Binary AcidsContain hydrogen and a monoatomic anion (e.g. Cl-, S2-)Most common binary acids are halogen (e.g., HCl, HBr)Acid names:The prefix “hydro” + the halogen base name + the suffix “ic” + the word acidEx: HBr- Hydrobromic acidOxoacidsIf oxoanion name ends in:-ate-iteCorresponding acid ends in:-ic-ousPractice: Naming Compounds and Acids:Molecular compound, an ionic compound, or an acid.Name or give formulas for the compoundsK2Cr2O7Na3NNO2H2CrO4Sulfurous acidIron(II) phosphateLewis StructuresLewis TheoryOctet Rule- elements are going to seek to find a way to have 8 electrons around them (except for H and He)(Atoms tend to lose, gain, or share electrons to obtain a set of 8 valence electrons)Lewis SymbolsChemical symbol for an atom surrounded by one or more dots representing valence electrons“Dots” arranged around elemental symbolFirst 4 electrons = unpaired (top, sides, bottom)Next 4 added to form pairsExamples: Na (one valence e-), Mg (two e-)Lewis Symbols for ElementsUnpaired dots= bonding capacityMain Group Elements: Members of same family have same # valence electrons, similar bonding capacitiesLewis Structures: Ionic BondsA nonmetal and a metalMetals lose valence electrons to achieve noble gas electron configurationNonmetal gain electrons to achieve noble gas electron configurationLewis Structure: Molecular CompoundsBonding pair of electronsPair of electrons shared between two atoms in a covalent bondSingle bond: two atoms sharing one pair e-H:H H—HLone pair: pair of e- that is not sharedDrawing Lewis StructuresAs told by the book:Determine the # of valence electrons:Sum valence electrons for all atoms in molecule; add subtract electrons to account for ionic chargesArrange atoms in pattern that shows how they are bonded:Atom with largest bonding capacity in the center; other atoms arranged around central; lowest bonding capacity (H) on peripheryConnect atoms with single bondsComplete octets of atoms connected to central atom by adding lone pairsCompare the # of electrons in structure to the # determined in stepAs told by the professor:Draw the Lewis structure (for H2O and Ch4)“Play connect the dots:“Clean it up”Check to see if following the rulesMultiple BondsDouble Bond:Two electron pairs shared by two atomsRepresented as a double line (=)Triple Bond:Three electron pairs shared by two atomsRepresented as triple lineCHEM 111 1nd Edition Lecture 15 Outline of Last Lecture I. Binary Ionic CompoundsII. Common Polyatomic IonsIII. Naming Molecular CompoundsIV. Rules for Using PrefixesOutline of Current Lecture II. Binary AcidsIII. OxoacidsIV. Lewis StructuresV. Multiple BondsCurrent Lecture Binary Acids- Contain hydrogen and a monoatomic anion (e.g. Cl-, S2-)- Most common binary acids are halogen (e.g., HCl, HBr)- Acid names:o The prefix “hydro” + the halogen base name + the suffix “ic” + the word acido Ex: HBr- Hydrobromic acid Oxoacids- If oxoanion name ends in:o -ateo -ite- Corresponding acid ends in:o -ico -ousThese notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Practice: Naming Compounds and Acids:Molecular compound, an ionic compound, or an acid.Name or give formulas for the compoundsK2Cr2O7Na3NNO2H2CrO4Sodium carbonateSulfurous acidIron(II) phosphate Lewis Structures Lewis Theory- Octet Rule- elements are going to seek to find a way to have 8 electrons around them (except for H and He)(Atoms tend to lose, gain, or share electrons to obtain a set of 8 valence electrons) Lewis Symbols- Chemical symbol for an atom surrounded by one or more dots representing valence electrons- “Dots” arranged around elemental symbolo First 4 electrons = unpaired (top, sides, bottom)o Next 4 added to form pairso Examples: Na (one valence e-), Mg (two e-) Lewis Symbols for Elements Unpaired dots= bonding capacity Main Group Elements: Members of same family have same # valence electrons, similar bonding capacities Lewis Structures: Ionic Bonds- A nonmetal and a metalo Metals lose valence electrons to achieve noble gas electron configurationo Nonmetal gain electrons to achieve noble gas electron configuration Lewis Structure: Molecular Compounds- Bonding pair of electronso Pair of electrons shared between two atoms in a covalent bondo Single bond: two atoms sharing one pair e- H:H H—Ho Lone pair: pair of e- that is not shared Drawing Lewis Structures As told by the book:- Determine the # of valence electrons:o Sum valence electrons for all atoms in molecule; add subtract electrons to account for ionic charges- Arrange atoms in pattern that shows how they are bonded:o Atom with largest bonding capacity in the center; other atomsarranged around central; lowest bonding capacity (H) on peripheryo Connect atoms with single bonds- Complete octets of atoms connected to central atom by adding lonepairs- Compare the # of electrons in structure to the # determined in step As told by the professor:- Draw the Lewis structure (for H2O and Ch4)- “Play connect the dots:- “Clean it up”- Check to see if following the rules Multiple Bonds- Double Bond: o Two electron pairs shared by two atomso Represented as a double line (=)- Triple Bond:o Three electron pairs shared by two atomso Represented as triple
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