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UGA CHEM 1211 - Chemistry - Chapter 7 - 1

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Metathesis ReactionsMetathesis ReactionsMetathesis ReactionsGas-Formation ReactionsGas-Formation ReactionsGas-Formation ReactionsSlide 7Slide 8Comparison of Ionic and Covalent CompoundsSlide 10Slide 11Lewis Dot Formulas of AtomsSlide 13Ionic BondingSlide 15Slide 16Slide 17Slide 18Slide 19Slide 20Slide 21Slide 22Slide 23Slide 24Slide 25Slide 26Slide 27Slide 28Slide 29Slide 30Slide 31Slide 32Slide 33Slide 34Slide 35Slide 361Metathesis Reactions•Precipitation Reactions •Molecular equation(s)3)aq(3aq)(32(aq)23CaCO +KNO 2 COK + )Ca(NO 2Metathesis Reactions•Molecular equation 2(s)43)aq(aq)(43(aq)2POCa +NaCl 6 PONa 2 + CaCl 3 3Metathesis Reactions•Molecular equation•2H+ + 2Cl- + 2Na+ + SO3(2-)  2Na+ + 2Cl- + H20 + SO2–2H+ + SO3 (2-)  H20 + SO2–Cl & Na = Spectator ions   g22)aq(aq)(32(aq)SO O H+NaCl 2 SONa + HCl2 4Gas-Formation Reactions•A gas-formation reaction is a type of reaction in which there is a formation of an insoluble or slightly soluble gas when there are no gaseous reactants.•Displacement reactions in which an active metal displaces from an acid or from water are gas-formation reactions; they are not metathesis reactions.•Only common gases that are very soluble in water are HCl and NH3.5Gas-Formation Reactions•Consider hydrochloric acid with calcium carbonate to form carbonic acid.Formula Unit2HCl(aq) + CaCO3 (s)  H2CO3 (aq) + CaCl2 (aq)Total Ionic2[H+(aq) + Cl-(aq)]  H2CO3 (aq) + CaCO3 (s) + [Ca2+(aq) + 2Cl-(aq)]Net Ionic2H+(aq) + CaCO3 (s)  H2CO3 (aq) + Ca2+(aq)6Gas-Formation Reactions•Enough heat is generated in the reaction to cause thermal decomposition of carbonic acid.H2CO3 (aq)  CO2 + H2O(l)•The net effect of the chemical reaction and subsequent decomposition is2HCl(aq) + CaCO3 (s)  CO2 + H2O(l) + CaCl2 (aq)7•Chemical bonding refers to the attractive forces that hold atoms together in compounds. •The electrons involved in bonding are usually those in the outermost (valence) shell.Ch. 7 Chemical Bondingend of chapter problems (partial list): 1,2,4 6,8, 10, 16, 20, 23, 24, 30, 38, 44, 46, 52, 578•Chemical bonds are classified into two types:oIonic bonding results from electrostatic attractions among ions, which are formed by the transfer of one or more electrons from one atom to another.oCovalent bonding results from sharing one or more electron pairs between two atoms.9Comparison of Ionic and Covalent Compounds•Melting point comparison –Ionic compounds are usually solids with high melting points•Typically > 400oC–Covalent compounds are gases, liquids, or solids with low melting points•Typically < 300oC•Solubility in polar solvents (remember like dissolves like)–Ionic compounds are generally soluble–Covalent compounds are generally insoluble10•Solubility in polar solvents–Ionic compounds are generally soluble–Covalent compounds are generally insoluble•Solubility in nonpolar solvents–Ionic compounds are generally insoluble–Covalent compounds are generally soluble•Conductivity in molten solids or liquids–Ionic compounds generally conduct electricity•They contain mobile ions–Covalent compounds generally do not conduct electricity11•Conductivity in aqueous solutions–Ionic compounds generally conduct electricity•They contain mobile ions–Covalent compounds are poor conductors of electricity•Formation of Compounds–Ionic compounds are formed between elements with large differences in electronegativity•Often a metal and a nonmetal–Covalent compounds are formed between elements with similar electronegativities•Usually two or more nonmetals12Lewis Dot Formulas of Atoms•The # and arrangements of e in the outermost shells of atoms determine the chemical and physical properties of the elements as well as the kinds of chemical bonds they form.•Lewis dot formulas or Lewis dot representations are a convenient bookkeeping method for tracking valence electrons.–Chemical bonding involves only the valence e which are usually the e in the outermost occupied s and p orbitals. They are chemically important.Table 7-1, p. 25214Ionic BondingFormation of Ionic CompoundsIonic bonding is the attraction of oppositely charged ions (cations [+] and anions [-]) in large numbers to form a solid. Such a solid cpd is called an ionic solid.•An ion is an atom or a group of atoms possessing a net electrical charge.•Ions come in two basic types:1. positive (+) ions or cations•These atoms have lost 1 or more electrons.2. negative (-) ions or anions•These atoms have gained 1 or more electrons.15Clicker Q: How many valence e does Cl have?•Monatomic ions consist of one atom.•Examples:–Na+, Ca2+, Al3+ - cations–Cl-, O2-, N3- -anions•Polyatomic ions contain more than one atom.–NH4+ - cation–NO2-,CO32-, SO42- - anionsClicker Q: How many valence e does C have?16•Ionic bonds are formed by the attraction between cations and anions, usually, to form solids.•When the electronegativity difference (∆EN), between 2 elements is large (as between a metal and a nonmetal), the elements are likely to form a compound by ionic bonding.•Commonly, metals react with nonmetals to form ionic compounds.•The formation of NaCl is one example of an ionic compound formation.172Li + F2 → 2LiF•The underlying reason for the formation of LiF lies in the electron configurations of Li and F. 1s 2s 2p Li  F  _These atoms form ions with these configurations. Li+  same configuration as [He] F- same configuration as [Ne]18•We can also use Lewis dot formulas to represent the neutral atoms and the ions they form.19•The Li+ ion contains two electrons, same as the helium atom. –Li+ ions are isoelectronic with helium.•The F- ion contains ten electrons, same as the neon atom.–F- ions are isoelectronic with neon. •Isoelectronic species contain the same number of electrons.20•The reaction of potassium with bromine is another example of a group IA metal with a Group VIIA non metal.–Write the reaction equation, then Lewis dot, then e config21•There is a general trend evident in the formation of these ions.•Cations become isoelectronic with the preceding noble gas.•Anions become isoelectronic with the following noble gas.22•In general for the reaction of IA


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