Chemistry - Organic Compounds - Quick Guides

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Study GuideChemistry–Organic Compounds1. Quiz: Structural Formulas1. QuestionThe electron configuration for carbon isAnswer Choices•1s² 2s¹ 2p³•1s² 2s² 2p²•1s² 2s³ 2p¹Correct Answer1s² 2s² 2p²Why This is CorrectCarbon has an atomic number of6, which means it has6 electrons.These electrons fill orbitals in order of increasing energy.•1s orbital holds2 electrons•2s orbital holds2 electrons•The remaining2 electronsgo into the 2p orbitalSo, the correct electron configuration of carbon is1s² 2s² 2p².For ExampleHydrogen (atomic number 1) has the electron configuration1s¹,while oxygen (atomic number 8) has1s² 2s² 2p⁴.2. QuestionIn order to completely fill the valence shell, carbon wants how many bonds?

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Study GuideAnswer Choices•2•3•4Correct Answer4Why This is CorrectCarbon has4 valence electronsin its outer shell. To achieve astable octet (8 electrons), carbonneeds4 more electrons. It does this by formingfour covalent bondswith other atoms, sharingelectrons to completely fill its valence shell.For ExampleIn methane (CH₄), carbon formsfour single bondswith four hydrogen atoms, which gives carbon afull valence shell and makes the molecule stable.3. QuestionA carbon atom has __________ valence electrons and needs __________ electrons to fill thevalence shell orbitals.Answer Choices•4, 2•4, 4•2, 4Correct Answer4, 4

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Study GuideWhy This is CorrectCarbon has4 valence electronsin its outer shell.To achieve a stable octet (8 electrons in the valence shell), itneeds 4 more electrons.Therefore, the correct pair is4 valence electrons and needs 4 electrons.For ExampleCarbon formsfour covalent bonds(like in methane, CH₄) to complete its valence shell.4. QuestionIn a structural formula, __________ are used to depict two electrons in a chemical bond.Answer Choices•dots•two small e⁻•a single lineCorrect Answera single lineWhy This is CorrectIn a structural formula, asingle linerepresents a pair of shared electrons between two atoms, whichmakes up a chemical bond.For ExampleIn the structural formula of hydrogen (H—H), the single line between the two hydrogen atoms showsone shared pair of electrons.5. QuestionA molecular formula tells the

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Study GuideAnswer Choices•number and types of atoms in the molecule•arrangement of the atoms in the molecule•total number of bonds in the moleculeCorrect Answernumber and types of atoms in the moleculeWhy This is CorrectA molecular formula shows which elements are present in a molecule and how many atoms of eachelement it contains. It doesnotshow how the atoms are arranged or bonded.For ExampleThe molecular formulaH₂Otells us there are two hydrogen atoms and one oxygen atom, but it doesnot show their arrangement.6. QuestionThe same molecular formula can representAnswer Choices•only one specific molecule•several different isomers•the physical state of the moleculeCorrect Answerseveral different isomersWhy This is CorrectA molecular formula shows only the number and types of atoms present in a molecule.

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Study GuideIt doesnotshow how those atoms are arranged. Because atoms can be connected in different ways,the same molecular formula can represent different compounds calledisomers.For Example:C₂H₆O can represent ethanol or dimethyl ether.7. QuestionThe structure of a molecule affectsAnswer Choices•only the chemical properties of the compound•only the physical properties of the compound•both the chemical and physical properties of the compoundCorrect Answerboth the chemical and physical properties of the compoundWhy This is CorrectThe structure of a molecule determines how its atoms are arranged and bonded. This arrangementaffects how the molecule reacts with other substances (chemical properties) and also influencescharacteristics such as melting point, boiling point, shape, andsolubility (physical properties).For ExampleGlucose and fructose have the same molecular formula but different structures. Because of this, theyshow differences in both physical properties (such as sweetness and solubility) and chemicalbehavior.8. QuestionIn organic chemistry, structure is just as important as ________.Answer Choices•composition•isomerism•nomenclature

