Unit 3- Chemical Bonding Study Guide

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Unit 3- Chemical Bonding Study Guide CHEMICAL BNDS 1. How are atoms held together? What is the attraction between? 2. What are the three characteristics of atoms that contribute to bonding? Explain each. 3. What is a solute? What is a solvent? Give an example of each. 4. For each of the 4 different types of bonds, explain the following a. Bond name b. What kinds of atoms are held together c. What is happening with the valence electrons in the bond d. Will the substance conduct electricity or dissolve in water? INIC BNDING 1. Explain what is happening in an ionic bond in terms of valence electrons, electronegativity, and ionization energy. 2. What is an electrostatic force? 3. Draw an example of a picture of an ionic bond between a metal and nonmetal. 4. What is noble gas envy? 5. What is an ion? What are the two types of ions? Explain their differences. 6. Fill in the following chart: Group #A # valence e- Lose/gain e-? xidation #? Type of ion? I A II A III A IV A V A VI A VII A VIII A 7. What type of ion do metals become? Nonmetals? 8. Does chemical bonding change the identity of the atoms? 9. What is a crystal lattice? Why do ionic compounds form a crystal lattice structure? Draw a picture of NaCl in a crystal lattice. INIC FRMULAS & NAMES 1. Explain how you figure out the chemical formula for an ionic compound. 2. Fill in the following chart: Element 1 (metal) Na # of valence electrons Charge of Element 1 Element 2 (nonmetal) # of valence electrons Charge of Element 2 Compound & Name

Mg Sr Be Ba Ca Li K Al Ga In Al Ca F Br Cl I Se Br N F S Rb (P 4 ) Ga (S 3 ) 3. What are polyatomic ions? 4. List ALL 11 polyatomic ions by name AND formula (with charge). 5. List the 5 steps for naming ionic compounds. 6. Write the correct name for the following compounds: a. Fe 2 (S 3 ) 3 b. RbI c. Na 3 P 4 d. CuCl 2 e. Ti 3 P 2 CVALENT BNDING 1. Explain in detail what a covalent bond is. 2. What is a molecular formula? Give two examples. 3. What is a structural formula? Draw the structural formulas for the two example molecular formulas in questions #2. 4. Explain the HNC 1234 rule. 5. Explain in detail how an atom can have more than one bond with another atom.

6. What are isomers? Draw two examples of isomers. 7. What are Lewis Dot Structures? Draw the Lewis Dot Structure for carbon, phosphorous, sulfur, and iodine. 8. Write a detailed explanation of the ctet Rule. 9. What is the mathematical formula for the number of covalent bonds a nonmetal will form? 10. How many dots are shown in a Lewis Dot Structure for a single bond? Double bond? Triple bond? 11. List the 4 strategies to create Lewis Dot Structures. 12. Fill in the following chart: Molecular Formula Lewis Dot Structure Structural Formula 1. Si 2 H 6 2. C 2 F 4 3. C 2 Br 2 4. SiH 4 5. SiH 2 6. CH 5 P 7. CH 3 N 8. HCP 9. SiH 4 2 10. CH 2 2 11. CS 2

VSEPR 1. What types of e- pairs are in a molecule? 2. What does VSEPR mean? 3. What are electron domains? 4. How does VSEPR contribute to the shape of a molecule? 5. Fill in the following chart: Molecule SiH 4 Structure # e- domains # bonded pairs # lone pairs Shape Bond angle PH 3 H 2 S Si 2 CH 2 S CF 3 H ELECTRNEGATIVITY & PLARITY 1. What is polarity? 2. Why are some molecules polar? Explain in detail. 3. What are some properties of polar molecules? 4. What are some properties of nonpolar molecules? 5. Explain how electronegativity can help determine the bond type in a molecule. 6. Explain how you can tell if an entire molecule will be polar or nonpolar. 7. Describe how polarity is related to the sense of smell. 8. Give a detailed explanation of why water and oil don t mix. 9. What are intermolecular forces? 10. What are three types of intermolecular/ van der Waals forces? Give an example of each. 11. Fill in the following chart: Molecule CCl 4 Lewis Dot Structure (use ctet Rule) Structural Formula (use HNC 1234) Shape 1. sketch ball & stick model 2. Write name of shape 3. Show direction of all dipoles (e- pull) according to electronegativity difference Is the entire molecule Polar or Nonpolar? Can we smell it? Will it dissolve in water? Type of IMF? (Intermolecular Force)

H 2 CH 2 C 2 NH 3 HSiCl 3

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