I Covalent Bonding Name: A. Molecular Compounds Molecule Molecular compound Chemical formula Molecular formula o Oxygen molecular formula = o Water molecular formula = o Sucrose molecular formula = B. Covalent Bond Formation C. H 2 Covalent Bond Formation a) b) c) d) D. Covalent Bond Characteristics Bond energy Bond length 3
4 Relationship between bond energy and length Covalent Bond Characteristics E. Multiple Covalent Bonds Double covalent bond Triple covalent bond Bond length and energy F. Covalent Network Solids 4
5 6.2.II Octet Rule & Lewis Structures Name: A. The Octet Rule Octet Rule Exceptions o o o Hydrogen Boron Main-group elements in Periods 3 and up B. Electron dot notation Electron-dot notation Sample Problem B a. Write the electron-dot notation for hydrogen. b. Write the electron-dot notation for nitrogen. C. Lewis Structures Unshared pairs of electrons (aka lone electrons) Structural formula D. Lewis Structure Rules
6 Sample Problem C: Draw the Lewis structure of iodomethane, CH 3 I. 1. Determine the type and number of atoms in the molecule. 2. Write the electron-dot notation for each type of atom in the molecule. 3. Determine the total number of valence electrons available in the atoms to be combined. 4. Arrange the atoms to form a skeleton structure for the molecule. If carbon is present, it is the central atom. Otherwise, the least-electronegative atom is central. Hydrogen, is never central. 5. Add unshared pairs of electrons to each nonmetal atom (except H) such that each is surrounded by eight electrons. Sample Problem D: Draw the Lewis structure for methanal, CH 2 O (aka formaldehyde). 1. Determine the type and number of atoms in the molecule. 2. Write the electron-dot notation for each type of atom in the molecule. 3. Determine the total number of valence electrons available in the atoms to be combined. 4. Arrange the atoms to form a skeleton structure for the molecule. Connect the atoms by electron-pair bonds. 5. Add unshared pairs of electrons to each nonmetal atom (except H) such that each is surrounded by eight electrons. 6. Count the electrons in the Lewis structure to be sure that the number of valence electrons used equals the number available. Subtract one or more lone pairs until the total number of valence electrons is correct. Move one or more lone electron pairs to existing bonds until the outer shells of all atoms are completely filled. 6
7 6.3 Ionic Bonding Name: A. Ionic Bonds Ionic compound o Crystalline solids Comparison to molecular compounds Formula unit (ionic formula) B. Ionic Bond Formation C. Ionic Bond Characteristics Lattice energy D. Ionic vs Covalent Bonding 7
8 E. Ionic vs Covalent Compounds Physical properties depend on: Physical Property Ionic Compound Molecular Compound Hardness Melting point Boiling point Solubility in H 2 O Conductivity Types of elements F. Polyatomic Ions 8
9 6.4 Metallic Bonding Name: A. Metallic Bonding Delocalized Sea of electrons B. Metallic Properties Electrical conductivity Thermal conductivity Malleability Ductility Luster o Caused by: C. Property Comparison 9
10 Metallic Ionic Compound Molecular Compound Covalent Network Solid Bonding Melting point / phase Conductivity Crystalline arrangement Solubility in H 2 O Example 10
11 6.5.I Intermolecular Forces Name: A. Intermolecular Forces Boiling point of a liquid 3 types Dipole I. Dipole-dipole a. Hydrogen Bonding II. Dipole-Induced Dipole III. London Dispersion Forces 11
12 12
13 6.5.II Molecular Geometry Name: A. Molecular Geometry Molecular polarity VSEPR Theory Sample Problem E: Use VSEPR theory to predict the molecular geometry of boron trichloride, BCl 3. Sample Problem F a) Use VSEPR theory to predict the shape of a molecule of carbon dioxide, CO 2. b) Use VSEPR theory to predict the shape of a chlorate ion, ClO 3-13
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