Chemistry PreAP Homework Packet COVALENT BONDING Name: Period: Chemistry Teacher: 1
Name Per.. Donic / Metallic / Covalent Bonding? Use vour covalent bonding notes to classifv the following as characterktics of a substance that contains ionic (I), metallic tm) or covalent (C) bondilÿg. 1, Contains a metal and a nonmetal ion (and possibly polyatomic ions) 2, Contains nonmetals and possibly metalloids 3, The smallest particle is the formula unit _o 4. The smallest particle is the molecule 5, Electrons are described as a mobile "sea" 6. Particles are held together by strong electrostatic forces 7, Particles are held together by relatively weal{ intermolecular forces 8, The elements in the compound share valence electrons 9, The elements in the compound gain and lose valence electrons 10, Are usually soluble in water 11. High thermal and electrical conductivity in their pure states 12. Are electrolytes when dissolved in water or molten (liquid) 13, Have low melting and boiling points 14. Have high melting and boiling points 15. Often exist as gases or vaporize easily at room temperature 16. Are crystalline solids at room temperature 17, Are soft if solid 18. Are lustrous, malleable, and ductile 19, Are hard, rigid and brittle 20, An example is MgCl2 2.1, An example is CCI4 22, Its structure looks like this: 23, Its structure looks like this: 24. Its structure looks like this:!,t ',ÿ',ÿ'ÿ;iÿ',;j2ÿ' 2
Name: Date: Period: Lewis Structures Practice Worksheet Draw the Lewis structures for the following compounds: 1) PBr3 2) N2H2 3) CH3OH (methanol) 4) nitrite ion 5) C2H4 6) phosphiteion 7) HBr 3
8) C2H5OH (ethanol) 9) N2F4!0) 02H2 Draw all of the possible resonance structures for the following ions or molecules: 11) nitrate ion: 12) formate ion (CliO2 -): 13) cyclobutadiene (04H4): 14) ozone (03): 4
Name Per. Moleeullar Geometry Worlcÿheeÿ (VSEF R) Draw the Lewis structure for each molecule or ion and then determine the geometry (shape). Molecule or IIon Lewis Structure -- Molecular Geometry 1. or Structural Formula (e.g. tetrahedra!, eÿco) SO3 2. SO3 2-3. SC12 4. PH3 5. SO2 6, NO3-7o CC14 8. CO2 5
Name Per, Deterrainiÿg Poÿarfiÿy of IVÿoÿecÿles J, Lewis Strÿcture }ÿoÿecaÿar Geometry (ÿcÿde 3D sketch of edeÿ w/dÿp_ÿesÿ Polar or No;tpolar? PH3, Nÿ3, CBr4, SO2, HCN 6ÿ B onds: BF3 6
Study Guide: Chemical Bonding. Define chemical bond, What electrons are involved in chemical bonding? 2, Explain the reason for chemical bonding in terms of stability and energy.. Bonds that involve the transfer of electrons are that involve the sharing of electrons are electrons roam fi'eely between multiple nuclei are bonds; bonds bonds, and bonds where bonds, 4ÿ Ionic bonds exist between and.5. Use electron dot diagrams to depict the formation of a) barium iodide b) cesium phosphide c) aluminum oxide 6, List 3 unique properties of ionic compounds. 7, List 3 unique properties of metals, 8. List 3 unique properties of molecular compounds. 9. A covalent bond involves a chemical bond between 2 atoms that are electrons. When atoms share electrons, each achieves a complete most atoms). Typically, covalent bonds involve what type(s) of elements? (for :[0. What is the definition of a single, double, and triple bond? 11. Provide an example of a compound for each type of bond in the previous question. 12. All diatomic elements form bonds. Diatomic elements include., and (ionic/polar covalent/nonpolar covalent) 1 '! t 13. structures depict the bonding in a molecule. The first step in drawing these structures is determining the number of in the molecule. 7
!4. When it is possible to write 2 or more valid Lewis structures for a rnolecule or ion, it is called. An example of a molecule or ion that shows this is Draw the resonance forms below:!5. Draw the Lewis structure for: water, sulfur dioxide, carbon tetraiodide, carbon monoxide, nitrite ion, carbon dioxide, ammonia, ethene (C2H4) and phosphate ion. 16. The theory states that because electron pairs shapes adjust so the valence electron pairs are as far apart as possible.., molecular!7. Determine the geometry or shape of each molecule or ion in #15. For ethene, determine the geometry around each carbon atom. 18. The degree of polarity of a bond between any two atoms can be determined by determining the difference in 19. A bond is considered nonpolar covalent if the electronegativity difference between the two atoms is ; polar covalent if the electronegativity difference is. and ionic if the electronegativity difference is ÿ ÿ_. ' 20. Ionic, nonpolar covalent, or polar covalent bond? a) H-P b) H-O c) LioF d) C-I e) P-Cl 21. (1) Draw Lewis structures for each molecule and determine its shape. (2) Draw a structural formula that shows the correct shape for each molecule and indicate the dipoles with arrow notation. (3) Determine whether the molecule is polar or nonpolar overall. a) NH3 b) CF4 c) C02 8