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Study GuideCorrect AnswercompositionWhy This is CorrectIn organic chemistry,compositiontells us what atoms are present in a compound, whilestructuretells us how those atoms are arranged. Both are equally important because compounds with thesame composition can have different structures and show different properties.For ExampleTwo compounds may both have the formula C₂H₆O, but one can be ethanol and the other dimethylether. They have the same composition, but different structures and different properties.9. QuestionWhat type of formula omits the carbon–hydrogen (C–H) bonds?Answer Choices•structural•molecular•condensed structuralCorrect Answercondensed structuralWhy This is CorrectAcondensed structural formulashows how atoms are connected but does not display everyindividual bond. Carbon–hydrogen (C–H) bonds are not written out; instead, hydrogen atoms aregrouped with the carbon atoms they are attached to.For ExampleEthane can be written asCH₃–CH₃in a condensed structural formula, instead of showing every C–Hbond separately.

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Study Guide10. QuestionIsopropyl alcohol andn-propanol have the same molecular formula, C₃H₇OH, yet their structures aredifferent. These compounds are known asAnswer Choices•alkenes•isomers•aldehydesCorrect AnswerisomersWhy This is CorrectIsomers are compounds that have thesame molecular formulabutdifferent structuralarrangementsof atoms. Although isopropyl alcohol andn-propanol both have the formula C₃H₇OH,the atoms are connected differently in each compound, giving them different structures andproperties.For ExampleButane and isobutane both have the molecular formula C₄H₁₀, but their structures are different, sothey are isomers.11. QuestionCarbon always forms __________ covalent bonds.Answer Choices•2•3•4

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Study GuideCorrect Answer4Why This is CorrectCarbon hasfour valence electronsin its outer shell. To achieve a stable octet (8 electrons), carbonshares electrons with other atoms and therefore formsfour covalent bonds. This bonding abilityallows carbon to form a wide variety of compounds.For ExampleIn methane (CH₄), one carbon atom forms four covalent bonds with four hydrogen atoms.2. Hydrocarbons2.1What Are Hydrocarbons?Hydrocarbons are compounds made using onlycarbonandhydrogenatoms.Even though they use just these two elements, hydrocarbons can forman enormous variety ofsubstances.These compounds are very important in everyday life. They make uppetroleum and natural gas,which are major sources of fuel and raw materials for industry.2.2Alkanes: Hydrocarbons with Single Bonds

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Study GuideHydrocarbons that containonly single covalent bonds between carbon atomsare calledalkanes.Examples include:•Propane•Butane•IsobutaneAlkanesdo notcontain:•Double bonds•Triple bonds•Ring structuresThese features make alkanes thesimplest class of hydrocarbons.As the number of carbon atoms increases, the number of possible structures also increases.2.3Isomers: Same Formula, Different StructuresWhen a molecule has more than one way to connect its carbon atoms, it formsisomers.Isomers have:•The same molecular formula•Different arrangements of carbon atomsThe identity of an isomer depends onhow the carbon atoms are bonded, not on how the moleculelooks when drawn.Understanding ButaneFigure 1. Both molecules are the same isomer of butane.

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Study GuideFigure 2. The condensed structural formula of butane.Sometimes molecules may look different in drawings, but they are still thesame compound.In butane:•A straight chain drawing and a bent chain drawing represent thesame isomer•Both have the samecondensed structural formulaSo, these drawings donotrepresent different isomers.2.4Alkenes: Hydrocarbons with Double BondsFigure 3. Ethylene—an alkene.Analkeneis a hydrocarbon that containsat least one carbon–carbon double bond.Ethylene (Ethene)•The simplest alkene•Molecular formula:C₂H₄Each carbon atom still formsfour bonds, filling its valence shell with eight electrons.

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