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Types of Chemical Bonds Academic Chemistry Unit 7: Properties of Covalent Compounds Textbook Readings and Homework: 6-1 Introduction to Chemical Bonding p. 161 - 163 6-2 Covalent Bonding & Molecular Compounds p. 164 – 175 7-1 Chemical Names and Formulas p. 211 – 215 EOC’s p. 195 # 9, 12, 13, 39, 41, 46, 64ab and p. 235 # 9-11 P 163 #3a,b,c p. 175 #2,3,4 p. 215 #4 f,g,h Vocabulary: Chemical Bond (6.1) Ionic Bonding (6.1) Covalent Bonding (6.1) Non-polar Covalent Bond (6.1) Polar Covalent Bond (6.1) Polar (6.1) Molecule (6.2) Molecular Compound (6.2) Chemical Formula (6.2) Molecular Formula (6.2) Diatomic Molecule (6.2) Bond Length (6.2) Bond Energy (6.2) Octet Rule (6.2) Electron-dot Notation (6.2) Lone Pair (6.2) Lewis Structures (6.2) Structural Formula (6.2) Single Bond (6.2) Double Bond (6.2) Triple Bond (6.2) Resonance (6.2) Molecular Polarity (6.5) Objectives: 1. 2. 3. 4. Relate the electron configuration of an atom to its chemical reactivity. Describe the process of forming a covalent bond. Describe the change in energy and stability that takes place as a covalent bond is formed. Distinguish between nonpolar and polar covalent bonds based on differences in electronegativity. 5. Draw Lewis structures to show the arrangement of valence electrons among atoms in molecules and polyatomic ions. 6. Explain the differences between single, double, and triple covalent bonds. 7. Name simple covalent compounds using prefixes, roots, and suffixes. Activities and Labs: 1. Lab: DHMO Research 2. Lab: Ionic vs Covalent 1 Classify the following compounds as ionic (Metal + nonmetal), covalent (nonmetal + nonmetal) or both (compounds containing a polyatomic ion) 1. CaCl2 11.MgO 2. CO2 12.NH4Cl 3. H2O 13.HCl 4. BaSO4 14.KI 5. K2O 15.NaOH 6. NaF 16.NO2 7. Na2CO3 17.AlPO4 8. CH4 18.FeCl3 9. SO3 19.P2O5 10.LiBr 20.N2O3 2 Covalent Bonding Covalent bonding occurs when two or more nonmetals share electrons, attempting to attain a stable octet of electrons at least part of the time. For example: xx H Cl xx xx Cl xx + x . .x xx H xx Remember that hydrogen is content with 2 electrons Show how covalent bonding occurs in each of the following pairs of atoms. Atoms may share one, two or three pairs of electrons. H + H (H2) F + F (F2) H + S (H2S) S + Br (SBr2) H + O (H2O) N + H (NH3) 3 Use the equations to correctly draw the Lewis Structure and Structural Formula for each of the following. N = number of bonding atoms except hydrogen. All Single Bonds One Double Bond One Triple Bond *Or Two Double Bonds Molecule Dot Notation Calculation 6(N) + 2 = VE 6(N) + 2 = VE + 2 6(N) + 2 = VE + 4 Lewis Structure IBr CH3Br C2HCl SiCl4 F2O SO3 ONCl 4 Structural Formula CO O2 O3 SNI CHP N2O2 S2Si 5 Rules for Naming Binary Covalent Compounds A binary covalent compound is composed of two different nonmetal elements. For example, a molecule of chlorine trifluoride, ClF3 contains 1 atom of chlorine and 3 atoms of fluorine. Rule 1. The element with the lower group number is written first in the name; the element with the higher group number is written second in the name. Rule 2. If both elements are in the same group, the element with the higher period number is written first in the name. Rule 3. The second element in the name is named as if it were an anion, i.e., by adding the suffix -ide to the name of the element. Rule 4. Greek prefixes (see the table given to you in class) are used to indicate the number of atoms of each nonmetal element in the chemical formula for the compound. Exception: if the compound contains one atom of the element that is written first in the name, the prefix "mono-" is not used. Name the following covalent compounds. Formula Name Formula 1 NO3 9 NF3 2 N2O5 10 CO2 3 S2Cl2 11 SO3 4 XeO3 12 CCl4 5 Cl2O7 13 NH3 6 HBr 14 PO2 7 P4O10 15 SO2 8 P4O6 16 CO 6 Name Writing Formulas for Covalent Compounds Follow these steps for writing formulas for binary covalent compounds when you are given a systematic name. Notice that they are the reverse of the steps for writing names from chemical formulas. Write the symbols for the elements in the order mentioned in the name. Write subscripts indicated by the prefixes. If the first part of the name has no prefix, assume it is mono-. Write the formulas for these covalent compounds. Name Formula Name 1 Dinitrogen pentoxide 10 Tribromine octoxide 2 Carbon monoxide 11 Dichlorine pentoxide 3 Hydrogen iodide 12 Carbon tetrafluoride 4 Iodine bromide 13 Sulfur hexafluoride 5 Diphosphorus pentoxide 14 Carbon dioxide 6 Phosphorous tribromide 15 Carbon tetrahydride 7 Diboron silicide 16 Dinitrogen trioxide 8 Chlorine dioxide 17 Nitrogen trifluoride 9 Xenon tetrafluoride 18 Disilicon hexabromide Formula 7 Covalent Compound Scavenger Hunt 1) List three covalent objects that can be found in the sinks in this classroom: a) ________________________________________________ b) ________________________________________________ c) ________________________________________________ 2) Haikus are three line Japanese poems where the first line has five syllables, the second has seven syllables, and the third has five syllables. Write a haiku about how the electrons behave when a covalent compound is formed. 3) Find one example of an edible covalent compound somewhere in the book and give its name, molecular formula, and empirical formula. Name: ________________________________________________ Molecular formula: ____________________________________________ Empirical formula: ____________________________________________ 4) Give the names and molecular formulas of five covalent compounds that has “oxide” somewhere in the name. These compounds must actually exist, so don’t just make them up! a) ________________________________________________ b) ________________________________________________ c) ________________________________________________ d) ________________________________________________ e) ________________________________________________ 8 5) Describe how a blind person might determine if a compound is ionic or covalent if they were working alone in a laboratory. 6) Ask somebody who is not in your group the following question: “If you were a chemical, would you want to be ionic or covalent, and why?” Write their answer below: 7) Draw the Lewis structures of any three covalent molecules whose formulas can be found in the Appendix of your book: 9